Download Question Bank for Pre Board Exam(XII Chemistry)

SOLID STATE
1. Which kind of defect is found in KCL crystal?
2. Why urea has a sharp melting point but glass does not have?
3. A NaCl crystal is found to have Cs Cl structure. Guess how it might have happened?
4. Why is Frenkel defect not found in pure alkali metal halides?
5. NaCl and Cs Cl have similar formula. Then why they have different structures?
6. Non-stoichiometric cuprous oxide,CU2O can be prepared in laboratory.
In this oxide, copper to oxygen ratio is slightly less than 2:1.Can you account for the fact that
the substance is a p-type semiconductor?
7. In a crystalline solid ,anions C are arranged in cubic close packing . Cations A occupy 50%of the
tetrahedral voids and cations B occupy 50% of the octahedral voids .
What is the formula of the soiids?
8. How many lattice points are presents in ECC unit cell?
9.What kind of interaction are present in the molecular crystalline solid?
10.Write a similarities and difference between metallic and ionic crystal.
11.What is meant by the term ‘forbidden zone’ in reference to band theory of solids ?
12.’Crystaline solids are anisotropic in nature.’What does this statement mean ?
13.Which stoichiometric defect in crystals increases the density of a solid ?
14.What type of semiconductor is obtained when silicon is doped with arsenic ?
15.Give an example of an ionic compound which shows Frenkel defect.
16.Name the non-stoichiometric point defect responsible for colour in alkali halides.
17.Name the crystal defect which lowers the density of an ionic crystal.
18.What is the maximum possible coordinatin number of an atom in an hcp crystal
structure of an element ?
19.What is the number of tetrahedral voids in a unit cell of a cubic close-packed
structure ?
20.What is the co-ordination number of an octahedral voids ?
21.What is the formula of a compound in which the element Y forms ccp lattice and atoms of X
occupy 1/3rd of tetrahedral voids.
22.Nam the type of point defect that occur in a crystal of Zinc sulphide.
23.In Nacl Crystal, Cl- ions are in fcc arrangement calculate the number of Cl- ions in its unit
cell.
24.What type of crystal defect is produced when Nacl is doped with MgCl2.
25. How does the electrical conductivity of metallic conductors vary with temperature
26.What type of stochiometric defect is shown by (i) ZnS and (ii) CsCl?
27.What is the coordination number for
(a) an octahedral void
(b) a tetrahedral void.
28.Arrange simple cubic, bcc and fcc lattice in decreasing order of the fraction
unoccupied space.?
of the
29.What are anisotropic substances?
30.Why are amorphous solids isotropic in nature?
31.Why glass is regarded as an amorphous solid?
32What type of stochiometric defect is shown by (i) ZnS and (ii) CsCl?
33.If the formula of a compound is A2B, which sites would be occupied by A ions?
34.What is the coordination number for (a) an octahedral void (b) a tetrahedral void.
35. How many octahedral voids are there in 1 mole of a compound having cubic closed
packed structure?
36.Arrange simple cubic, bcc and fcc lattice in decreasing order of the fraction of the
unoccupied space.
37.In Corundum, O2– ions from hcp and Al3+ occupy two third of octahedral voids. Determine
the formula of corundum.
38.Why is Frenkel defect not found in pure alkali metal halides?
39.Which point defect is observed in a crystal when a vacancy is created by an atom missing
from a lattice site.
40. Why does conductivity of silicon increase with the rise in temperature?
41.Name the crystal defect which lowers the density of an ionic crystal.
42 What makes the crystal of KCl sometimes appear violet?
43 Which point defect in ionic crystal does not alter the density of the relevant solid?
44.Name one solid in which both Frenkel and Schottky defects occur.
45.Which type of defects are known as thermodynamic defects?
46.In a p-type semiconductor the current is said to move through holes.Explain.
47. Solid A is very hard, electrical insulator in solid as well as in molten state and melts at
extremely high temperature. What type of solid is it?
48. What are anistropic substances.
49Why are amorphous solids isotropic in nature?
50.Why glass is regarded as an amorphous solid?
51. Define the term 'crystal lattice.’
52. Define the term voids.
53.What type of stochiometric defect is shown by (i) ZnS and (ii) CsCl?
[Hint. : (i) Frenkel defect (ii) Schottky defect]
54. If the formula of a compound is A2B, which sites would be occupied by A ions?
[Hint. : Number of A ions is double to B ions, so ions will occupy tetrahedral voids]
55. What is the coordination number for
(a) an octahedral void
(b) a tetrahedral void.
[Hint. : (a) 6; (b) 4 ]
*56. How many octahedral voids are there in 1 mole of a compound having cubic closed packed
structure?
[Ans. : 1 mole]
13. Arrange simple cubic, bcc and fcc lattice in decreasing order of the fraction of the unoccupied
space.
[Hint. : fcc < bcc < sc]
57. How much space is empty in a hexagonal closed packed solid?
58. An element crystallises separately both in hcp and ccp structure. Will the two structures have the
same density? Justify your answer.
[Hint : Both crystal structures have same density because the percentage of occupied space is
same.]
58.. In NaCl crystal, Cl– ions form the cubic close packing. What sites are occupied by Na+ ions.
59. In Corundum, O2– ions from hcp and Al3+ occupy two third of octahedral voids. Determine the
formula of corundum. [Ans. : Al2O3]
60.. Why is Frenkel defect not found in pure alkali metal halides?
61. Which point defect is observed in a crystal when a vacancy is created by an atom missing from
a lattice site.
62. Define the term ‘doping’.
63. Why does conductivity of silicon increase with the rise in temperature.
64. Name the crystal defect which lowers the density of an ionic crystal.
[Ans. : Schottky defect]
65. What makes the crystal of KCl sometimes appear violet?[Hint : F-Centre]
66. Which point defect in ionic crystal does not alter the density of the relevant solid?
67. Name one solid in which both Frenkel and Schottky defects occur.
68. Which type of defects are known as thermodynamic defects?
[Ans. : Stoichiometric defects]
69. In a p-type semiconductor the current is said to move through holes. Explain.
70. Solid A is very hard, electrical insulator in solid as well as in molten state and melts at extremely
high temperature. What type of solid is it?
[Hint : Covalent solid]
2marks
1What type of stoichiometric defect is shown by (i) ZnS and (ii) CsCl?
2.If the formula of a compound is A2B, which sites would be occupied by A ions?
3.What is the coordination number for
(a) an octahedral void
(b) a tetrahedral void.
4.Give suitable reason for the following–
(a) Ionic solids are hard and brittle.
(b) Copper is malleable and ductile.
5. Account for the following :
(a) Glass objects from ancient civilizations are found to become milky in appearance.
(b) Window glass panes of old buildings are thicker at the bottom than at the top.
6. What happens when ferrimagnetic Fe3o4is heated to 850 K and why?
7. Give reasons:
(a)Why is frenkel defect found in AgCl?
(b)What is the difference between Phosphorus doped and Gallium doped semiconductor?
8. If radius of an atom of element is 150pm and it crystallizes as FCC lattices .
What is the face length of unit cell?
9. Sodium metal crystallizes in body centred cubic lattice with the cell edge=4.29 A0
What is the radius of sodium atom?
10. The composition of a sample of wustite is Fe 0.93O 1.00
What percentage of the iron is present in the form of Fe(III)?
11. In terms of band theory, what is the difference
(i) between conductor and an insulator.
(ii) between a conductor and a semi conductor.
12. If NaCl is doped with 10-3 mol % of SrCl2,what is the concentration of cation vacancies?
13. Silver crystallizes with face centred cubic unit cell has a length of 439pm.
What is the radius of an atom of silver?
(Assume that each face of atom is touching the four corner atoms)
Atoms of element B form hcp lattice and those of the element A occupy 2/3rd of
tetrahedral voids. What is the formula of the compound formed by these elements A
and B ?
15.Explain the following terms with suitable examples of each:
(i)
Ferromagnetism
(ii)
Antiferromagnetism
16.Gold (atomic radius=0.144 nm) crystallises in a face centered unit cell. What is the
length of a side of the cell ?
17.Silver forms ccp lattice and X-ray studies of its crystals show that the edge length of
its unit cell is 408.6 pm. Calculate the density of silver. (Atomic mass= 107.9 u)
18.What type of defect can arise when a solid is heated ? Which physical property is
affected by it and in what way ?
19.Calculate the packing efficiency in body centered cubic solid.
20.Gold crystallises in fcc structure. Each side of this unit cell has a length of 407 pm.
Calculate the atomic mass of gold if its density is 19.47 g cm-3. (NA=6.02 X 1023)
21.The edge of fcc unit cell of Al is 404 pm. Calculate the radius of Aluminium ion.
14.
1. Calculate the distance between Na+ and Ci- ion in NaCl crystal if the density is 2.165g/cc.
(molar mass of NaCl=58.5g/mol.)
1.
2.
3.
4.
A copper crystal has a face centred cubic structure Atomic radius of the copper
atom is 128 pm. Calculate the density of copper. (Atomic mass of copper= 63.5)
Classify the following as either a p-type or n-type semi-conductor.
(i)
Ge doped with In (ii) B doped with Si
Explain the following
(i) Zinc oxide is white but it turns yellow on heating
(ii) Frenkel defect is not found in pure alkali metal halides
5.
Explain the following with suitable examples
(i) Ferromagnetism
(ii) Ferrimagnetism
Define F–centre. Mention its one consequence ?
2.
In a fcc arrangement of A and B atoms A are present at the corners of the unit cell and B
are present at the face centres. If one atom of A is missing from its position at the
corner, what is the formula of the compound?
1. Explain how electrical neutrality is maintained in compounds showing Frenkel and
Schottky
defect.
2. Gold crystallizes in an FCC unit cell. What is the length of a side of the cell(r=0.144mm)
3. Classify each of the following as either a p-type or n-type semi-conductor.
a) Ge doped with In
b) B doped with Si
4. In terms of band theory what is the difference between a conductor, an insulator and a
semiconductor?
5. CaCl2 will introduce Scotty defect if added to AgCl crystal. Explain
6. What type of substances would make better permanent magnets, ferromagnetic or
7. ferromagnetic, why?
8. In a crystalline solid, the atoms A and B are arranged as follows:a. Atoms A are arranged in ccp array.
b. Atoms B occupy all the octahedral voids and half of the tetrahedral voids. What is the
9. In compound atoms of element Y forms ccp lattice and those of element X occupy 2/3rd
of
tetrahedral voids. What is the formula of the compound?
10. Silver forms ccp lattice and X –ray studies of its crystal show that the edge length of its
unit cell is 408.6 pm. Calculate the density of silver (Atomic wt= 107.9u).
11. Explain how you can determine the atomic mass of an unknown metal if you know its
mass density and the dimensions of unit cell of its crystal.
12. Calculate the packing efficiency of a metal crystal for a simple cubic lattice.
13. Define the following terms in relation to crystalline solids:
(i) Unit cell
(ii) Coordination number
Give one example in each case
14. Account for the following:
(i) Schottky defects lower the density of related solids.
(ii) Conductivity of silicon increases on doping it with phosphorus.
15. Aluminium crystallises in an fcc structure. Atomic radius of the metal is 125 pm. What is
the length of the side of the unit cell of the metal?
1. List four distinctions between crystalline and amorphous solids with one example of each.
2. Give suitable reason for the following–
(a) Ionic solids are hard and brittle.
(b) Copper is malleable and ductile.
3. Define F–centre. Mention its one consequence.
4. What is packing efficiency. Calculate the packing efficiency in body-centered cubic crystal.
5. Explain :
(a) List two differences between metallic and ionic crystals.
(b) Sodium chloride is hard but sodium metal is soft.
6. Account for the following :
(a) Glass objects from ancient civilizations are found to become milky in appearance.
(b) Window glass panes of old buildings are thicker at the bottom than at the top.
7. Why is graphite soft lubricant and good conductor of electricity?
8. What do you understand by the following types of stacking sequences :
(a) AB AB ............... (b) A B CABC .................
What kind of lattices do these sequences lead to?
9. Derive the formula for the density of a crystal whose length of the edge of the unit cell is known?
10. Explain how much portion of an atom is located at
(a) corner
(b) body centre
(c) face-centre and (d) edge centre of a cubic unit
cell.
11. In a fcc arrangement of A and B atoms A are present at the corners of the unit cell and B are
present at the face centres. If one atom of A is missing from its position at the corner, what is the
formula of the compound?
[Ans. :
A7B24]
12. A compound made up of elements ‘A’ and ‘B’ crystallises in a cubic close packed structure.
Atoms A are present on the corners as well as face centres, whereas atoms B are present on the
edge-centres as well as
body centre. What is the formula of the compound?
[Ans.
AB]
13. Explain the terms :
(a) Intrinsic semiconductor
(b) Extrinsic semiconductor.
14. Explain how vacancies are introduced in a solid NaCl crystal when divalent cations are added to
it.
15. What is meant by non-stoichiometric defect? Ionic solids which have anionic vacancies due to
metal excess defect develop colour. Explain with the help
of suitable example.
16. Define the term ‘point defects’ Mention the main difference between stoichiometric and nonstoichiometric point defects.
17. A compound MpXq has cubic close packing (ccp) arrangement of X. Its unit cell structure is show
below :
Determine the empirical formula of the compound.
[Ans :
MX2]
18. The concentration of cation vacancies in NaCl crystal doped with CdCl2 is found to be 6.02 x
1016 mol–1. What is the concentration of CdCl2 added to it?
[Ans : 10–5
mol% CdCl2]
19. Iron changes its crystal structure from body contred to cubic close backed structure when heated
to 916°C. Calculate the ratio of the density of the BCC crystal to that of CCP crystal. Assume that the
metallic radius of the
atom does not change.
[Ans : 1]
3marks
1. Write the relationship between atomic radius (r) and edge length (a) of
cubic unit cell for
(a) Simple cubic unit cell
(b) Body-centred cubic unit cell
(c) Face-centred cubic unit cell
2. Define a semiconductor? Describe the two main types of semiconductors
when it is doped with
(a) group 13 element, (b) group 15 element.
3. Explain the following terms with one example each :
(a) Ferrimagnetism (b) Antiferromagnetism
(c) 13-15 compounds
4. Examine the defective crystal lattice given below and answer the following
questions :
(a) Name the crystal defect present in ionic solid.
(b) Out of AgCl and NaCl, which is most likely to show this type of defect and why?
(c) Why this defect is also known as dislocation defect?
5. Tungsten crystallizes in body centred cubic unit cell. If the edge of the unit
cell is 316. 5pm, calculate the radius of tungsten atom?
1. Alluminium crystallizes in a cubic close packed structure. Its metallic radius is 125pm.
(a)What is the length of the side of the unit cell?
(b)How many unit cells are there in 1.00 cm 3 of aluminium?
[3]
2.The unit cell of an element of atomic mass 108 and density 10.5 gcm-3 is a cube with edge length 409
pm.
Find the structure of the crystal lattice (simple cubic, FCC or BCC)
[3]
3. What is a semiconductor? Describe the two main types of semiconductors and explain mechanisms
for their conduction.
4. Silver crystallises with face-centred cubic unit cells. Each side of the unit cell has a length of 409 pm.
What is the radius of an atom of silver? (Assume that each face atom is touching the four cor ner
atoms.)
5. The density of copper metal is 8.95 g cm–3. If the radius of copper atom be 127.8 pm, is the copper unit
cell simple cubic, body-centred cubic or face-centred cubic?
(Given: atomic mass of Cu = 63.54 g mol–1 and NA = 6.02 × 1023 mol–1)
6.(a). Explain how you can determine the atomic mass of an unknown metal if you know its mass density
and the dimensions of unit cell of its crystal.
(b)Calculate the packing efficiency of a metal crystal for a simple cubic lattice.
1. Silver crystallises in a fcc lattice. If the edge length of the unit cell is 4.07 X 10-8 cm and
density of silver is 10.5 g cm-3, calculate the atomic mass of silver.
( NA = 6.02 X 1023 atoms mol-1 )
2. (i)
Phosphorus doped silicon is a semiconductor.
(ii)
Schottky defect lowers the density of a solid.
(iii) Some of the very old glass objects appear slightly milky instead of being
transparent.
3. (a)
With reference to crystal structure, what is meant by coordination number ?
(b)
What is the coordination number of atoms
(i) in a cubic closed packed structure,
(ii)in a body centered cubic structure ?
4. How will you distinguish between the following pairs of terms ?
(a) Hexagonal close packing and cubic close packing
(b) Crystal lattice and Unit cell
(c) Tetrahedral void and octahedral void.
5. Determine the type of cubic lattice to which a given crystal belongs if it has edge length
of 290 pm and density is 7.80 g cm-3.
(Molecular mass = 56 g mol-1)
6.
7.
8.
12.
Niobium Crystallizes in a body centred cubic structure. It is density is 8.55 g cm3
. Calculate atomic radius of niobium, given that its atomic mass is 93 u.
A Sample of ferrous oxide has actual formula Fe0.93O1.00. In this sample what
fraction of metal ions are Fe2+ ions? What type of non-stoichiometric defect is
present in this sample?
Copper crystallizes in face centred cubic lattice and has density of 8-93 g/cm3.
Calculate the radius of copper atom (At. Mass of cu = 63.5u, Avogadro’s constant
NA = 6.02 x 1023 mol-1)
An element crystallises in a cubic close packed structure having a fcc unit cell of an edge
200 pm. Calculate the density if 200 g of this element contain 24 × 1023 atoms?
1. An element crystallizes in FCC structure; 200 g of this element has 4.12X 1024 atoms. If
the
density of A is 7.2g cm, calculate the edge length of unit cell.
2. Niobium crystallizes in bcc structure. If its density is 8.55 cm–3, calculate atomic radius of
[At.Mass of Niobium = 92.9u, NA = 6.022x 1023 atoms mol –1].
3. If radius of octahedral void is r and radius of atom in close packing is R, derive the
relationshipbetween r and R.
4. Non stoichiometric cuprous oxide can be prepared in the laboratory. In this oxide,
copper to
oxygen ratio is slightly less than 2:1 can u account for the fact that the substance is a ptype
semiconductor?
5. The unit cell of an element of atomic mass 50u has edge length 290pm. Calculate its
density the element has bcc structure (NA =6.022x 1023 atoms mol –3).
6. Calculate the density of silver which crystallizes in face centered cubic form. The
distance
between nearest metal atoms is 287pm (Ag= 107.87g mol –1, NA= 6.022x 1023 atoms mol
–1
).
7. What is the distance between Na+ and Cl –ions in NaCl crystal if its density 2.165g cm–3.
NaCl crystallizes in FCC lattice.
8. Analysis shows that Nickel oxide has Ni 0.98 O 1.00 what fractions of nickel exist as Ni2+
ions and Ni3+ ions?
9. Find the type of lattice for cube having edge length of 400pm, atomic wt. = 60 and
density=6.25g/cc.
10. Niobium (Nb) crystallizes in a body-centred cubic (bcc) structure. If its density is 8.55 g
cm-3 ,
Calculate the atomic radius of niobium. (Atomic mass of Nb = 93 u; NA = 6.02 x1023 mol 1
)
11. Explain with suitable examples the following:
(a) n-type and p-type semiconductors
(b) F-centre
(c) Ferromagnetism
12. How would you account for the following?
a) Frenkel defects are not found in alkali metal halides.
b) Schottky defects lower the density of related solids.
c) Impurity doped silicon is a semiconductor.
13. What is a semiconductor? Describe the two main types of semiconductors and explain
mechanisms
for their conduction.
14. Iron has a body-centred cubic unit cell with a cell edge of 286.65 pm. The density of iron
is 7.87g cm–3.
Use this information to calculate Avogadro’s number (At. mass of Fe = 56g mol–1).
15. Silver crystallises with face-centred cubic unit cells. Each side of the unit cell has a length
of 409 pm. What is the radius of an atom of silver? (Assume that each face atom is
touching the four corner atoms.)
16. The well known mineral fluorite is chemically calcium fluoride. It is known that in one
unit cell of this mineral there are 4 Ca2+ ions and 8 F– ions and that Ca2+ ions are
arranged in a fcc lattice. The F– ions fill all the tetrahedral holes in the face centred
cubic lattice of Ca2+ ions. The edge of the unit cell is5.46 × 10–8 cm in length. The density
of the solid is 3.18 g cm–3. Use this information to calculate Avogadro's number (Molar
mass of CaF2 = 78.08 g mol–1)
17. The density of copper metal is 8.95 g cm -3 . If the radius of copper atom is 127.8 pm, is
the copper unit cell a simple cubic, a body-centred cubic or a face-centred cubic
structure? (Given: At. mass of Cu=63.54 g mol -1 and NA = 6.022 × 1023 mol -1)
18. The density of copper metal is 8.95 g cm–3. If the radius of copper atom be 127.8 pm, is
the copper unit cell simple cubic, body-centred cubic or face-centred cubic? (Given:
atomic mass of Cu = 63.54 g mol–1 and NA = 6.02 × 1023 mol–1)
19. Silver crystallises in fcc lattice. If the edge length of the unit cell is 4.07 × 10–8 cm and the
density of the crystal is 10.5 g cm–3, calculate the atomic mass of silver. (NA = 6.02 ×
1023 atoms mol–1)
20. 1. Write the relationship between atomic radius (r) and edge length (a) of cubic unit cell for
21.
(a) Simple cubic unit cell
22.
(b) Body-centred cubic unit cell
23.
(c) Face-centred cubic unit cell
24. (a) a = 2r (b) a = 4/√3 r (c) a = 2 √2r
25.
26. 2. Define a semiconductor? Describe the two main types of semiconductors when it is doped
with
27.
(a) group 13 element,
(b) group 15 element.
28. 3. Explain the following terms with one example each :
29.
(a) Ferrimagnetism
(b) Antiferromagnetism (c) 13-15 compounds
30. 4. Tungsten crystallizes in body centred cubic unit cell. If the edge of the unit cell is 316.
5pm, calculate the
radius of tungsten atom?
31. 5. Iron has a body centred cubic unit cell with a cell dimension of 286.65 pm. The density of
iron is 7.874 g cm–3. Use this information to calculate Arogadro number.
32. (At. Mass of Fe = 55.845u).
VALUE BASED QUESTION (4 MARKS)
1. Ram lives in a village of Hariyana.His vallage gets electricity for 6 to 8 hours at
night.Hehas used solar panels to produce electricity.He uses CFL and LED lamps in stead
of bulbs and tube lights which save lots of electricity. After reading this passage, answer
the following questions:
(a) What values are associated with Ram?
(b) What is meant by photovoltaic material? Give one example.
(c) Why is solar power generation is better than thermal power plants?
(d) Why is solar power not popular in India?
2. Mr.Sahu has heavy machines in his factory which he maintains regularly by getting them
serviced and used graphite powder as lubricant. Mr.Roy also has heavy machines in his
factory but he does not get them tuned using lubricants. His machines make a lot of
noise and do not work efficiently. After reading this passage, answer the following
questions:
(a) What are the values associated with Mr. Sahu which Mr.Roy does not have?
(b) Why is graphite a suitable lubricant for machines? Give two reasons.
(c) Why should we get our machines serviced regularly?
(d) Is graphite crystalline or amorphous solid?Give its shape.
5marks
1.The well known mineral fluorite is chemically calcium fluoride. It is known that in one unit
cell of this mineral there are 4 Ca2+ ions and 8F– ions and that Ca2+ ions are arranged in afcc
lattice. The F– ions fill all the tetrahedral holes in the fcc lattice of Ca2+ ions. The edge of the unit
cell is 5.46 ×
10–8 cm in length. The density of the solid is 3.18 g cm–3. Use this information to
calculate Avogadro’s number (Molar mass of CaF2 = 78.08 g mol–1]
2. The density of copper metal is 8.95 g cm–3. If the radius of copper atom
is 127 pm, is the copper unit cell a simple cubic, a body-centred cubic or
a face centred cubic structure?
3. A metallic element has a body centered cubic lattice. Edge length of unit cell is 2.88 × 10–8
cm. The density of the metal is 7.20 gcm–3. Calculate
(a) The volume of unit cell.
(b) Mass of unit cell.
(c) Number of atoms in 100 g of metal.
SOLUTION
1. Give an example of ‘liquid in solid’ type solution
2. Which type of solid solution will result by mixing two solid components with large
difference in the sizes of their molecules?
3. What is meant by semimolar and decimolar solutions?
4. What will be the mole fraction of water in C2H5OH solution containing equal number of
moles of water and C2H5OH?
5. Which of the following is a dimensionless quantity : molarity, molality or mole fraction?
6. 1. Measurement of which colligative property is preferred for determination of molar mass of
biomolecules?
7. 2. State Raoult’s law for a solution containing volatile components.
8. 3. Define osmotic pressure.
9. 4. What is meant by reverse osmosis?
10. 5. State the main advantage of molality over molarity as the unit of concentration.
11. 5. Why are aquatic species more comfortable in cold water than in warm water?
12. 6. Out of 1M sugar solution and 1M urea solution which have higher boiling point?
13. 7. Give reason when 30ml ethanol and 30ml water are mixed the volume of the solution is more
than 60ml.
14. 8. Why do doctors advise gargles by saline water in case of sore throat?
15. How is molality of a solution different from its molarity ?
16. Define osmotic pressure.
17. What is meant by reverse osmosis ?
18. State Raoult’s law for a solution containing volatile components.
19. What is the expected value of van’t Hoff factor for K3[Fe(CN)6] in dilute solution ?
20. Of 0.1 molal solution of glucose and sodium chloride respectively, which one will have a
21.
22.
23.
24.
25.
26.
27.
higher boiling point ?
Define Henry’s law about solubility of gas in a liquid.
What change is observed in boiling point of a liquid at higher altitude ?
Why do doctors advise gargles by saline water in case of sore throat /
Why is osmotic pressure considered as a colligative property ?
A mixture of chlorobenzene and bromobenzene forms nearly ideal solution but a
mixture of chloroform and acetone does not. Why?
2.
If kf for water is 1.86 K kg mol–1, what is the freezing point of 0.1 molal solution
of a substance which undergoes no dissociation or association of solute?
3.
Liquid ‘Y’ has higher vapour pressure than liquid ‘X’, which of them will have
higher boiling point?
28.
29. Give an example of ‘liquid in solid’ type solution.
30. Which type of solid solution will result by mixing two solid components with large
difference in the sizes of their molecules?
31. What is meant by semimolar and decimolar solutions?
32. What will be the mole fraction of water in C2H5OH solution containing equal number of
moles of water and C2H5OH?
33. Which of the following is a dimensionless quantity : molarity, molality or mole fraction?
34. 6. 10 g glucose is dissolved in 400 g. of solution. Calculate percentage concentration of
the solution.
35. 7. Gases tend to be less soluble in liquids as the temperature is raised.
36.
37.
38.
39.
Why?
State the conditions which must be satisfied if an ideal solution is to be formed.
A mixture of chlorobenzene and bromobenzene forms nearly ideal solution but a
mixture of chloroform and acetone does not. Why?
How is the concentration of a solute present in trace amount in a solutionexpressed?
N2 and O2 gases have KH values 76.48 kbar and 34.86 kbar respectively at 293 K
temperature. Which one of these will have more solubility in water?
What are isotonic solutions?
Why do doctors advise patients with high blood pressure to take less common salt?
Give one use of Revese osmosis?
What is the effect of temperature on solubility of the gas in liquid?
Why osmotic pressure is a colligative properties?
40.
41.
42.
43.
44.
45. 1. Give an example of ‘liquid in solid’ type solution.
46. 2. Which type of solid solution will result by mixing two solid components with large
difference in the sizes of their molecules?
47. 3. What is meant by semimolar and decimolar solutions?
48. 4. What will be the mole fraction of water in C2H5OH solution containingequal number of
moles of water and C2H5OH?
[Ans. : 0.5]
49. 5. Which of the following is a dimensionless quantity : molarity, molality or mole fraction?
50.
[Ans. :
mole fraction]
51. 6. 10 g glucose is dissolved in 400 g. of solution. Calculate percentage concentration of the
solution
52.
[Ans. :
2.5% w/w]
53. 7. Gases tend to be less soluble in liquids as the temperature is raised. Why?
54. 8. State the conditions which must be satisfied if an ideal solution is to be formed.
55. 9. A mixture of chlorobenzene and bromobenzene forms nearly ideal solution but a mixture
of chloroform and acetone does not. Why?
56. 10. How is the concentration of a solute present in trace amount in a solution expressed?
57. *12. N2 and O2 gases have KH values 76.48 kbar and 34.86 kbar respectively at 293 K
temperature. Which one of these will have more solubility in water?
58. *13. Under what condition molality and molarity of a solution are identical.Explain with
suitable reason.
59. *14. Addition of HgI2 to KI (aq.) shows decrease in vapour pressure. Why?
60. 15. What will happen to the boiling point of the solution formed on mixing two miscible liquids
showing negative deviation from Raoult’s law?
61. 16. Liquid ‘Y’ has higher vapour pressure than liquid ‘X’, which of them will have higher
boiling point?
62. 17. When 50 mL of ethanol and 50 mL of water are mixed, predict whether the volume of the
solution is equal to, greater than or less than 100 mL.Justify.
63. 18. Which type of deviation is shown by the solution formed by mixing cyclohexane and
ethanol?
64. 19. A and B liquids on mixing produce a warm solution. Which type of deviation from Raoult’s
law is there?
65. 20. Define cryoscopic constant (molal freezing point depression constant.)
66. 21. Mention the unit of ebulioscopic constant (molal boiling point elevation constant.)
67. 22. If kf for water is 1.86 K kg mol–1, what is the freezing point of 0.1 molal solution of a
substance which undergoes no dissociation or association of solute?
68. [Hint : Tf = iKf . m]
69. 24. What is reverse osmosis? Give one large scale use of it.
70. *25. What is the maximum value of van’t Hoff factor (i) for Na2SO4 . 10H2O?
71. [Ans. : i = 3]
72. 26. What is the value of van’t Hoff factor (i) if solute molecules undergo
73. dimerisation. [Ans. : i = 0.5]
74. 27. Under what condition is van’t Hoff factor less than one?
75. [Ans. : Association]

2marks
1Explain the following :
(a) Solubility of a solid in a liquid involves dynamic equilibrium.
(b) Ionic compounds are soluble in water but are insoluble in nonpolar solvents
2. Give two examples each of a solution :
(a) showing positive deviation from Raoult’s Law.
(b) showing negative deviation from Raoult’s Law.
3. Draw vapour pressure vs composition (in terms of mole fraction) diagram
for an ideal solution.
4. Define azeotropes with one example of each type.
5. Draw the total vapour pressure vs. mol fraction diagram for a binary solution exhibiting nonideal behaviour with negative deviation.
(i)Ideal solution
(ii)Azeotrope
2 .A solution of glucose (C6H12O6) in water is labeled as 10% by weight. What would be the
Molality of the solution?(Molar mass of glucose = 180 g mol–1)
3. 1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of
benzene by 0.40 K. Find the molar mass of the solute. (Kf for benzene = 5.12 kg mol–1)
4. The density of water of a lake is 1.25 g (mL)–1and 1kg of this water contains 92g of Na+ions.
What is the molarity of Na+ions in the water of the lake ? (Atomicmassof Na = 23.00 u)
5. Why do gases always tend to be less soluble in liquids as the temp. is raised?
6. At 25°C the saturated vapour pressure of water is 3.165 kPa(23.75 mm Hg).Find the saturated vapour
pressure of a 5% aqueous solution of urea (car amide) at the same temperature.(Molar mass of urea =
60.05 g
mol–1)
7. Explain the following:
(i) Henry’s law about dissolution of a gas in a liquid.
(ii) Boiling point elevation constant for a solvent.
8. Non-ideal solutions exhibit either positive or negative deviations from Raoult's law. What are these
deviations and why are they caused? Explain with one example for each type
1. A sugar syrup of weight 214.2 g contains 34.2 g of sugar (C12H22O11). Calculate (i)
mole fraction of sugar, (ii) molality of sugar syrup.
2. (a) Solution of NaCl boils at higher temperature than water. Explain.
(b) Why do doctors advise people with high blood pressure to take less common
salt ?
3. Derive the relationship between relative lowering of vapour pressure and mole fraction of
the volatile liquid.
4. What type of deviation (positive or negative ) from ideal behaviour will be shown by the
solution of cyclohexane and ethanol ? Give suitable reason.
5. 0.5 g of KCl was dissolved in 100g water and the solution originally at 200C, froze at 0.240C.Calculate the percentage ionization of salt.(Kf per 1000 g of water =1.86 K/m)
6. State Henry’s law. Why do gases tend to be less soluble in liquids as the
temperature is raised.
7. What are positive and negative deviations from Raoult’s law. Explain with one
example for each.
8. Calculate the amount of benzoic acid required for preparing 250 ml of 0.15 m
solution in methanol.
9. (i)
What would be the value of Van’t Hoff factor for a dilute solution of K2SO4
in water ?
(ii) Which of the following has higher boiling point and why?
10. Define Azeotropes and explain briefly minimum boiling and maximum boiling
azeotrope with suitable example.
11. Benzene and toluene form a nearly ideal solution. At a certain temperature, calculate
the vapour pressure of solution containing equal moles of the two substances.
12. [Given : P°Benzene = 150 mm of Hg, P°Toluene = 55 mm of Hg]
13. 2.
When 1 mole of NaCl is added to 1 litre water, the boiling point increases? When
1 mole of CH3OH is added to 1 litre water, the boiling point decreases? Suggest reasons.
1. State Henry’s law correlating the pressure of a gas and its solubility in a solvent and
mention two applications of the law.
2. State Raoult’s law for solutions of volatile liquids. Taking suitable examples explain the
meaningof positive and negative deviations from Raoult’s law.
3. Define the term osmotic pressure. Describe how the molecular mass of a substance can
be determined by a method based on measurement of osmotic pressure?
4. Define osmotic pressure. How is it that measurement of osmotic pressures is more
widely used for determining molar masses of macromolecules than the rise in boiling
point or fall in freezing point of their solutions?
5. Derive an equation to express that relative lowering of vapour pressure for a solution is
equal to the mole fraction of the solute in it when the solvent alone is volatile.
6. Differentiate between molality and molarity of a solution. What is the effect of change
in temperature of a solution on its molality and molarity?
7. Non-ideal solutions exhibit either positive or negative deviations from Raoult's law.
What are these deviations and why are they caused? Explain with one example for each
type.
8. Define the terms, ‘osmosis’ and ‘osmotic pressure’. What is the advantage of using
osmotic pressureas compared to other colligative properties for the determination of
molar masses of solutes in solutions.
9. State the following:
(i) Raoult’s law in its general form in reference to solutions.
(ii) Henry’s law about partial pressure of a gas in a mixture.
10 Differentiate between molarity and molality of a solution. Explain how molarity value of
a solution can be converted into its molality.
11 A 0.561 m solution of an unknown electrolyte depresses the freezing point of water by
2.93°C. What is Van’t Hoff factor for this electrolyte? The freezing point depression
constant (Kf) for water is 1.86°C kg mol–1.
12 A 1.00 molal aqueous solution of trichloroacetic acid (CCl3COOH) is heated to its boiling
point. The solution has the boiling point of 100.18°C. Determine the van’t Hoff factor for
trichloroacetic acid. (Kb for water = 0.512 K kg mol–1)
13 Define the following terms:
(i) Mole fraction (ii) Isotonic solutions
(iii) Van’t Hoff factor (iv) Ideal solution
12 (a) Define any two of the following terms:
(i) van’t Hoff factor (ii) Mole fraction
(iii) Ebullioscopic constant
(b) State Raoult’s law.
13 The density of water of a lake is 1.25 g (mL)–1 and one kg of this water contains 92 g of
Na+ ions. whatis the molarity of Na+ ions in the water of the lake? (Atomic mass of Na =
23.00 u)
14 18 g of glucose, C6H12O6 (Molar Mass = 180 g mol–1) is dissolved in 1 kg of water in a
sauce pan. At what temperature will this solution boil? (Kb for water = 0.52 K kg mol–1,
boiling point of pure water = 373.15 K)
15 Henry’s law constant (kH) for the solution of methane in benzene at 298 K is 4.27 ×105
mm Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.
16 (i) Why is an increase in temperature observed on mixing chloroform and acetone?
(ii) Why does sodium chloride solution freeze at a lower temperature than water?
17. Write the anode and cathode reactions occurring in a commonly used mercury cell. How
is the overall reaction represented?
1. Explain the following :
(a) Solubility of a solid in a liquid involves dynamic equilibrium.
(b) Ionic compounds are soluble in water but are insoluble in nonpolar solvents.
2. Give two examples each of a solution :
(a) showing positive deviation from Raoult’s Law.
(b) showing negative deviation from Raoult’s Law.
3. Draw vapour pressure vs composition (in terms of mole fraction) diagram for an ideal solution.
4. Define azeotropes with one example of each type.
5. Draw the total vapour pressure vs. mol fraction diagram for a binary solution exhibiting non-ideal
behaviour with negative deviation.
6. The vapour pressure curve for three solutions having the same non-volatile solute in the same
solvent are shown. The curves are parallel to each other and do not intersect. What is the correct
order of the concentrations of the solutions.
[Hint. : A < B
< C]
7. Show that the relative lowering of vapour pressure of a solvent is a colligative property.
8. Benzene and toluene form a nearly ideal solution. At a certain temperature, calculate the vapour
pressure of solution containing equal moles of the two substances.
[Given : P°Benzene = 150 mm of Hg, P°Toluene = 55
mm of Hg]
9. What is meant by abnormal molecular mass? Illustrate it with suitable examples.
*10. When 1 mole of NaCl is added to 1 litre water, the boiling point increases? When 1 mole of
CH3OH is added to 1 litre water, the boiling point decreases? Suggest reasons.
11. Can we separate water completely from HNO3 solution by vapourisation? Justify your answer.
*12. 1 gram each of two solutes ‘A’ and ‘B’ (molar mass of A > molar mass of B) are dissolved
separately in
100 g each of the same solvent. Which solute will show greater elevation in boiling point and Why?
13. How relative lowering in vapour pressure is related with depression in
freezing point and elevation in boiling point?
3marks
1.Write the relationship between atomic radius (r) and edge length (a) of
cubic unit cell for
(a) Simple cubic unit cell
(b) Body-centred cubic unit cell
(c) Face-centred cubic unit cell
2. Define a semiconductor? Describe the two main types of semiconductors
when it is doped with
(a) group 13 element, (b) group 15 element.
3. Explain the following terms with one example each :
(a) Ferrimagnetism (b) Antiferromagnetism
(c) 13-15 compounds
4. Examine the defective crystal lattice given below and answer the following
questions :
(a) Name the crystal defect present in ionic solid.
(b) Out of AgCl and NaCl, which is most likely to show this type of defect and why?
(c) Why this defect is also known as dislocation defect?
5. Tungsten crystallizes in body centred cubic unit cell. If the edge of the unit
cell is 316. 5pm, calculate the radius of tungsten atom?
1. What mass of ethylene glycol (molar mass = 62.0 g mol–1) must be added to 5.50 kg of
water to lower the freezing point of water from 0°C to – 10.0°C? (Kf for water = 1.86 K kg mol–1)
2. Calculate the freezing point depression for 0.0711 m aqueous solution of sodium sulphate, if it is
completely ionised in solution. If this solution actually freezes at – 0.320 °C, what is the value of Van’t
Hoff factor for it at the freezing point? (Kf for water is 1.86°C mol–1)
3. Calculate the temperature at which a solution containing 54 g of glucose, (C6H12O6 ), in 250 g of water
will
freeze. (Kf for water =1.86 K mol-1 kg)
4. 5.100 mg of a protein is dissolved in enough water to make 100 mL of a solution. If this solution
has an osmotic pressure 13.3 mm Hg at 25° C, what is the molar mass of protein?
(R = 0.0821 L atm mol–1 K–1 and 760 mm Hg = 1 atm.)
5.Derive an equation to express that relative lowering of vapour pressure for a solution is equal to
the mole fraction of the solute in it when the solvent alone is volatile.
6.What concentration of nitrogen should be present in a glass of water at room temperature? Assume a
temperature of 25° C, total pressure of 1 atmosphere and mole fraction of nitrogen in air of 0.78. [KH
for
nitrogen = 8.42 × 10–7 M/mm Hg]
7.Calculate the freezing point depression for 0.0711 m aqueous solution of sodium sulphate, if it is
completely ionised in solution. If this solution actually freezes at – 0.320 °C, what is the value of
Van’t
Hoff factor for it at the freezing point? (Kf for water is 1.86°C mol–1)
1. 2 g of benzoic acid ( C6H5COOH) dissolved in 25 g of benzene shows a depression in
freezing point equal to 1.62 K. Molal depression constant for benzene is 4.9 K kg
mol-1. What is the percentage association of acid if it forms dimer in solution ?
2. 45 g of ethylene glycol (C2H6O2) is mixed with 600 g of water.
Calculate:
(a) Freezing point of depression, (b) freezing point of the solution ( Kf for water = 1.86 K
kg mol-1; Atomic mass : C=12, H=1, O=16u)
3. Explain the following :
(i)
Freezing point depression constant for a solvent
(ii)
Effect of pressure on solubility of gas in liquid
(iii) Maximum boiling azeotropes
4. (i)
Define ebullioscopic constant.
(ii)
What are isotonic solutions ? Give one example.
(iii)
Why should intravenous injections be isotonic with body fluids ?
5. (a)
What is the effect of temperature on vapour pressure of a liquid ?
(b)
Calculate the molal lowering of vapour pressure of water at 100 0C. Vapour
pressure of pure water is 760 mm Hg.
A solution containing 30g of non-volatile solute exactly in 90g of water has a vapour pressure of
2.8 kPa at 298 K. Furhter, 18 g of water is then added to the solution and the new
vapour pressure becomes 2.9 kPa at 298 K. Calculate :
(i) molar mass of the solute
(ii) Vapour pressure of water at 298 K.
1 (a) State Henry’s Law.
(b) If O2 is bubbled through water at 393 K, how many millimoles of O2 gas would be
dissolved in 1L of water? Assume that O2 exerts a pressure of 0.95 bar. (Given KH for O2
= 46.82 bar at 393K).
2 Given reason for the following :–
(a) Aquatic species are more comfortable in cold waters than in warm waters.
(b) To avoid bends scuba divers use air diluted with helium.
(c) Cold drinks bottles are sealed under high pressure of CO2.
3 Why should a solution of a non-volatile and non-eletrolyte solute boil at a higher
temperature? Explain with the help of a diagram. Derive the relationship between molar
mass and elevation in boiling point.
4 Account for the following :–
(a) CaCl2 is used to clear snow from roads in hill stations.
(b) Ethylene glycol is used as antifreeze solution in radiators of vehicles in cold
countries.
(c) The freezing point depression of 0.01 m NaCl is nearly twice that of 0.01 m glucose
solution.
5 Why do colligative properties of solution of a given concentration are found to give
abnormal molecular weight of solute. Explain with the help of suitable examples.
6 Give reasons for the following :–
(a) RBC swell up and finally burst when placed in 0.1% NaCl solution.
(b) When fruits and vegetables that have been dried are placed in water, they slowly
swell and return to original form.
7. Calculate the temperature at which a solution containing 54 g of glucose, (C6H12O6 ), in
250 g of water will freeze. (Kf for water =1.86 K mol-1 kg)
8. Calculate the amount of KCl which must be added to 1 kg of water so that its freezing
point is depressed by 2 K.
(Kf for water =1.86 K kg mol-1, Atomic mass K = 39, Cl = 35.5)
9. 100 mg of a protein is dissolved in just enough water to make 10.0 mL of solution. If this
solution has an osmotic pressure of 13.3 mm Hg at 25oC, what is the molar mass of the
protein?
(R = 0.0821 L atm mol–1 K–1 and 760 mm Hg = 1 atm.)
10. Calculate the freezing point depression expected for 0.0711m aqueous solution of Na
2SO4 . If this solution actually Freezes at -0.320°C, what would be the value of van't Hoff
factor? (Kf for water is 1.86°C mol -1).
11. A solution prepared by dissolving 1.25 g of oil of winter green (methyl salicylate) in 99.0
g of benzene has a boiling point of 80.31°C. Determine the molar mass of this
compound. (B.P. of pure Benzene = 80.10°C and Kb for benzene = 2.53°C kg mol–1)
12. A solution of glycerol (C3H8O3; molar mass = 92 g mol -1) in water was prepared by
dissolving some glycerol in 500 g of water. This solution has a boiling point of 100.42°C.
What mass of glycerol was dissolved to make this solution? Kb for water = 0.512 K kg
mol -1.
13. What mass of NaCl (molar mass = 58.5 g mol–1) must be dissolved in 65 g of water to
lower the freezing point by 7.5°C? The freezing point depression constant, Kf for water
is 1.86 K kg mol–1 Assume van’t Hoff factor for NaCl is 1.87.
14. What mass of ethylene glycol (molar mass = 62.0 g mol–1) must be added to 5.50 kg of
water to lower the freezing point of water from 0°C to – 10.0°C? (Kf for water = 1.86 K
kg mol–1)
15. 15 g of an unknown molecular substance was dissolved in 450 g of water. The resulting
solution freezes at – 0.34°C. What is the molar mass of the substance? (Kf for water =
1.86 K kg mol–1).
16. A solution prepared by dissolving 8.95 mg of a gene fragment in 35.0 mL of water has an
osmotic pressure of 0.335 torr at 25°C. Assuming that the gene fragment is a nonelectrolyte, calculate its molar mass.
17. What mass of NaCl must be dissolved in 65.0 g of water to lower the freezing point of
water by 7.50°C? The freezing point depression constant (Kf) for water is 1.86 C/m.
Assume van’t Hoff factor for NaCl is 1.87. (Molar mass of NaCl = 58.5 g).
18. Calculate the amount of KCl which must be added to 1 kg of water so that the freezing
point is depressed by 2 K. (Kf for water = 1.86 K kg mol–1)
19. A solution of glycerol (C3H8O3) in water was prepared by dissolving some glycerol in 500
g of water. This solution has a boiling point of 100.42 °C while pure water boils at 100 °C.
What mass of glycerol was dissolved to make the solution?
(Kb for water = 0.512 K kg mol–1)
20. 15.0 g of an unknown molecular material was dissolved in 450 g of water. The resulting
solution was found to freeze at – 0.34 °C. What is the molar mass of this material? (Kf
for water = 1.86 K kg mol–1)
21. At 25°C the saturated vapour pressure of water is 3.165 kPa (23.75 mm Hg). Find the
saturated vapour pressure of a 5% aqueous solution of urea (carbamide) at the same
temperature. (Molar mass of urea = 60.05 g mol–1)
22. Calculate the freezing point depression expected for 0.0711 m aqueous solution of
sodium sulphate. If the solution actually freezes at – 0.320 °C, what is the actual value of
van’t Hoff factor at this temperature? (Kf for water = 1.86 K kg mol–1)
23. Determine the osmotic pressure of a solution prepared by dissolving 2.5 × 10–2 g of
K2SO4 in 2 L of water at 25oC, assuming that it is completely dissociated.(R = 0.082 L atm
K–1 mol–1, Molar mass of K2SO4 = 174 g mol–1).
1. (a) State Henry’s Law.
(b) If O2 is bubbled through water at 393 K, how many millimoles of O2 gas would be dissolved in 1L
of water? Assume that O2 exerts a pressure of 0.95 bar.
(Given KH for O2 = 46.82 bar at 393K).
2. Given reason for the following :–
(a) Aquatic species are more comfortable in cold waters than in warm waters.
(b) To avoid bends scuba divers use air diluted with helium.
(c) Cold drinks bottles are sealed under high pressure of CO2.
3. Why should a solution of a non-volatile and non-eletrolyte solute boil at a higher temperature?
Explain with the help of a diagram. Derive the relationship between molar mass and elevation in
boiling point.
4. Account for the following :–
(a) CaCl2 is used to clear snow from roads in hill stations.
(b) Ethylene glycol is used as antifreeze solution in radiators of vehicles in cold countries.
(c) The freezing point depression of 0.01 m NaCl is nearly twice that of 0.01 m glucose solution.
5. Why do colligative properties of solution of a given concentration are found to give abnormal
molecular weight of solute. Explain with the help of suitable examples.
6. Give reasons for the following :–
(a) RBC swell up and finally burst when placed in 0.1% NaCl solution.
(b) When fruits and vegetables that have been dried are placed in water, they slowly swell and return
to original form.
(c) A person suffering from high blood pressure is advised to take less amount of table salt.
*7. Glycerine, ethylene glycol and methanol are sold at the same price per kg. Which would be
cheaper for preparing an antifreeze solution for the radiator of an automobile? [Ans. : Methanol]
*8. Determine the correct order of the property mentioned against them :
(a) 10% glucose (p1), 10% urea (p2), 10% sucrose (p3) [Osmotic pressure]
(b) 0.1 m NaCl, 0.1 m urea, 0.1 m MgCl2 [Elevation in b.pt.]
(c) 0.1 m CaCl2, 0.1 m sucrose, 0.1 m NaCl [Depression in f.pt.]
9. For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in 100 g of water, the
elevation in boiling point at 1 atm pressure is 2°C. Assuming concentration of solute is much lower
than the concentration of solvent, determine the vapour pressure (mm of Hg) of the solution.
[Given : Kb for water = 0.76 kg mol–1] [Ans.: 724 mm
of Hg]
10. 15.0 g of an unknown molecular substance was dissolved in 450 g of water. The resulting
solution was fund to freeze at –0.34°C. What is the molar mass of this substance. (Kf for water =
1.86 K kg mol–1).
5marks
1. The well known mineral fluorite is chemically calcium fluoride. It is known that in one unit
cell of this mineral there are 4 Ca2+ ions and 8F– ions and that Ca2+ ions are arranged in afcc
lattice. The F– ions fill all the tetrahedral holes in the fcc lattice of Ca2+ ions. The edge of the unit
cell is 5.46 ×
10–8 cm in length. The density of the solid is 3.18 g cm–3. Use this information to calculate
Avogadro’s number (Molar mass of CaF2 = 78.08 g mol–1]
2. The density of copper metal is 8.95 g cm–3. If the radius of copper atom
is 127 pm, is the copper unit cell a simple cubic, a body-centred cubic or
a face centred cubic structure?
3. A metallic element has a body centered cubic lattice. Edge length of unit cell is 2.88 × 10–8
cm. The density of the metal is 7.20 gcm–3. Calculate
(a) The volume of unit cell.
(b) Mass of unit cell.
(c) Number of atoms in 100 g of metal.
1.(a) Differentiate between molarity and molality for a solution. How does a change in temperature
influence their values?
(b) Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of
water. (Molar mass of MgBr2= 184 g) (Kf for water = 1.86 K kg mol–1)
2.(a) Define the terms osmosis and osmotic pressure. Is the osmotic pressure of a solution a
colligative property? Explain.
(b) Calculate the boiling point of a solution prepared by adding 15.00 g of NaCl to 250.00 g of
water. (Kb for water = 0.512 kg mol–1),(Molar mass of NaCl = 58.44 g)
3 (a) Non-ideal solutions exhibit either positive or negative deviations from Raoult's law.What are
these deviations and how are they caused?
(b) What mass of NaCl (molar mass = 58.5 g mol–1) must be dissolved in 65g of water to lower
the freezing point by 7.50°C? The freezing point depression constant, Kf for water is 1.86 K kg
mol–1. Assume van't Hoff factor for NaCl is 1.87.
4.(a) Define the terms osmosis and osmotic pressure. What is the advantage of using osmotic
pressure as compared to other colligative properties for the determination of molar masses of
solutes in solution?
(b) A solution prepared from 1.25 g of oil of wintergreen (methyl salicylate) in 99.0 g of benzene
has a boiling point of 80.31°C. Determine the molar mass of this compound. (Boiling point of
pure benzene = 80.10°C and Kb for benzene = 2.53°C kg mol–1).
5. What is meant by:
(i) Colligative properties
(ii) Molality of a solution.
(b) What concentration of nitrogen should be present in a glass of water at room temperature?
Assume a temperature of 25° C, total pressure of 1 atmosphere and mole fraction of nitrogen in
air of 0.78. [KH for nitrogen = 8.42 × 10–7 M/mm Hg]
1. (a)
Assuming complete ionisation, calculate the expected freezing point of
solution prepared by dissolving 6.00 g of Glauber’s salt, Na2SO4.10 H2O in
0.1kg ofH2O. (Kf for H2O =1.86 K kg mol-1 )
[At. Mass of Na =23, S =32, O = 16, H = 1u]
(b) Two liquids X and Y boil at 110 0C and 130 0C respectively. Which of them has
higher vapour pressure at 50 0C ?
2. (a)
Define the following terms :
(i)
Mole fraction
(ii)
Van’t Hoff factor
(b) 100 mg of protein is dissolved in enough water to make 10.0 ml of a
Solution. If the solution has an osmotic pressure of 13.3 mm Hg at 25 0C, what
is the molar mass of protein ?
(R = 0.0821 L atm mol-1 K-1 and 760 mm Hg = 1 atm)
3. (a)
List any four factors on which the colligative properties of a solution depend.
(b)
Calculate the boiling point of one molar aqueous solution
(density =1.06 g ml-1) of KBr.
[ Given : Kb for H2O = 0.52 K kg mol-1, Atomic mass : K =39, Br =80 ]
4. 2O(a) Explain why a solution of chloroform and acetone shows negative deviation
from Raoult’s law.
(b)
Phenol associates in bezene to certain extent to form a dimer. A solution
containing 20g of phenol in 1.0 kg of benzene has its freezing point lowered
by 0.69 K. Calculate the fraction of phenol that has dimerised.
[Given Kf for benzene = 5.1 Km-1]
(a) Give reason for the following
7.
(i)
At higher altitudes, people suffer from a disease called anoxia
(ii)
When mercuric iodide is added to an aq. Solution of KI, the freezing point
is raised.
(b)
100 mg of a protein is dissolved in just enough water to make 10.0 ml of
solution. If this solution has an osmotic pressure of 13.3 mmHg at 250C,
what is the molar mass of the protein ?
(a)
Explain elevation in boiling point with the help of vapour pressure and
temperature curve of a solution and explain why it is elevated ?
(b)
Calculate the freezing point of a solution when 3 gm of CaCl2
(M=111g/mol) was dissolved in 100g of water, assuming CaCl2 undergoes
complete ionization.
8.
(a)
Define
(i) Molarity
(ii) Molality
(b)
A 5% solution (by mass) of cane sugar in water has a freezing point of 271
k. Calculate the freezing point of a 5% glucose in water if the freezing point of
pure water is 273.15 k.
9.
(a)
Why does vapour pressure of a liquid decreases when a non-volatile
solute is added to it ?
(b)
State Raoult’s law for dilute solution.
(c)
A solution containing 30 g of a non volatile solute exactly in 90 g water has
a vapour pressure of 2.8 kpa at 298 k. Further 18 g of water is then added to the
solution, the new vapour becomes 2.9 kps at 298 K. Calculate
(i)
Molar
mass of the solute
(ii)
Vapour pressure of the solute at 298 K
1. (a) Non-ideal solutions exhibit either positive or negative deviations from Raoult's law.
What are these deviations and how are they caused?
(b) What mass of NaCl (molar mass = 58.5 g mol–1) must be dissolved in 65g of water to
lower the freezing point by 7.50°C? The freezing point depression constant, Kf for water
is 1.86 K kgmol–1. Assume van't Hoff factor for NaCl is 1.87.
2. (a) Define the terms osmosis and osmotic pressure. What is the advantage of using
osmotic pressure as compared to other colligative properties for the determination of
molar masses of solutes in solution?
(b) A solution prepared from 1.25 g of oil of wintergreen (methyl salicylate) in 99.0 g of
benzene has a boiling point of 80.31°C. Determine the molar mass of this compound.
(Boiling point of pure benzene = 80.10°C and Kb for benzene = 2.53°C kg mol–1).
3. (a) Differentiate between molarity and molality for a solution. How does a change in
temperature influence their values?
(b) Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in
200 g of water. (Molar mass of
MgBr2= 184 g) (Kf for water = 1.86 K kg mol–1)
4. (a) Define the terms osmosis and osmotic pressure. Is the osmotic pressure of a solution
a colligative property? Explain.
(b) Calculate the boiling point of a solution prepared by adding 15.00 g of NaCl to 250.00
g of water. (Kb for water = 0.512 kg mol–1),(Molar mass of NaCl = 58.44 g)
5. (a) State the following:
(i) Henry’s law about partial pressure of a gas in a mixture.
(ii) Raoult’s law in its general form in reference to solutions.
(b) A solution prepared by dissolving 8.95 mg of a gene fragment in 35.0 mL of water has
an osmotic pressure of 0.335 torr at 25°C. Assuming the gene fragment is a nonelectrolyte,determine its molar mass.
6. (a) Differentiate between molarity and molality in a solution. What is the effect of
temperature change on molarity and molality in a solution?
(b) What would be the molar mass of a compound if 6.21g of it dissolved in 24.0 g of
chloroform form a solution that has a boiling point of 68.04°C. The boiling point of pure
chloroform is 61.7°C and the boiling point elevation constant, Kb for chloroform is
3.63°C/m
7. (a) Define the following terms:
(i) Mole fraction (ii) Ideal solution
(b) 15.0 g of an unknown molecular material is dissolved in 450 g of water. The resulting
solution freezes at – 0.34°C. What is the molar mass of the material? (Kf for water =
1.86 K kg mol–1)
8. (a) Explain the following:
(i) Henry’s law about dissolution of a gas in a liquid.
(ii) Boiling point elevation constant for a solvent.
(b) A solution of glycerol (C3H8O3) in water was prepared by dissolving some glycerol in
500 g of water. This solution has a boiling point of 100.42°C. What mass of glycerol was
dissolved to make this solution? (Kb for water = 0.512 K kg mol–1)
9. (a) State Raoult’s law for a solution containing volatile components. How does Raoult’s
law become a special case of Henry’s law?
(b) 1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing
point of benzene by 0.40 K. Find the molar mass of the solute. (Kf for benzene = 5.12 kg
mol–1)
10. (a) Define the following terms:
(i) Ideal solution (ii) Azeotrope (iii) Osmotic pressure
(b) A solution of glucose (C6H12O6) in water is labelled as 10% by weight. What would be
the molality of the solution? (Molar mass of glucose = 180 g mol–1)
(a) What are ideal solutions? Write two examples.
(b) Calculate the osmoic pressure in pascals exerted by a solution prepared by dissolving 1.0g of
polymer of molar mass 185000 in 450 mL of water at 37°C.
2. (a) Describe a method of determining molar mass of a non-volatile solute from vapour pressure
lowering.
(b) How much urea (mol. mass 60 g mol–1) must be dissolved in 50g of water so that the vapour
pressure at the room temperature is reduced by 25%? Also calculate the molality of the solution
obtained.
[Ans. : 55.55 g and
18.5 m]
3. (a) Why is the freezing point depression considered as a colligative property?
(b) The cryoscopic constant of water is 1.86 km–1. Comment on this statement.
(c) Calculate the amount of ice that will separate out on cooling solution containing 50 g of ethylene
glycol in
200 g H2O to –9.3°C. (Kf for water = 1.86 K kg mol–1) [Ans. : 38.71g]
4. (a) Define osmotic pressure.
(b) Why osmotic pressure is preferred over other colligative properties for the determination of
molecular masses of macromolecules?
(c) What is the molar concentration of particles in human blood if the osmotic pressure is 7.2 atm at
normal body temperature of 37°C?
ELECTROCHEMISTRY
1mark
1.
2.
3.
4.
5.
What is the EMF of the cell when the cell reaction attains equilibrium?
What is the electrolyte used in a dry cell?
How is cell constant calculated from conductance values?
What flows in the internal circuit of a galvanic cell.
Define electrochemical series.
1. Given that the standard electrode potential (E°) of metals are:
K+ K = – 2.93 V, Ag+ /Ag = 0.80V, Cu 2+ /Cu = 0.34 V, Mg2+ / Mg = −2.37V, Cr 3+ / Cr
= −0.74V,
Fe2+ / Fe = −0.44V.
Arrange these metals in an increasing order of their reducing power
2. Express the relation between conductivity and molar conductivity of a solution held in a cell
1. 3.Why conductivity of an electrolyte decreases with the decrease in concentration
2. What is meant by limiting molar conductivity ?
3. What is a primary cell ? Give an example.
4. State Faraday’s second law of electrolysis.
5. Write the correct representation of the cell :
2 Cr(s) + 3 Cd2+(aq)
2 Cr3+ (aq) + 3 Cd(s)
6. What is the sign of ∆G for electrolytic cell ?
7. Write Nernst equation for the reaction
8.
2 Cr(s) + 3 cd2+ (aq) 2 Cr3+(aq) + 3 cd(s)
9. 2.
Write any two advantages of a fuel cell
10. 3.
How many Faradyas of Charge are required to convert 1 mole cr2O72- to
3+
Cr .
11. 4.
Define Molar conductivity.
12. 5.
Rusting of ion is quicker in saline water than in ordinary water. Give
reason.
13. (2 Marks)
14. 6.
What type of battery is dry cell? Write the over all reaction occurring in dry
cell.
15. 7.
The conductivity of a 0.20 m solution of Kcl at 298 k is 0.0248 S cm-1.
Calculate its molar conductivity.
16. 8.
Calculate equilibrium constant for the reaction
17.
Fe(s) + Cd2+(aq) Fe2+(aq) + Cd(s)
18.
Given E0 Cd2+/cd = -0.40 v
E0 Fe2+/Fe = -0.44v
19. 9.
Define Kohlrausch’s Law. Mention one application of the law.
20. 10.
(a)
(i) Calculate the standard free energy change for the following
21.
reaction at 250C.
22.
Au(s) + Ca2+aq (1M) Au 3+ (aq, 1M) + Ca(s)
E 0 Au 3+ / Au = + 1.50v
E 0Ca 2+ / Ca = − 2.87v
23.
0
24. (ii) Predict whether the reaction will be spontaneous or not at 25 C. Which of the
above two half cells will act as an oxidizing agent and which one be a reducing
agent ?
25. (b)
The conductivity of 0.001 M acetic acid is 4 x 10-5 S/cm. Calculate the
dissociation constant of acetic acid, if Λ0m for acetic acid is 390.5 Scm2/mol.
26.
27. (11)
28.
(a)
Calculate ∆G 0 and log Kc for the following reaction at 298 K
2 Al( s ) + 3Cu 2 + (aq) → 2 A13+ (aq) + 3Cu ( s)
0
ECell
= 2.02v
Given
0
Using the E values of A and B, predict which is better for coating the
surface of iron
31.
[ E 0 ( Fe 2 + / Fe) = − 0.44v] to prevent corrosion and Why ?
0
2+
E 0 ( B 2 + / B ) = − 0.14v
32.
Given E ( A / A) = − 2.37v
29.
30. (b)
33.
34. 12.
Value Based Question
35. Manu and his father went to a shop to purchase a battery for their inverter. Shop
36.
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
Keeper showed them two types of batteries, one with lead plates and the other
with Cadmium plates. The battery with cadmium plates was more expensive.
Manu’s father wanted to purchase lead battery as it was cheaper.
(i)
As a student of Chemistry, why would you suggest to Manu’s father to buy
the expensive cadmium plate battery. Give two reasons.
(ii)
What are the values associated with the above decisions.
Express the relation between conductivity and molar conductivity of a solution.
What is primary cell? Give an example.
What is meant by ‘limiting molar conductivity’?
Express the relation between conductivity and molar conductivity of a solution held in a
cell?
Express the relation among the conductivity of solution in the cell, the cell constant and
the resistance of solution in the cell.
. What is the effect of temperature on molar conductivity?
2. Why is it not possible to measure single electrode potential?
3. Name the factor on which emf of a cell depends:4. What are the units of molar conductivity?
5. Write Nernst equation –
For the general cell reaction
aA+bB→cC+dD
6. What is the EMF of the cell when the cell reaction attains equilibrium?
7. What is the electrolyte used in a dry cell?
8. How is cell constant calculated from conductance values?
9. What flows in the internal circuit of a galvanic cell.
10. Define electrochemical series.
2marks
1. How can you increase the reduction potential of an electrode.?
For the reaction
Mn+(aq) + ne- → M (s)
2. Electrolysis of KBr(aq) gives Br2 at anode but KF(aq) does not give F2. Give reason.
3. What happens when a piece of copper is added to
(a) an aq solution of FeSO4
(b) anAq solution of FeCl3?
4. Define corrosion. Write chemical formula of rust
5. What is cell constant? How it is determined?
. Conductivity of 0.00241M acetic acid solution is 7.896 x10-5 S cm-1. Calculate its molar
conductivity in this
solution. If Λom For acetic acid is 390.5 S cm2 mol-1, what would be its dissociation constant?
2. In the button cells widely used in watches and other devices the following reaction takes
place:
Zn(s) + Ag2O+ H2O(l) →Zn+2 (aq) + 2Ag(s) + 2OH (aq)
Determine ∆G° for the reaction. (Given: E° Zn 2+ /Zn = -0.76 V and E° Ag +/ Ag = 0.34 V)
3. The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm-1. Calculate its molar
conductivity in this
solution.
4. What type of cell is a lead storage battery? Write the anode and the cathode reactions and the
overall cell
reaction occurring in the use of a lead storage battery.
5. Corrosion is essentially an electrochemical phenomenon. With the help of a diagram explain
the reactions
occurring during the corrosion of iron kept in open atmosphere. 2
6. Define the term molar conductivity and indicate how molar conductivity of a substance
changes with change
in Concentration of a weak electrolyte and a strong electrolyte in its solution
7. How many moles of mercury will be produced by electrolyzing 1.0 M. Hg (NO3)2 solution
with
a current of 2.00 A for 3 hours?
8. Write the anode and cathode reactions occurring in a commonly used mercury cell. How is the
overall
Reaction represented?
9. Determine the values of equilibrium constant (KC) and ∆G° for the following reaction:
Ni(s) + 2Ag+(aq) → Ni2+(aq) + 2Ag(s), E° = 1.05 V
(1 F = 96500 C mol–1)
10. The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S cm2 mol–1.
11. The electrical resistance of a column of 0.05 M NaOH solution of diameter 1 cm and length
50 cm is
5.55 × 103 ohm. Calculate its resistivity, conductivity and molar conductivity
12. A strip of nickel metal is placed in a 1-molar solution of Ni (NO3)2 and a strip of silver metal
is
Placed in a 1-molar solution of AgNO3. An electrochemical cell is created when the two
Solutions are connected by a salt bridge and the two strips are connected by wires to a
Voltmeter. Write the balanced equation for the overall reaction occurring in the cell and
calculate the
Cell potential
13. The conductivity of 0.20 M solution of KCl at 298 K is 0.025 S cm–1. Calculate it’s molar
Conductivity.
14.Calculate the time to deposit 1.27g of copperat cathode when a current of 2A was passed
through the
solution of CuSO4 .(Molar mass of Cu=63.5gmol ,1F=96500C mol-1 )
1. How much time would it take in minute to deposit 1.18 g of metallic copper on a metal
object when a current of 2.0 A is passed through the electrolytic cell containing Cu2+ ions
?
[Cu=63.5 g mol-1 , 1 F =96,500 C mol-1]
2. (a) Why does a dry cell become dead after a long time, even if it has not been used ?
(b) Why does a mercury cell gives a constant voltage throughout its life ?
3. How does molar conductivity vary with concentration for (i) weak electrolyte and for (ii)
strong electrolyte ? Give reason for these variations.
4. Calculate Ecell for the cell
Al I Al3+(0.01M) II Fe2+ (0.02M) I Fe
଴
଴
Given ‫ܧ‬஺௟
యశ /஺௟ = -1.66V and ‫ܧ‬ி௘ మశ /ி௘ = -0.44V
5. The conductivity of a 0.20m solution of KCl at 298 K is 0.o248 S cm-1.Calculate its
molar conductivity.
6. The conductivity of a 0.20 M solution of KCl at 298 K is 0.0248 S cm-1. Calculate its molar
conductivity
7. Formulate the galvanic cell in which the following reaction takes place:
Zn(s) + 2Ag + (aq) → Zn 2+ (aq) + 2Ag
State:
(i) Which one of its electrodes is negatively charged?
(ii) The reaction taking place at each of its electrode.
(iii) The carriers of current within this cell.
8. The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500ῼ.
What is the cell constant if the conductivity of 0.001 M KCl solution at 298 K is 0.146x103
S cm-1 ?
9. The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm-1. Calculate its molar
conductivity in this solution.
10. What type of cell is a lead storage battery? Write the anode and the cathode reactions
and the overall cell reaction occurring in the use of a lead storage battery.
11. Two half cell reactions of an electrochemical cell are given below:
MnO-4 (aq ) + 8H+ (aq ) + 5e →Mn+2 ( aq) + 4H O(l ), Eo = 1.51V
Sn 2+ (aq) = Sn 4+ (aq) + 2e- , E°= + 0.15 V
Construct the redox equation from the two half cell reactions and predict if this reaction
favours
formation of reactants or product shown in the equation.
12. Corrosion is essentially an electrochemical phenomenon. With the help of a diagram
explain the
reactions occurring during the corrosion of iron kept in open atmosphere.
13. Define the term molar conductivity and indicate how molar conductivity of a substance
changes with
change in concentration of a weak electrolyte and a strong electrolyte in its solution.
14. Express the relation among the cell constant, the resistance of the solution in the cell
and the
conductivity of the solution. How is the conductivity of a solution related to its molar
conductivity?
15. The chemistry of corrosion of iron is essentially an electrochemical phenomenon.
Explain the reactions occurring during the corrosion of iron in the atmosphere.
16. The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S cm2
mol–1.
Calculate the conductivity of this solution.
17. The conductivity of 0.20 M solution of KCl at 298 K is 0.025 S cm–1. Calculate its molar
conductivity.
1. How can you increase the reduction potential of an electrode.?
For the reaction
Mn+(aq) + ne-- → M (s)
2. Calculate emf of the following cell at 298K
Zn/Zn2+ (10-4 M) || Cu2+ (10-2M)/Cu
Given E0 Zn2+/Zn=-0.76V
E0Cu2+/Cu=+0.34V
Q 3. Electrolysis of KBr(aq) gives Br2 at anode but KF(aq) does not give F2. Give reason.
3. What happens when a piece of copper is added to
(a) an aq solution of FeSO4
(b) an Aq solution of FeCl3?
4. Define corrosion. Write chemical formula of rust. Corrosion is a process of
determination of metal as a result of its reaction with air and water, surrounding it. It is
due to formulation of
sulphides, oxides, carbonates, hydroxides, etc. Formula of rust- Fe2O.XH2O
5. Write short notes on reduction and oxidation potentials.
6. How are standard electrode potentials measured?
7. What is cell constant? How it is determined?
8. what is conductivity water
9. Why it is necessary to platinize the electrodes of a conductivity cell before it is used
for conductance measurement?
10. Why mercury cell gives the constant voltage.
11. What is fuel cell, write reaction involved in h2-o2 fuel cel.
3marks
1. Write any three differences between potential difference and e.m.f.
2. Why an electrochemical cell stops working after sometime?
3.For the standard cell
i. identify the cathode and the anode as the current is drawn from the cell.
ii. Write the reaction taking place at the electrodes.
1. iii. Calculate the standard cell potential.
4 Can we store copper sulphate in
(i)Zinc vessel
(ii) Silver vessel?
Give reasons.
Given
5 Define electrode potential. Why absolute value of reduction potential of
electrode cannot be determined?
. A copper-silver cell is set up. The copper ion concentration in it is 0.10 M. The concentration of
silver ion is
not known.The cell potential measured 0.422 V. Determine the concentration of silver ion in
the cell.
(Given: E 0 Ag+ /Ag. = 0.80V, E 0. Cu /Cu+ 2 = 0.34 V o
2. Three electrolytic cells A, B and C containing solutions of zinc sulphate, silver nitrate and
copper sulphate,
respectively are Connected in series. A steady current of 1.5 ampere was passed through
them until 1.45 g
of silver were deposited at the Cathode of cell B. How long did the current flow? What mass
of copper and
what mass of zinc were deposited in the Concerned cells? (Atomic masses of Ag = 108, Zn =
65.4, Cu = 63.5)
3 .A voltaic cell is set up at 25° C with the following half-cells Al3+ (0.001 M) and Ni2+ (0.50
M).
Write an equation for the reaction that occurs when the cell generates an electric current and
Determine the
cell potential. (Given: ENi /Ni2+ = –0.25 V, EAl /Al3+ = –1.66 V)
4. One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution
Of unknown concentration. The other half-cell consists of a zinc electrode in a 0.10 M
solution
Of Zn (NO3)2. A voltage of 1.48 V is measured for this cell. Use this information to calculate
the
Concentration of silver nitrate solution.(Given EZn 2+ /Zn = – 0.763 V, EAg+/Ag =0.80 V)
5 The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 Ω.
What
Cell constant if the conductivity of 0.001 M KCl solution at 298 K is 0.146 × 10–3 S cm–1?
6. Conductivity of 2.5 x 10-4 M methanoic acid is 5.25 x 10-5 S cm-1. Calculate its molar
conductivity and
degree of dissociation. Given: λ0(H+) = 349.5 Scm2mol-1 and λ0(HCOO-) = 50.5S cm2mol-1.
7 (a) Calculate ∆rGo for the reaction
Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s)
Given: Ecello = +2.71V, 1 F = 96500 C mol–1
(b) Name the type of cell which was used in Apollo space programme for providing electrical
Power
8.
1. Calculate ∆G0 and the equilibrium constant for the cell reaction :
Cl2 + 2I- → 2 Cl- + I2
଴
଴
ష =1.36 V , ‫ܧ‬ூ
Given ‫ܧ‬஼௟
= 0.536 V
మ /಺
మ /஼௟
2.
Calculate the number of coulombs required to deposit 12.7 g of copper when blue vitriol
is electrolysed.[At. Mass of copper = 63.5 g]
3. The electrical resistance of a column of diameter 2 cm and length 25 cm containing
0.01M NaOH solution is 6 X 10-4 ohms. Calculate its resistivity, conductivity, and molar
conductivity.
4. What is nickel-cadmium cell ? State its one merit and demerit over lead storage cell.
Write the overall reaction that occurs during discharging of this cell.
5. Molar conductivity at infinite dilution for NH4Cl, NaOH and NaCl solutions at 298 K are
respectively 129.8, 217.4 and 108.9 S cm2 mol-1 and ᴧ௠ of 10-2 M solution of NH4OH is
9.33 S cm2 mol-1 . Calculate the degree of dissociation of NH4OH.
6. Conductivity of 0.00241M acetic acid solution is 7.896 x10-5 S cm-1. Calculate its molar
conductivity in this solution. If ∆°୫ for acetic acid is 390.5 S cm2 mol-1, what would be
its dissociation constant?
7. Three electrolytic cells A, B and C containing solutions of zinc sulphate, silver nitrate and
copper sulphate, respectively are connected in series. A steady current of 1.5 ampere
was passed throug h them until 1.45 g of silver were deposited at the cathode of cell B.
How long did the current flow? What mass of copper and what mass of zinc were
deposited in the concerned cells? (Atomic masses of Ag = 108, Zn = 65.4, Cu = 63.5
8. In the button cells widely used in watches and other devices the following reaction takes
place :
Zn(s) + Ag2O+ H2O→ Zn+2 (aq) + 2Ag(s) + 2OH- (aq)
Determine ∆ rG° for the reaction.
(Given : E° Zn 2+ /Zn =0.76 V and E° Ag+/ Ag= 0.34 V)
9. Write the Nernst equation and determine the e.m.f. of the following cell at 298 K:
Mg (s) | Mg2+ (0.001M) | | Cu 2+ (0.0001M) | Cu (s)
(Given : E° Mg 2+ /Mg= -2.375 V, E° Cu 2+ /Cu = +0.34 V)
10. Define conductivity and molar conductivity for the solution of an electrolyte. How do
they vary when the concentration of electrolyte in the solution increases?
11. Corrosion is essentially an electrochemical phenomenon. Explain the reactions occurring
during corrosion of iron kept in an open atmosphere.
12. A copper-silver cell is set up. The copper ion concentration in it is 0.10 M. The
concentration of silver ion is not known. The cell potential measured 0.422 V. Determine
the concentration of silver ion in the cell.
(Given: E 0. Ag+ /Ag =80V, E 0 Cu+2 /Cu = 34 V)
1. Write any three differences between potential difference and e.m.f.
2. Why an electrochemical cell stops working after sometime?
3. for the standard cell
Cu(s)/Cu+(aq)|| Ag+(aq)/Ag(s)
E0 cell 2+/Cu = +0.34 V
E0 cell 2+ =+0.34 V
E0 Ag+/Ag =+0.80 V
i. identify the cathode and the anode as the current is drawn from the cell.
ii. Write the reaction taking place at the electrodes.
iii. Calculate the standard cell potential.
2. Can we store copper sulphate in (i)Zinc vessel (ii) Silver vessel? Give reasons.
Given E0 Cu2+/Cu = +0.34V, E0Zn2+/Zn= -0.76V) , E0Ag+/Ag = +0.80V
3. How many grams of chlorine can be produced by the electrolysis of molten NaCl with
a current of 1.02 A for 15 min?
4. What is understood by a normal hydrogen electrode? Give its significance.
5. Define electrode potential. Why absolute value of reduction potential of electrode
cannot be determined?
6. Write the equation showing the effect of concentration on the electrode potential.
7. Derive the relationship between Gibb’s free energy change and the cell potential.
8. How Nernst equation can be applied in the calculation of equilibrium constant of any
cell reaction.?
9. The cell reaction as written is spontaneous if the overall EMF of the cell is positive.
Comment on this statement.
5marks
1. Explain the term electrolysis. Discuss briefly the electrolysis of (i) molten
NaCl (ii) aqueous sodium chloride solution (iii) molten lead bromide (iv)
Water
2. state and explain Faraday’s laws of electrolysis. What is Electrochemical
equivalent?
3. What do you understand by ‘electrolytic conduction’? what are the factors
on which electrolyte conduction depends.? What is the effect of temperature
on electrolytic conduction?
4. Crude copper containing Fe and Ag as contaminations was subjected to
electro refining by using a current of 175 A for 6.434 min. The mass of anode
was found to decrease by 22.260 g, while that of cathode was increased by
22.011 g. Estimate the % of copper, iron and silver in crude copper.
.(a) Define molar conductivity of a substance and describe how for weak and strong electrolytes,
molar
conductivity changes With concentration of solute. How is such change explained?
(b) A voltaic cell is set up at 25 oC with the following half cells:
Ag+ (0.001 M) | Ag and Cu2+ (0.10 M) | Cu
What would be the voltage of this cell? (Eo cell = 0.46 V)
2.(a) State the relationship amongst cell constant of a cell, resistance of the solution in the cell
and conductivity
of the solution. How is molar conductivity of a solute related to conductivity of its solution?
(b) A voltaic cell is set up at 25oC with the following half-cells:
Al | Al3+ (0.001 M) and Ni | Ni2+ (0.50 M)
Calculate the cell voltage [Eo Ni2+/Ni = – 0.25 V, Eo Al/Al3+ = – 1.66 V]
3. (a) State Kohlrausch law of independent migration of ions. Write an expression for the molar
Conductivity of acetic acid at infinite dilution according to Kohlrausch law.
(b) Calculate Λ°m for acetic acid. Given that Λ°m (HCl) = 426 S cm2 mol–1Λ°
m (NaCl) = 126 S cm2 mol–1Λ°m (CH3COONa) = 91 S cm2 mol–1
4. (a) Write the anode and cathode reactions and the overall reaction occurring in a lead storage
battery.
(b) A copper-silver cell is set up. The copper ion concentration is 0.10 M. The concentration
of
Silver ion is not known. The cell potential when measured was 0.422 V. Determine the
Concentration of silver ions in the cell. (Given E 0.80V, E 0.34 V)
5. The standard electrode potential (E°) for Daniel cell is + 1.1 V. Calculate the ∆G° for the
reaction
Zn(s) + Cu 2 + (aq) → Zn 2 + (aq) + Cu(s)
(1 F = 96500 C mol–1).
6. Calculate the emf of the following cell at 25oC:
Ag(s) Ag+ (10–3 M) | | Cu 2 + (10–1 M) | Cu (s)
(Given Ecello = + 0.46 V and log 10n = n.)
7. (a) State Kohlrausch’s law of independent migration of ions. Mention one application of
Kohlrausch’s law.
(b) The resistance of a conductivity cell containing 10–3 M KCl solution at 25ºC is 1500 Ω.
What is
The cell constant if conductivity of 10–3 M KCl solution at 25°C is 1.5 × 10–4 S cm–1?
1. (a) The molar conductivity of 1.5 M solution of an electrolyte is found to be 138.9 S cm2
mol-1. Calculate the conductivity of solution.
(b) Define conductivity and molar conductivity for the solution of an electrolyte. Discuss
their variation with concentration.
2. (a) Explain with one example each the terms weak and strong electrolytes.
(b)Write the Nerst equation and calculate the emf of the following cell :
Fe(s) I Fe2+(0.001M) II (1M) I H2(g) I Pt (s)
଴
(‫ܧ‬ி௘
మశ/ಷ೐ =-0.44 V)
3. (a) (i) Represent the galvanic cell in which the reaction
Zn(s) + 2Ag+(aq)→ Zn2+(aq) + 2 Ag(s) takes place.
(ii) Which electrode is negatively charged ?
(iii)Write reaction taking place at each electrode.
(b)Calculate the number of coulombs required for the oxidation 1 mole of water to
oxygen as per the equation :
2H2O→ 4H+ + O2 +4e4. What type of battery is lead storage battery ? Write the anode and cathode reactions and
overall cell reaction occurring in the operation of a lead storage battery.
5. (a) State the relationship amongst cell constant of a cell, resistance of the solution in the
cell and conductivity of the solution. How is molar conductivity of a solute related to
conductivity of its
solution?
(b) A voltaic cell is set up at 25oC with the following half-cells:
Al / Al3+ (0.001 M) and Ni / Ni2+ (0.50 M)
Calculate the cell voltage [Eo Ni2+/Ni = – 0.25 V, E oAl/Al3+ = – 1.66 V]
6. What type of a cell is the lead storage battery? Write the anode and the cathode
reactions and the overall reaction occurring in a lead storage battery while operating.
(b) A voltaic cell is set up at 25°C with the half-cells Al | Al3+ (0.001 M) and Ni | Ni2+ (0.50
M).
Write the equation for the reaction that occurs when the cell generates an electric
current and
determine the cell potential.(Given: Eo Ni2+ /Ni = –0.25V, Eo Al3+ Al =–1.66V).
7. (a) Express the relationship amongst cell constant, resistance of the solution in the cell
and
conductivity of the solution. How is molar conductivity of a solute related to
conductivity of its solution.
(b) Calculate the equilibrium constant for the reaction.
Fe(s) + Cd2+ (aq ) ⇌ Fe+2 (aq) + Cd(s) (Given: Eo Cd2+/ Cd= – 0.40V,EoFe+2 /Fe = -0.44V)
8. (a) Define the term molar conductivity. How is it related to conductivity of the related
solution?
(b) One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate
solution of unknown concentration. Its other half-cell consists of a zinc electrode
dipping in 1.0 M solution of Zn(NO3)2. A voltage of 1.48 V is measured for this cell. Use
this information to calculate the concentration of silver nitrate solution used.
(E 0 Zn+2 / Zn =76V, E 0 Ag2+ /Ag =80V)
9. (a) State Kohlrausch law of independent migration of ions. Write an expression for the
molar conductivity of acetic acid at infinite dilution according to Kohlrausch law.
(b) Calculate Ʌ°m for acetic acid.Given that Ʌ°m (HCl) = 426 S cm2 mol–1 ,Ʌ°m (NaCl) = 126
S cm2 mol–1Ʌ°m (CH3COONa) = 91 S cm2 mol–1
10. Write the anode and cathode reactions and the overall reaction occurring in a lead
storage battery.
(b) A copper-silver cell is set up. The copper ion concentration is 0.10 M. The
concentration of silver ion is not known. The cell potential when measured was 0.422 V.
Determine the concentration of silver ions in the cell. (Given E 0.Ag+ / Ag = 80V, E 0CU2+ /Cu
= 34 V)
11. (a)How many moles of mercury will be produced by electrolysing 1.0 M. Hg(NO3)2
solution with a current of 2.00 A for 3 hours?
(b) A voltaic cell is set up at 25° C with the following half-cells Al3+ (0.001 M) and Ni2+
(0.50 M).
Write an equation for the reaction that occurs when the cell generates an electric
current and
determine the cell potential.(Given: [Eo Ni2+/Ni = – 0.25 V, E oAl/Al3+ = – 1.66 V]
8. (a) Define osmotic pressure.
(b) Why osmotic pressure is preferred over other colligative properties for the
determination of molecular masses of macromolecules?
(c) What is the molar concentration of particles in human blood if the osmotic pressure
is 7.2 atm at normal body temperature of 37°C?
. Explain the term electrolysis. Discuss briefly the electrolysis of (i) molten NaCl (ii)
aqueous sodium chloride solution (iii) molten lead bromide (iv) water.
2. state and explain Faraday’s laws of electrolysis. What is Electrochemical equivalent?
3. What do you understand by ‘electrolytic conduction’? what are the factors on which
electrolyte conduction depends.? What is the effect of temperature on electrolytic
conduction?
4. How is electrolytic conductance measured experimentally?
5. Describe normal hydrogen electrode and its applications.
CHEMICAL KINETICS
1. The gas phase decomposition of acetaldehyde
CH3CHO → CH4+CO
Follows the rate law.
What are the units of its rate constant ?
2 Give one example of pseudo first order reaction.
3. The conversion of molecules X to Y follows the second order of kinetics. If
concentration of X is increased 3 times, how will it affect the rate of
formation of Y.
4. The rate law for a reaction is
Rate = K [A] [B] 3/2
Can the reaction be an elementary process? Explain.
5. Name the factors on which the rate of a particular reaction depends.
1. Define the term ‘order of reaction’ for chemical reactions.
2. Define: Elementary reaction in a process
3 What do you mean by Rate of a reaction
1. Give an example of pseudo first order reaction.
2. For the reaction 2X →X2, the rate of reaction becomes three times when the
concentration of X is increased 27 times. What is the order of the reaction /
3. The rate law for the decomposition of N2O5 is :rate = k[N2O5]. What is the
significance of ‘k’ in this equation ?
4. The specific rate of reaction is 4.2 X 10-3mol L-1 S-1. What is the order of reaction ?
5. 1 litre of 2 M acetic acid is mixed with 1 litre of 3M ethyl alcohol to form an ester.
What would be the decrease in the initial rate if each solution is diluted by an equal
volume of water ?
6. State the order with respect to each reactant and overall reaction.
7. H2O + 3I- + 2H+ → 2H2O + I3 Rate = k[H2O]1 [I- ]1
8. 2.
The conversion of molecules X to Y follows the second order of kinetics. If
concentration of X is increased 3 times, how will it affect the rate of formation of
Y.?
9. Mention the units of rate of reaction
10. Define the term ‘order of reaction’ for chemical reactions.
11. Define ‘rate of a reaction’.
12. Identify the order of reaction from the following unit for its rate constant: L mol–1s–
1
13. Identify the order of reaction for which the rate constant is expressed in units of L–1
mol s–1.
14. Define ‘activation energy’ of a reaction.
15. Write the unit of first order rate constant of a gaseous reaction if the partial
pressure of gaseous reactant is given in bar.
16. 1. The gas phase decomposition of acetaldehyde
17. CH3CHO → CH4+CO
18. Follows the rate law.
19. What are the units of its rate constant.
20. 2. State the order with respect to each reactant and overall reaction.
21. H2O + 3I- + 2H+ → 2H2O + I3
22. Rate = k[H2O2]1[I-]1
23. 3. Give one example of pseudo first order reaction.
24. 4. The conversion of molecules X to Y follows the second order of kinetics. If
concentration of X is increased 3 times, how will it affect the rate of formation of Y.
25. 5. The rate law for a reaction is
26. Rate = K [A] [B] 3/2
27. Can the reaction be an elementary process? Explain.
28. 6. What do you understand by ‘rate of reaction’?
29. 7. Name the factors on which the rate of a particular reaction depends.
30. 8. Why rate of reaction does not remain constant throughout?
31. 9. Define specific reaction rate or rate constant.
32. 10. What is half-life period of a reaction?
2marks
1.The rate of a particular reaction quadruples when the temperature changes
from 293K to 313K. Calculate activation energy.
2. If the decomposition of nitrogen oxide as
2N2O5────> 4NO2 + O2
follows a first order kinetics.
(i)
Calculate the rate constant for a 0.05 M solution if the instantaneous rate is 1.5 x 106
mol/l/s?
3. Write the difference between order and molecularity of reaction.
4. Define Threshold energy and activation energy. How they are related?
5. List the factors affecting the rate of reaction.
Identify the order of reaction from the following unit for its rate constant: L mol–1s–1
2. Distinguish between ‘rate expression’ and ‘rate constant’ of a reaction.
3. The rate constant for a first order reaction is 60 s–1. How much time will it take to reduce the
initial
concentration of the reactant to1/10 of its initial value?
4. What do you understand by the rate law and rate constant of a reaction? Identify the order of a
reaction if the units of its rate constant are: (i) L–1 mol s–1 (ii) L mol–1 s–1.
5. A first order decomposition reaction takes 40 minutes for 30% decomposition. Calculate its
t1/2value.
6. What is meant by the ‘rate constant, k’ of a reaction? If the concentration is expressed in mol
L-1units and time
in seconds, what would be the units for k (i) for a zero order reaction and (ii) for a first order
reaction?
7. A reaction is of second order with respect to a reactant. How will the rate of reaction be
affected if the
concentration of this reactant is (i) doubled (ii) reduced to half?
8. Define the following: (i) Elementary step in a reaction (ii) Rate of a reaction.
9. A reaction is of first order in reactant A and of second order in reactant B. How is the rate of
this
reaction affected when (i) the concentration of B alone is increased to three times
(ii) the concentrations of A as well as B are doubled?
10. The rate constant for a reaction of zero order in A is 0.0030 mol L–1 s–1. How long will it take
for the
initial concentration of A to fall from 0.10 M to 0.075M?
11..Explain the following terms: (i) Order of a reaction (ii) Molecularity of a reaction.
1. What do you understand by zero order reaction ? Identify the reaction order from
the following units.
(i)
S-1
(ii)
L2mol-2 s-1
2. The following values for the first order rate constant were obtained for a certain
reaction ;
Temperature
K(s-1)
25
3.46 X 10-5
31
1.35 X 10-4
Calculate the activation energy.
3. Distinguish between order and molecularity of a reaction.
4. The half life for a first order reaction is 5 X 104 s. Calculate the rate constant of the
reaction and amount of reactant left after 30 min if we start with 1 g of reactant.
5. A first order reaction has rate constant 1.15 X 10-3 s-1 . How long will it take for 5 g
reactant to reduce to 3 g ?
6. A reaction is second order in A and first order in B.
a. Write the differential rate equation
b. How is the rate affected on increasing the concentration of A three times.
7. For the reaction AB, the rate of reaction becomes 27 times when the
concentration of A is increased three times. What is the order of the reaction.
8. What is half life period? Derive an expression for half life period in case of first
order reaction.
9. Differentiate order and molecularity.
10. The rate constant for a zero order reaction is 0.0030 mol L-1 S-1. How long will it
take for the initial concentration of the reactant to fall fro 0.10 m to 0.075 m ?
11. What are Pseudo unimolecular reactions? Explain with the help of a suitable
example.
2 . If the decomposition of nitrogen oxide as 2N2O5────>
4NO2 + O2 follows a first order kinetics. (i) Calculate the rate constant for a 0.05
M solution if the instantaneous rate is 1.5 x 10-6 mol/l/s?
A first order decomposition reaction takes 40 minutes for 30% decomposition. Calculate
its t1/2 value
2. What is meant by the ‘rate constant, k’ of a reaction? If the concentration is expressed in
mol L-1
units and time in seconds, what would be the units for k (i) for a zero order reaction and
(ii) for a
first order reaction?
3. Explain with an example, what is a pseudo first order reaction?
4. Show that time required for 99.9% completion of the first order reaction is 10 times of
t1/2 for first order chemical reaction
5. Define the following terms giving an example for each:
(i) The order of a reaction
(ii) The molecularity of a reaction
6. What is meant by a pseudo first order reaction? Give an example of a pseudo first order
reaction and write the rate equation for the same.
7. A reaction is of second order with respect to a reactant. How will the rate of reaction be
affected if the concentration of this reactant is (i) doubled (ii) reduced to half?
8. Define the following: (i) Elementary step in a reaction (ii) Rate of a reaction
1.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
A reaction is of first order in reactant A and of second order in reactant B. How is the rate
of this
reaction affected when (i) the concentration of B alone is increased to three times
(ii) the concentrations of A as well as B are doubled?
The rate constant for a zero order reaction is 0.0030 mol L–1 s–1. How long will it take for
the initial
concentration of the reactant to fall from 0.10 M to 0.075 M?
Distinguish between ‘rate expression’ and ‘rate constant’ of a reaction.
1. The rate of a particular reaction quadruples when the temperature changes from 293K
to 313K. Calculate activation energy.
2. If the decomposition of nitrogen oxide as
2N2O5────> 4NO2 + O2
follows a first order kinetics.
(i) Calculate the rate constant for a 0.05 M solution if the instantaneous rate is 1.5 x 10-6
mol/l/s?
ii) What concentration of N2O6 would give a rate of 2.45 x 10-5 mol L-1s-1
3) Write the difference between order and molecularity of reaction.
4) Define Threshold energy and activation energy. How they are related?
5(a). Draw a schematic graph showing how the rate of a first order reaction changes in
concentration of reactants.
(b). rate of reaction is given by the equation
Rate = k [A] 2[B]
What are the units of rate constant for this reaction?
6. List the factors affecting the rate of reaction.
7. Explain with suitable example, how the molecularity of a reaction is different from the
order of a reaction.
8. Define the term ‘rate constant’ of ‘specific reaction rate’.
9. What is half life period? Derive and expression for half-life period in case of a first
order reaction.
3marks
1. The rate constant for first order reaction is 60/s. How much time will it take to reduce the
concentration of the reaction to 1/10 of its initial value.
2. The rate of most of reaction double when their temperature is raised from 298k to 308k.
Calculate the activation energy of such a reaction.
3. A first order reaction takes 69.3 min for 50% completion. Set up on equation for
determining the time needed for 80% completion.
4. The decomposition of NH3 on platinum surface is a zero order reaction. What are the rate
of production of N2 and H2.
5.
How is the rapid change in concentration of reactants/products monitored for
1. fast reactions.
2. The rate of a reaction increases four times when the temperature changes from 300 K to
320 K.
Calculate the energy of activation of reaction, assuming that it does not change with
temperature.
4.
(R = 8.314 J K–1 mol–1).
3.
5. 2. Nitrogen pentoxide decomposes according to equation:
6.
2N2O5(g)→4NO2(g) + O2(g).
[N2O5] (M)
Time (min)
0.400
0.00
0.289
20.0
0.209
40.0
0.151
60.0
0.109
80.0
7.
8. This first order reaction was allowed to proceed at 40°C and the data below were
collected:
9. (a) Calculate the rate constant. Include units with your answer.
10. (b) What will be the concentration of N2O5 after 100 minutes?(c) Calculate the initial
rate of reaction
11. 3. The thermal decomposition of HCO2H is a first order reaction with a rate constant of
2.4 × 10–3 s–1
12.
at a certain temperature. Calculate how long will it take for three-fourths of initial
quantity of
13.
HCO2H to decompose. (log 0.25 = – 0.6021).
14. 4. For the reaction 2NO(g) + Cl2(g) 2NOCl(g),
15.
the following data were collected. All the measurements were taken at 263 K:
Experiment No.
16.
17.
18.
Initial [NO] (M)
Initial [Cl2] (M)
Initial rate of
disappearance
of Cl2 (M/min)
0.60
1.20
2.40
?
1
0.15
0.15
2
0.15
0.30
3
0.30
0.15
4
0.25
0.25
(a) Write the expression for rate law.
(b) Calculate the value of rate constant and specify its units.
(c) What is the initial rate of disappearance of Cl2 in experiment 4?
19. 5. For a chemical reaction R → P, the variation in the
20. concentration ln [R] vs. time t plot is given as
21.
For this reaction
22.
(i) what is the order of the reaction?
23. (ii) what is the slope of the curve?
24. (iii) what is the unit of rate constant ‘k’?
25. 6. For a decomposition reaction, the values of rate constant k at two different temperature
are
26. given k1 = 2.15 × 10–8 L mol–1 s–1 at 650 K, k2 = 2.39 × 10–7 L mol–1 s–1 at 700 K
–1
27. Calculate the value of activation energy (Ea) for this reaction. (R = 8.314 J K
mol–1)
–1
28. 7. A first order reaction has a rate constant of 0.0051 min . If we begin with 0.10M
concentration of the
29. reactant, what concentration of reactant will remain in solution after 3 hours?
1. The rate constant for a first order reaction is 60 s-1.How much time will it take to reduce
the concentration of the reactant to 1/10th of its initial value ?
2. The rate of a particular reaction doubles when the temperature changes from 27 0C to 37
0
C. Calculate the activation energy of such reaction.
3. The half life for radioactive decay of 14C is 5730 years. An archaeological artitact
contained wood had only 80 % of the 14C found in a living tree. Estimate the age of the
sample.
4. A reaction is first order in A and second order in B.
(i)
Write the differential rate equation.
(ii)
How is rate affected on increasing the concentration of B three times ?
(iii) How is the rate affected when the concentrations of both A and B doubled ?
5. Prove that the time required for the completion of 3/4th of the reaction of first order is
twice the time required for the completion of half of the reaction.
6. A first order reaction takes 69.3 min for 50% completion. Set up on equation for
determining the time needed for 80% completion and determine the time needed ?
1. The rate constant for a first order reaction is 60 s-1. How much time will it take to reduce
the initial concentration of the reactant to 1/16 th of its initial value?
2. What is meant by zero order reaction? Derive an integrated rate equation for a zero order
reaction.
3. (a) Write two points of difference between order of reaction and molecularity of a
reaction.
(b) Write one point of difference between rate of reaction and rate constant.
4. Draw a graph between fraction of molecules and kinetic energy of the reacting species for
two different temperatures :
(a) Room temperature
(b) Temperature 10°C higher than the room temperature
(c) Indicate the fraction of additional molecules which react at (t +10)°C
5. A first order reaction has a rate constant of 0.0051 min–1. If we begin with 0.10M
concentration of the reactant, what concentration of reactant will remain in solution after
3 hours?
6. For a decomposition reaction the values of rate constant k at two different temperatures
are given below: k1 = 2.15 × 10–8 L mol–1 s–1 at 650 K, k2 = 2.39 × 10–7 L mol–1 s–1 at
700 K
Calculate the value of activation energy for this reaction. (R = 8.314 J K–1 mol–1)
7. The rate constant for a reaction of zero order in A is 0.0030 mol L–1 s–1. How long will it
take for the
initial concentration of A to fall from 0.10 M to 0.075M?
8. The rate of a reaction increases four times when the temperature changes from 300 K to
320 K.
Calculate the energy of activation of reaction, assuming that it does not change with
temperature. (R = 8.314 J K–1 mol–1)
9. Nitrogen pentoxide decomposes according to equation:
2N2O5(g→4NO2(g) + O2(g).
This first order reaction was allowed to proceed at 40°C and the data below were
collected:
[N2O5] (M)
Time (min)
0.400
0.00
0.289
20.0
0.209
40.0
0.151
60.0
0.109
80.0
(a) Calculate the rate constant. Include units with your answer.
(b) What will be the concentration of N2O5 after 100 minutes?
(c) Calculate the initial rate of reaction
10. A first order reaction has a rate constant value of 0.00510 min–1.If we begin with 0.10 M
concentration of the reactant, how much of the reactant will remain after 3.0 hours?
11. For the reaction
2NO(g) + Cl2(g) →2NOCl(g),
the following data were collected. All the measurements were taken at 263 K:
Initial [NO]
Initial [Cl2]
Experiment
Initial rate of
No.
(M)
(M)
disappearance
of Cl2 (M/min)
1
0.15
0.15
0.60
2
0.15
0.30
1.20
3
0.30
0.15
2.40
4
0.25
0.25
?
(a) Write the expression for rate law.
(b) Calculate the value of rate constant and specify its units.
(c) What is the initial rate of disappearance of Cl2 in experiment 4?
Q1. The rate constant for first order reaction is 60/s. How much time will it take to reduce the
concentration of the reaction to 1/10 of its initial value.
2. The rate of most of reaction double when their temperature is raised from 298k to 308k.
Calculate the activation energy of such a reaction.
3. A first order reaction takes 69.3 min for 50% completion. Set up on equation for determining
the time needed for 80% completion.
4. Following reaction takes place in one step
2NO + O2→ 2NO2
How will the rate of the reaction of the above reaction change if the volume of reaction vessel is
diminished to 1/3 of its original volume? Will there be any change in the order of reaction with
reduced volume?
5. The decomposition of NH3 on platinum surface is a zero order reaction. What are the rate of
production of N2 and H2. If k= 2.5 x 10-4
6. How is the rapid change in concentration of reactants/products monitored for
fast reactions.
7. What are photochemical reactions? Give two examples,
8. What is the effect of temperature on the rate of reaction? Explain giving
reasons.
9. Comment on free energy change of ‘photochemical reactions’.
10. State the role of activated complex in a reaction and state its relation with
activation energy.
5marks
1. What do you understand by order of a reaction? How does rate law differfrom law of mass
action? Give two example of each of the reactions of
(i)zero order
(ii) first order
(iv)
second order
2. Briefly explain the effect of temperature on the rate constant of a reaction.
The gas phase decomposition of CH3OCH3 follows first order of kinetics
CH3OCH3 → CH4 (g) + H2 (g) + CO (g)
The reaction is carried out at a constant volume of the container at 5000C andhas t1/2 =14.5min.
Initially only dimethyl ether is present at a pressure of 0.40 atm. What is the totalpressure of the
system after 12 min? Assume ideal behavior.
3. For the reaction, the energy of activation is 75KJ / mol. When the energy ofactivation of a
catalyst is lowered to 20KJ / mol. What is the effect of catalyst onthe rate of reaction at 200C.
4. What do you understand by the rate of a reaction? How it is expressed?How it is the rate of
reaction determined?
1. (a) A reaction is of first order in A and of second order in B. Write the differential rate
equation for this reaction.
How will its initial rate be affected if the concentration of both A and B are together doubled?
(b) The rate constant k of a reaction increases four times when the temperature changes from
300 K
to 320 K. Calculate the activation energy for the reaction. (R = 8.314 J mol -1 K -1)
2. (a) List the factor which affect the rate of a chemical reaction.
(b) The half-life for radioactive 14 C is 5730 years. The wooden part of an archaeological
artifact has
only 80% of the 14 C activity found in fresh wood. Calculate the age of the artefact.
3. Decomposition of phosphine (PH3) at 120°C proceeds according to the equation:
4PH3(g) P4(g) + 6H2(g)
It is found that this reaction follows the following rate equation: Rate = k[PH3]
The half-life of PH3 is 37.9 s at 120°C.
(i) How much time will be required for 3/4 of PH3 to decompose?
(ii) What fraction of the original amount of PH3 will remain un decomposed after 1 minute?
4..Hydrogen peroxide, H2O2 (aq) decomposes to H2O(l) and O2(g) in a reaction that is of first
order in
H2O2 and has a rate constant, k = 1.06 × 10–3 min–1.
(i) How long will it take 15% of a sample of H2O2 to decompose?
(ii) How long will it take 85% of a sample of H2O2 to decompose?
1. (a) Explain the following terms (i)Order of a reaction; (ii)Molecularity of a reaction
(b)The rate of a reaction increases four times when the temperature changes from
300 K to 320 K. Calculate the energy of activation of the reaction, assuming that it
does not change with temperature.( R= 8.314 J k-1 mol-1)
2. (a) Derive the general expression for the half –life of a first order reaction.
(b)The decomposition of NH3 on platinum surface is a zero order reaction. What are
the rates of production of N2 and H2 if k = 2.5 x 10-4 mol L-1 s-1 ?
3. The thermal decomposition of HCOOH is a first order reaction with a rate constant of
2.4 X 10-3 s-1 at a certain temperature. Calculate how long will it take for ¾ of initial
quantity of HCOOH to decompose ? ( Log 0.25 = -0.6021)
4. Hydrogen peroxide, H2O2 (aq) decomposes to H2O (l) and O2 (g) in a reaction i.e
of first order in H2O2 and has a rate constant, k= 1.06 X 10-3 min-1.
(i)
How long it will take 15 % of a sample of H2O2 to decompose ?
(ii)
How long it will take 85 % of a sample of H2O2 to decompose ?
5. (a) Reaction between NO2 and F2 to give NO2F takes place by the following
mechanism :
slow
NO2(g) + F2(g)
NO2F + F(g)
fast
NO2(g) + F2(g)
NO2F (g)
Derive rate law from above mechanism.
(b)The conversion of X and Y follows second order kinetics. If the concentration of X
is increased to three times how will it affect the rate of formation of Y and why ?
1.
A reaction is second order in A and first order in B.
(a) Write the differential rate equation
(b) How is the rate affected on increasing the concentration of A three times.
2.
For the reaction AB, the rate of reaction becomes 27 times when the concentration
of A is increased three times. What is the order of the reaction.
What is half life period? Derive an expression for half life period in case of first order
reaction.
Differentiate order and molecularity.
The rate constant for a zero order reaction is 0.0030 mol L-1 S-1. How long will it take
for the initial concentration of the reactant to fall fro 0.10 m to 0.075 m ?
3.
4.
5.
(5 Marks)
6.
(a) Derive integrated rate equation for rate constant of a zero order reaction.
(b)
For the first order thermal decomposition reaction, the following data were
obtained.
C2H5Cl(g) C2H4(g) + Hcl(g)
Time/Sec
Total Pressure/atm
0
0.30
300
0.50
Calculate rate constant.
(Given log2 = 0.301, log3 = 0.4771, Log 4 = 0.6021)
7.
(a)
What is rate of reaction? Write two factors that affect the rate of a reaction.
(b)
The rate of a first order reaction becomes quadruples when temperature increases
from 250 to 450 C. Calculate the energy of activation.
8.
(a)
Define (i) Activation energy (ii) Order of a reaction
(b)
Show that in a first order reaction, time required for completion of 99.9% is 10
times the time required for the completion of half of the reaction.
(5 Marks)
9.
(a)
What is pseudo first order reaction. Given one example?
(b)
Consider the following data for the reaction A+BP
Initial
Conc.[A]
Initial Conc.
[B]
Initial rate
1
0.10 M
1.0 M
2.1 x 10-3
2
0.20 M
1.0 M
8.4 x 10-3
3
0.20 M
2.0 M
8.4 x 10-3
Determine the order of reaction with respect to A and with respect to B and the
overall order of the reaction.
1. (a) Derive the general form of the expression for the half-life of a first order reaction.
(b) The decomposition of NH3 on platinum surface is a zero order reaction. What are the
rates of production of N2 and H2 if k = 2.5 x 10-4 mol-1 L s-1?
2. (a) List the factors on which the rate of a chemical reaction depends.
(b) The half-life for decay of radioactive 14 C is 5730 years. An archaeological artefact
containing
wood has only 80% of the 14 C activity as found in living trees. Calculate the age of the
artefact .
3. (a) A reaction is of first order in A and of second order in B. Write the differential rate
equation
for this reaction .How will its initial rate be affected if the concentration of both A and B
are together doubled?
(b) The rate constant k of a reaction increases fourfold when the temperature changes
from 300 K
to 320 K. Calculate the activation energy for the reaction. (R = 8.314 J mol -1 K -1)
4. Decomposition of phosphine (PH3) at 120°C proceeds according to the equation:
4PH3 (g) → P4(g) + 6H2(g)
It is found that this reaction follows the following rate equation:
Rate = k[PH3]
The half-life of PH3 is 37.9 s at 120°C.
(i) How much time will be required for 3/4 of PH3 to decompose?
(ii) What fraction of the original amount of PH3 will remain undecomposed after 1
minute?
5. Hydrogen peroxide, H2O2 (aq) decomposes to H2O(l) and O2(g) in a reaction that is of
first order in
H2O2 and has a rate constant, k = 1.06 × 10–3 min–1.
(i) How long will it take 15% of a sample of H2O2 to decompose?
(ii) How long will it take 85% of a sample of H2O2 to decompose?
6. (a) A reaction is second order in A and first order in B.
(i) Write the differential rate equation.
(ii) How is the rate affected on increasing the concentration of A three times?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
(b) A first order reaction takes 40 minutes for 30% decomposition. Calculate t 1/2 for this
reaction.
7. For a first order reaction, show that time required for 99% completion is twice the time
required
for the completion of 90% of reaction.
(b) Rate constant ‘k’ of a reaction varies with temperature ‘T’ according to the equation:
ாೌ
ଵ
log k= log A –
ቀ ቁ
ଶ.ଷ଴ଷோ ்
Where Ea is the activation energy. When a graph is plotted for log k vs.1/T, a straight line
with a
slope of – 4250 K is obtained. Calculate ‘Ea’ for the reaction. (R = 8.314 JK–1 mol–1)
(Given log 1.428 = 0.1548)
1. What do you understand by the rate of a reaction? How it is expressed? How it is the rate of
reaction determined?
2. What do you understand by order of a reaction? How does rate law differ from law of mass
action? Give two example of each of the reactions of
(i) zero order (ii) first order (iii) second order
3. Derive the equation for the rate constant for a first order reaction. What would be the units of
the first order rate constant if the concentration is expressed in mole per litre and time in seconds.
4. Explain why the rate of reaction increases with increase in temperature.
5. Briefly explain the effect of temperature on the rate constant of a reaction
SURFACE CHEMISTRY
1mark
1. Why does a gas mixed with another gas not form a colloidal system?
2.Why are adsorbate particles attracted and retained on the surface of
adsorbent?
3.Explain the terms sorption and desorption.
4. Chemisorption is highly specific.” Illustrate with an example.
5. “Adsorbents in finely divided form are more effective.” Why?
1. What type of forces are responsible for the occurrence of physisorption?
2. Which has higher enthalpy of adsorption: physisorption or chemisorption?
3. Define desorption.
4. What is the effect of temperature on chemisorptions?
5. Give one example of each sol and gel.
6. Define the term” Tyndall effect”.
7. What causes Brownian movement in a colloidal solution?
8. What is the coagulation process?
9. What is an emulsion?
10. What are lyophobic colloids? Give one example for them.
11. Name the temperature above which micelles formation takes place.
12. Define peptization.
13. Give an example each of” Oil in water” and “water in oil” emulsion.
14. What is shape selective catalysis?
1. How does chemical adsorption of a gas on a solid vary with temperature ?
2. Define the enthalpy of adsorption.
3. How does the addition of alum purify water /
4. In what way a sol different from a gel ?
5. Of NH3 and N2 which gas will be adsorbed more readily on the surface of charcoal and
why ?
6. Why is a finely divided substance more effective as an adsorbent ?
7. Which has a higher enthalpy of adsorption, Physisorption or chemisorptions ?
8. What is meant by critical micelle concentration ?
9. What is a Brownian movement ?
10. To which colloidal system does milk belong ?
11. What is the effect of temperature on chemisorption ?
12.
Give one example each of Sol and gel.
13.
Give one example each of oil in water and water in oil emulsion.
14.
Why is adsorption always exothermic.
15.
Write the dispersed phase and dispersion medium in smoke.
16. What are the physical states of dispersed phase and dispersion medium in foam rubber?
17. 2.
Which of the following is more effective in coagulating positively charged
hydrated ferric oxide sol : (i) KCl
(ii) CaSO4
(iii) K3 [Fe(CN)6 ].
1. What are the physical states of dispersed phase and dispersion medium of froth?
2. What is the cause of Brownian movement among colloidal particles?
3. Arrange the solutions: True solution, colloidal solution, suspension in decreasing order of
their particles size?
4. Give an example of micelles system?
5. Why is it necessary to remove CO when ammonia is obtained by Haber’s process?
6. How is adsorption of a gas related to its critical temperature?
7. What is meant by Shape Selective Catalyst?
8. Of the physiorption & chemisorptions, which type of adsorption has higher enthalpy of
adsorption?
9. Write down the Example of Positive Sol?
10. Mention two ways by which lyophilic colloids can be coagulated.
11. Define the term ‘Tyndall effect’.
12. What is the ‘coagulation’ process?
13. What is an emulsion?
14. Define ‘electrophoresis’.
15. What is meant by ‘shape-selective catalysis’ of reactions?
16. What are lyophobic colloids? Give one example for them.
17. Define ‘peptization’.
18. Why is the adsorption phenomenon always exothermic?
18. How does chemical adsorption of a gas on a solid vary with temperature ?
19. Define the enthalpy of adsorption.
20. How does the addition of alum purify water /
21. In what way a sol different from a gel ?
22. Of NH3 and N2 which gas will be adsorbed more readily on the surface of charcoal and
why ?
23. Why is a finely divided substance more effective as an adsorbent ?
24. Which has a higher enthalpy of adsorption, Physisorption or chemisorptions ?
25. What is meant by critical micelle concentration ?
26. What is a Brownian movement ?
27. To which colloidal system does milk belong ?
9. What is the effect of temperature on chemisorption ?
10. Give one example each of Sol and gel.
11. Give one example each of oil in water and water in oil emulsion.
12. Why is adsorption always exothermic.
13. Write the dispersed phase and dispersion medium in smoke.
14. What are the physical states of dispersed phase and dispersion medium in foam rubber?
15. Which of the following is more effective in coagulating positively charged hydrated
ferric oxide sol : (i) KCl
(ii) CaSO4
(iii) K3 [Fe(CN)6 ].
19. What are the physical states of dispersed phase and dispersion medium of froth?
20. What is the cause of Brownian movement among colloidal particles?
21. Arrange the solutions: True solution, colloidal solution, suspension in decreasing order of
their particles size?
22. Give an example of micelles system?
23. Why is it necessary to remove CO when ammonia is obtained by Haber’s process?
24. How is adsorption of a gas related to its critical temperature?
25. What is meant by Shape Selective Catalyst?
26. Of the physiorption & chemisorptions, which type of adsorption has higher enthalpy of
adsorption?
27. Write down the Example of Positive Sol?
28. Mention two ways by which lyophilic colloids can be coagulated.
29. Define the term ‘Tyndall effect’.
30. What is the ‘coagulation’ process?
31. What is an emulsion?
32. Define ‘electrophoresis’.
33. What is meant by ‘shape-selective catalysis’ of reactions?
34. What are lyophobic colloids? Give one example for them.
35. Define ‘peptization’.
36. Why is the adsorption phenomenon always exothermic?
1. Why does a gas mixed with another gas not form a colloidal system?
(a) 2. Why are adsorbate particles attracted and retained on the surface of adsorbent?
(b) 3. Explain the terms sorption and desorption.
(c) 4. “Chemisorption is highly specific.” Illustrate with an example.
(d) 5. “Adsorbents in finely divided form are more effective.” Why?
(e) 6. Name two compounds used as adsorbent for controlling humidity. [Ans. : Silica
gel, Alumina gel]
(f) 7. Mention one shape selective catalyst used to convert alcohol directly into gasoline.
(g) 8. ‘Generally high temperature is favourable for chemisorption.’ Why?
(h) 9. Name the catalyst used in the following process :
(i) (a) Haber’s process for the manufacture of NH3 gas.
(j) (b) Ostwald process for the manufacture of nitric acid.
(k) 10. Explain the relationship given by Freundlich in adsorption isotherm.
(l) 11. Which group elements show maximum catalytic activity for hydrogenation
reactions?
(m) [Hint : 7–9 group elements]
(n) 12. Why gas masks are used by miners in coal mines while working?
(o) 13. Write the chemical reaction involved in the preparation of sulphur sol.
(p) 14. Name the enzyme which converts milk into curd. [Ans. : lactobacilli]
(q) 15. What are the optimum temperature and pH at which enzymes are highly active.
(r) [Ans. : Temperature 298–310K and pH 5 to 7]
(s) 16. What are the physical states of dispersed phase and dispersion medium in foam
rubber.
(t) 18. What is the composition of colloidion solution?
(u) 19. Why do colloidal particles show Brownian movement?
(v) [Hint : Due to unbalanced bombardment of the particles by the molecules
(w) of the dispersion medium]
(x) 21. State the sign of entropy change involved when the molecules of a substances get
adsorbed on a solid surface.
(y) 22. Why does sky appear blue to us?
(z) 23. What happens when hydrated ferric oxide and arsenious sulphide sols are mixed
in almost equal proportions?
(aa) 24. Gelatin is generally added to ice-cream. Why?
(bb) [Hint : Ice-cream is water in oil type emulsion and gelatin acts as emulsifier].
(cc) 25. How is lake test for aluminium ion based upon adsorption?
(dd) [Hint : Al2O3.xH2O has the capacity to adsorb the colour of blue litmus from the
solution]
(ee) 26. What is saturation pressure in Freundlich’s isotherm?
(ff) 27. Mention the two conditions for the formation of micelles. [Hint. : CMC and Tk]
(gg) 28. How is Brownian movement responsible for the stability of sols?
(hh) [Hint : Stirring effect due to Brownian movement does not allow the particles to
settle down.]
(ii) 29. Which of the following is more effective in coagulating positively charged
hydrated ferric oxide sol :
(jj) (i) KCl (ii) CaSO4 (iii) K3 [Fe(CN)6].
(kk) 30. State the purpose of impregnating the filter paper with colloidion solution.
(ll) 31. Mention one use of ZSM–5 catalyst.
1. 1. What type of forces are responsible for the occurrence of physisorption?
2. 2. Which has higher enthalpy of adsorption: physisorption or chemisorption?
3. 3. Define desorption.
4. 4. What is the effect of temperature on chemisorptions?
5. 5. Give one example of each sol and gel.
6. 6. Define the term” Tyndall effect”.
7. 7. What causes Brownian movement in a colloidal solution?
8. 8. What is the coagulation process?
9. 9. What is an emulsion?
10. 10. What are lyophobic colloids? Give one example for them.
11. 11. Name the temperature above which micelles formation takes place.
12. 12. Define peptization.
13. 13. Give an example each of” Oil in water” and “water in oil” emulsion.
14. 14. What is shape selective catalysis?
2marks
SHORT ANSWER-I(2MARKS)
1. Define the following: (i) Peptization (ii) Reversible sols
2. Define the following terms giving an example of each: (i) Emulsion (ii) Hydrosol
3. Explain how to phenomenon of adsorption finds application in the following processes:
(i) Production of vacuum (ii) Heterogeneous catalysis
4. Write four distinguishing features operative between chemisorption and physisorption.
5. What is meant by coagulation of a colloidal solution? Name any method by which
coagulation of lyophobic sols can be carried out.
6. Define the following terms:(i) Aerosol(ii) Coagulation of colloids
7. Name the two groups into which phenomenon of catalysis can be divided. Give an
example of each group with the chemical equation involved.
8. What is meant by coagulation of a colloidal solution? Describe briefly any three methods
by which coagulation of lyophobic sols can be carried out.
9. Write the dispersed phase and dispersion medium of the following colloidal systems: (i)
Smoke (ii) Milk
10. What are lyophilic and lyophobic colloids? Which of these sols can be easily coagulated
on the addition of small amounts of electrolytes?
1. 1. Write three distinct features of chemisorptions which are not found in
physisorptions.
2. 2. Name the two groups into which Catalysis can be divided. Give an example of
each group with the chemical equation involved.
3. 3. Write the dispersed phase and dispersion medium of the following colloidal
systems:
4. (i) Smoke
(ii) Milk
5. 4. Classify colloids where the dispersion medum is water. State their characteristics
and write an example ofeachof these classes.
6. 5.(a) What happens when a freshly prepared Fe(OH)3 is shaken with water containing
a small quantity of FeCl3?
7. (b)Why is a finely divided substance more effective as an adsorbent?
8. 6. Explain what is observed when
9. (i) An electric current is passed through a colloidal sol.
10. (ii) When abeam of light is passed through a colloidal solution.
11. 7. Write the dispersed phase and dispersion medium of the given colloids.
12. (i) Cheese
(ii) Fog
13. 8. What is the difference between Oil/water type and water/Oil type emulsions? Give
an example of each type.
1. Why are some medicines more effective in the colloidal form ?
2. On the basis of Hardy Schulze rule explain why the coagulating power of phosphate
is higher than chloride.
3. How does a delta form at the meeting place of sea and river water ?
4. What is meant by coagulation of a colloidal solution ? Name any method by which
coagulation of a lyophobic sols can be carried out.
5. Write the dispersed phase and dispersion medium of the colloidal systems:
(a) Smoke
(b) Milk
6. What is the difference between (O/W) type and (W/O) type emulsions. Give
example of each type.
7. How are the following sols produced ?
(a) Sulphur sol
(b) Collodion
8. Explain the following terms with an example of each :
(i)
Emulsification
(ii)
Chemisorption
9. Distinguish between homogeneous and heterogeneous catalysis.
10. What is the lyophilic and lyophobic colloids ?
11. Why are some medicines more effective in the colloidal form ?
12. On the basis of Hardy Schulze rule explain why the coagulating power of phosphate
is higher than chloride.
13. How does a delta form at the meeting place of sea and river water ?
14. What is meant by coagulation of a colloidal solution ? Name any method by which
coagulation of a lyophobic sols can be carried out.
15. Write the dispersed phase and dispersion medium of the colloidal systems:
(b) Smoke
(b) Milk
16. What is the difference between (O/W) type and (W/O) type emulsions. Give
example of each type.
17. How are the following sols produced ?
(b) Sulphur sol
(b) Collodion
18. Explain the following terms with an example of each :
(ii)
Emulsification
(ii)
Chemisorption
19. Distinguish between homogeneous and heterogeneous catalysis.
20. What is the lyophilic and lyophobic colloids ?
16. 1.
Define the terms : (a) Helmholtz electrical double layer. (b) Zeta potential. How
can the two emulsions can be distinguished : (a) oil in water type (O/W) and (b) water in
oil type (W/O
11. Define the following: (i) Peptization (ii) Reversible sols
12. Define the following terms giving an example of each: (i) Emulsion (ii) Hydrosol
13. Explain how to phenomenon of adsorption finds application in the following processes:
(ii) Production of vacuum (ii) Heterogeneous catalysis
14. Write four distinguishing features operative between chemisorption and physisorption.
15. What is meant by coagulation of a colloidal solution? Name any method by which
coagulation of lyophobic sols can be carried out.
16. Define the following terms:(i) Aerosol(ii) Coagulation of colloids
17. Name the two groups into which phenomenon of catalysis can be divided. Give an
example of each group with the chemical equation involved.
18. What is meant by coagulation of a colloidal solution? Describe briefly any three methods
by which coagulation of lyophobic sols can be carried out.
19. Write the dispersed phase and dispersion medium of the following colloidal systems: (i)
Smoke (ii) Milk
20. What are lyophilic and lyophobic colloids? Which of these sols can be easily coagulated
on the addition of small amounts of electrolytes?
17.
What is adsorption? Give reason why a finely divided substance is more effective
as an adsorbent.
18.
(b)
How does the addition of alum purify water ?
19.
(c)
Sky appears blue in colour. Explain ?
20.
21. 7.
(a)
Heat of adsorption is great for chemisorption than physisorption. Why ?
22.
(b)
What is Zeolite?
23.
(c)
Differentiate between peptization and coagulation.
24.
25. 8.
(a)
What is shape selective catalysis ? Given an example in which shape
selectivity of the catalyst is exhibited.
26.
(b)
Define (i) Peptization (ii) Zeta potential
27.
28. 9.
Explain the following temrs
29.
(a)
Electrophoresis
(b) Tyndal Effect
(c) Dialysis
30.
31. 10.
(a)
Differentiate Lyophilic and Iyopobic Sol.
32.
(b)
What is adsorption isotherm. Write the expression for adsorption of gases
on solids in reference to Freundlich adsorption isotherm.
33.
34. 11.
Explain the following observations
35.
(a)
Passing an electric current through a colloidal Solution.
36.
(b)
Ferric hydroxide solution coagulates on addition of a solution of
potassium sulphate.
(c) Colloidal “ particles scatter light
(mm) 35. Explain the effect of temperature on the extent of physical and chemical
adsorption.
(nn) 36. Define the term peptization and mention its cause.
(oo) 38. Write the factors upon which the catalytic reaction of shape-selective catalyst
depends?
(pp) [Hint : (a) Pore structure of the catalyst; (b) Size and shape of the reactant and
product molecules.]
(qq) 39. Mention two examples of emulsifying agents for o/w emulsions and w/o
emulsions.
(rr) 40. Suggest a mechanism of enzyme catalysed reaction.
(ss) 41. A small amount of silica gel and a small amount of anhydrous calcium chloride
are placed separately in two beakers containing water vapour. Name of phenomenon
that takes place in both the beakers.
(tt) [Hint : Silica gel – Adsorption, Anhydrous CaCl2–Absorption, as it forms CaCl2.
2H2O)
(uu) 42. Write the differences between adsorption and absorption?
(vv) 43. How can physisorption be distinguished from chemisorption?
(ww) 45. In what way these are different : (a) a sol and a gel (b) a gel and an emulsion.
(xx) 46. State “Hardy Schulze Rule” with one example.
(yy) 47. What is an emulsifying agent? What role does it play in forming an emulsion?
(zz) 48. Define the terms :
(aaa) (a) Helmholtz electrical double layer.
(bbb) (b) Zeta potential.
(ccc) 50. Mention the two necessary conditions for the observation of Tyndall Effect.
(ddd) 51. Account for the following :
(eee) (a) Artificial rain can be caused by spraying electrified sand on the clouds.
(fff) (b) Electrical precipitation of smoke.
(ggg) 52. Write chemical equations for the preparation of sols :
(hhh) (a) Gold sol by reduction.
(iii)(b) hydrated ferric oxide sol by hydrolysis.
(jjj)53. How can the two emulsions can be distinguished :
(kkk) (a) oil in water type (O/W) and
(lll)(b) water in oil type (W/O)
SHORT ANSWER-II(3MARKS)
14. What are lyophilic and lyophobic sols? Give one example of each type. Which one of
these two types of sols is easily coagulated and why?
15. Discuss the effect of pressure & temperature on the adsorption of gases on solids?
16. Explain what is observed when
17. (i) an electrolyte, KCl, is added to a hydrated ferric oxide sol.
18. (ii) an electric current is passed through a colloidal solution.
19. (iii) a beam of strong light is passed through a colloidal solution.
20. Explain what is observed when
21. (i) a beam of light is passed through a colloidal solution.
22. (ii) an electrolyte NaCl, is added to hydrated ferric oxide sol.
23. (iii) an electric current is passed through a colloidal sol.
24. How are the following colloids different from each other in respect of dispersion
medium and dispersed phase? Give one example of each type.
(i) An aerosol
(ii) A hydrosol
(iii) An emulsion
25. What is the difference between multimolecular and macromolecular colloids? Give
one example of each. How are associated colloids different from these two types of
colloids?
26. What happens in the following activities and why?
27. (i) An electrolyte is added to a hydrated ferric oxide sol in water.
28. (ii) A beam of light is passed through a colloidal solution.
29. (iii) An electric current is passed through a colloidal solution.
30. How are the following colloids different from each other in respect of their dispersion
medium and dispersed phase? Give one example of each. (i) Aerosol (ii) Emulsion
(iii) Hydrosol
31. Explain how the phenomenon of adsorption finds application in each of the following
processes:
(i) Production of vacuum
(ii) Heterogeneous catalysis
(iii) Froth floatation process
32. Define each of the following terms: (i) Micelles
(ii) Peptization (iii)
Desorption
33. Classify colloids where the dispersion medium is water. State their characteristics and
write an example of each of these classes.
34. Describes some features of catalysis by Zeolites?
35. 1. Define the following terms: (i) Aerosol (ii) Coagulation of colloids (iii)
Electrophoresis
36. 2. What are lyophillic and lyophobic colloids? Give an example of each type. Which
one of these is easily coagulated and why?
37. 3. What is the difference between multimolecular and macromolecular colloids? Give
one example of each. How are associated colloids different from these two types of
colloids?
38. 4. Explain the following observations:
39. (i) Lyophillic colloid is more stable than lyophobic colloid.
40. (ii) Coagulation takes place when sodium chloride solution is added to a colloidal
solution of ferric hydroxide.
(iii) Sky appears blue in colour
1. Define each of the following terms:
(i)
Micelles
(ii)
Peptization
(iii) Desorption
2. Explain what is observed when
(i)
An electric current is passed through a sol.
(ii)
A beam of light is passed through a sol.
(iii) An electrolyte (say NaCl) is added to Ferric hydroxide sol.
3. Explain the following terms :
(i)
Electrophoresis
(ii)
Dialysis
(iii) Tyndall effect
4. What is the difference between multimolecular and macromolecular colloids ?
Give one example of each type, How are associated colloids different from these two
types of colloids ?
5. How are the following colloids different from each other in respect of their dispersion
medium and dispersed phase ? Give one example of each.
(i)
Aerosol
(ii)
Emulsion
(iii) Hydrosol
6. Explain the following observations:
(a) Lyophilic colloid is more stable than lyophobic colloid.
(b) Coagulation takes place when NaCl solution is added to a colloidal solution of
Fe(OH)3.
(c) Sky appears blue in colour.
7. (a) What are micelles ? How do they differ from ordinary colloidal particles ? Give
two examples of micelle forming substances.
(b)State Hardy-Schulze rule
(c) State the principle of electrodialysis
8. Give four differences between physical and chemical adsorption. What is the effect
of temperature on chemical adsorption ?
37. Explain the following terms with suitable examples :
(i)
Gel
(ii)
Aerosol
(iii) Hydrosol
38. Discuss the effect of pressure and temperature on the adsorption of gases ion solids.
Describe the application of adsorption in controlling humidity.
39.
What happens : (a) by persistent dialysis of a sol.
(b) when river water
meets the sea water.
(c) when alum is applied on cuts during
bleeding.
1. What are lyophilic and lyophobic sols? Give one example of each type. Which one of
these two types of sols is easily coagulated and why?
2. Discuss the effect of pressure & temperature on the adsorption of gases on solids?
3. Explain what is observed when
4. (i) an electrolyte, KCl, is added to a hydrated ferric oxide sol.
5. (ii) an electric current is passed through a colloidal solution.
6. (iii) a beam of strong light is passed through a colloidal solution.
7. Explain what is observed when
8. (i) a beam of light is passed through a colloidal solution.
9. (ii) an electrolyte NaCl, is added to hydrated ferric oxide sol.
10. (iii) an electric current is passed through a colloidal sol.
11. How are the following colloids different from each other in respect of dispersion
medium and dispersed phase? Give one example of each type.
(i) An aerosol
(ii) A hydrosol
(iii) An emulsion
12. What is the difference between multimolecular and macromolecular colloids? Give
one example of each. How are associated colloids different from these two types of
colloids?
13. What happens in the following activities and why?
14. (i) An electrolyte is added to a hydrated ferric oxide sol in water.
15. (ii) A beam of light is passed through a colloidal solution.
16. (iii) An electric current is passed through a colloidal solution.
17. How are the following colloids different from each other in respect of their dispersion
medium and dispersed phase? Give one example of each. (i) Aerosol (ii) Emulsion
(iii) Hydrosol
18. Explain how the phenomenon of adsorption finds application in each of the following
processes:
(i) Production of vacuum
(ii) Heterogeneous catalysis
(iii) Froth floatation process
19. Define each of the following terms: (i) Micelles
(ii) Peptization (iii)
Desorption
20. Classify colloids where the dispersion medium is water. State their characteristics and
write an example of each of these classes.
21. Describes some features of catalysis by Zeolites?
(mmm)54. Write the difference between
(nnn) (a) catalysts and enzymes
(ooo) (b) promoters and poisons
(ppp) 55. Write the steps of ‘Modern Adsorption Theory of Heterogenous Catalysis.’
(qqq) 56. Mention the two important features of solid catalysts and explain with the help
of suitable examples.
(rrr) 57. How are the following colloids different from each other in respect of
dispersion medium and dispersed phase? Give one example of each type.
(sss) (a) An aerosol (b) A hydrosol (c) An emulsion.
(ttt)58. What happens :
(uuu) (a) by persistent dialysis of a sol.
(vvv) (b) when river water meets the sea water.
(www) (c) when alum is applied on cuts during bleeding.
(xxx) 59. Distinguish between multimolecular, macromolecular and associated colloids
with the help of one example of each.
(yyy) 60. (a) Which property of colloids is responsible for the sun to look red at the time
of setting?
(zzz) (b) C2H2 on addition with H2 forms ethane in presence of palladium catalyst but
if reaction is carried in the presence of barium sulphate and quinoline, the product is
ethene and not ethane. Why?
(aaaa) [Ans. (a) Sun is at horizon and blue part of the light is scattered away by the
(bbbb) dust particles as light has to travel a long distance through the atmosphere.
VALUE BASED QUESTION (4 MARKS)
1. Ram noticed that the barber applied alum on his face after saving. He also observed his
wife dissolved alum to purify muddy water.He thinks that it is all about colloidal
chemistry and the properties of colloidal solutions. He discussed these values with his
wife as she is from humanities background. After reading this passage, answer the
following questions:
(a) What values are associated with this Ram’s actions?
(b) What do you mean by the term coagulation?
(c) How can the coagulation of lyophilic sols be done?
(d) Write the properties of colloidal solution.
2. Colloidal solutions are used as medicines. Colloidal medicines, are more effective
because they have large surface area and therefore , easily assimilated.
(cccc) Name a colloidal solution used in eye lotion.
(dddd) What is the used of colloidal gold?
(eeee) What is milk of magnesia? Give its use.
GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF
ELEMENTS(CH-6)
1marks
1. Nam What are collectors in froth flotation process?
2. Give one example e three metals which occur in native state in nature.
3. Give the names and formulae of three ores which are concentrated by
froth floatation process.
4.Among Fe, Cu, Al and Pb, which metal (s) can not be obtained by smelting.
5.What is the thermodynamic criteria for the feasibility of a reaction?
1. An ore of galena (PbS) is concentrated with zinc blende (ZnS). Name one chemical which can be used
to concentrate galena by froth flotation method.
2. Why is only sulphide ores are concentrated by froth flotation process?
3. What is the function of collectors in the froth flotation process for the concentration of ores?
4. What is liquation?
5. What name is given to carbon reduction process for extracting the metal?
6. What is the role of cryolite in the metallurgy of aluminium?
7. Which reducing agent is used to get copper from the leached low grade copper ore?
8. Zinc act as a reducing agent in the extraction of silver. Comment.
1.
2.
3.
4.
5.
6.
7.
Differentiate between a mineral and an ore.
What type of ores can be concentrated by magnetic separation method .
Name the method used for removing gangue from sulphide ores.
How is copper extracted from a low grade ore of it?
What is the role of collectors and stabiliser in froth floatation method?
Name the reducing agent used in aluminothermic(thermite)process.
Copper matte is charged into a silica lined converter in extraction of copper. What is the
role of silica lining here?
8. What is meant by the term pyrometallurgy ?
9. Name the process of heating in presence of oxygen so as to convert suphide ore to oxide
ore.
10. What is meant by the term chromatography ?
11. What is the role of flux in metallurgical process ?
12. Out of C andCO ,which is the better reducing agent for ZnO.?
13. Why sulphide ores are converted to oxide ore before reduction.
14. How is cast iron different from pig iron.
15. How are metals used as semiconductors refined?What is principle ofmethod used.
16. What is the composition of copper matte?
17. What are collectors in froth flotation process? Give one example.
1.
2.
3.
4.
5.
6.
7.
8.
9.
Why is the froth floatation method selected for the concentration of sulphide ores?
What is meant by the term ‘pyrometallurgy’?
Name two metals which occur in nature as oxides.
Differentiate between a mineral and an ore.
What type of ores can be concentrated by magnetic separation method?
What is the role of graphite in the electrometallurgy of aluminium?
How is copper extracted from a low grade ore of it?
What is the role of collectors in Froth Floatation process?
Write the reaction involved in the extraction of silver after the silver ore has been
leached with NaCN.
10. What is the role of a depressant in Froth Floatation process for the concentration of a
sulphide ore?
(a) 1. Name three metals which occur in native state in nature.
(b) 2. What are collectors in froth flotation process? Give one example.
(c) *3. Give the names and formulae of three ores which are concentrated by froth floatation
process.
(d)
(e)
(f)
(g)
(h)
(i)
(j)
(k)
(l)
4. Among Fe, Cu, Al and Pb, which metal (s) can not be obtained by smelting.
5. What is the thermodynamic criteria for the feasibility of a reaction?
8. Why can’t aluminium be reduced by carbon?
9. Name the most important form of iron. Mention its one use.
10. Name the impurities present in bauxite ore.
11. What is the composition of copper matte?
12. Which from of copper is called blister copper?
13. What are froth stabilizers? Give two examples.
14. A sample of galena is contaminated with zinc blend. Name one chemical which can
be used to concentrate galena selectively by froth floatation method.
(m) 15. What are the constituents of German silver?
(n) 16. Why is froth floatation process selected for concentration of the sulphide ore?
(o) 17. Write the reaction involved in the extraction of copper from low grade ores.
(p) 18. Although aluminium is above hydrogen in the electrochemical series, it is stable in air
and water. Why?
(q) 19. Which method of purification is represented by the following reaction
(r) Ti(s) + 2I2, (g) 523K→ Ti I4(g) 1700K→ Ti(s) + 2I2(g)
(s) 20. Zinc is used but not copper for the recovery of metallic silver from the complex
[Ag(CN)2]–, although electrode potentials of both zinc and copper are less than that of
Ag. Explain why?
(t) [Hint : Zinc reacts at faster rate as compared with copper, further zinc is cheaper than
copper].
(u) 21. Write the composition of motlen mixture which is electrolysed to extract aluminium.
2marks
1. Name the method that is used for refining of
(i) Nickel
(ii) Copper (iii) Zirconium.
2. Name the principal ore of aluminium. Explain the significance of leaching in the extraction of
aluminium.
3. State briefly the principle of (i) froth flotation process (ii) Refing by liquation.
4. Describe the principle of (i) Vapour phase refining of titanium metal (ii) Electrolytic refining.
5. Give two requirements of vapour phase refining.
6. Outline the principle of (i) Zone refining. (ii) Chromatographic method.
7. Describe the (i) principle of Mond process for refining of nickel.
(ii) Role of NaCN in the extraction of silver.
8. Explain the role of (i) CO in the extraction of nickel. (ii) Zinc in the extraction of silver.
(iii) Graphite rod in the electrometallurgy of aluminium.
1. Write the principle involved in each of the following processes :
(i)
Mond process of refining of Nickel.
(ii)
Column chromatography for purification of rare elements.
2. Name the chief ore each of copper and aluminium. Name the method used for the
concentration of these two ores.
3. Explain the role of
(i)
Cryolite in the electrolytic reduction of alumina,
(ii)
Carbon monoxide in the purification of nickel.
4. Which methods are usually employed for purifying the following metals.
i)Nickel ii)Germanium
Mention the principle behind each one of them.
5. What is the significance of leaching in the extraction of aluminium?
6. Name one example each of (i) acidic flux and (ii) basic flux.
7. Although thermodynamically feasible, in practice, magnesium metal is not used for the
reduction of alumina in the metallurgy of aluminium. Why ?
8. I) Copper can be extracted by hydrometallurgy but not zinc. Explain.
Ii)Why the extraction of copper from pyrite ores is more difficult than
that from its oxide ore through reduction.
9. Name the chief ores of following in the earth’s crust :
(a) Al (b) Ca (c) Na (d) Pb
10. Give one example of the following for extraction of metal
(i)
Auto-reduction
(ii)
H2 is used as reducing agent.
11. What is froth floatation method ? What is the role of of depressant .Explain with one
example.
12.Explain the role of each of the following in the extraction of metals from their ores :
i)NaCN in the extraction of gold from gold ore /silver from silver ore.
1.
2.
3.
4.
5.
6.
7.
8.
ii) SiO2 in the extraction of copper from copper matte..
iii)carbon dioxide in the extraction of Al.
The graphite electrodes in the extraction of ‘alluminium’ by Hall-Heroult process need to
be changed frequently. Why?
Why is the reduction of a metal oxide easier if metal formed is in liquid state at the
temperature of reduction?
Explain the role of
(i) Cryolite in the electrolytic reduction of alumina.
(ii) Carbon monooxide in the purification of nickel.
Describe the underlying principle of each of the following metal refining methods:
(i) Electrolytic refining of metals
(ii) Vapour phase refining of metals
Describe the role of the following:
(i) NaCN in the extraction of silver
(ii) CO in the purification of nickel
State the principles on which the following operations are based:
(i) Zone refining (ii) Vapour phase refining.
State the principle on which each of the following processes operates:
(i) Recovery of silver after the silver ore has been leached with NaCN.
(ii) Electrolytic refining of a metal.
(iii)Vapour phase refining of a metal.
Describe the following:
(i) The role of cryolite in electrometallurgy of aluminium.
(ii) The role of carbon monoxide in the refining of crude nickel.
9. Name one chief ore each of copper and aluminium. Name the method used for
concentration of these two ores
10. (a) Which solution is used for the leaching of silver metal in the presence of air in the
metallurgy of silver?
(b) Out of C and CO, which is a better reducing agent at the lower temperature range in
the blast furnace to extract iron from the oxide ore?
11. (a) Which of the following ores can be concentrated by froth floatation method and
why?
Fe2O3, ZnS, Al2O3.
(b) What is the role of silica in the metallurgy of copper?
12. What is the composition of ‘Copper matte’?
(a) Name the method used for removing gangue from sulphide ores.
(b) How is wrought iron different from steel?
13. How can you separate alumina (Al2O3) from silica present in bauxite ore? Write the
chemical equations for the reactions involved
(a) *22. What is hydrometallurgy? Give one example where it is used for metal extraction.
(b) 23. Name the process for the benefaction/concentration of (i) an ore having lighter
impurities (ii) sulphide ore.
(c) 24. Mention the role of cryolite in the extraction of aluminium.
(d) 25. Mention the role of following :
(e) (a) SiO2 in the metallurgy of Cu.
(f) (b) CaCO3 in the metallurgy of Fe.
(g) (c) CO in the metallergy of iron
(h) (d) I2 in the purification of zirconium.
(i) 26. Extraction of copper directly from sulphide ore is less favourable than from its oxide
through reduction. Explain.
(j) 27. The graphite electrodes in the extraction of ‘alluminium’ by Hall-Heroult process need
to be changed frequently. Why?
(k) 28. Write the chemical formulae of the following ores (a) Haematite (b) Magnetite (c)
Limonite (d) Siderite.
(l) 29. Give equations for the industrial extraction of zinc from calamine.
(m) 30. Name the elements present in anode mud during refining of copper. Why does it
contain such elements?
(n) 31. Write the Chemical reactions taking place in different zones in the blast furnace for
the extraction of iron from its ore.
(o) 32. How are impurities separated from bauxite ore to get pure alumina?
(p) 33. Why is the reduction of a metal oxide easier if metal formed is in liquid state at the
temperature of reduction?
(q) 34. What is pyrometallurgy? Explain with one example.
(r) 35. Write the method to produce Copper matte from copper pyrites.
(s) *38. Copper can be extracted by hydrometallurgy but not zinc. Explain why?
3marks
1. Describe the role of (i) Iodine in the refining of Zirconium
.(ii) NaCN in the extraction of gold from gold ore
(iii)SiO2.in the extraction of copper from copper matte. Write the chemical equations for the involved
reactions.
2. Write the chemical reactions which take place in the following operations:
(i) Electrolytic reduction of Al2O3 (ii) Isolation of Zinc from Zinc blende.
(iii) Mond’s process for refining of nickel.
3. Describe how the following changes are brought about:
(i) Pig iron into steel
(ii) Zinc oxide into Zinc. (iii) Impure Titanium into pure
Titanium.
4. What is the chief ore of iron? Write the chemical reactions taking place in the extraction of iron from
its ore.
1.
(i)
Roasting
(ii)
Calcination (iii) Smelting
2. State the role of
(i)
NaCN in froth floatation process
(ii)
Iodine in the refining of titanium/Zirconium.
(iii) Graphite rod in the electrolytic reduction of alumina
4...Write the reaction involved in the following process.
i) Zinc in the extraction of silver.
ii)Leaching of bauxite ore to prepare pure alumina i
ii)Refining of zirconium/Titanium by Ven-Arkel method.
5.Write the principle of each of the following processes :
i)Zone refining
ii)Electrolytic refining
iii)Liquation method. iv)Vapour phase refining
v) Froath flotation method vi) Magnetic separation
6..Describe how the following changes are brought about..
i)Pig iron to steel ii)Zinc oxide to metallic zinc.iii)Impure copper to pure copper.
7.Write down the reaction taking place in different zones in different zones in the blast furnace
during the extraction of iron.
Explain the role of
(a)
SiO2 in the extraction of copper.
(b)
Graphite in the metallurgy of aluminum
(c)
NacN in both floatation process.
2.
Outline the principles behind the refining of Metals by
(a)
Zone refining method
(b)
Vapour Phase refining method
(c)
Chromatographic method
3.
(a)
(b)
4.
Describe the role of
5.
Out of C and CO, which is better reducing agent for ZnO.
Explain the principle of the method of electrolytic refining of metals. Give
one example.
(i)
Carbon monoxide in the purification of nickel
(ii)
Cryolite in the metallurgy of aluminium
(iii)
Iodine in the refining of Zirconium
Value Based Question
Ram visited he house of his friend Shyam and found that all the water taps were
rusted. On enquiry he came to know that these were iron taps. Ram advised his
friend to use either chrome plated or nickel plated taps. Shyam accepted his
advise.
(i)
Why did iron taps get rusted ?
(ii)
What is the purpose of Chrome plating or nickel plating.
(iii)
What is the name of the process ?
(iv)
What is the value associated with this ?
1. State briefly the principles which serve as basis for the following operations in
metallurgy:
(i) Froth floatation process
(ii) Zone refining
(iii) Refining by
liquation
2. Explain the basic principles of following metallurgical operations:
(i) Zone refining
(ii) Vapour phase refining
(iii) Electrolytic
refining
3. Write the chemical reactions which take place in the following operations :
(i) Electrolytic reduction of Al2O3 .
(ii) Isolation of zinc from zinc blende.
(iii) Mond’s process for refining nickel
4. Describe how the following changes are brought about:
(i) Pig iron into steel.
(ii) Zinc oxide into metallic zinc.
(iii) Impure titanium into pure titanium.
5. Describe the role of
(i) NaCN in the extraction of gold from gold ore.
(ii) SiO2 in the extraction of copper from copper matte
(iii) Iodine in the refining of Zirconium
Write chemical equations for the involved reactions
6. Explain the role of each of the following in the extraction of metals from their ores:
(i) CO in the extraction of nickel.
(ii) Zinc in the extraction of silver.
(iii) Silica in the extraction of copper
7. Write the reactions involved in the following processes:
(i) Leachiing of bauxite ore to prepare pure alumina.
(ii) Refining of zirconium by van Arkel method.
(iii) Recovery of gold after gold ore has been leached with NaCN solution
(a) *40. State the principles of refining of metal by the following methods.
(b)
(a) Zone refining (b) Electrolytic refining (c) Vapour phase refining.
(c) 41. How is pure copper obtained from its principle ore? Write the chemical reactions
occurring during the
(d)
extraction.
(e) 42. Name the method of refining of the following metals –
(f)
(a) Hg (b) Sn (c) Cu (d) Ge (e) Ni (f) Zr
(g)
(h) 45. In the cynamide extraction rocess of silver pon argentite ore, name the oxidising and
reducing agents. Write the chemical equations of the reactions involved.
VALUE BASED QUESTION (4 MARKS)
1. Magnesium is more electropositive than aluminium, therefore it can be reduced
alumina thermodynamically, but in India aluminium is being extracted by electrolytic
reduction and not chemical reduction.
(a) Under what conditions magnesium can reduce alumina?
(b) Although thermodynamically feasible, in practice, magnesium metal is not used to
reduce alumina. Explain.
(c) What are the values involved in using electrolytic reduction instead of chemical
reduction for the extraction of aluminium.
2. Metals are very useful in our daily life. Aluminium powder is used in white paints. It is
used as a reducing agent. Alloys containing aluminium, being light, are useful, Utensils
of aluminium are more popular than brass. Metals like gold, silver, iron, copper, zinc are
very useful in our daily life.
(i) Which metal foils are used as wrappers for chocolates, medicines, chapaties, etc.?
(j) Why are aluminium vessels preferred over copper and bronze vessels?
(k) What values are possessed by people using aluminium instead of copper?
5MARKS
1.The well known mineral fluorite is chemically calcium fluoride. It is known that in one unit
cell of this mineral there are 4 Ca2+ ions and 8F– ions and that Ca2+ ions are arranged in afcc
lattice. The F– ions fill all the tetrahedral holes in the fcc lattice of Ca2+ ions. The edge of the unit
cell is 5.46 ×
10–8 cm in length. The density of the solid is 3.18 g cm–3. Use this information to calculate
Avogadro’s number (Molar mass of CaF2 = 78.08 g mol–1]
2. The density of copper metal is 8.95 g cm–3. If the radius of copper atom is 127 pm, is the
copper unit cell a simple cubic, a body-centred cubic or a face centred cubic structure?
3. A metallic element has a body centered cubic lattice. Edge length of unit cell is 2.88 × 10–8
cm. The density of the metal is 7.20 gcm–3. Calculate
(a) The volume of unit cell.
(b) Mass of unit cell.
(c) Number of atoms in 100 g of metal.
The p-Block Elements (CH-7)
1 MARK QUESTIONS
1.Give reasons for the following: (a) Nitric oxide becomes brown when released in air.
(b)PCl5 is ionic in nature in the solid state.
2.In which one of the two structures,NO2+ and NO2-,the bond angle has a higher value?
3.Why is the bond angle in PH3 molecule lesser than that in NH3 molecule?
4..Assign a reason for each of the following statements: Phosphorous (P4) is more reactive than nitrogen
(N2).
5.Arrange the following in the increasing order of their basic character: NH3,PH3,AsH3,SbH3,BiH3
6.What is the basicity of H3PO3 and why?
7.Why does NO2 dimerises?
8.Fluorine does not exhibit any positive oxidation state.Why?
9.Why is BiH3 the strongest reducing agent amongst all the hydrides of Group 15 elements?
10.Name two poisonous gases which can be prepared from chlorine gas?
11.What is the covalency of nitrogen in N2O5 ?
12.What is the basicity of H3PO3?
1
13.Why does NO2 dimerises?
14.Why is the single N-N bond weaker than the single P-P bond?
15.Why does NH3 act as a Lewis base
1. Draw the structure of XeF6.
2. Which is a stronger reducing agent, SbH3 or BiH3 and why ?
3. What is the basicity of H3PO2 acid and why ?
4. Why does NO2 dimerise ?
5. What is the oxidation number of phosphorus in H3PO2 molecule ?
6. Nitrogen is relatively inert as compared to phosphorus, why ?
(I)
Write one chemical reaction to show that conc. H2SO4 is a strong oxidising
agent. .
7.
8. Give an example of a compound in which the oxidation state of chlorine is +7.
9. Why does oxygen not show the oxidation state of +4 and +6 like sulphur ?
10. Why is OF6 compound not known ?
11. Why is NH3 good complexing agent ?
12. Oxygen-Oxygen bond length in ozone is same.Explain.
13. Which of the xenon fluoride molecule is isostructural with IF5 ? Draw the structure of its
molecule.
14. Which is the strongest oxidising agent among ClO4-, BrO4- and IO3- ?
15. Nitrogen does not form pentahalides. Give reason.
16. In which one of the two structures NO2+ And NO2-the bond angle has higher value?
17. Which has higher electron gain enthalpy with negative sign,sulphur or oxygen?
18. NF3 is exothermic but NCl3 is endothermic why?
19. Flourie does not exhibit positive oxidation state?
20. Which is a stronger acid in aq. Solution-HCl or HI?
21. The tendency to exhibit – 3 oxidation state, decreases down the group in group 15
elements. Explain.
22. The boiling point of PH3 is lesser than NH3 . Why?
23. Write disproportionation reaction of H3PO3 ?
24. With what neutral molecule ClO– is isoelectronic?
25. What is cause of bleaching action of chlorine water? Explain it with chemical equation
26. In which one of the two structures, NO2+ and NO2- , the bond angle has a higher value?
27. Mention all the oxidation states exhibited by chlorine in its compounds.
28. Why is Bi (V) a stronger oxidant than Sb (V)?
29. Why is red phosphorus less reactive than white phosphorus?
30. Which one has higher electron gain enthalpy with negative sign, sulphur or oxygen?
31. Why does NO2 dimerise?
32. NF3 is an exothermic compound but NCl3 is endothermic compound.
33. ClF3 molecule has a T-shaped structure and not a trigonal planar one.
34. What is the oxidation number of phosphorus in H3PO2 molecule
35. Draw the structure of O3 molecule.
36. Fluorine does not exhibit any positive oxidation state. Why?
37. Nitrogen is relatively inert as compared to phosphorus. Why?
38. Which is a stronger acid in aqueous solution—HCl or HI, and why?
39. H2S is less acidic than H2Te . Why?
40. Noble gases are the least reactive elements, Why?
41. Mention the optimum conditions for the industrial manufacture of ammonia by Haber’s
process.
42. Which one of PCl4+ and PCl4– is not likely to exist and why?
43. Which is a stronger reducing agent, SbH3 or BiH3, and why?
44. Explain all the bonds in SF4 are not equivalent.
45. Although the H-bonding in hydrogen fluoride is much stronger than that in water, yet
water has a much higher boiling point than hydrogen fluoride. Why?
46. 1.In group 15 elements, there is considerable increase in covalent radius from N to P but
small increase from As to Bi. Why?
47. 2. The tendency to exhibit – 3 oxidation state, decreases down the group in group 15
elements. Explain.
48. 3. Maximum covalence of Nitrogen is ‘4’ but the heavier elements of group 15 show
covalence greater than ‘4’. Why?
49. 4. Nitrogen exists as a diatomic molecule with a triple bond between the two atoms, whereas
the heavier
50. elements of the group do not exist as E2 at room temperature. Assign a reason.
51. 5. The ionization enthalpies of group 15 elements are higher than those of corresponding
members of group 14
52. and 16 elements. Assign the reason.
53. 6. The boiling point of PH3 is lesser than NH3. Why?
54. 7. NO2 dimerises to form N2O4. Why?
55. 8. Draw the structure of N2O5 molecule.
56. 9. How does ammonia solution react with Ag+ (aq)? Write the balanced chemical equation.
57. 10. Why does NH3 forms intermolecular hydrogen bonds whereas PH3 does not?
58. 11. Write disproportionation reaction of H3PO3?
59. 12. How does NH3 acts as a complexing agent?
60. 13. Why HF is the weakest acid and HI is the strongest.
61. 14. Explain why halogens are strong oxidising agents.
62. 15. Why is Bi(V) a stronger oxidant than Sb(V)?
63. 16. Why SF4 is easily hydrolysed, whereas SF6 is resistant to hydrolysis?
64. 17. Bond dissociation enthalpy of F2 is less than that of Cl2. Why?
65. 18. Write the reaction of PCl5 with heavy water.
66. 19. How many P – O – P bonds are there in cyclotrimetaphosphoric acid?
67. 20. In group 16, the stability of +6 oxidation state decreases and that of +4 oxidation state
increases down the group. Why?
68. 21. Why we can not prepare HBr by heating KBr with sulphuric acid.
69. 24. Fluorine exhibit only –1 oxidation state whereas other halogens exhibit +ve oxidation
states also. Explain.
70. 25. Arrange the following oxoacids of chlorine in increasing order of acidic strength.
71.
HOCl, HOClO, HOClO3, HOClO3
72. *26. The majority of known noble gas compounds are those of Xenon. Why?
73. *27. “Hypophosphorus acid is a good reducing agent.” Justify with an example.
74. *28. Draw the structure of H4P2O7 and find out its basicity?
75.
*29. Arrange the following triatomic species in the order of increasing bond angle. NO2, NO2+,
NO2–
76.
77.
78.
79.
80.
81.
30. With what neutral molecule ClO– is isoelectronic?
31. Draw the structure of H2S2O8 and find the number of S–S bond if any.
32. What is cause of bleaching action of chlorine water? Explain it with chemical equation?
*33. Electron gain enthalpy of fluorine is more negative than that of chlorine.
*34. Which one of the following is not oxidised by O3. State the reason.
Kl, FeSO4, K2MnO4, KMnO4
2marks
1.How would you account for the following:
(i)Sulphur hexafluoride is less reactive than sulphur tetrafluoride.
(ii)Of the noble gases only xenon forms known chemical compounds.
2.Compare the structural shapes of the following species: SF6 and SF4 ?
3..Answer the following:
(i)Which neutral molecule would be isoelectronic with ClO-?
(ii)Of Bi(V) and Sb(V) which may be a stronger oxidizing agent and why?
4.(a)Draw the structures of the following:
(i) XeF4 (ii)H2S2O7
5.(a)Complete the following reaction equations:
(i)P4 + NaOH + H2O
(ii)Cu + HNO3(dilute)
6.Complete the following reaction equation:
(i)XeF4 + H2O
(ii)I2 + H2O + Cl2
7.Explain the following facts giving appropriate reason in each case :
(i)NF3 is an exothermic compound whereas NCl3 is not. (ii)All the bonds in SF4 are not equivalent.
8.What happens when
(i)PCl5 is heated ?
(ii)H3PO3 is heated?
Write the reactions involved .
9.Draw the structures of the following molecules:
(i) XeOF4 (ii) H3PO3
10.How are interhalogen compounds formed ?What general compositions can be assigned to them?
11.Draw the structures of the following molecules:
(i) XeF6 (ii)H2S2O7 (iii)BiH3 is the strongest reducing agent amongst all the hydrides of Group 15
elements.
12.Draw the structures of the following molecules:
(i)N2O5
(ii)XeF2
13.Complete the following equations :
(i)P4 + H2O
(ii)XeF4 + O2F2
14.Draw the structures of the following :
(i) XeF2
(ii) BrF3
15.Complete the following equations:
(i)Ag +PCl
(ii)CaF2 + H2SO4
16.Draw the structures of the following :
(i)XeF4 (ii)HClO4
17.Draw the structures of the following :
(i)XeO3 (ii)H2SO4
18 .Name the two most important allotropes of sulphur. Which one of the two is stable at room
temperature?
What happens when the stable form is heated above 370K?
19.(i)Write the condition to maximize the yield ofH2SO4 by contact process.
(ii)Why is Ka2 <<Ka1 for H2SO4 in water?
20 .Complete the following chemical equations:
(i) Ca3P2 + H2 O
(ii)Cu + H2SO4 (Conc.)
21.Arrange the following in order of property indicated against each set:
(i)HF,HCl,HBr,Hi -increasing bond dissociation enthalpy. (ii)H2O,H2S,H2Se,H2Te -increasing acidic
character.
22.(a)Draw the structures of the following molecules:
(ii)H2SO4
(i)XeOF4
1. State reasons for each of the following ;
(II)
All P−Cl bonds in PCl5 molecule are not equivalent.
(III) Sulphur has greater tendency for catenation than oxygen.
2. Complete the following reactions :
(i)
XeF6 + H2O →
(ii)
FeSO4 + H2SO4 + Cl2 →
3. Draw the structure and predict the shape of
(i)
XeO3 and
(ii)
BrF3
4. Give reason for the following :
(a) Deep sea divers use a mixture of He (80%) and O2 (20%) instead of air for breathing.
(b) Among the hydrogen halides, HF is least volatile, whereas HCl is most volatile.
5. Write the chemical equation for the reactions which occur when :
(i)
SO2 reacts with hydrogen sulphide (H2S)
(ii)
Sulphur dioxide reacts with sodium chlorate in strongly acidic solution.
6. Account for the following
(i)
PbCl4 is more covalent than PbCl2
(ii)
SF6 is kinetically an inert substance
7.
Write balanced chemical equations for the following
(a)
H3PO3 is added to AgNO3 solution.
(b)
Chlorine gas is passed through hot and concentration NaOH
Solution.
8. (a)
Explain the structure of the following.
(i)
Xe F2
(ii) Br F3
(b)
Complete the following equation
9.
Cl2 + F2 (excess) 10.
Account for the following
(i)
ICl is more reactive than I2.
(ii)
Bi (V) is a stronger oxidizing agent than Sb(v)
1.
2.
.
Draw the structures of BrF3 , XeOF4 using VSEPR theory.
Complete the equations
(i) (NH4 ) 2 Cr2O7heat→
3.
4.
(ii) NH4Cl (aq) + NaNO2 (aq) →
(i) Interhalogen compounds are more reactive than halogens except F2 . Why?
(ii) Give one important use of ClF3 .
“Hypophosphorus acid is a good reducing agent.” Justify with an example.
1. Assign a reason for each of the following statements:
(i) Ammonia is a stronger base than phosphine.
(ii) Sulphur in vapour state exhibits a paramagnetic behaviour.
2. Draw the structure of the following molecules: (i) SF4 (ii) XeF4
3. Assign reasons for the following :
(i) In liquid state, hydrogen chloride is a stronger acid than hydrogen fluoride.
(ii) Phosphorus (P4 ) is much more reactive than nitrogen (N2 ).
4. Draw the structures of the following molecules:
(i) XeF4 (ii) BrF3
5. Complete the following chemical reaction equations:
(i) P4( s) +NaOH (aq) +H2O( l ) →
(ii) I- (aq ) + H2O(l) + O3(g ) →
6. Complete the following chemical reaction equations:
(i) XeF2 + H2O →
(ii) PH3 + HgCl2 →
7. Draw the structures of the following molecules:
(i) BrF3 (ii) H2S2O7
8. State reasons for the following observations:
(i) The enthalpies of atomisation of transition elements are quite high.
(ii) There is a greater horizontal similarity in the properties of the transition elements
than of the main group elements.
9. Draw the structures of white phosphorus and red phosphorus. Which one of these two
types of phosphorus is more reactive and why?
10. Complete the following chemical reaction equations::
(i) P4 + SO2Cl2 →
(ii) XeF4 + H2O →
11. Complete the following chemical reaction equations:
(i) I2 + HNO3 → (ii) HgCl2 + PH3→
12. State reasons for each of the following:
(i) The N–O bond in NO2 – is shorter than the N–O bond in NO3 – .
(ii) SF6 is kinetically an inert substance.
13. State reasons for each of the following:
(i) All the P—Cl bonds in PCl5 molecule are not equivalent.
(ii) Sulphur has greater tendency for catenation than oxygen.
.
2. Why is red phosphorus denser and less chemically reactive than white phosphorus?
3. Give chemical reaction in support of the statement that all the bonds in PCl5 molecule are not
equivalent.
4. Account for the following :
(a) XeF2 has linear structure and not a bent structure.
(b) Phosphorus show marked tendency for Catenation.
5. Draw the structures of BrF3, XeOF4, XeO3 using VSEPR theory.
6. Write the conditions that favour the formation of ammonia gas along with the reactions involved in
Haber’s Process.
7. Write the chemical equations of the following reactions
(a) Glucose in heated with conc. H2SO4.
(b) Sodium nitrate is heated with conc. H2SO4.
Complete the following reactions :
heat→
(ii) N4H Cl (aq) + NaNO2 (aq) →
9. (i) NH2CONH2 + H2O →
(ii) FeCl3 (aq) + NH4OH →
10. (i) Ca3 P2 + H2 O (l) →
(ii) I2 + HNO3 (conc.) →
11. (i) Ba(N3)2heat→
(ii) 4H3PO3 heat→
12. (i) PH4I + KOH →
(ii) HgCl2 + PH3 →
13. (i) PCl3 + 3H2O →
(ii) S + H2SO4 (conc.) →
14. (i) Al2O3(s) + NaOH (aq) + H2O(l) →
8. (i) (NH4)2 Cr2O7
(ii) HCl + O2 2 CuCl →
→
(ii) XeF4 + H2O →
16. (i) Na2SO3 + Cl2 + H2O →
(ii) NaHCO3 + HCl →
15. (i) Ca(OH)2 + Cl2
17. (i) XeF6 + H2O Completehydrolysis →
(ii) XeF6 + H2O Partialhydrolysis →
→
(ii) Zn + HNO3 (dil) →
19. (i) Zn + HNO3 (conc) →
18. (i) NO3– + Fe2+ + H+
(ii) P4 + HNO3 (conc)
→
20. (i) NH3 + O2Pt/Rh→
→
21. (i) P4 + SOCl2 →
(ii) P4 + SO2Cl2 →
22. (i) PbS + O3 →
(ii) KI + H2O + O3 →
23. (i) MnO4– + SO2 + H2O →
(ii) Zn + HNO3 →(dil)
24. (i) NH3 (Excess) + Cl2 →
(ii) NH3 + Cl2 (Excess) →
25. (i) Cl2 + NaOH (cold and dil) →
(ii) Cl2 + NaOH (hot & conc) →
26. (i) Fe + HCl →
(ii) Cl2 + F2 (Excess) →
27. (i) U + ClF3 →
(ii) FeSO4 + H2SO4 + Cl2 →
(ii) P4 + NaOH + H2O
28. (i) What is the covalency of N in N2O5?
(ii) Explain why phosphorus forms pentachloride whereas nitrogen and bismuth do not?
29. (i) The acidic character of hydrides of group 15 increases from H2O to H2Te. Why?
(ii) Dioxygen is a gas while sulphur (S8) is a solid. Why?
30. (i) Interhalogen compounds are more reactive than halogens except F2. Why?
(ii) Give one important use of ClF3.
31. (i) Write the composition of bleaching powder.
(ii) What happens when NaCl is heated with conc. H2SO4 in the presence of MnO2. Write the
chemical equation.
32. Arrange the following in the decreasing order of their basicity. Assign the reason :
PH3, NH3, SbH3, AsH3, BiH3.
*33. A colourless and a pungent smelling gas which easily liquifies to a colourless liquid and freezes
to a white
crystalline solid, gives dense white fumes with ammonia. Identify the gas and write the chemical
equation for
its laboratory preparation. [Hint : HCl]
*34. Complete following disproportionation reactions.
(a) P4 + NaOH + H2O
→
(b) HNO2H+ →
35. Arrange the following trichlorides in decreasing order of bond angle NCl3 PCl3, AsCl3, SbCl3
36. Suggest reason why only known binary compounds of noble gases arefluorides and oxides of
Krypton, Xenon.
37. Which fluorinating agent are oftenly used instead of F2? Write two chemical equations showing
their use as fluorinating agents.
38. (a) Hydrolysis of XeF6 is not regarded as a redox reaction. Why?
(b) Write a chemical equation to represent the oxidising nature of XeF4.
39. Write Chemical equation :
(a) XeF2 is hydrolysed
(b) PtF6 and Xenon are mixed together.
3marks
1. (i) How is HNO3 prepared commercially?
(ii) Write chemical equations of the reactions involved.
(iii) What concentration by mass of HNO3 is obtained?
2. (i) How does O3 react with lead sulphide? Write chemical equation.
(ii) What happens when SO2 is passed in acidified KMnO4 solution?
(iii) SO2 behaves with lime water similar to CO2.
3. Assign reason for the following :
(i) Sulphur in vapour state exhibits paramagnetism.
(ii) F2 is strongest oxidising agent among halogens.
(iii) In spite of having same electronegativity, oxygen forms hydrogen bond while chlorine does not.
4. Give appropriate reason for each of the following :
(i) Metal fluorides are more ionic than metal chlorides.
(ii) Perchloric acid is stronger than sulphuric acid.
(iii) Addition of chlorine to KI solution gives it a brown colour but excess of Cl2 makes it colourless.
5. Explain why :
(i) No chemical compound of helium is known.
(ii) Bond dissociation energy of fluorine is less than that of chlorine.
(iii) Two S–O bonds in SO2 are identical.
6. Out of the following hydrides of group 16 elements, which will have :
(i) H2S (ii) H2O (iii) H2Te
(a) lowest boiling point
(b) highest bond angle
(c) highest electropositive hydrogen.
7. (i) How is XeO3 prepared from XeF6? Write the chemical equation for the reaction.
(ii) Draw the structure of XeF4.
8. (i) Thermal stability of hydrides of group 16 elements decreases down the group. Why?
(ii) Compare the oxidising powers of F2 and Cl2 on the basis of bond dissociation enthalpy,
electron gain
ethalpy of halogens and hydration enthalpy of halide ions.
(iii) Write the chemical equation for the reaction of copper metal with conc. HNO3.
*9. An unknown salt X reacts with hot conc. H2SO4 to produce a brown coloured gas which
intensifies on
addition on copper turnings. On adding dilute ferrous sulphate solution to an aqueous solution of
X and
then carefully adding conc. H2SO4 along the sides of the test tube, a brown complex Y is formed
at the
interface between the solution and H2SO4. Identify X and Y and write the chemical equation
involved in
the reaction.
10. Assign reason to the following :
(i) Noble gases have large positive values of electron gain enthalpy.
(ii) Helium is used by scuba divers.
11. Arrange the following in the order of the property indicated for each set–
(a) F2, Cl2, Br2, I2 (Increasing bond dissociation energy).
(b) HF, HCl, HBr, HI (decreasing acid strength).
(c) NH3, PH3, ASH3, SbH3, BiH3 (decreasing base strength).
*12. A transluscent while waxy solid (A) on heating in an inert atmosphere is converted to its
allotropic form (B),
Allotrope (A) on reaction with very dilute aqueous NaOH liberates a highly poisonous gas (C)
having a
Rotten fish smell, with excess of chlorine forms D which hydrolyses to form compound (E).
Identify the
compounds (A) to (E).
13. Write balanced equation for the following reactions :
(a) Zn is treated with dilute HNO3.
b) NaCl is heated with H2SO4 in the presence of MnO2.
(c) Iodine is treated with conc. HNO3.
14. X2 is a greenish yellow gas with pungent offensive smell used in purification of water. It partially
dissolves in
H2O to give a solution which turns blue litmus red. When X2 is passed through NaBr Solution,
Br2 is btained.
(a) Identify X2, name the group to which it belongs.
(b) What are the products obtained when X2 reacts with H2O? Write chemical equation.
(c) What happens when X2 reacts with hot and conc. NaOH? Give equation.
15. Assign the appropriate reason for the following:
(a) Nitrogen exists as diatomic molecule and phorphorous as P4, Why?
(b) Why does R3P = 0 exist but R3N = 0 does not ? (R = an alkyl group).
(c) Explain why fluorine forms only one oxoacid, HOF.
1.Draw the structures of the following:
(i) PCl5(g (ii)S8(g) (iii)ClF3(g)
2.Complete the following chemical equations:
(i)Ca3p2(s) + H2O(l)
…………………
(ii)Cu2+(aq) + NH3 (aq)
……………….
(excess)
(iii)F2(g) + H2O(l)
……………………..
4.Explain the following situations:
(i) In the structure of HNO3 molecule, the N-O bond (121pm) is shorter than N-OH bond (140 pm).
(ii) SF4 is easily hydrolysed whereas SF6 is not easily hydrolysed .
(iii) XeF2 has a straight linear structure and not a bent angular structure.
(b)Explain the following observations:
(i) Phosphorous has a greater tendency for catenation than nitrogen.
(ii)The negative value of electron gain enthalpy is less for fluoride than that for chlorine.
(iii)Hydrogen fluoride has a much higher boiling point than hydrogen chloride.
5.Arrange the following in order of the property mentioned:
(i)PH3,NH3,SbH3,AsH3 ( increasing basic strength)
(ii)HCL,HBr,HI,HF
(increasing acid strength)
(iii)HClO4,HClO,HClO2 (increasing oxidizing power)
6.How would you account for the following:
(i)NF3 is an exothermic compound but NCl3 is not.
(ii)The acidic strength of compounds increase in the order:
PH3<H2S<HCl
(iii)SF6 is kinetically inert.
7.Account for the following:
(i)PCl5 can act as an oxidizing agent but not as a reducing agent.
(ii)Dioxygen is a gas but sulphur is a solid.
(iii)Halogens are coloured.
8.Complete the following chemical equations:
(i) P4 + SO2Cl2
(ii)XeF2 + H2O
(iii)I2 + HNO3(conc.)
(i)XeF2 (ii)H2S2O8
9.Write the types of isomerism exhibited by the following complexes:
(i) [Co(NH3)5Cl]SO4 (ii)[Co(en)3]3+ (iii)[Co(NH3)6] [Cr(CN)6]
10.Give reasons for the following :
(i)R3P=O exists but R3N=O does not, where R is an alkyl group.
(ii) PbCl4 is more covalent than PbCl2.
(iii)At room temperature, N2 is much less reactive.
11.Give reasons for the following :
(i)Oxygen is a gas but sulphur is a solid.
(ii)O3 acts as a powerful oxidizing agent .
12.Give reasons for the following :
(i)Though nitrogen exhibits +5 oxidation state,it does not form pentahalide.
(ii)Electron gain enthalpy with negative sign of Fluorine is less than that of chlorine.
(iii)The tho oxygen-oxygen bond lengths in ozone molecule are identical.
13.Account for the following:
(i) White phosphorous is more reactive than red phosphorous.
(ii)SnCl4 is more covalent than SnCl2.
(iii)O3 is a powerful oxidizing agent.
14.Complete the following equations:
(i)PCl5 +H2O
(ii)XeF2 +PF5
(iii)NaN3
HEAT
15.Draw the structures of the following molecules:
(i)PCl5 (ii)H4P2O7 (iii)ClF3
16.Draw the structures of the following:
(i)Solid PCl5 (ii)H2S2O8 (iii)Xeo3
17 (i)PCl5 is more covalent than PCL3.
(ii)Iron on reaction with HCl forms FeCl2 and not FeCl3.
(iii)The two o-o bond lengths in the ozone molecule are equal.
18 .Account for the following:
(i)Bi(V) is a stronger oxidizing agent than Sb(V).
(ii)N-N single bond is weaker than P-P single bond.
(iii)Noble gases have very low boiling points.
19.(a)Draw the structures of the following compounds:
(i)XeF4
(ii)N2O5
(b)Write the structural differences between white phosphorous and red phosphorous.
20.Account for the following :
(i)Sulphur in vapour form exhibits paramagnetic behavior.
(ii)SnCl4 is more covalent than SnCl2.
(iii)H3PO2 is a stronger reducing agent than H3PO3.
21.Give reasons for the following:
(i) (CH3)3 P=0 exists but (CH3)3 N=O does not.
(ii)Oxygen has less electron gain enthalpy with negative sign than sulphur.
(iii)H3PO2 is a stronger reducing agent than H3PO3.
1. Draw the structure of the following molecules :
(i)
NF3
(ii)
H2S2O8
(iii) H3PO3
2. Account for the following :
(i)
PCl5 can act as an oxidising agent but not as a reducing agent.
(ii)
Dioxygen is a gas but sulphur is a solid.
(iii) Halogens are coloured.
3. Write balanced chemical equations for the following reactions :
(i)
Chlorine is passed through hot conc. NaOH solution.
(ii)
XeF6 is hydrolysed,
(iii) Excess of SO2 reacts with sodium hydroxide solution.
4. Arrange the following in order of the property mentioned ;
(i)
PH3, NH3, SbH3, AsH3 (increasing basic strength)
(ii)
HCl, HBr, HI, HF ( increasing acid strength )
(iii) HClO4, HClO, HClO2 (increasing oxidising power)
5. Mention three areas in which H2SO4 plays an important role.
(i) How does O3 react with lead sulphide? Write chemical equation.
(ii) What happens when SO2 is passed in acidified KMnO4 solution?
(iii) SO2 behaves with lime water similar to CO2 .
2.
Assign the appropriate reason for the following:
(a) Nitrogen exists as diatomic molecule and phorphorous as P4 , Why?
(b) Why does R3P = 0 exist but R3N = 0 does not ? (R = an alkyl group).
(c) Explain why fluorine forms only one oxoacid, HOF.
1. Write chemical equations for the following processes:
2.
3.
4.
5.
6.
7.
(i) Chlorine reacts with a hot concentrated solution of sodium hydroxide.
(ii) Orthophosphorous acid is heated
(iii) PtF6 and xenon are mixed together.
Complete the following chemical equations:
(i) Ca 3P2 (s) + H2O(l) →
(ii) Cu 2+ (aq) + NH3 (aq) (excess) →
Account for the following:
(i) NH3 is a stronger base than PH3.
(ii) Sulphur has a greater tendency for catenation than oxygen.
(iii) Bond dissociation energy of F2 is less than that of Cl2.
Explain the following situations:
(i) In the structure of HNO3 molecule, the N—O bond (121 pm) is shorter than N—OH
bond (140 pm).
(ii) SF4 is easily hydrolysed whereas SF6 is not easily hydrolysed.
(iii) XeF2 has a straight linear structure and not a bent angular structure.
How would you account for the following:
(i) NCl3 is an endothermic compound while NF3 is an exothermic one.
(ii) XeF2 is a linear molecule without a bend.
The electron gain enthalpy with negative sign for fluorine is less than that for chlorine,
still fluorine is a stronger oxidising agent than chlorine
Answer the following:
(i) What is the basicity of H3PO3 and why?
(ii) Why does fluorine not play the role of a central atom in interhalogen compounds?
(iii)Why do noble gases have very low boiling points
4marks
1. Scientists have claimed that chloroform (CFC) and other gases emitted from the exhaust
system of supersonic aeroplanes might be slowly depleting the concentration of the
ozone layer in the upper atmosphere.
(a) Name the gas emitted by the exhaust of supersonic jet aeroplanes.
(b) What are the other sources of ozone depleting gases?
(c) Mentions the values that are leant by the students in this depletion of ozone layer.
(d) How does nitric oxide deplete the ozone layer?
2. Ozone is formed in upper atmosphere by photochemical reaction involving dioxygen.
Ozone absorbs UV radiations and protects earth and inhabitants from harmful UV
radiations from sun.
It is prepared by passing silent electric discharge through oxygen gas in the laboratory.
௎௏௢௥ ௦௜௟௘௡௧ ௘௟௘௖௧௥௜௖ ௗ௜௦௖௛௔௥௚௘
3O2(g)
ሱۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛۛሮ 2O3(g)
(a) What is the cause of depletion of ozone layer?
(b) Why is silent electric discharged used for preparation of ozone?
(c) Which is better oxidizing agent: O3 or F2? Explain.
(d) Should we ban CFCs? What are the value associated with it?
Though nitrogen exhibits +5 oxidation state, it does not form pentahalides. Give reason.
2.
Draw the structure of XeF6 molecule.
3.
With what neutral molecule is Clo isoelectronic.
4.
Nitric Oxide (NO) is paramagnetic in gaseous state where as solid and liquid NO
is diamagnetic. Give Reason.
5.
H3PO2 is a stronger reducing agent than H3PO3. Explain.
6.
Why does NO2 dimerise ?
7.
What is the barocity of H3PO2 and why ?
LONG ANSWER TYPE QUESTIONS (5 - MARK QUESTIONS)
1. How is PH3 prepared in the laboratory? How is it purified? How does the solution of PH3 in water
react on
irradiation with light and on absorption in CuSO4? How can you prove that PH3 is basic in nature?
Write the chemical equations for all the reactions involved.
2. Assign a possible reason for the following :
(a) Stability of +5 oxidation state decreases and that of +3 oxidation state increases down
the group 15 elements.
(b) H2O is less acidic than H2S.
(c) SF6 is inert while SF4 is highly reactive towards hydrolysis.
(d) H3PO2 and H3PO3 act as good reducing agents while H3PO4 does not.
(e) Noble gases have comparatively large size in their respective periods.
3. (a) How is XeF6 prepared from the XeF4? Write the chemical equation for the reaction.
(b) Deduce the structure of XeF6 using VSEPR theory.
(c) How does XeF2 reacts with PF5?
(d) Give one use each of helium and neon.
(e) Write the chemical equation for the hydrolysis of XeF4.
4. (a) Why does nitrogen show anomalous behaviour? Discuss the trend of chemical reactivity of
group 15
elements with. (a) oxygen (b) halogens (c) metals
(b) H3PO3 is a dibasic acid. Why?
5. (a) Arrange the following in the order of their increasing acid strength.
(i) Cl2O7, SO2, P4O10
(b) How is N2O gas prepared? And draw its structure.
(c) Give one chemical reaction to show O3 is an oxidising agent.
*6. A white waxy, translucent solid, M, insoluble in water but soluble in CS2, glows in dark. M
dissolves in NaOH
in an inert atmosphere giving a poisonous gas (N). Also M catches fire to give dense white fumes
of Q :
(a) Identify M, N and Q and write the chemical equations of the reactions involved.
(b) M exists in the form of discrete tetrahedral molecules. Draw its structure.
(c) M on heating at 573 K is changed into other less reactive form, Q, which is nonpoisonous, insoluble
in water as well as in CS2 and does not glow in dark, Identify Q and draw its structure.
7. Give reason for each of the following :
(a) NH3 is more basic than PH3.
(b) Ammonia is a good complexing agent.
(c) Bleaching by SO2 is temporary.
(d) PCl5 is ionic in solid state.
(e) Sulphur in vapour state exhibits paramagnetism.
1.(a)Complete the following reaction equations:
(i)PCl5 + H2O(excess)
(ii)F2 + H20
(b) Explain the following observations:
(i)No distinct chemical compound of helium is known.
(ii)Phosphorous has a greater tendency for catenation than nitrogen.
(iii)In solution of H2SO4 in water,the second dissociation constant Ka2 ,is less than the first
dissociation constant Ka1 .
2.(a)Give reasons for the following :
(i)Bond enthalpy of F2 is lower than that of Cl2.
(ii)PH3 has lower boiling point than NH3.
(b)Draw the structures of the following molecules:
(i) BrF3
(ii) (HPO3)3
(iii)XeF4
3.(a)Account for the following:
(i) Helium is used in driving apparatus.
(ii)Fluorine does not exhibit positive oxidation state.
(iii)Oxygen shows catenation behavior less than sulphur.
(b)Draw the structures of the following molecules:
4.(a) Account for the following :
(i)Bi is a strong oxidizing agent in the +5 state.
(ii)PCl5 is known but NCl5 is not known.
(iii)Iron dissolves in HCl to form FeCl2 and not FeCl3.
(b) Draw the structures of the following :
(i)XeOF4
(ii)HClO4
5. (a)Draw the structures of the following :
(i)H2S2O8
(ii)Red P4
(b)Account for the following :
(i)Sulphur in vapour state exhibits paramagnetism.
(ii)Unlike xenon , no distinct chemical compound of helium is known.
(iii)H3PO2 is a stronger reducing agent than H3PO3.
6..(a) Arrange the following in order of property indicated for each set:
(i)HF,HCl,HBr,HI – Increasing acid strength.
(ii)NH3,PH3,AsH3,SbH3,BiH3 -increasing reducing power.
(b)Draw the structures of the following molecules:
(i)N2O5
(ii)H3PO2
(iii)XeF6
1. Account for the following ;
(i)
Xe has highest polarising power.
(ii)
Halogens are coloured.
(iii) Noble gases are mostly chemically inert.
(iv)
Nitrogen does not form pentahalides.
(v)
Bismuth is a strong oxidising agent in pentavalent state.
2. (a) Complete the following chemical equations ;
(i)
F2 + H2O →
(ii)
Ca3P2 + H2O →
(iii)
XeF4 + H2O→
(c) Draw structures of the following species :
(i)
H2S2O7
(ii)
NO33. Give appropriate reasons for each of the following observations :
(i)
Sulphur vapour exhibits some paramagnetic behaviour.
(ii)
Interhalogen compounds are more reactive than halogens.
(iii) Of the noble gases only xenon is known to form real chemical compounds.
(iv)
Despite lower electron affinity F2is stronger oxidising agent than Cl2.
Nitrogen shows little tendency for catenation, whereas phosphorus shows a clear
tendency for catenation
12.
(a)
(b)
13.
(a)
(b)
14.
(a)
Draw the structures of
(ii)
Xe OF4
(i)
H4P2O7
Give reason for the following
(i)
Noble gases have comparatively large atomic sizes
(ii)
H2S is more acidic than H2O
(iii)
Ozone is thermodynamically unstable
Complete the following reactions
(i)
Ca3P2 + H2O (ii)
Pcl5 + D2O Give reason for the following
(i)
Pcl5 is more covalent than Pcl3
(ii)
NH3 is a stronger base than pH3
(iii)
Bond enthalpy of F2 is lower than that of Cl2
Give Reason
(i)
ClF3 is known but FCl3 is not known.
(b)
15.
1.
(ii)
Sulphur shows greater tendency for catenation than oxygen
(iii)
Red Phosphorous is less reactive than white phosphorous
Complete the following reactions
(i)
P4 + NaOH + H2O (ii)
Cu + HNO3 (dil.) (a)
Arrange the following in order of property – indicated against each set.
(i)
HF, Hcl, HBr, HI Increasing bond dissociation enthalpy
(ii)
H2O, H2S, H2Se, H2Te Increasing acidic strength
(iii)
NH3, PH3, ASH3, SbH3, BiH3 – Increasing basic strength
(b)
Draw the structures of
(i)
H2S2O7
(ii) HclO3
How is PH3 prepared in the laboratory? How is it purified? How does the solution of PH3
in water react on irradiation with light and on absorption in CuSO4 ? How can you prove
that PH3 is basic in nature? Write the chemical equations for all the reactions involved
1. (a) Assign reasons for the following :
(i) Bi (V) is a stronger oxidising agent than Sb (V).
(ii) Of the noble gases only xenon is known to form established chemical compounds.
(b) Draw the structures of the following molecules :
(i) H2S2O7 (ii) BrF3 (iii) XeF2
2. Complete the following chemical reaction equations :
(i) Ca 3P2 + H2O →
(ii) XeF4 + H2O →
(b) How would you account for the following observations :
(i) NH3 is a stronger base than PH3 .
(ii) Sulphur in vapour state exhibits paramagnetism.
(iii) Hydrogen fluoride has a higher boiling point than hydrogen chloride.
3. (a) Draw the structures of the following:
(i) H2S2O8(ii) HClO4
(b) How would you account for the following:
(i) NH3 is a stronger base than PH3.
(ii) Sulphur has a greater tendency for catenation than oxygen.
(iii) F2 is a stronger oxidising agent than Cl2.
4. Draw the structures of the following:
(i) H2S2O7
(ii) HClO3
(b) Give an explanation for each of the following observations:
(i) In the structure of HNO3, the N – O bond (121 pm) is shorter than the N – OH bond
(140 pm)
(ii) All the P – Cl bonds in PCl5 are not equivalent.
(iii)
ICI is more reactive than I2.
5. (a) Draw the structure of the following:
(i) H3PO2
(ii) BrF3
(b) How would you account for the following observations:
(i) Phosphorus has a greater tendency for catenation than nitrogen.
(ii) Bond dissociation energy of fluorine is less than that of chlorine.
(iii) No chemical compound of helium is known.
(a) Draw the structures of the following:
(i) N2O5
(ii) XeOF4
(b) Explain the following observations:
(i) The electron gain enthalpy of sulphur atom has a greater negative value than that of
oxygen atom.
(ii) Nitrogen does not form pentahalides.
(iii)In aqueous solutions HI is a stronger acid than HCl.
6. (a) Draw the structures of the following:
(i) XeF4
(ii) H2S2O7
(b) Explain the following observations:
(i) Phosphorus has a greater tendency for catenation than nitrogen.
(ii) The negative value of electron gain enthalpy is less for fluorine than that for chlorine.
(iii) Hydrogen fluoride has a much higher boiling point than hydrogen chloride.
UNIT-8
d – AND f – BLOCK ELEMENTS
1marks
1. Write the electronic configuration of Cr3+ ion (atomic number of Cr = 24)?
2. Explain CuSO4. 5H2O is blue while ZnSO4 and CuSO4 are colourless?
3. Why is the third ionisation energy of Manganese (Z = 25) is unexpectedly high?
4. Which element among 3d– transition elements, exhibit the highest oxidation state?
5. Silver (Ag) has completely filled d-orbitals (4d10) in its ground state. How can you say that it is a
transition element.

6. In 3d series (Sc → Zn), the enthalpy of atomisation of Zn is low. Why?
7. Out of the following elements, identify the element which does not exhibit variable oxidation state?
Cr, Co, Zn.
8. The +3 oxidation state of lanthanum (Z = 57), gadolinium (Z = 64) and lutetium (Z = 71) are
especially stable
Why?
10. Mention one consequence of Lanthanoid Contraction?
11. The first ionization enthalpies of 5d– series elements is higher than those of 3d and 4d series
elements why?
12. Why Mn2+ compounds are more stable than Fe2+ compounds towards oxidation to their +3 state?
14. Calculate the magnetic moment of Cu2+ (Z = 29) on the basis of “spin-only” formula.
15. What is the shape of chromate ions?
16. Why does vanadium pentoxide act a catalyst?
17. What are interstitial compounds?
18. The transition metals and their compounds are known for their catalytic activity. Give two specific
reasons to
justify the statement.
19. Write the chemical equation for the reaction of thiosulphate ions and alkaline potassium
permanganate.
20. Mention the name and formula of the ore from which potassium dichromate is prepared.
21. Write the electronic configuration of Lu3+ (At. No. = 71).
22. What is the most common oxidation state of actinoids?
23. Write the names of the catalyst used in the :
(a) Manufacture of sulphuric acid by contact process.
(b) Manufacture of polythene.
24. Mention the name of the element among lanthanoids known to exhibit +4 oxidation state.
25. Name one ore each of manganese and chromium.
26. Why is Cd2+ ion white?
*27. Draw the structure of dichromate anion.
*28. Arrange the following monoxides of transition metals on the basis of decreasing basic character
TiO, VO, CrO, FeO.[Hint : TiO > VO > CrO > FeO]
1. Actinoids exhibit greater range of oxidation states than lanthanoids. Explain.
2. What is meant by ‘lanthanoid contraction’?
3. Silver (Ag) has completely filled d-orbitals (4d10) in its ground state. How can you say
that it is a transition element.
4. 2.
Why Mn2+ compounds are more stable than Fe2+ compounds towards oxidation
to their +3 state?
5. 3.
Why does vanadium pentoxide act a catalyst?
6. 4.
Draw the structure of dichromate anion.?
7. 5.
Write the chemical equation for the reaction of thiosulphate ions and alkaline
potassium permanganate.
8. What is meant by lanthanoid contraction ?
9. Write the outer electronic configuration of Cr atom (Z=24 )
10. Complete and balance the following chemical equation ;
Cr2O72- + I- + H+ →
11. Out of Cr2+ and Cr3+, which one is stable in aqueous solution ?
12. Wrire outer electronic configuration of lanthanoids.
13. Arrange the given in increasing order of acidic character-CrO3, CrO, Cr2O3.
14. Why are transition metals called d-block elements ?
15. Why is KMnO4 kept in dark bottles ?
16. Which property of the transition metals makes them good catalyst ?
17. Why is the third ionisation energy of manganese(At no.=25) unexpectedly high ?
2marks
2.Assign reasons for the following:
(i)Copper(I) ion is not known in aqueous solution.
(ii)Actinoids exhibit greater range ofoxidation states than lanthanoids.
3.How would you account for the following:
(i)Cr2+ is educing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidizing agent.
4.Describe the preparation of
(i)Potassium dichromate from sodium chromate and
(ii)KMnO4 from K2MnO4.
5.(a) Which metal in the first transition series(3d series) exhibits +1 oxidation states most frequently and
why?
(b)Which of the following cations are coloured in aqueous solutions and why?
Sc3+ , V3+ , Ti4+ , Mn2+
6.Answer the following questions:
(i)Which element in the first series of transition elements does not exhibit variable oxidation states
and why?
(ii)Why do actinoids ,in general,exhibit a greater range of oxidation states than the lanthanoids?
1.Write the chemical equation, when the yellow colour of aqueous solution of Na2CrO4 changes to
orange on passing CO2 gas?
2. The stability of Cu2+ (aq) is more than that of Cu+ (aq). Why?
3. Indicate the steps in the preparation of
(a) K2Cr2O7 from Chromite ore.
(b) KMnO4 from Pyrolusite ore.
4. Give reason for : –
(a) In permanganate ions, all bonds formed between manganese and oxygen are covalent.
(b) Permanganate titrations in presence of hydrochloric acid are unsatisfactory.
5. Write complete chemical equations for
(a) oxidation of Fe2+ by Cr2O7 2– in acidic medium
(b) oxidation of Mn2+ by MnO4 – in neutral or faintly alkaline medium.
6.
(a) Why do transition metals show high melting points?
(b) Out of Fe and Cu, which one would exhibit higher melting point?
7. Describe giving reason which one of the following pairs has the property indicated :
(a) Cr2+ or Fe2+ (stronger reducing agent).
(b) Co2+ or Ni2+ (lower magnetic moments).
8. Of the ions Co2+, Sc3+, Cr3+ which one will give colourless aqueous solution and how will each of
them
respond to magnetic field and why?
9. Complete the following equations :
(a) MnO2 + KOH + O2 → (b) Na2Cr2O7 + KCl →
10. Transition metals show low oxidation states with carbon monoxide.
11.Assign reason for the following :
(a) Transition elements have higher values of enthalpies of atomisation.
(b) The enthalpy of atomisation of zinc is the lowest in 3d - series.
12. Account for the following :
(a) Copper shows its inability to liberate hydrogen gas from the dilute acids.
(b) Scandium (Z = 21) does not exhibit variable oxidation states.
13. Copper (I) compounds undergo disproportionation. Write the chemical equation for the reaction
involved
and give reason.
14. The following two reactions of MNO3 with Zn are given.
(a) Zn + conc. HNO3 → Zn(NO3)2 + X + H2O
(b) Zn + dil.HNO3 → Zn(NO3)2 + Y + H2O
Identify X and Y and write balanced equations.
15. Titanium shows magnetic moment of 1.73 BM in its compound. What is the oxidation number of
Ti in the
compound?
16. Account for the following :
(a) Transition metals and majority of their compounds act as good catalysts.
(b) From element to element, actionoid contraction is greater than lanthanoid contraction
17. Calculate the number of electrons transferred in each case when KMnO4 acts as an oxidising
agent to give
(i) MnO2 (ii) Mn2+ (iii) Mn(OH)3 (iv) MnO42– respectively.
18. Calculate the number of moles of KMnO4 that is needed to react completely with one mole of
sulphite ion in
acidic medium.
1. Assign a reason for each of the following:
(i) The third ionization energy of Mn (Z = 25) is higher than that of either Cr (Z = 24) or Fe
(Z = 26).
(ii) Simple copper (I) salts are not stable in aqueous solutions.
2. Discuss the relative stability in aqueous solutions of +2 oxidation state among the
elements : Cr, Mn, Fe and Co. How would you justify this situation? (At. Nos. Cr = 24, Mn
= 25, Fe = 26, Co = 27)
3. Assign a reason for each of the following:
(i) The third ionization energy of Mn (Z = 25) is higher than that of either Cr (Z = 24) or Fe
(Z = 26).
(ii) Simple copper (I) salts are not stable in aqueous solutions.
4. State reasons for the following observations:
(i) The enthalpies of atomisation of transition elements are quite high.
(ii) There is a greater horizontal similarity in the properties of the transition elements
than of the main group elements.
5. Explain the following observations:
(i) Generally there is an increase in density of elements from titanium (Z = 22) to copper
(Z = 29) in the first series of transition elements.
(ii) Transition elements and their compounds are generally found to be good catalysts in
chemical
reactions.
6. Explain the following observations:
(i) Transition elements generally form coloured compounds.
(ii) Zinc is not regarded as a transition element.
7. Describe the preparation of (i) Potassium dichromate from sodium chromate, and (ii)
KMnO4 from K2MnO4
8. Assign reasons for each of the following:
(i) Transition metals generally form coloured compounds.
(ii) Manganese exhibits the highest oxidation state of +7 among the 3d series of
transition elements.
9. Explain giving reasons:
(i) Transition metals and their compounds generally exhibit a paramagnetic behaviour.
(ii) The chemistry of actinoids is not as smooth as that of lanthanoids.
1.
2.
The stability of Cu2+ (aq) is more than that of Cu+ (aq). Why?
Complete the equations :
(a)
MnO4
– + NO2– + H+ -
(b) KMnO4 --513 k→
3.
Account for the following :
(a) Transition metals and majority of their compounds act as good catalysts
(b) From element to element, actionoid contraction is greater than lanthanoid
contraction
4.
Write complete chemical equations for
(a) oxidation of Fe2+ by Cr2 O7 2- in acidic medium
(b) oxidation of Mn2+ by MnO4- in neutral or faintly alkaline medium
.
Give reason for the following
(i)
The enthalpies of atomization of transition elements are high.
(ii)
The transition metals and many of their compounds act as good catalyst.
2.
Assign reasons for the following
(i)
Copper (I) ion undergoes disproportionation in the aqueous solution.
(ii)
Actinoids exhibits greater range of oxidations states than lanthanoids.
3.
Write the preparation of KMno4 from pyrolusite ore (MnO2).
4.
Describe the preparation of potassium dichromate from chromite ore.
1. Assign reasons for the following :
(i)
Copper (I) ion is not known in aqueous solution.
(ii)
Actinoids exhibit greater range of oxidation states than lanthanoids.
2. Write complete chemical equation for :
(i)
Oxidation of Fe2+ by Cr2O72- in acidic medium.
(ii)
Oxidation of S2O32- by MnO4- in neutral aqueous medium.
3. Why is the +2 oxidation state of manganese quite stable, while the same is not true for
iron ? [Mn=25, Fe=26]
4. Explain the following giving reasons :
(i)
It is difficult to separate the lanthanoid elements in pure state.
(ii)
The first ionisation energies of 5d transition elements are higher than those of the
3d or 4d transition elements of the corresponding groups.
5. Explain :
(i)
Co2+ is easily oxidised to Co3+ in the presence of a strong ligand.
(ii)
CO is a stronger complexing reagent than NH3.
3marks
1.Give reasons for the following observations:
(i)Mn(II) ion shows maximum paramagnetic character amongst the bivalent ions of first transition
series.
(ii)Scandium (At.no.21)salts are white.
(ii)In a transition series of metals, the metal which exhibits the greatest number of oxidation states
occurs in the
middle of the series.
2.How would you account for this following:
(i)The oxidizing power of oxo anions are in the order
VO2+<Cr2072-<MnO4(ii)The third ionization enthalpy of manganese (Z=25) is exceptionally high.
(iii)Cr2+ is a stronger reducing agent than Fe2+.
3.How would you account for the following chemical equations?
(i)Transition metals exhibit variable oxidation states.
(ii)Zr (Z=40) and Hf (Z==72) have almost identical radii.
(iii)Transition metals and their compounds act as catalyst.
4.Complete the following chemical equations:
(i)Cr2O2-7 + 6Fe2+ + 14H+
(ii)2CrO2-4 +2H+
(iii)2MnO4- + 5C2O2-4 +16H+
1. Account for the following :
(a) La(OH)3 is more basic than Lu(OH)3
(b) Zn2+ salts are white.
(c) Cu(I) compounds are unstable in aqueous solution and undergo disproportination.
2. Describe the oxidising action of potassium dichromate with following. Write ionic equations for its
reaction
with.
(a) Iodide ion (b) Iron (II) (c) H2S.
3. (a) Deduce the number of 3d electrons in the following ions :
Fe3+, Cu2+ and Sc3+.
(b) Why do transition metals form alloys.
(c) Write any two characteristics of interstitial compounds.
4. What happens when
(a) thiosulphate ions react with alkaline KMnO4.
(b) ferrous oxalate reacts with acidified KMnO4.
(c) sulphurous acid reacts with acidified KMnO4
Write the chemical equations for the reactions involved.
5. Name the catalysts used in the
(a) manufacture of ammonia by Haber’s Process
(b) oxidation of ethyne to ethanol
(c) photographic industry.
*6. Among TiCl4, VCl3 and FeCl2 which one will be drawn more strongly into a magnetic field and
why?
7. How do you account for the following?
(a) With the same d-orbital configuration (d4), Cr2+ is a reducing agent while Mn3+ is an
oxidiising agent.
(b) The actinoids exhibit a larger number of oxidation states than the corresponding
members in the
lanthanoid series.
(c) Most of transition metal ions exhibit characteristic colours in aqueous solutions
1. Describe the trends in the following properties of the first series of the transition
elements :
(i) Oxidation states (ii) Atomic sizes
Magnetic behaviour of dipositive gaseous ions (M2+)
2. Compare actinoids and lanthanoids with reference to their :
(i) electronic configurations of atoms
(ii) oxidation states of elements
(iii) general chemical reactivity of elements.
3. Explain the following observations:
(i) Transition metals form compounds which are usually coloured.
(ii) Transition metals exhibit variable oxidation states.
(iii) The actinoids exhibit a greater range of oxidation states than the lanthanoids.
4. How would you account for the following:
(i) Many of the transition elements and their compounds can act as good catalysts.
(ii) The metallic radii of the third (5d) series of transition elements are virtually the same
as those of the corresponding members of the second series.
(iii) There is a greater range of oxidation states among the actinoids than among the
lanthanoids
5. Explain the following observations:
(i) With the same d-orbital configuration (d4) Cr2+ ion is a reducing agent while Mn3+ ion
is an oxidising agent.
(ii) Cu+ ion is not stable in aqueous solutions.
(iii) Among the 3d series of transition elements, the largest number of oxidation states
are exhibited by manganese.
6. How would you account for the following:
(i) The oxidising power of oxoanions are in the order VO2+ < Cr2 O72- < MnO4– .
(ii) The third ionization enthalpy of manganese (Z = 25) is exceptionally high.
(iii) Cr2+ is a stronger reducing agent than Fe2+.
7. Explain the following observations:
(i) La3+ (Z = 57) and Lu3+ (Z = 71) do not show any colour in solutions.
(ii) Among the divalent cations in the first series of transition elements, manganese
exhibits the maximum paramagnetism.
(iii) Cu+ ion is not known in aqueous solutions.
8. Explain the following observations:
(i) The enthalpies of atomisation of transition metals are quite high.
(ii) There is a close similarity in physical and chemical properties of the 4 d and 5 d series
of the transition elements, much more than expected on the basis of usual family
relationship.
(iii) The members in the actinoid series exhibit larger number of oxidation states than
the corresponding members in the lanthanoid series.
9. Explain the following:
(i) The transition elements have great tendency for complex formation.
(ii) There is a gradual decrease in the atomic sizes of transition elements in a series with
increasing atomic numbers.
(iii)
Lanthanum and Lutetium do not show colouration in solutions.
(At. No.: La = 57, Lu = 71)
How do you account for the following?
(a) With the same d-orbital configuration (d4), Cr2+ is a reducing agent while Mn3+ is an
oxidiising agent.
(b) The actinoids exhibit a larger number of oxidation states than the corresponding
members in the lanthanoid series.
(c) Most of transition metal ions exhibit characteristic colours in aqueous solutions
2.
What happens when
(a) thiosulphate ions react with alkaline KMnO4.
(b) ferrous oxalate reacts with acidified KMnO4.
(c) sulphurous acid reacts with acidified KMnO4
Write the chemical equations for the reactions involved.
3
(a) Deduce the number of 3d electrons in the following ions :
Fe3+, Cu2+ and Sc3+.
(b) Why do transition metals form alloys.
(c) Write any two characteristics of interstitial compounds.
What is lanthanoid contraction. Mention its important consequences.
6.
What is meant by disproportionation? Give two examples of disproportionation
reaction in aqueous solution of d-block elements.
7.
(a)
What is interstitial compound ?
(b)
Complete the following reactions
(i) Cr2O72- + H2S + H+ (ii) MnO4- + 2 H2O + 3e alk. Medium
8.
Account for the following
(i)
Mn2O7 is acidic where as Mno is basic
(ii)
Zr and Hf exhibit similar properties
(iii)
Transition metal forms a large number of complex compounds
9.
Answer the following
(i)
In the 3d transition series copper has exceptionally positive E0(M2+/m)
value. Why?
(ii)
Zn2+ salts are colourless. Why ?
(iii)
In 3d transition series which element is a strong reducing agent in +2
oxidation state and why ?
10.
(a)
A blackish brown coloured solid ‘A’ when fused with an alkali metal
hydroxide in the presence of air produces a dark green coloured compound ‘B’
which upon electrolytic oxidation in alkaline medium give a dark purple coloured
compound ‘C’. Identify A, B, and C. Write the reactions involved.
1. With the help of equations explain the preparation of potassium dichromate from
chromite ore. Why is K2Cr2O7 preferred over Na2Cr2O7 in volumetric analysis ?
2. Describe the preparation of potassium permanganate from pyrolusite ore. Write the
chemical equations for the reaction involved.
3. Give reasons :
(i)
Size of trivalent lanthanoids cation decreases with increase in the atomic number.
(ii)
Transition metal fluorides are ionic in nature, whereas bromides and chlorides are
usually covalent in nature.
(iii) Chemistry of all the lanthanoids is quite similar.
4. Compare the chemistry of actinoids with that of lanthanoids with reference to
(i)
Electronic configuration
(ii)
Oxidation states
(iii) Chemical reactivity.
5. Complete the following reactions :
(i)
Cr2O72- + H+ + Fe2+→
(ii)
MnO4- + I- + H+ →
(iii) Cu2+ + I- →
.
LONG ANSWER TYPE QUESTIONS (5 - MARK QUESTIONS)
1. A green compound ‘A’ on fusion with NaOH in presence of air forms yellow compound ‘B’ which
on acidification with dilute acid, gives orange solution of compound ‘C’. The orange solution when
reacted with equimolar ammonuim salt gives compound ‘D’ which when heated liberates nitrogen
gas and compound ‘A’. Identify compounds A to D and write the chemical equation of the reactions
involved.
2. Assign reasons for the following :
(a) There is no regular trends in E° values of M2+/M systems in 3d series.
(b) There is gradual decrease in the ionic radii of M2+ ion in 3d series.
(c) Majority of transition metals form complexes.
(d) Ce3+ can be easily oxidised to Ce4+
(e) Tantalum and palladium metals are used to electroplate coinage metals.
3. Account for the following :
(a) Actinoids display a variety of oxidation states.
(b) Yb2+ behaves as a good reductant.
(c) Cerium (iv) is a good analytical reagent.
(d) Transition metal fluorides are ionic in nature while chlorides and bromides are covalent in
nature.
(e) Hydrochloric acid attacks all the actinoids.
*4. Explain by giving suitable reason :
(a) Co(II) is stable in aqueous solution but in the presence of complexing agent it is readily
oxidised.
(b) Eu2+, Yb2+ are good reductants whereas Tb4+ is an oxidant.
(c) AgCl dissolves in ammonia solution
(d) Out of Cr2+ or Fe2+, which one is a stronger reducing agent?
(e) The highest oxidation state is exhibited in oxoanions of a transition metal.
5. When a white crystalline compound A is heated with K2Cr2O7 and conc. H2SO4, a reddish brown
gas B is
evolved, which gives a yellow coloured solution C when passed through NaOH. On adding
CH3COOH and
(CH3COO)2 Pb to solution C, a yellow coloured ppt. D is obtained. Also on heating A with NaOH
and passing
the evolved gas through K2HgI4 solution, a reddish brown precipitate E is formed. Identify A, B, C,
D and E
and write the chemical equations for the reactions involved.
*6. (a) Describe the preparation of potassium dichromate (K2Cr2O7). Write the chemical equations of
the
reactions involved.
(b) “The chromates and dichromates are interconvertible by the change in pH of medium.” Why?
Give
Chemical equations in favour of your answer.
7. Explain giving reasons :
(a) Transition metals are less reactive than the alkali metals and alkaline earth metals.
(b) Elements in the middle of transition series have higher melting points.
(c) The decrease in atomic size of transition elements in a series is very small.
8. (a) Compare the chemistry of the actinoids with that of lanthanoids with reference to—
(i) electronic configuration
(ii) oxidation states
(iii) chemical reactivity.
(b) How would you account for the following :
(i) of the d4 species, Cr2+ is strongly reducing while Mn3+ is strongly oxidising.
(ii) the lowest oxide of a transition metal is basic whereas highest is amphoteric or acidic.
9. (a) What is meant by disproportionation of an oxidation state. Give one example.
(b) Explain why europium (II) is more stable than Ce(II)?
10. (a) For M2+/M and M3+/M2+ systems, the E values for some metals are as follows :
Cr2+/Cr = – 0.9V and Cr3+/Cr2+ = – 0.4V Mn2+/Mn = – 1.2 V and Mn3+/Mn2+ = + 1.5V
Fe2+/Fe = – 0.4V and Fe3+/Fe2+ = + 0.8V
Use this data to comment upon :
(i) the stability of Fe3+ in acid solution as compared to that of Cr3+ and Mn3+
(ii) the ease with which iron can be oxidised as compared to a similar process for either chromium
or
manganese.
(b) How is the variability in oxidation states of transition metals different from that of the nontransition metals?
Illustrate with examples.
1. Assign reasons for the following:
(i) The enthalpies of atomisation of transition elements are high.
(ii) The transition metals and many of their compounds act as good catalysts.
(iii) From element to element the actinoid contraction is greater than the lanthanoid
contraction.
(iv) The E° value for the Mn 3+ / Mn 2+ couple is much more positive than that of Cr 3+ / Cr
2+
.
(v) Scandium (Z = 21) does not exhibit variable oxidation states and yet it is regarded as
a transition element.
2. (a) What may be the possible oxidation states of the transition metals with the following
d electronic configurations in the ground state of their atoms: 3d 3 4s 2 , 3d5 4s 2 and 3d 6
4s 2 . Indicate relative stability of oxidation states in each case.
(b) Write steps involved in the preparation of (i) Na 2CrO4 from chromite ore and (ii)
K2MnO4 from pyrolusite ore.
3. Complete the following chemical reaction equations:
(i)
MnO4-(aq ) + C2 O42-(aq) + H + (aq ) →
(ii)
(ii) Cr2O72-(aq ) + F –(aq) + H + (aq ) →
(b) Explain the following observations about the transition/inner transition elements:
(i) There is in general an increase in density of element from titanium (Z = 22) to copper
(Z = 29).
(ii) There occurs much more frequent metal-metal bonding in compounds of heavy
transition elements (3rd series).
(iii) The members in the actinoid series exhibit a large number of oxidation states than
the corresponding members in the lanthanoid series.
4. (a)Complete the following chemical equations for reactions:
(i)
MnO4-(aq ) + S2O32-(aq) + H2O(i ) →
(ii)
Cr2 O72-(aq) + H2S(g) + H+(aq) →
(b) Give an explanation for each of the following observations:
(i) The gradual decrease in size (actinoid contraction) from element to element is
greater among the actinoids than that among the lanthanoids (lanthanoid contraction).
(ii) The greatest number of oxidation states are exhibited by the members in the middle
of a transition series.
(iii) With the same d-orbital configuration (d4) Cr2+ ion is a reducing agent but Mn3+ ion is
an oxidising agent.
5. Explain the following observations:
(i) Transition elements are known to form many interstitial compounds.
(ii) With the same d4 d-orbital configuration Cr2+ ion is reducing while Mn3+ ion is
oxidising.
(iii) The enthalpies of atomisation of the transition elements are quite high.
6. (a) What is meant by the term lanthanoid contraction? What is it due to and what
consequences does it have on the chemistry of elements following lanthanoids in the
periodic table?
(b) Explain the following observations:
(i) Cu+ ion is unstable in aqueous solutions.
(ii) Although Co2+ ion appears to be stable, it is easily oxidised to Co3+ ion in the presence
of a strong ligand.
(iii) The Eo Mn 2+/ Mn value for manganese is much more than expected from the trend
for other elements in the series.
1.
2.
A green compound ‘A’ on fusion with NaOH in presence of air forms yellow compound
‘B’ which on acidification with dilute acid, gives orange solution of compound ‘C’. The
orange solution when reacted with equimolar ammonuim salt gives compound ‘D’
which when heated liberates nitrogen
gas and compound ‘A’. Identify compounds A to D and write the chemical equation of
the reactions involved
(a) Describe the preparation of potassium dichromate (K2Cr2O7). Write the chemical
equations of the reactions involved.
(b) “The chromates and dichromates are interconvertible by the change in pH of
medium.” Why? Give chemical equations in favour of your answer.
1. Account for the following :
(i)
Transition elements have higher boiling points.
(ii)
Zn, Cd and Hg are normally not regarded as transition elements.
(iii) Sc forms no coloured ions yet it is regarded as transition elements,
(iv)
Transition elements show variable oxidation states.
(v)
Zr resembles with Hf.
2. (a) Write the electronic configutation of Ce3+ ion, and calculate the magnetic
moment on the basis of spin-only formula.[Atomic No. of Ce =58]
(b) Account for the following :
(i)
The enthalpies of atomisation of the transition metals are high.
(ii)
The lowest oxide of a transition metal is basic, the highest is
amphoteric/acidic.
(iii) Cobalt (II) is stable in aqueous solution but in the presence of complexing
agents, it is easily oxidised.
1.(a)How do you prepare:
(i)K2MnO4 from MnO2?
(ii)Na2Cr2O7 from Na2CrO4?
(b) Account for the following:
(i)Mn2+ is more stable than Fe2+ towards oxidation to +3 state.
(ii)The enthalpy of atomization is lowest for Zn in 3d series of the transition elements.
(iii)Actinoids elements show wide range of oxidation states.
2.(i)Name the element of 3d transition series which shows maximum number of oxidation states. Why
does it show so?
(ii)Which transition metal of 3d series has positive Eo(M2+/M) value and why?
(iii)Out of Cr3+and Mn3+ ,which is a stronger oxidizing agent and why?
(iv)Name a member of the lanthanoid series which is well known to exhibit +2 oxidation state.
(v)Complete the following equation:
MnO-4 +8H+ + 5e3. (a)Give reasons for the following:
(i)Mn3+ is a good oxidizing agent.
(ii)EoM2+ /M values are not regular for first row transition metals(3d series).
(iii)Although ‘F’ is more electronegative than ‘O’,the highest Mn fluoride is MnF4,whereas the highest
oxide is
Mn2O7.
(b)Complete the following equations:
(i) 2CrO42- + 2H+
HEAT
(ii)KMnO4
4.(a)Why do transition elements show variable oxidation states?
(i)Name the element showing maximum number of oxidation states among the first series of
transition metals from
Sc (Z=21) to Zn (Z=30).
(ii)Name the element which shows only +3 oxidation state.
(b)What is lanthnoid contraction ? Name an important alloy which contains some of the lanthanoid
metals.
5.Assign reasons for the following :
(i)In the series Sc(Z=21) to Zn(Z=30),the enthalpy of atomization of Zn is the lowest.
(ii)Zr and Hf have almost identical radii.
(iii)Transition metals show variable oxidation states .
(iv)The EO M2+/M value for copper is positive (+0.34v).
(v)Cr2+ is a very good reducing agent.
6.Describe the preparation of KMnO4 from pyrolusite ore (MnO2).How does the acidified permanganate
solution react
with the following:
(i)Fe2+ ions (ii)Oxalic acid (C2O4H2)
Write the ionic equations for the reactions involved.
7.(a)Complete the following equations :
(i)Cr2O72- + 2OH(ii)MnO4- + 4H+ + 3e(b)Account for the following:
(i)Zn is not considered as a transition element.
(ii)Transition metals form a large number of complexes.
(iii)The Eo value for the Mn3+/Mn2+ couple is much more positive than that for Cr3+ /Cr2+ couple.
8. (i)With reference to structural variability and chemical reactivity ,write the differences between
lanthanoids and
actinoids.
(ii)Name a member of the lanthanoid series which is well known to exhibit +4 oxidation states.
(iii)Complete the following equation:
MnO4- +8H+ +5 e(iv)Out of Mn3+ and Cr3+, which is moreb paramagnetic and why?
9.Complete the following equations:
(i)2MnO-4 +5S2- +16H+
(ii)Cr2O72- + 2 OH10.(a)What are the different oxidation states exhibited by the lanthanoid?
(b) Write two characteristics of the transition elements.
( c)Which of the 3d-block el;ements may not be regarded as the transition elements and why?
11.Assign suitable reasons for the following :
(a)The Mn2+ compounds are more stable than Fe2+ towards oxidation to their +3 state.
(b)In the 3d series from Sc (Z=21) to Zn (Z=30),the enthalpy of atomization of Zn is the lowest.
©Sc3+ is colourless in aqueous solutions , whereas Ti3+ is coloured.
12. Complete the following equations :
(i)2MnO4- + 5NO2- + 6H+
(ii)Cr2O2-7 + 14 H+ + 6e13.Complete the following equations :
(i)2MnO4- + 5SO2-3 + 6H
(ii)2CrO2-4 + 2H+
Unit - 9
CO-ORDINATION COMPOUNDS
1marks
1. Define the term coordination compound?
2. Write the names of counter ions in
(i) Hg [Co (SCN)4] and (ii) [Pt(NH3)4] Cl2.
3. Write the oxidation state of nickel in [Ni(CO)4]
*4. What is the coordination number of central atom in [Co(C2O4)3]3–?
5. What is the coordination number of iron in [Fe (EDTA)]– ? [Ans. : 6]
6. Write the name of a complex compound used in chemotherapy.
[Ans. : Cis–Platin. [Pt(NH3)2 Cl2]
7. Name the compound used to estimate the hardness of water volumetrically.
8. Give the IUPAC name of [Pt Cl2 (NH2CH3) (NH3)2] Cl.
*9. How many geometrical isomers are possible for the tetrahedral complex [Ni(CO)4].
10. Arrange the following in the increasing order of conductivity in solution.
[Ni(NH3)6]Cl2; [Co(NH3)6]Cl3 and [CoCl2(en)2] Cl
11. Arrange the following ligands in increasing order of(Crystal field splitting energy) for
octahedral
complexes with a particular metal ion.
Cl –, NH3, I –, CO, en.
12. Write I.U.P.A.C. name of Tollens’ reagent.
13. Which is more stable? K3[Fe(CN)6] or K4[Fe(CN)6]
14. Calculate the overall dissociation equilibrium constant for the [Cu(NH3)4]2+ ion. Given that
overall stability constant for this complex is 2.1 × 1013.
*15. What is a chelate ligand? Give one example.
16. Write the I.U.P.A.C. name of Li[AlH4].
17. Name one homogeneous catalyst used in hydrogenation of alkenes.
*18. Name the types of isomerism shown by coordination entity : [CrCl2(Ox)2]3–
*19. [Ti(H2O)6]Cl3 is coloured but on heating becomes colourless. Why?
*20. Write the IUPAC name of ionization isomer of [Co(NH3)5(SO4)] Br
*21. Write the formula and the name of the coordinate isomer of [Co(en)3] [Cr(CN)6].
Give an example of linkage isomerism.
Give an example of coordination isomerism.
What is an ambidentate ligand? Give an example.
What do you understand by ‘denticity of a ligand’?
Why is CO a stronger ligand than Cl–?
Name the following coordination compound: K3[CrF6]
Write the hybridisation of the complex [NiCl4]2–. (Atomic number of Ni = 28)
Give an example of the role of coordination compounds in biological systems.
Why CO is a stronger ligand than NH3 for many metals
Write the name of a complex compound used in chemotherapy ?
2.
Give the IUPAC name of [Pt Cl2 (NH2CH3) (NH3)2] Cl.
3.
Write the formula and the name of the coordinate isomer of [Co(en)3] [Cr(CN)6].
1.
2.
3.
4.
5.
6.
7.
8.
4. Write the IUPAC names of the following compoundCH2Br – CH = CH – CH2 – C - CH
Write the structure of following halogen compounds
1-bromo-4-sec-butyl-2–methylebenzene.
Arrange1-chloropropane, isopropyl chloride, 1-chlorobutane
Increasing order of boiling point
5.
Why is CO stronger ligand than Cl- ?
Give the chemical formula of pentaamminechlorocobalt(III) Chloride.
What is the oxidation state of Ni in [Ni(CO)4] ?
Which of the two is more stable K4[Fe(CN)6] or K3[Fe(CN)6] ?
Give an example of chelate complex.
Write IUPAC name of K3[Fe(C2O4)3].
Write coordination isomer of :
[Cr(en)3] [Co(CN)6].
8. What is ambidentate ligand ?
1.
2.
3.
4.
5.
6.
7.
1.Why is [NiCl4]2- paramagnetic?
{Ni=28}
2.Why is CO astronger ligand than Cl-?
3.Name the following coordination compound:K3[CrF6].
4.Write the IUPAC name of [Pt(NH3)4Cl2]Cl2.
5.Which of the following is more stable complex and why?
[Co(NH3)6]3+ and [Co(en)3]3+
6.What type of isomerism is shown by the following complex:
[Co(NH3)6][Cr(CN)6]?
7.What type of isomerism is exhibited by the following complex :
[Co(NH3)5SO4]Cl.
2marks
*22. Write two differences between a double salt and a coordination compound with the help of
an example of
each.
23. Mention the main postulates of Werner’s Theory.
24. Define (a) Homoleptic and (b) Heteroleptic complexes with the help of one example of each.
25. In the following coordination entity : [Cu(en)2]2+
(a) Identify the ligand involved and
(b) Oxidation state of copper metal.
27. Calculate the magnetic moments of the following complexes :
(i) [Fe(CN)6]4–
(ii) [CoF6]3–
28. Explain the following :
(a) [Fe(CN)6]3– is an inner orbital complex whereas [FeF6]3– is an outer orbital
complex.
(b) NH3 acts as complexing agent but NH4 + does not.
29. What type of structural isomerism is represented by the following complexes:
(a) [Mn(CO)5(SCN)] and [Mn(CO)5(NCS)]
(b) [Co(NH3)5(NO3)] SO4
30. How are complex compounds applicable in (a) electroplating of silver, gold or other noble
metals
(b) in photography.
31. Explain on the basis of Valance Bond Theory that diamagnetic [Ni(CN)4]2– has square
planar structure and
paramagnetic [NiCl4]2– ion has tetrahedral geometry.
23. Explain as to how the two complexes of nickel [Ni(CN)4]2– and Ni(CO)4 have different
structures but do not differ in their magnetic behaviours. (At. no. of Ni = 28).
34. Draw the structures of geometrical isomers of the coordination complexes–
[Co(NH3)3Cl3] and [CoCl2(en)2]+
35. Write the IUPAC name of the complexes :
(a) [NiCl2 (PPh3)2] (b) [Co(NH3)4 Cl(NO2)] Cl (c) K[Cr(H2O)2 (C2O4)2]
36. Using IUPAC norms write the formulae for the following :
(a) Terabromidocuprate (II)
(b) Pentaamminenitrito–O– Cobalt (III)
*37. How does EDTA help as a cure for lead poisoning?
37. A complex is prepared by mixing CoCl3 and NH3 in the molar ratio of 1:4. 0.1 m solution of
this complex was
found to freeze at –0.372°C. What is the formula of the complex?
Kf of water = 1.86°C/m
[Hint : Tf = i Kf × m = i 1.86 0.1
Tf(obs) = 0.373°C
This means each molecule of complex dissociates into two ions.
Hence the formula is i = 2
*38. The [Mn(H2O)6]2+ ion contains five unpaired electrons while [Mn(CN)6]4– ion contains
only one unpaired
electron. Explain using Crystal Field Theory:
1.
2.
3.
4.
5.
Name the following coordination compounds according to IUPAC system of
nomenclature:
(i) [Co(NH3)4 (H2O) Cl]Cl2 (ii) [CrCl2(en)2]Cl, (en = ethane –1, 2 – diamine)
Explain the following terms: (i) Crystal field splitting in an octahedral field (ii)
Spectrochemical series.
(a) Write the IUPAC name of the complex [CoBr2(en)2]+.
(b) What type of isomerism is shown by the complex [Co(NH3 )5 SO4 ]Br?
Write the formulae for the following coordination compounds:
(i) Tetraammineaquachloridocobalt (III) chloride
(ii) Potassiumtetracyanonickelate (II)
Explain the following cases giving appropriate reasons:
(i) Nickel does not form low spin octahedral complexes.
(ii) Co2+ is easily oxidised to Co3+ in the presence of a strong ligand.
1.
Explain the following :
(a) [Fe(CN)6]3– is an inner orbital complex whereas [FeF6]3– is an outer orbital
complex.
(b) NH3 acts as complexing agent but NH4+ does not.
2
What type of structural isomerism is represented by the following complexes:
(a) [Mn(CO)5(SCN)] and [Mn(CO)5(NCS)]
(b) [Co(NH3)5(NO3)] SO4
3
Explain on the basis of Valance Bond Theory that diamagnetic
[Ni(CN)4]2–
has square planar structure and paramagnetic
tetrahedral geometry
How will you bring about the following conversions?
(i) benzene to 3-bromonitrobenzene
(ii) ethanol to but-1-yne
2
Explain the following reactions with suitable example :
(i) Finkelstein reaction.
[NiCl4]2– ion has
3
4
5
6
(ii) Swarts reaction.
Give a chemical test to distinguish between the following pairs of compounds:
(i) chlorobenzene and cyclohexylchloride.
(ii) vinyl chloride and ethyl chloride.
Give mechanism of the following reactions :
(i) (CH3)3C – Cl + O – H ––>(CH3)3 C – OH
(ii) CH3 – Cl + OH–>CH3 – OH
Which compound in each of the following pairs will react faster in SN2
reaction with OH– and why?
(i) CH3Br or CH3I
(ii)(CH3)3CClorCH3Cl
Give reasons for the following :
(i) The bond length of C–Cl bond is larger in haloalkanes than that in haloarenes.
(ii) Although alkyl halides are polar in nature but are not soluble in Water
1. What is the coordination number of central ion in octahedral complex ? Why does NH3
form complex but NH4+ ion does not ?
2. Using valence bond theory, predict the shape and magnetism(paramagnetic or
diamagnetism) of [Co(CO)4]-.[At. No. of Co=27]
3. CuSO4.5H2O is blue in colour while CuSO4 is colourless. Why ?
4. Account for the following :
[Cr(NH3)6]3+ is paramagnetic and octahedral whereas [Ni(CN)4]2- is diamagnetic and
square planar.
5. Illustrate the geometrical isomerism with the help of an example [Pt(NH3)4Cl2]2+.
3marks
1.Describe the state of hybridization ,the shape and the magnetic behavior of the following
complexes :
(i) [Cr(H2O)2(C2O4)2](ii)[Co(NH3)2(en)2]3+
(en = ethane-1, 2-diamine)
(At.NOs :Cr=24, Co=27)
2.Write the IUPAC name of [Pt(NH3)3(NO)Cl2]Br2.
3.Name the following coordination compounds and draw their structures :
(i)[CoCl2(en)2]Cl
(ii)[Pt(NH3)2Cl(NO2)] (At no. Co=27,Pt=78)
4.Draw the structures of isomers ,if any,and write the names of the following complexes:
(i) [Cr(NH3)4Cl2]+
(ii) [Co(en)3]3+
5.Explain the following:
[Fe(CN)6]4- and [Fe(H2O)6]2+ are of different colours in dilute solutions.
6.State a reason for each of the following situations:
(i)CO is a stronger complexing reagent than NH3.
(ii)The molecular shape of Ni(Co)4 is not the same as that of [Ni(CN)4]2-.
7.Square planar complexes (of MX2L2type) with coordination number of 4 exhibit geometrical
isomerism, whereas
tetrahedral complexes with similar composition do not.Why?
8.Write the IUPAC NAME OF THE COMPLEX [Cr(NH3)4Cl2]+ . What type of isomerism does
it exhibit?
9.Write the state of hybridization,shape and IUPAC name of the complex [CoF6]3- .
10.Write the state of hybridization ,shape and IU[PAC name of the complex [Ni(CN4]2-.
11.Write the state of hybridization ,shape and IUPAC name of the complex [Co(NH3)6]3+.
1.Explain the following terms giving a suitable example in each case :
(i) Ambident Ligand
(ii)Denticity of a ligand
(iii)_Crystal field splitting in an octahedral field.
2.Name the following coordination entities and draw the structures of their sterioisomers:
(i)[Co(en)2Cl2]+
(ii)[Cr(C2O4)3]3(iii)[Co(NH3)3Cl3]
3.Explain the following cases giving appropriate reasons :
39. Account for the following —
(i) [NiCl4]2– is paramagnetic while [Ni(CO)4] is diamagnetic though both are
tetrahedral.
(ii) [Fe(H2O)6]3+ is strongly paramagnetic whereas [Ni(NH3)6]2+ weakly
paramagnetic.
(iii) [Co(NH3)6]3+ is an inner orbital complex whereas [Ni(MH3)6]2+ is in outer orbital
complex.
40. Compare the following complexes with respect to their shape, magnetic behaviours and the
hybrid orbitals
involved.
(a) [CoF6]3–
(b) [Cr(NH3)6]3+
(c) [Fe(CN)6]4–
[Atomic Number : Co = 27, Cr = 24, Fe = 26]
41. Draw the structure of
(a) cis-dichloridotetracyanochromate (II) ion
(b) mer-triamminetrichloridocobalt (III)
(c) fac-triaquatrinitrito–N–cobalt (III)
42. Name the central metal atom/ion present in (a) Chlorophyll (b) Haemoglobin (c) Vitamin B12.
43. A metal complex having composition Cr(NH3)4 Cl2Br has been isolated in two forms ‘A’
and ‘B’. The form ‘A’
reacts with AgNO3 solution to give white precipitate which is readily soluble in dilute
aqueous ammonia,
whereas ‘B’ gives a pale yellow precipitate which is soluble in concentrated ammonia
solution. Write the
formula of ‘A’ and ‘B’. Also mention the isomerism which arises among ‘A’ and ‘B’.
44. Write the limitations of Valence Bond Theory.
45. Draw a sketch to show the splitting of d-orbitals in an octahedral crystal field state for a d4
ion. How the
actual electronic configuration of the split d-orbitals in an octahedral crystal field is decided
by the relative
values of 0 and pairing energy (P)?
*46. For the complex [Fe(en)2Cl2]Cl identify
(a) the oxidation number of iron.
(b) the hybrid orbitals and the shape of the complex.
(c) the magnetic behaviour of the complex.
(d) the number of geometrical isomers.
(e) whether there is an optical isomer also?
(f) name of the complex. [At. no. of Fe = 26]
48. A chloride of fourth group cation in qualitative analysis gives a green coloured complex [A]
in aqueous
solution which when treated with ethane –1, 2-diamine (en) gives pale yellow solution [B]
which on
subsequent addition of ethane –1, 2-diamine turns to blue/purple [C] and finally to violet
[D]. Identify [A], [B],
[C] and [D] complexes,
(a)What is a ligand? Give an example of a bidentate ligand.
(b) Explain as to how the two complexes of nickel, [Ni (CN) 4 ]2- and Ni (CO) 4 have
different structures but do not differ in their magnetic behaviour. (Ni = 28)
2. Write the IUPAC name and describe the magnetic behaviour (diamagnetic or
paramagnetic) of thefollowing coordination entities:(i) [Cr (H2O) 2 (C2O4 ) 2 ](ii) [Co
(NH3 )5 Cl]2+ (iii) [NiCl4 ]2(At. Nos. : Cr = 24, Co = 27, Ni = 28)
1.
3.
4.
5.
6.
7.
8.
9.
10.
For the complex [Fe(en)2Cl2]Cl, (en = ethylene diamine), identify
(i) the oxidation number of iron.
(ii) the hybrid orbitals and the shape of the complex.
(iii) the magnetic behaviour of the complex.
(iv) the number of geometrical isomers.
(v) whether there is an optical isomer also, and
(vi) name of the complex. (At. no. of Fe = 26)
Compare the following complexes with respect to their shape, magnetic behaviour and
the hybrid orbitals involved:
(i) [CoF4]2– (ii) [Cr(H2O)2(C2O4)2]– (iii) [Ni(CO)4] (Atomic number: Co = 27, Cr = 24,
Ni = 28)
Giving a suitable example for each, explain the following:
(i) Crystal field splitting (ii) Linkage isomerism (iii) Ambidentate ligand.
Compare the following complexes with respect to structural shapes of units, magnetic
behaviour and hybrid orbitals involved in units:[Co(NH3 ) 6 ]+3 , [Cr(NH )6 ]+3 , Ni(CO)4
(At No.: Co = 27, Cr = 24, Ni = 28)
Three geometrical isomers are possible for [Co(en)(H2O)2(NH3)2]3+. Draw molecular
structure of these three isomers and indicate which one of them is chiral.
Explain the following giving an example in each case: (i) Linkage isomerism (ii) An
outer orbital complex (iii) A bidentate ligand
Write the name, stereochemistry and magnetic behaviour of the following: (At. nos. Mn =
25, Co = 27, Ni = 28) K4[Mn(CN)6] (ii) [Co(NH3)5Cl]Cl2 (iii) K2[Ni(CN)4]
For the complex [Fe(en)2 Cl2] Cl, identify the following:
(i) Oxidation number of iron. (ii) Hybrid orbitals and shape of the complex.
(iii) Magnetic behaviour of the complex.
(iv) Number of its geometrical
isomers.
(v) Whether there may be optical isomer also.
(vi) Name of the complex
1.
Account for the following —
(i) [NiCl4]2– is paramagnetic while [Ni(CO)4] is diamagnetic though both are
tetrahedral.
(ii) [Fe(H2O)6]3+ is strongly paramagnetic whereas [Ni(NH3)6]2+ weakly
paramagnetic.
(iii) [Co(NH3)6]3+ is an inner orbital complex whereas [Ni(MH3)6]2+ is in outer orbital
complex
Draw optical isomers of [Fe(OX)3]3(b)
When a co-ordination compound p+Cl4. 6NH3 is mixed with AgNO3, 4 moles of
Agcl was precipitated per mole of the compound. Write
(i)
Structural formula of the complex
(ii)
IUPAC name of the complex
2.
(a)
(b)
Write IUPAC name of [Pt (NH3)2 Cl2]Cl2
[Cr (NH3)6]3+ is paramagnetic while [Ni(CN)4]2- is diamagnetic. Explain Why?
3.
(a)
(b)
Draw the geometrical isomers of [CoCl2(en)2]+
Using valence bond theory explain the hybridization, and magnetic behaviour of
[CO (CN)6]3- ion.
4.
(a)
(b)
give example of a ambidentate and a chelating ligand.
Draw a diagram to show the splitting of d-orbitals in an Octahedral crystal field.
Explain how the actual configuration is decided by the magnitude of ∆0 value.
1. (a) A coordination compound has the formula CoCl3 .4NH3. It does not liberate
ammonia but forms a precipitate with AgNO3. Write the structure and IUPAC
name of the complex compound.
(b)Name a ligand which is bidentate and give an example of the complex formed by
this ligand.
2. Explain the following cases giving appropriate reasons ;
(i)
Nickel (II) does not form low spin octahedral complexes.
(ii)
The ∏-Complexes are known for the transition metals only.
(iii) Co2+ is easily oxidised to Co3+ in the presence of a strong ligand.
3. What is the difference between inner orbiteal and outer orbital octahedral complexes?
Illustrate with the help of an example.
4. Explain the following giving an example in each case :
(i)
Linkage isomerism
(ii)
An outer orbital complex
(iii) Ambidentate ligand
(i)Nickel(II) does not form low spin octahedral complexes.
(ii)The π-complexes are known for the transition metals only.
(iii) Co2+ is easily oxidized to Co3+ in the presence of a strong ligand.
4.Write the IUPAC names of the following coordination compounds:
(i) [Cr(NH3)3Cl3] (ii) K3[Fe(CN)6]
(iii)[CoBr2(en)2]+,(en=ethylene diamine)
5. For the complex [NiCl4]2-,write
(i)the IUPAC name (ii)the hybridization type, (iii)the shape of the complex.
6.What is meant by crystal field splitting energy? On the basis of crystal field theory, write the
electronic configuration
of d4 in terms of t2g and eg in an octahedral field when
(i)
0>p
(ii)
0<p
7.(a)Write the IUPAC name of the complex [CoBr2(en)2]+
(b)What type of isomerism is shown by the complex [Co(NH3)5SO4]Br?
(c)Why is CO a stronger ligand than NH3 in complexes?
8.(a)What type of isomerism is shown by each of the following complexes:
(i)[Pt(NH3)2Cl2]
(ii)[Co(NH3)5(NO2)]Cl2
(b)Give an example of the role of coordination compounds in biological systems.
9. (i)Write the IUPAC name of the complex [Cr(NH3)4Cl2]Cl.
(ii)What type of isomerism is exhibited by the complex [Co(en)3]3+ ?
(iii)Why is[NiCl4]2- paramagnetic but Ni(CO)4] is diamagnetic?
{At nos. Cr=24,Co=27,Ni=28}
VALUE BASED QUESTION (4 MARKS)
1. Hemoglobin, the is red pigment of blood, which acts as oxygen carrier is a coordination
compound. The deficiency of Iron leads to anaemia. Vitamins are also essential for
growth of our body , Vitamins B12 deficiency leads to pernicious anaemia.
(a) Name the complex present in vitamin B12.Which metal is present in it?
(b) What are the sources of iron in our body?
(c) What are the values possessed by people taking iron rich diet?
(d) Name the vitamin which helps in absorption of iron by our body?
Co-ordination compounds have an important role in the field of medicines. Out of these,
the compound cic-platin is quite effective against cancer. It inhibits the growth of tumors
leading to cancer.
(a)
What is the chemical formula and name of the complex.
(b)
How does it behave as an anti-cancer agent ?
(c)
Why is trans isomer not effective ?
(d)
What is the value associated with the use of cic-platin.
HALOALKANE AND HALOARENE (CH-10)
1mark
1.Write the IUPAC names of the following compound.
2.Write the IUPAC names of the following compound.
3. Write the structure of following compound
2-chloro-3-methylpentane
4. Write the structure of following compound
1-bromo-4-sec-butyl-2–methylebenzene
5. Arrange the following in the increasing order of boiling points
bromomethane, chloromethane, dichloromethane
1. What happens when bromine attacks CH2 = CH—CH2—C ≡ CH?
2
3.Write the IUPAC name of the following compound: (CH3)3 CCH2Br
4.Draw the structure of the following compound:
4-Bromo-3-methylpent-2-ene
5. Complete the following chemical equation:
CH3CH2CH= CH2 + HBr Peroxide

→ ..................
6.What happens when CH3—Br is treated with KCN?
1Write the IUPAC name of the following compound :
CH2 = CH−CH2−C≡CH
2. Haloalkanes react with KCN to form alkyl cyanide as main product while AgCN
form isocyanides as the chief product. Explain
3. A solution of KOH hydrolyses CH3CHClCH2CH3 and CH3CH2CH2CH2Cl. Which
one of these ismore easily hydrolysed
4. Draw the structure of the following compound: 4-Bromo-3-methylpent-2-ene
5. Write the IUPAC name of the following compound:
(CH3)3 CCH2Br
6. How would you convert ethanol to ethene?
7. Why are halo arenes more stable or less reactive than halo alkanes towards
electrophillic substitution reaction/
8. What is meant by chirality of a compound? Give an example.
9. Write the structure of 2-(2-bromo phenyl)butane.
10. Write the structure of 4- tert butyl -3-iodo heptane.
11. Why alkyl halides are generally not prepared in the laboratory by free radical
halogenations of alkanes?
(a)
(b)
(c)
(d)
(e)
(f)
1 Write the IUPAC names of the following compoundCH2Br – CH = CH – CH2 – C - CH
2 Write the structure of following halogen compounds
1-bromo-4-sec-butyl-2–methylebenzene.
Arrange1-chloropropane, isopropyl chloride, 1-chlorobutane
Increasing order of boiling point
1. Answer the following questions:
(i) What is meant by chirality of a compound? Give an example.
(ii) Which one of the following compounds is more easily hydrolysed by KOH and why?
CH3CHClCH2CH3 or CH3CH2CH2Cl
2.
3.
4.
5.
6. Chlorobenzene is extremely less reactive towards a nucleophilic substitution reaction. Give two reasons
for the same.
7. Write chemical equations when
(i) ethyl chloride is treated with aqueous KOH.
(ii) chlorobenzene is treated with CH3COCl in presence of anhydrous AlCl3 .
8 (a) Which alkyl halide from the following pairs would you expect to react more rapidly by SN2
mechanism and why?
(b) Racemisation occurs in SN1 reactions. Why?
SECTION-C (THREE MARKS)
1.Answer the following:
(i) Identify chiral in CH3CHOHCH2CH3 and CH3CHOHCH3.
(ii) Among the following compounds, which one is more easily hydrolysed and why?
CH3CHCICH2CH3 or CH3CH2CH2CH2Cl
(iii) Which of these will react faster in SN2 displacement and why?
1-bromopentane or 2-bromopentane
2. (a) Why does p-dichlorobenzene have a higher m.p. than its o- and m- isomers?
(b) Why is (±) – Butan-2-ol is optically inactive?
3. Give reasons for the following:
(i) Ethyl iodide undergoes SN2 reaction faster than ethyl bromide.
(ii) (±) 2–Butanol is optically inactive.
(iii) C–X bond length in halobenzene is smaller than C–X bond length in CH3–X.
4.
(2MARKS)
1. Which compound in each of the following pairs will react faster in SN2 reaction
with —OH? Why?
(i) CH3Br or CH3I (ii) (CH3 )3CCl or CH3Cl
2. Complete the following reaction equations:
(i) C6H5N2Cl + KI →
୮ୣ୰୭୶୧ୢୣ
(ii)CH3CH2CH= CH2 + HBrሱۛۛۛۛۛሮ
3. Write the IUPAC names of the following compounds :
(i) (CH3 )3 CCH2Br
(ii)C6H5 -CH2 –Cl
4. Which one of these compounds is more easily hydrolysed by KOH solution and
why?
CH3 CHCICH2CH3Or CH3CH2CH2CH2Cl
5. How would you obtain
(i)2-phenyl acetic acid from toluene.
(ii) 2-Methylpropene from 2methylpropanol?
6. What are ambident nucleophiles? Explain giving an example.
7. Explain as to why
(i) Alkyl halides, though polar, are immiscible with water.
(ii) Grignard’s reagents should be prepared under anhydrous conditions.
8. Explain why
(i) the dipole moment of chlorobenzene is lower than that of cyclohexyl chloride.
(ii) haloalkanes are only slightly soluble in water but dissolve easily in organic
solvents.
9. (a) Why does p-dichlorobenzene have a higher m.p. than its o- and m- isomers?
(b) Why is (±) – Butan-2-ol is optically inactive?
10. Account for the following:
(i) The C—Cl bond length in chlorobenzene is shorter than that in CH3—Cl.
(ii) Chloroform is stored in closed dark brown bottles.
11. Propose reaction for the preparation of(1) ally1 iodide and(2) ally1 fluoride from
prop- 1- ene?
SHORT ANSWER-II(3MARKS)
(i) State one use each of DDT and iodoform.
(ii) Which compound in the following couples will react faster in SN2
displacement and why?
(a) 1-Bromopentane or 2-bromopentane
(b) 1-Bromo-2-methylbutane or 2-bromo-2-methylbutane.
2. How would you differentiate between SN1 and SN2 mechanisms of substitution
reactions? Give one example of each.
3. Answer the following:
(i) Identify chiral in CH3CHOHCH2CH3 and CH3CHOHCH3.
1.
(ii) What is known as a racemic mixture? Give an example.
(iii) Of the two bromoderivatives, C6H5CH(CH3)Br and C6H5CH(C6H5)Br, which
one is more reactive in SN1 substitution reaction and why?
4. Rearrange the compounds of each of the following sets in order of reactivity
towards SN2 displacement:
(i) 2-Bromo-2-methylbutane, 1-Bromopentane, 2-Bromopentane
(ii) 1-Bromo-3-methylbutane, 2-Bromo-2methylbutane, 3-Bromo-2-methylbutane
(iii) 1-Bromobutane, 1-Bromo-2, 2-dimethylpropane, 1-Bromo-2-methylbutane
5. Although chlorine is an electron withdrawing group, yet it is ortho-, para-directing
in electrophilic aromatic substitution reactions. Explain why it is so?
6. Give reasons for the following:
(i) Ethyl iodide undergoes SN2 reaction faster than ethyl bromide.
(ii) The order of reactivity of haloalkanes is
RI > RCl > RBr
iii)Neopentyl chloride does not follow ܵே 2 mechanism
7(a) Write a chemical test to distinguish between ;
(i)
Chlorobenzene and Benzylchloride
(ii)
Chloroform and carbon tetrachloride.
(b)Why is methyl chloride hydrolysed more easily than chlorobenzene ?
7.Convert :
(i) Chlorobenzene to p-nitrophenol
(ii)Butane-1-ol to But-1-ene
iii)Ethanol to but 1-yne.
8. a.Haloalkanes undergo nucleophillc substitution reactions while haloarenes
undergo
electrophilic substitution reactions. Explain?
b. The following reaction gives two products. Write the structures of the
products.
ୟ୪ୡ.୏୓ୌ
C6H5CH2CHCIC6H5 ୌୣୟ୲
C.An organic compound C8H18 on monochlorination gives a single monochloride
. Write
the structure of the hydrocarbon.
9.a. Give the structural formula and IUPAC name of DDT.
b.Explain the following in one or two sentences :
(i)Allyl chloride is hydrolysed more readily than n-propyl chloride.
(ii)Vinyl chloride is hydrolysed more slowly than ethyl chloride.
10.Explain the following :
a. The treatment of alkyl chlorides with aqueous KOH leads to the formation
of alcohols but in presence of
alcoholic KOH, alkenes are the major products.
b. Haloalkanes react with KCN to form alkyl cyanides as main product while
AgCN forms isocyanides as the
major product.
c.neopentyl bromide undergoes nucleophilic substitution reaction very slowly
1.
11
VALUE BASED QUESTION (4 MARKS)
1. The chloroflurocarbon compounds of methane and ethane are collectively
known as freons. They are extremely stable and unreactive, non-toxic, noncorrosive and easily liquefiable gases.
(g) Write the formula of Freon-12.
(h) Give two uses of chloroflurocarbons.
(i) What is the harmful effect of having CFCs?
(j) Do you think use of CFCs banned? Give reason.
(k) 1 How will you bring about the following conversions?
(l)
(i) benzene to 3-bromonitrobenzene
(m) (ii) ethanol to but-1-yne
(n)
(o) 2
Explain the following reactions with suitable example :
(p) (i) Finkelstein reaction.
(q) (ii) Swarts reaction.
(r) 3
Give a chemical test to distinguish between the following pairs of
compounds:
(i) chlorobenzene and cyclohexylchloride.
(s)
(t)
(ii) vinyl chloride and ethyl chloride.
(u) 4 Give mechanism of the following reactions :
(v)
(i) (CH3)3C – Cl + O – H ––>(CH3)3 C – OH
(w) (ii) CH3 – Cl + OH–>CH3 – OH
(x) 5 Which compound in each of the following pairs will react faster in SN2
reaction with OH– and why?
(y)
(z)
(i) CH3Br or CH3I
(aa)
(ii)(CH3)3CClorCH3Cl
(bb) 6
Give reasons for the following :
(cc) (i) The bond length of C–Cl bond is larger in haloalkanes than that in haloarenes.
(dd) (ii) Although alkyl halides are polar in nature but are not soluble in Water
(ee)
)
1. Explain as to why haloarenes are much less reactive than haloalkanes towards
nucleophilic substitution reactions
2. A solution of KOH hydrolyses CH3CHClCH2CH3 and CH3CH2CH2CH2Cl. Which one of these
is more easily hydrolysed
3. Which is a stronger acid in aqueous solution—HCl or HI, and why?
4. Draw the structure of the following compound: 4-Bromo-3-methylpent-2-ene
5. Write the IUPAC name of the following compound: (CH3)3 CCH2Br
6. How would you convert ethanol to ethene?
7. Which will react faster in SN2 displacement, 1-bromopentane or 2-bromopentane, and
why?
8. What is meant by chirality of a compound? Give an example.
9. What happens when CH3—Br is treated with KCN?
10. What happens when ethyl chloride is treated with aqueous KOH?
SHORT ANSWER-I(2MARKS)
11. Which compound in each of the following pairs will react faster in SN2 reaction with —
OH? Why?
(i) CH3Br or CH3I (ii) (CH3 ) 3 CCl or CH3Cl
12. Complete the following reaction equations:
(i) C6H5N2Cl + KI →
୮ୣ୰୭୶୧ୢୣ
(ii) CH3CH2CH= CH2 + HBr ሱۛۛۛۛۛሮ
13. Write the IUPAC names of the following compounds :
(i) (CH3 ) 3 CCH2Br
(ii)C6H5 -CH2 –Cl
14. Which one of these compounds is more easily hydrolysed by KOH solution and why?
CH3 CHCICH2CH3 Or CH3CH2CH2CH2Cl
15. How would you obtain
(i) Picric acid (2, 4, 6-trinitrophenol) from phenol, (ii) 2-Methylpropene from 2methylpropanol?
16. What are ambident nucleophiles? Explain giving an example.
17. Explain as to why
(i) Alkyl halides, though polar, are immiscible with water.
(ii) Grignard’s reagents should be prepared under anhydrous conditions.
18. Explain why
(i) the dipole moment of chlorobenzene is lower than that of cyclohexyl chloride.
(ii) haloalkanes are only slightly soluble in water but dissolve easily in organic solvents.
19. (a) Why does p-dichlorobenzene have a higher m.p. than its o- and m- isomers?
7.
8.
9.
10.
11.
12.
13.
SHORT ANSWER-II(3MARKS)
(i) State one use each of DDT and iodoform.
(ii) Which compound in the following couples will react faster in SN2 displacement and
why?
(a) 1-Bromopentane or 2-bromopentane
(b) 1-Bromo-2-methylbutane or 2-bromo-2-methylbutane.
How would you differentiate between SN1 and SN2 mechanisms of substitution
reactions? Give one example of each.
Answer the following:
(i) Identify chiral in CH3CHOHCH2CH3 and CH3CHOHCH3.
(ii) Among the following compounds, which one is more easily hydrolysed and why?
CH3CHCICH2CH3 or CH3CH2CH2CH2Cl
(iii) Which of these will react faster in SN2 displacement and why? 1-bromopentane or
2-bromopentane
Answer the following:
(i) Haloalkanes easily dissolve in organic solvents, why?
(ii) What is known as a racemic mixture? Give an example.
(iii) Of the two bromoderivatives, C6H5CH(CH3)Br and C6H5CH(C6H5)Br, which one is more
reactive in SN1 substitution reaction and why?
Rearrange the compounds of each of the following sets in order of reactivity towards
SN2 displacement:
(i) 2-Bromo-2-methylbutane, 1-Bromopentane, 2-Bromopentane
(ii) 1-Bromo-3-methylbutane, 2-Bromo-2methylbutane, 3-Bromo-2-methylbutane
(iii) 1-Bromobutane, 1-Bromo-2, 2-dimethylpropane, 1-Bromo-2-methylbutane
Although chlorine is an electron withdrawing group, yet it is ortho-, para-directing in
electrophilic aromatic substitution reactions. Explain why it is so?
Give reasons for the following:
(i) Ethyl iodide undergoes SN2 reaction faster than ethyl bromide.
(ii) (±) 2–Butanol is optically inactive.
(iii) C–X bond length in halobenzene is smaller than C–X bond length in CH3–X.
VALUE BASED QUESTION (4 MARKS)
2. The chloroflurocarbon compounds of methane and ethane are collectively known as
freons. They are extremely stable and unreactive, non-toxic, non-corrosive and easily
liquefiable gases.
(ff) Write the formula of Freon-12.
(gg) Give two uses of chloroflurocarbons.
(hh) What is the harmful effect of having CFCs?
(ii) Do you think use of CFCs banned? Give reason.
[1 Marks Questions]
1. What happens when CH3-Br is treated with KCl?
2. Write the structure of 2-(2-bromophenyl) butane.
3. Which will react faster in SN2 displacement, 1 – bromopentane or 2 – bromopentane. Why?
4. Write the structure of 4- tert.butyl-3 iodoheptane.
5. Write a chemical reaction in which the iodide ion replaces the diazonium group in a diazonium salt?
[2 Marks Questions]
a) Chlorobenzene is extremely less reactive towards a nucleophilic substitution reaction.Give two
reasons for the same.
b) Which one of the following pairs undergoes SNl substitution reaction faster and . why ?
i)
ii)
CH2Cl or
I
or
Cl
Cl
c) Complete the reaction :i)
C6H5N2Cl+ KI→
ii)
CH3 – CH2 – CH = CH2 + HBr
d) Suggest a possible reason:
1. The order of reactivity of haloalkanes is RI > RBr > RCl.
2. Neo pentyl chloride ,(CH3)3 C - CH3Cl does not follow SN2 mechanism.
e) Discuss the mechanism of SN1 reaction of haloalkanes.
[3 Marks Questions]
1) Although chlorine is an electron withdrawing group, yet it is ortho, para directing in
electrophilic aromatic substitution reaction. Explain why is it so?
2) Write a chemical test to distinguish between
a) Chlorobenzene and benzylchloride
b) CHCl3 and CCl4
c) Why is methyl chloride hydrolysed more easily than chlorobenzene .
3) i) State one use of DDT and iodoform.
ii) Which compound in the following couples will react faster in SN2 displacement and why ?
1- bromo – 2 methylbutane or
2- bromo – 2 methylbutane.
4) Explain why
1. The dipole moment of cholorobenzene is lower than that of cyclohexyl chloride.
2. Alkyl halides though polar are immiscible with water ?
3. In the pair, (CH3)3 --C—Cl and CH3Cl, CH3Cl will react faster in SN2 reaction with –OH?
Alcohols,phenols and ethers(CH-11)
Section-A (1MARK)
1. Write the structure of the molecule of a compound whose IUPAC name is
1-phenylpropan-2-ol
2. Draw the structural formula of 1-phenylpropan-1-one molecule
3. Write the mechanisms of the following reactions:
(i) Hydration of ethene to ethanol
(ii) Dehydration of ethanol, giving ethene.
4.
5. How would you convert ethanol to ethene?
6. Draw the structure of 2, 6-Dimethylphenol.
7. Which of the following isomers is more volatile: o-nitrophenol or p-nitrophenol?
1. Draw the structure of hex-1-en-3-ol compound.
2. Write the chemical equation for the preparation of phenol from
benzene using oleum and sodium hydroxide.
3. How can phenol be distinguished from carboxylic acid ?
4. Name the product obtained when 2-butanol is refluxed with SOCl2
in presence of pyridine as solvent.
5. How is t-butyl alcohol obtained from acetone ?
6. What happens when 2-propanol is treated with HCl in presence of
anhydrous ZnCl2 ?
7. What happens when phenol is treated with excess of nitrating
mixture ?
8. Give the IUPAC name of the following compound: CH3-C(CH3)=C(Br)-CH2-OH
9. Give the IUPAC name of the following compound: H2C =CH—CH(OH) —CH2—
CH2—CH3
10. Draw the structure of 2, 6-Dimethylphenol.
11. Of the two alcohols; (a) CH2=CH—CH2OH and (b) CH2=CH—CH2—CH2OH,
which one will react more easily with conc. HCl in the presence of ZnCl2?
12. Arrange the following compounds in the increasing order of their acid strengths:
4-nitrophenol, phenol, 2,4,6-trinitrophenol
6.Acid-catalysed dehydration of tert- butanol is faster than that of n- butanol
.Explains?
2
3
Write IUPAC names of the following compound
CH3CH2OCH2CH2CH2Cl
Write the structure of the compounds whose name is given below :
3, 5-dimethoxyhexane-1, 3, 5-triol
Arrange the following in the increasing order of property shown :
phenol, o-nitrophenol, m-nitrophenol, p-nitrophenol. (Acid strength)
4 .What is the function of ZnCl2 (anhyd) in Lucas test for distinction between 1°, 2° and 3°
alcohols.
5 .Nitrophenol is more acidic than o-methoxyphenol . Explain
1. Arrange the following compounds in an increasing order of their acid strengths:
(CH3 ) 2 CHCOOH, CH3CH2CH(Br)COOH, CH3CH(Br)
CH2COOH
2. Give the IUPAC name of the following compound: CH3C(CH3)=C(Br)-CH2-OH
3. Give the IUPAC name of the following compound: H2C =CH—
CH(OH) —CH2—CH2—CH3
4. Draw the structure of 2, 6-Dimethylphenol.
5. Of the two alcohols; (a) CH2=CH—CH2OH and (b) CH2=CH—
CH2—CH2OH, which one will react more easily with conc. HCl
in the presence of ZnCl2?
6. Ethanol is soluble in water. Why?
7. Arrange the following compounds in the increasing order of their
acid strengths:
4-nitrophenol, phenol, 2,4,6-trinitrophenol
8.Write the chemical equation for the preparation of phenol from benzene using oleum and sodium
hydroxide.
9.Phenyl methyl ether reacts with HI to give phenol and methyl iodide and not iodobenzene and methyl
alcohol. Why?
10.Why is the preparation of ether by acid catalysed dehydration of secondary alcohol not a suitable
method?
11.How can you convert Anisole to phenol?
12.Write the equation involved in the reaction
Williamsons Ether Synthesis.
2MARKS
1. How will you convert
a) Propene to Propan-1-ol?
b) Enthnal to Propan-2-ol?
2. Explain
a) Alcohols are more soluble in water than the hydrocarbons of
comparable masses
b) Ortho-Nitrophenol is more acidic than ortho-methoxyphenol.
3. How will you convert?
a) Benzyl chloride to benzyl alcohol.
b) Methyl magnesium bromide to 2-methylpropan-2-ol.
4. Give one chemical test to distinguish between
a) Phenol and Benzoic Acid
b) 1-propanol and 2-propanol
5. How will you convert?
1. Propan-2-ol to propanone.
2. Phenol to 2,4,6-tribromophenol
1. Illustrate the following reactions giving a chemical equation for each:
(i) Kolbe's reaction, (ii) Williamson synthesis.
2.Explain the following reactions with an example for each:
(i) Reimer-Tiemann reaction
(ii) Friedel-Crafts reaction.
3.
4. Alcohols react both as nucleophiles as well as electrophiles. Write one reaction of each type
and
describe its mechanism.
5.
6. Name the reagents used in the following reactions:
(i) Nitration of phenol to 2, 4, 6-trinitrophenol
(ii) Butanal to Butanol
(iii) Friedel-Crafts acetylation of anisole
(iv) Oxidation of primary alcohol to aldehyde
7.
8.
9. How will you convert:
(i) Propene to Propan–2–ol?
(ii) Phenol to 2, 4, 6 – trinitrophenol?
10. How will you convert the following?
(i) Propan–2–ol to propanone. (ii) Phenol to 2, 4, 6–tribromophenol
1. Explain the mechanism of following reaction :
Conc.H2SO4
2C2H5OH
C2H5OC2H5 +H2O
413 K
2. Nitration of phenol gives only ortho and para products. Give reasons.
3. Write equations for preparation of propan-2-ol from (i) an alkene and (ii) a Grignard
reagent.
4. How would you obtain
(i)
Picric acid (2, 4, 6-trinitrophenol) from phenol
(ii)
2-Methylpropene from 2-methylpropanol ?
5. Give one chemical test to distinguish between the following pairs of compounds :
(i)
Phenol and Benzoic acid
1-Propanol and 2-Propanol
1. Alcohols react both as nucleophiles as well as electrophiles. Write one reaction
of each type and describe its mechanism.
2. How would you carry out the following conversions?
(i) Ethyl magnesium chloride to propan-1-ol(ii) Benzyl chloride to benzyl alcohol
3. Give a chemical equation for each of the following reactions:
(i) Williamson’s synthesis (ii) Reimer-Tiemann reaction
4. Explain the mechanism of each of the following processes:
(i) Acid catalysed dehydration of an alcohol
(ii) Hydration of ethene to
yield ethanol.
5. Illustrate the following reactions giving a chemical equation for each:
(i) Kolbe's reaction, (ii) Friedel-Crafts reaction
6. How are the following conversions carried out?
(i)phenol to picric acid(2,4,6,trinitro phenol.), (ii) Methyl magnesium bromide to
2-methylpropan-2-.
7. How are the following conversions carried out?
8. (i) Propene to Propan-2-ol (ii) phenol to para- bromo phenol.
9. Illustrate the following name reactions giving a chemical reaction equation for
each:
(i) Kolbe’s reaction of phenol
(ii) Friedel-Crafts’ acetylation of anisole..
10. Explain the following behaviours:
(i) Alcohols are more soluble in water than the hydrocarbons of comparable
molecular masses.
(ii) Ortho-nitrophenol is more acidic than ortho-methoxyphenol.
11. How will you convert:(i) Propene to Propan–1–ol?(ii) phenol to benzoquinone.
12.Give the product and show the steps in
1. hydration of cyclobutylethene in dil. H2SO4
2. dehydration of cyclobutylcarbinol
1
Give a chemical test to distinguish between the following pair of
(a) phenol and anisole
(b) ethanol and diethyl ether
2
Write the mechanism of acid catalysed dehydration of alcohols :
3
Describe the following reactions with example
(a) Williamson synthesis
(b) Reimer-Tiemann reaction.
How will you convert
(i) propene to propan-l-ol.
4
compounds
1. Alcohols react both as nucleophiles as well as electrophiles. Write
one reaction of each type and describe its mechanism.
2. How would you carry out the following conversions?
(i) Ethyl magnesium chloride to propan-1-ol (ii) Benzyl chloride
to benzyl alcohol
3. Give a chemical equation for each of the following reactions:
(i) Williamson’s synthesis (ii) Reimer-Tiemann reaction
4. Explain the mechanism of each of the following processes:
(i) Acid catalysed dehydration of an alcohol
(ii) Hydration of
ethene to yield ethanol.
5. Illustrate the following reactions giving a chemical equation for
each:
(i) Kolbe's reaction, (ii) Friedel-Crafts reaction
6. How are the following conversions carried out?
(i) Benzyl chloride to benzyl alcohol, (ii) Methyl magnesium
bromide to 2-methylpropan-2-ol.
7. Write the mechanisms of the following reactions:
(i) Hydration of ethene to ethanol
(ii) Dehydration of ethanol,
giving ethene.
8. How are the following conversions carried out?
9. (i) Propene to Propan-2-ol (ii) Ethyl magnesium chloride to
Propan-1-ol
10.
Illustrate the following name reactions giving a chemical
reaction equation for each:
(i) Kolbe’s reaction of phenol
(ii) Friedel-Crafts’ acetylation of
anisole.
[3 Marks Questions]
1. Account For The following
a) Propanol has higher B.P than Butane.
b) o-Nitrophenol is more acidic than o-methoxyphenol.
2.
3.
4.
5.
c) Prepration of Etheres by acid Dehydration of 2˚ or 3˚ alcohol
is not a suitable method.
A compound A(C6H6O) on oxidation by PCC gave B, which on
treatment with aqueous alkali and subsequent heating furnished
C. B on oxidation by KMnO4 forms a monobasic carboxylic
acid with molar mass 16gm mol- deduce the structure of A,B,C
Explain the mechanism for :a) Addition of Grignard’s reagent to the carbonyl group of
compound forming an adduct followed by hydrolysis.
b) Acid catalysed dehydration of an alcohol forming an alkene.
c) Acid catalised hydration of an alkene forming an alcohol.
Name the reagent used in following conversions
a) A primary alcohol to an aldehyde.
b) Butan-2-one to butan-2-ol.
c) Phenol to 2,4,6-tribromophenol.
State the product of :a) CH3CH2CH2OCH3 + HBr
b)
OC2H5
+ HBr
HI
c) (CH3)3 C-OC2H5
6. How could you account for
1.phenols are more acidic than alcohols.
The boiling points of ethers are much lower than those of the
alcohols of comparable molar masses?
1. How would you convert the following:
(i) Phenol to benzoquinone
(ii) Propanone to 2-methylpropan-2-ol
(iii) Propene to propan-2-ol
2. Explain the following observations:
(i) The boiling point of ethanol is higher than that of methoxymethane.
(ii) Phenol is more acidic than ethanol.
(iii) o-and p-nitrophenols are more acidic than phenol
3. How would you obtain the following:
(i) Benzoquinone from phenol
(ii) 2-Methylpropan-2-ol from methylmagnesium bromide
(iii) Propan-2-ol from propane
4.Name the reagents which are used in the following conversions:
(i) A primary alcohol to an aldehyde
(ii) Butan-2-one to butan-2-ol
(iii) Phenol to 2, 4, 6-tribromophenol
5.Name the different reagents needed to perform the following reactions:
(i) Phenol to benzene
(ii) Dehydration of propan-2-ol to propene
(iv) Dehydrogenation of ethanol to ethanol
1. State the products of the following reactions :
(i) CH3−CH2−CH2−O−CH3 + HBr
(ii)
OC2H5
+ HBr
HI
2.
3.
4.
5.
(iii) (CH3)3C−OC2H5
Account for the following :
(i) The boiling point of ethanol is higher than that of methanol.
(ii) Phenol is a stronger acid than an alcohol
(iii) The boiling point of ethers are lower than isomeric alcohols,
How would you convert the following :
(i) Phenol to benzoquinone
(ii) Propanone to 2-methylpropan-2-ol
(iii) Propene to propan-2-ol
Name the reagents used in the following reactions :
(i) Oxidation of a primary alcohol to carboxylic acid.
(ii) Oxidation of a primary alcohol to an aldehyde.
(iii) Bromination of phenol to 2, 4,6-tribromophenol.
Write short notes on :
(i) Reimer-Tiemann reaction
(ii) Kolbe’s reaction
(iii) Williamson’s synthesis
6. Account for the following :
(i) Propanol has higer boiling point than butane.
(ii) Ortho-nitrophenol is more acidic than ortho-methoxyphenol.
(iii) Preparation of ethers by acid dehydration of secondary or
tertiary alcohols is not a suitable method.
1. Explain the following observations:
(i)The boiling point of ethanol is higher than that of methoxymethane.
(i ) Phenol is more acidic than ethanol
ii).o-and p-nitrophenols are more acidic than phenol.
2.complete the reaction.
(iv)
(v)
(vi)
CH3−CH2−CH2−O−CH3 + HBr
C6H5OC2H5+ HBr
HI
(CH3)3C−OC2H5
:
2. Draw the structure and name the product formed if the following alcohols are
oxidized. Assume that an excess of oxidizing agent is used. (i)
CH3CH2CH2CH2OH (ii) 2-butenol (iii) 2-methyl-1-propanol
3. Although phenoxide ion has more number of resonating structures than
carboxylate ion,carboxylic acid is a stronger acid than phenol. Give two reasons.
.
3.An aromatic compound ‘A’ on treatment with CHCl3/KOH gives two compounds ‘B’
and ‘C’. Both B and C give the same product ‘D’ when distilled with Zinc dust. Oxidation
of D gives E having molecular formula C7H6O2. The sodium salt of E on heating with
soda-lime gives F which may also be obtained by distilling A with zinc dust. Identify A to
F.
1
An alcohol A (C4H10O) on oxidation with acidified potassium dichromate gives
carboxylic acid B (C4H8O2). Compound A when dehydrated with conc. H2SO4 at 443 K
gives compound C. Treatment of C with aqueous H2SO4 gives compound D (C4H10O)
which is an isomer of A. Compound D is resistant to oxidation but compound A can be
easily oxidised. Identify A, B, C and D and write their structures
4. Explain the following observations:
(i)The boiling point of ethanol is higher than that of
methoxymethane.
(ii) Phenol is more acidic than ethanol.
(iii) o-and p-nitrophenols are more acidic than phenol.
5. How would you convert the following:
(a)Phenol to benzoquinone
(b) Propanone to 2-methylpropan-2-ol
(c)Propene to propan-2-ol
6. Draw the structure and name the product formed if the following
alcohols are oxidized. Assume that an excess of oxidizing agent is
used. (i) CH3CH2CH2CH2OH (ii) 2-butenol (iii) 2-methyl-1propanol
7. Although phenoxide ion has more number of resonating structures
than carboxylate ion, carboxylic acid is a stronger acid than
phenol. Give two reasons.
VALUE BASED QUESTION (4 MARKS)
1. Ethane-1,2-diol (ethylene glycol) is dihydric alcohol. It is used as a
coolant in radiators of vehicles and aeroplanes. It is also used as
antifreeze especially in cold countries. It is used in manufacture of
terylene. It is used as solvent and preservative.
(a) How is ethylene converted into ethylene glycol?
(b) Why ethylene glycol used as antifreeze?
(c) Name the monomer of terylene.
(d) Why should we not use terylene cloths in kitchen?
ALDEHYDES,KETONES AND CARBOXYLIC ACIDS(CH-12)
SECTION-A (1MARK)
1. What is Tollen’s reagent? Write one usefulness of this reagent
2. Give IUPAC name of the following compound:
(CH3)2C=CHCOCH3
3. Arrange the following compounds in an increasing order of their acid strengths:
(CH3 ) 2 CHCOOH, CH3CH2CH(Br)COOH, CH3CH(Br) CH2COOH
4. Write the structure of 3-oxopentanal.
5. Draw the structure of 3-methylbutanal.
6. Arrange the following compounds in increasing order of their reactivity in nucleophilic
addition
reactions: ethanal, propanal, propanone, butanone
7. Give simple test to distinguish between
Pentan-2-one and Pentan-3-one
1. Write the structure of pent-2-en-al.
2. What is Tollen’s reagent ? Write one usefulness of this reagent.
3. Complete the following reaction and give the names of the major products ;
C6H5CONH2 + HONO
4. What happens when ethanoyl chloride is subjected to Rosenmund reduction ?
5. What happens when benzoic acid is treated with conc. HNO3 and conc. H2SO4 ?
Give chemical equation.
6. Write structures of the products of the following reaction :
(C6H5CH2)2Cd + 2CH3COCl
7. What happens when methanol reacts with CH3MgBr followed by hydrolysis ?Give
chemical equation.
8. Give chemical test to distinguish between phenol and benzoic acid.
9. Illustrate Decarboxylation reaction with an example.
10. Illustrate the following reaction :
Cross- aldol condensation.
1.
2.
3.
4.
5.
6.
7.
VERY SHORT ANSWER(1MARKS)
Arrange the following compounds in an increasing order of their acid strengths:
(CH3 )2 CHCOOH, CH3CH2CH(Br)COOH, CH3CH(Br) CH2COOH
Write the IUPAC name of the following compound: CH3COCH2COCH3
Why are lower members of aldehydes easily miscible with water?
Write the structure of 3-oxopentanal.
Write the structural formula of 1-phenylpentan-1-one.
What is Tollen’s reagent? Write one usefulness of this reagent.
Give IUPAC name of the following compound: (CH3)2C=CHCOCH3
8. Draw the structure of 2-hydroxy cyclopentanecarbaldehyde.
9. Arrange the following compounds in increasing order of their reactivity in
nucleophilic addition reactions: ethanal, propanal, propanone, butanone.
.
10. Rearrange the following compounds in the increasing order of their boiling points:
CH3—CHO, CH3—CH2—OH, CH3—CH2—CH3
01.
02.
Write the IUPAC name of the compound
HOOC – CH2 – CH – CH2 – COOH
|
COOH
Name and complete the following chemical reaction
RCH2COOH (i) X2 / red P (ii) H2O
03.
Distinguish between propanal and propanone
04.
Arrange the following in increasing order of their reactivity towards nucliophilic addition
reaction
CH3CHO , CH3COOH , CH3CH2 OH
05.
Arrange the following in increasing order of their reactivity towards nucliophilic addition
reaction
C6H5COCH3 , CH3CHO
, CH3 COCH3
11. Arrange the following compounds in an increasing order of their acid strengths:
(CH3 ) 2 CHCOOH, CH3CH2CH(Br)COOH, CH3CH(Br) CH2COOH
12. Write the IUPAC name of the following compound: CH3COCH2COCH3
13. Why are lower members of aldehydes easily miscible with water?
14. Write the structure of 3-oxopentanal.
15. Write the structural formula of 1-phenylpentan-1-one.
16. What is Tollen’s reagent? Write one usefulness of this reagent.
17. Give IUPAC name of the following compound: (CH3)2C=CHCOCH3
18. Draw the structure of 3-methylbutanal
19. Arrange the following compounds in increasing order of their reactivity in nucleophilic
addition reactions: ethanal, propanal, propanone, butanone.
20. Draw the structure of hex-1-en-3-ol compound.
21. Rearrange the following compounds in the increasing order of their boiling points:
CH3—CHO, CH3—CH2—OH, CH3—CH2—CH3
1. Rearrange the following compounds in the increasing order of their boiling points
CH3 –CHO, CH3—CH2—OH, CH3—CH2—CH3
2. Give Chemical test to distinguish between benzophenone and acetophenone.
3. Illustrate the following reaction Cross An ldol condensation
4. What is Tollen’s Reagent? Write one usefulness of this reagent.
5. Draw the structure of 3-oxopentanal.
6. Complete the following reaction
஺௟஼௟ଷ
C6H6+ RCOCl ሱۛۛሮ
7. Give chemical test to distinguish between phenol and benzoic acid?
8. How are the following conversion carried out?
A) Acetic acid to methylamine
B) Acetaldehyde to methane
9. State reason
A)Monochloro ethanoic acid is a weaker acid than dichloroethanoic acid.
B)Benzoic acid is a stronger acid than ethanoic acid.
10. How are the following conversion carried out?
A) Acetic acid to methylamine
B) Acetaldehyde to methane
11. . Write IUPAC name of
COOH
CL
Br
12. Illustrate Decarboxylation reaction with an example.
SECTION-B (2MARK)
1. (a) Illustrate the following reactions giving one example for each :
(i) Cannizzaro reactio(ii) Decarboxylation
2. (a) Give chemical tests to distinguish between the following pairs of compounds:
(i) Ethanal and propanal
(ii) Phenol and Benzoic acid
3. Give chemical tests to distinguish between:
(i) Acetaldehyde and benzaldehyde
(ii) Propanone and propanol.
4. (a) How are the following obtained?
(i) Benzoic acid from ethyl benzene.
(ii) Benzaldehyde from toluene.
5. (a) Give chemical tests to distinguish between the following:
(i) Benzoic acid and ethyl benzoate
(ii) Benzaldehyde and acetophenone.
6. Give chemical tests to distinguish between Propanol and propanone
1. Give a chemical test to distinguish between the following pairs of compounds :
(i)
Propanal to propanone
(ii)
Benzaldehyde to bezoic acid.
2. Complete the following reaction and give the names of major products :
Dil. NaOH
(i)
CH3CHO
Conc. NaOH
(ii)
HCHO
∆
3. Although phenoxide ion has more number of resonating structure than carboxylate ion,
carboxylic acid is a stronger acid than phenol. Why ?
4. Explain :
(a) There are two -NH2 groups in semicarbazide. However only one such group is
involved in the formation of semicarbazones.
(b) Cyclohexanone forms cyanohydrins in good yield but 2,2,6-trimethyl-cyclohexanone
does not.
5. How will you account for the following :
(a) Chloroacetic acid is stronger acid than acetic acid
Ethers posseses a net dipole moment even if they are symmetrical in nature
1. Describe the following reactions:
(ii)
Etard’s reaction. (ii) Cross aldol condensation
2. How are the following obtained?
(i) Benzoic acid from ethyl benzene.
(ii) Benzaldehyde from toluene.
3.Complete the following reaction and give the names of major products :
(iii)
(iv)
Dil. NaOH
CH3CHO
Conc. NaOH
HCHO
∆
4.Give explanation for the followings
(i) Although phenoxide ion has more number of resonating structures than
carboxylate ion , carboxylic acid is a stronger acid than phenol.
(ii) There are two NH2 group in semicarbazide however only one is involved in
the formation of semi carbozones.
5.Write the structures of A and B in the following reactions
H2 , pd – BaSO4
NH2OH
(i)
C H3 COCl -------------------->
A --------------------> B
(i) CO2
PCl5
(ii)
C H3 MgBr --------------------> A --------------------> B
(ii) H3+O
6.Distinguish between
(i) C6 H5 COCH3 and C6 H5 CHO
(ii) C H3 COOH and HCOOH
01.
02.
03.
04.
Give explanation for the followings
(i) Although phenoxide ion has more number of resonating structures than carboxylate
ion , carboxylic acid is a stronger acid than phenol.
(ii) There are two NH2 group in semicarbazide however only one is involved in the
formation of semi carbozones.
Write the structures of A and B in the following reactions
H2 , pd – BaSO4
NH2OH
(i)
C H3 COCl -------------------->
A --------------------> B
(i) CO2
PCl5
(ii)
C H3 MgBr --------------------> A --------------------> B
(ii) H3+O
Distinguish between
(i) C6 H5 COCH3 and C6 H5 CHO
(ii) C H3 COOH and HCOOH
An organic compound X having molecular formula C4H8O gives orange red ppt with 2, 4
DNP reagent . It does not reduce Tollen’s reagent but gives yellow ppt of iodo form on
heating with NaOI , compound X on redulton with LiAlH4 gives compound Y , which
undergoes dehydration reaction on heating with conc H2 SO4 to form but-2-ene. Identify
the compound X and Y .
05.
06.
07.
Write chemical equation involved in the following reaction.
(i) Clemmenson reduction
(ii) Hell-Volhard-Zelinsky reaction
Convert the following
(i) Toulene to benzaldehyde
(ii) Ethanoyl chloride to ethanol
Convert the following
(i) P-notro benzoic acid has higher Ka value than benzoic acid.
(ii) Acetone is highly soluble in water, but benzophenone is not
3. Describe the following reactions:
(iii) Cannizaro reaction (ii) Cross aldol condensation
4. How are the following obtained?
(i) Benzoic acid from ethyl benzene. (ii) Benzaldehyde from toluene.
5. Give chemical tests to distinguish between compounds in the following pairs of
substances:
(i) Ethanal and Propanal
(ii) Benzoic acid and Ethyl benzoate
6. Give chemical tests to distinguish between the following:
(i) Benzoic acid and ethyl benzoate
(ii) Benzaldehyde and acetophenone.
1. Although phenoxide ion has more number of resonating structures than carboxylate ion,
carboxylic acid is a stronger acid than phenol. Give two reason.
2. Explain:
a. There are two ---NH2 groups in semicarbazide.However only one such group is involved in
the formation of semicarbazones.
b. Cyclohexanone forms cyanohydrins in good yield but 2,2,6-trimethyl-cyclohexanone does
not.
3. Draw the structures of:
a. 3-methylbutanal
b. P-nitropropiophenone
4. Convert:A) Acetic acid to methylamine
B) Acetaldehyde to methane
SECTION-C (3MARK)
1. How will you bring about the following conversions?
(i) Benzoic acid to benzaldehyde
(ii) Ethanal to but-2-enal
(iii) Propanone to propene
Give complete reaction in each case.
2. How would you account for the following:
(i) Aldehydes are more reactive than ketones towards nucelophiles.
(ii) The boiling points of aldehydes and ketones are lower than of the corresponding
acids.
(iii) The aldehydes and ketones undergo a number of addition reactions
3.
5.
6.
7. An organic compound with molecular formula C9H10O forms 2,4-DNP derivative, reduces
Tollen’s reagent and undergoes Cannizzaro’s reaction. On vigorous oxidation it gives
1,2-benzenedicarboxylic acid. Identify the compound.
8.Arrange the following compounds in increasing order of their property as indicated:
(i) Acetaldehyde, Acetone, Methyl tert-butyl ketone (reactivity towards HCN)
(ii) Benzoic acid, 3,4-Dinitrobenzoic acid, 4-Methoxybenzoic acid (acid strength)
(iii) CH3CH2CH(Br)COOH, CH3CH(Br)CH2COOH, (CH3)2CHCOOH (acid strength)
1. How will you convert :
(i)
Acetophenone to ethylbenzene
(ii)
Acetamide to m-nitrobenzoic acid
(iii) Benzoic acid to 3-bromobenzoic acid
2. Illustrate :
(i)
Cannizzaro’s reaction
(ii)
Clemmensen reduction
(iii) Etard’s reaction
3. An aliphatic compound ‘A’ with a molecular formula C3H6O reacts with
phenylhydrazine to give compound ‘B’ . Reaction of ‘A’ with I2 in alkaline medium on
warming, gives a yellow precipitate ‘C’. Identify the compounds A, B and C.
4. What happens when :
(i)
An aqueous solution of sodium acetate is electrolysed?
(ii)
Calcium acetate is dry distilled?
(iii) Sodium benzoate is heated with soda lime?
5. Identify A, B and C in the following sequence 0f reactions
COOH
+ NH3
COOH
heat
A
strong
B
heating
C
1. Name the reagents which are used in the following conversions:
(i) A primary alcohol to an aldehyde
(ii) Butan-2-one to butan-2-ol
(iii) Phenol to 2, 4, 6-tribromophenol
2. Explain the mechanism of the following reactions:
(i)
Addition of Grignard’s reagent to the carbonyl group of a compound
forming an adduct followed by hydrolysis.
ii)Identify A, B and C in the following sequence 0f reactions
COOH
heat
+ NH3
COOH
A
strong
B
C
heating
.
3. Give reasons for the following:
(i) Ethanal is more reactive than acetone towards nucleophilic addition reaction.
(ii) (CH3)3C—CHO does not undergo aldol condensation.
(iii)Carboxylic acids are higher boiling liquids than alcohols.
4. Give reason
(i) The α – hydrogen atom of aldehyde and ketone are acidic in nature
(ii) Oxidation of aldehyde is easier than ketone
(iii) CH2 == CH – COOH is more acidic than CH3CH2 COOH
05.
06.
07.
01.
02.
03.
Give reason
(i) Aldehydes are more reactive than ketone towards nucliphilic addition reaction
(ii) Benzoic acid does not give Friedal craft reaction
(iii) Benzaldehyde does not undergo aldol condensation reaction.
Arrange the following in the increasing order of
(i) Ethanol , Propane , ethanol , Methoxy methane (boiling point)
(ii) Formaldehyde , acetone , acetaldehyde (reactivity toward HCN)
(iii) Benzoic acid , 4-methoxy benzoic acid , 4- nitro benzoic acid (acid strength)
Give reason
(i) Chloro acetic acid is more acidic than acetic acid .
(ii) Carboxylic acids have higher boiling points than alcohol.
(iii) 4-nitro benzoic acid is more acidic than 4-methoxy benzoic acid.
An aldehyde A (C11H10O) which does not undergo self aldol condensation but gives
benzaldehyde and two moles of B on reductive Ozonolysis. The compound B on
oxidation with Silver ion gives oxalic acid . Identify compound A and B and write down
the reactions involved .
Carry out the following conversions in not more than two steps
(i) Phenylmagnesium bromide to benzoic acid
(ii) Acetaldehyde to but-2-enal
(iii) Benzene to m-nitro acetophenone
Draw the structures of the following derrivations
(i) 2,4- dinitrophenyl hydrozone of benzaldehyde
(ii) Acetaldehyde dimethyl acetal
04.
05.
06.
07.
08.
(iii) Cyclopropanone oxine
Give reason
(i) The α – hydrogen atom of aldehyde and ketone are acidic in nature
(ii) Oxidation of aldehyde is easier than ketone
(iii) CH2 == CH – COOH is more acidic than CH3CH2 COOH
Give reason
(i) Aldehydes are more reactive than ketone towards nucliphilic addition reaction
(ii) Benzoic acid does not give Friedal craft reaction
(iii) Benzaldehyde does not undergo aldol condensation reaction.
Arrange the following in the increasing order of
(i) Ethanol , Propane , ethanol , Methoxy methane (boiling point)
(ii) Formaldehyde , acetone , acetaldehyde (reactivity toward HCN)
(iii) Benzoic acid , 4-methoxy benzoic acid , 4- nitro benzoic acid (acid strength)
Give reason
(i) Chloro acetic acid is more acidic than acetic acid .
(ii) Carboxylic acids have higher boiling points than alcohol.
(iii) 4-nitro benzoic acid is more acidic than 4-methoxy benzoic acid.
Identify A, B, C in the following reaction
Dil.H2SO4
CH
CH
dil NaOH
A
heat
B
C
HgSO4
1. Name the reagents which are used in the following conversions:
(i) A primary alcohol to an aldehyde
(ii) Butan-2-one to butan-2-ol
(iii) Phenol to 2, 4, 6-tribromophenol
2. Explain the mechanism of the following reactions:
(i) Addition of Grignard’s reagent to the carbonyl group of a compound forming an
adduct followed by hydrolysis.
(ii) Acid catalysed dehydration of an alcohol forming an alkene.
(iii) Acid catalysed hydration of an alkene forming an alcohol.
3. Give reasons for the following:
(i) Ethanal is more reactive than acetone towards nucleophilic addition reaction.
(ii) (CH3)3C—CHO does not undergo aldol condensation.
(iii) Carboxylic acids are higher boiling liquids than alcohols.
1. A compound A (C2H6O) on oxidation by PCC gave B which on Treatment with aq. Alkali and
subsequent heating furnished C. B on oxidation by KMnO4 forms a monocarboxylic acid with
molar mass 60 gm per mol .deduce the structure of A,B,C.
2. Give reason:A) Chloroacetic acid has higher pKa value than acetic acid.
B) Electorphilic substitution in benzoic acid takes place at meta position.
C) Carboxylic acid have higher b.p than alcohols of comparable molecular mass.
3. How do you obtain?
But-2-en-al from ethanol
4.
A)
B)
5.
Butanoic acid from butanol
Benzoic acid from ethyl benzene
Illustrate
Cannizzaro’s reaction
Clemmensen reduction
How do you account for the following:
a. Aldehydes are more reactive than ketones towards nucleophiles.
b. The b.p of aldehydes and ketones are lower than that of corresponding acids.
c. The aldehyde and ketones undergo a number of addition reactions
VALUE BASED QUESTION (4 MARKS)
1. Formaldehyde (methanal) is a gas at room temperature. It is soluble in water because it
is polar. It has pungent smell.
(a)
What is formalin? Give its use.
(b) Which thermoplastics can be made from formalin?
(c)
Name a medicine prepared from formaldehyde. Give its use.
[5-Mark Quetions]
1. (a) How would you account for the following :
(i)
Aldehydes are more reactive than ketones towards nucleophiles.
(ii)
The boiling points of aldehydes and ketones are lower than that of the
corresponding acids.
(iii)
The aldehydes and ketones undergo a number of addition reactions.
(b)Give chemical tests to distinguish between :
(i)
Acetaldehyde and benzaldehyde
(ii)
Propanone and Propanol
2. (a) Identify A, B and C in the following sequence of reactions :
(i)C2H5MgCl
conc. H2SO4
HBr + Preoxide
CH3CHO
A
B
C
(ii)H2O
(b)Predict the structure of the products formed when benzaldehyde is treated with
(i) Conc. NaOH
(ii) HNO3 / H2SO4 (at 273-383 K)
(a) How would you account for the following:
(i) Aldehydes are more reactive than ketones towards nucelophiles.
(ii) The boiling points of aldehydes and ketones are lower than of the
corresponding acids.
(iii) The aldehydes and ketones undergo a number of addition reactions.
(b) Give chemical tests to distinguish between:
(i) Acetaldehyde and benzaldehyde
ii) Propanone and propanol.
1.
1. (a) How will you bring about the following conversions?
(i) Ethanol to acetone (ii) Benzene to acetophenone
(iii) Benzoic acid to benzaldehyde
(b) Describe the following giving a suitable example in each case:
(i) Decarboxylation (ii) Cannizaro’s reaction
2. (a) An organic compound contains 69.77% carbon, 11.63% hydrogen and the
rest is oxygen. The molecular mass of the compound is 86. It does not reduce
Tollens’ reagent but forms an addition compound with sodium hydrogen sulphite
and gives positive iodoform test. On vigorous oxidation it gives ethanoic and
propanoic acids. Deduce the possible structure of theorganic compound.
(b) State reasons for the following:
(i) Monochloroethanoic acid has a higher pKa value than dichloroethanoic acid.
(ii) Ethanoic acid is a weaker acid than benzoic acid.
3. (a)State tests to distinguish between the following pairs of compounds :
(i) Propanal and propanone
(ii) Phenol and benzoic acid
(b) How will you bring about the following conversions :
(i) Propanone to propene
(ii) Benzaldehyde to benzophenone
(iii) Ethanol to 3-hydroxybutanal
4. Arrange the following compounds in an increasing order of their indicated
property:
(i) Benzoic acid, 4-Nitrobenzoic acid, 3,4-Dinitrobenzoic acid, 4-Methoxybenzoic
acid (acid
strength)
(ii) CH3CH2CH(Br)COOH, CH3CH(Br) CH2COOH, (CH3)2CHCOOH,
CH3CH2CH2COOH
(acid
strength)
(b) How would you bring about the following conversions:
(i) Acetamide to m- nitro benzoic acid.(ii) Benzoic acid to Benzaldehyde (iii)
Bromobenzene to 1-phenylethanol
5. (a) Explain the mechanism of a nucleophilic attack on the carbonyl group of an
aldehyde or a ketone.
(b) An organic compound (A) (molecular formula C8H16O2 ) was hydrolysed with
dilute sulphuric acid to give a carboxylic acid (B) and an alcohol (C). Oxidation of
(C) with chromic acid also produced (B). On dehydration (C) gives but-1-ene.
Write the equations for thereactions involved.
6. (a) Give chemical tests to distinguish between the following pairs of compounds:
(i) Ethanal and propanal (ii) Formic acid and acetic acid.
(b) How will you bring about the following conversions?
(i) Aceto phenone to ethyl benzene.(ii) Ethanal to but-2-enal(iii) Propanone to
propene Give complete
reaction in each case.
7. (a)Illustrate the following name reactions giving a chemical equation in each
case:
(i) Clemmensen reaction (ii) Cannizzaro’s reaction
(b) Describe how the following conversions can be brought about:
(i) Cyclohexanol to cyclohexan-1-one (ii) Ethylbenzene to benzoic acid
(iii) Bromobenzene to benzoic acid
8. Illustrate the following name reactions:
(i) Hell–Volhard–Zelinsky reaction
(ii) Wolff–Kishner reduction reaction
(b) How are the following conversions carried out:
(i) Ethylcyanide to ethanoic acid (ii) Butan-1-ol to butanoic acid(iii)
Methylbenzene to benzoic acid
Write chemical equations for the involved reactions.
9. (a) How will you prepare the following compounds starting with benzene?
(i) Benzaldehyde
(ii) Acetophenone.
3. (b). Identifytify A, B and C in the following sequence of reactions :
(i)C2H5MgCl
conc. H2SO4
B
CH3CHO
HBr + Preoxide
A
C
(ii)H2O
(b)Predict the structure of the products formed when benzaldehyde is treated
with
(i) Conc. NaOH
(ii) HNO3 / H2SO4 (at 273-383k)
10. (a) Give a possible explanation for each one of the following:
(i) There are two —NH2 groups in semicarbazide. However, only one such group
is involved in the formation of semicarbazones.
(ii) Cyclohexanone forms cyanohydrin in good yield but 2, 4, 6trimethylcyclohexanone does not.
(b) An organic compound with molecular formula C9H10O forms 2, 4-DNP
derivative, reducesTollen’s reagent and undergoes Cannizzaro’s reaction. On
vigorous oxidation it gives1,2-benzene-di-carboxylic acid. Identify the compound
11. (a) Describe the mechanism of the addition of Grignard reagent to the carbonyl
group of acompound to form an adduct which on hydrolysis yields an alcohol.
(b) Draw the structures of the following compounds:
(i) 3-Methylbutanal
(ii) Hexane-1,6-dioic acid
(iii) p-Nitropropiophenone
12. (i) How will you convert phenol to benzoic acid ?
(ii)An organic compound A having molecular formula C6H6O gives a
characteristic colour with aqueous FeCl3 solution. A on treatment with CO2
and NaOH at 400 K under pressure gives B which on acidification gives a
compound C. The compound C reacts with acetyl chloride to gives D
which is a popular pain killer. Deduce the structure of A, B, C and D.
13.An organic compound (A) having molecular formula C9H10O forms an orange
red precipitate (B) with 2, 4-DNP reagent. Compound (A) gives a yellow
precipitate (C) when heated in the presence of iodine and NaOH along with a
colourless compound (D). A does not reduce oxidation of (A) with chromic acid, a
carboxylic acid (E) of molecular formula C7H6O2 is formed. Deduce the structures
of the organic compounds (A) to (E).
01.
Write the structures of A, B, C, D, E in the following reactions.
CH3COCl
C6 H6
Zn Hg/ Conc HCl
A
Anhy. AlCl3
(i) KMnO4–KOH
B
NaOI
C
(ii) ∆ H3O+
D+E
02.
An organic compound A has characteristic odour on treatement with NaOH, it forms two
compound B and C. Compound B has molecular formula C7H8O , which on oxidation gives back
A . The compound C sodium salt of an acid. When C is treated with sodalime it gives an
aromatic hydrocarbon D. Deduce the structures of A, B, C, D and write the sequence of
reactions involved
2.
(a) How would you account for the following:
(i) Aldehydes are more reactive than ketones towards nucelophiles.
(ii) The boiling points of aldehydes and ketones are lower than of the corresponding
acids.
(iii) The aldehydes and ketones undergo a number of addition reactions.
(b) Give chemical tests to distinguish between:
(i) Acetaldehyde and benzaldehyde
ii) Propanone and propanol.
12. (a) How will you bring about the following conversions?
(i) Ethanol to acetone (ii) Benzene to acetophenone
(iii) Benzoic acid to benzaldehyde
(b) Describe the following giving a suitable example in each case:
(i) Decarboxylation (ii) Cannizaro’s reaction
13. (a) An organic compound contains 69.77% carbon, 11.63% hydrogen and the rest is
oxygen. The molecular mass of the compound is 86. It does not reduce Tollens’ reagent
but forms an addition compound with sodium hydrogen sulphite and gives positive
iodoform test. On vigorous oxidation it gives ethanoic and propanoic acids. Deduce the
possible structure of theorganic compound.
(b) State reasons for the following:
(i) Monochloroethanoic acid has a higher pKa value than dichloroethanoic acid.
(ii) Ethanoic acid is a weaker acid than benzoic acid.
14. (a)State tests to distinguish between the following pairs of compounds :
(i) Propanal and propanone
(ii) Phenol and benzoic acid
(b) How will you bring about the following conversions :
(i) Propanone to propene
(ii) Benzaldehyde to benzophenone
(iii) Ethanol to 3-hydroxybutanal
15. Arrange the following compounds in an increasing order of their indicated property:
(i) Benzoic acid, 4-Nitrobenzoic acid, 3,4-Dinitrobenzoic acid, 4-Methoxybenzoic acid
(acid strength)
(ii) CH3CH2CH(Br)COOH, CH3CH(Br) CH2COOH, (CH3)2CHCOOH, CH3CH2CH2COOH (acid
strength)
(b) How would you bring about the following conversions:
(i) Propanone to Propene (ii) Benzoic acid to Benzaldehyde (iii) Bromobenzene to 1phenylethanol
16. (a) Explain the mechanism of a nucleophilic attack on the carbonyl group of an aldehyde
or a ketone.
(b) An organic compound (A) (molecular formula C8H16O2 ) was hydrolysed with dilute
sulphuric acid to give a carboxylic acid (B) and an alcohol (C). Oxidation of (C) with
chromic acid also produced (B). On dehydration (C) gives but-1-ene. Write the equations
for thereactions involved.
17. (a) Give chemical tests to distinguish between the following pairs of compounds:
(i) Ethanal and propanal
(ii) Phenol and Benzoic acid
(b) How will you bring about the following conversions?
(i) Benzoic acid to benzaldehyde(ii) Ethanal to but-2-enal(iii) Propanone to propene Give
complete
reaction in each case.
18. (a)Illustrate the following name reactions giving a chemical equation in each case:
(i) Clemmensen reaction
(ii) Cannizzaro’s reaction
(b) Describe how the following conversions can be brought about:
(i) Cyclohexanol to cyclohexan-1-one (ii) Ethylbenzene to benzoic acid
(iii) Bromobenzene to benzoic acid
19. Illustrate the following name reactions:
(i) Hell–Volhard–Zelinsky reaction
(ii) Wolff–Kishner reduction reaction
(b) How are the following conversions carried out:
(i) Ethylcyanide to ethanoic acid (ii) Butan-1-ol to butanoic acid(iii) Methylbenzene to
benzoic acid
Write chemical equations for the involved reactions.
20. (a) How will you prepare the following compounds starting with benzene?
(i) Benzaldehyde
(ii) Acetophenone.
(b) Give chemical tests to distinguish between the following pairs of compounds:
(i) Ethanal and Propanal (ii) Benzaldehyde and Acetophenone (iii) Phenol and Benzoic
acid.
21. (a) Explain the mechanism of nucleophilic attack on a carbonyl group of an aldehyde or
a ketone.
(b) How would you bring about the following conversions?
(i) Propanone to Propene (ii) Ethanol to 3-hydroxybutanal (iii) Benzaldehyde to
Benzophenone.
1. A organic compound with molecular formula C9H10O forms 2,4 DNP derivative reduces
Tollen’s reagent and undergoes cannizzaro reaction
On vigorous oxidation, it gives 1,2 benzene carboxylic acid. Identify the compound.
2. Identify A,B & C :CHCHO
஼ଶுହெ௚஼௟
ሱۛۛۛۛۛۛۛሮ ‫ܣ‬
ሱۛۛۛሮ
ுଶௌைସ
‫ܤ‬
ሱۛۛۛۛۛۛሮ
௉௘௥௢௫௜ௗ௘
‫ܥ‬
3. A ketone A (C4H8O) which undergoes a haloform reaction gives compound on reduction B on
heating with H2SO4 gives a compound C which forms mono-ozonide D. D on hydrolysis with
zinc dust gives only E. identify A,B,C,D AND E. Write the reaction involved
AMINES(CH-13)
1MARKS
1.Write IUPAC names of the following :
2. Write IUPAC names of the following :
3. What is Hoffman bromamide reaction?
4.Arrange the following in the increasing order of given property indicated.
(i)
C2H5NH2, (C2H5)2NH, (C2H5)3N and NH3, (Basic strength in aqueous solution).
5. Arrange the following in the increasing order of given property indicated.
Aniline, p-toluidine, p-nitroaniline. (Basic strength).
1.Why aniline is soluble in aqueous HCl.
.
2. Why do amines behave as nucleophiles?
3. Ethylamine is freely soluble in water whereas aniline is only slightly soluble.
4. Why is an alkylamine more basic than ammonia?
5. Arrange the following compounds in an increasing order of their basic strength in
aqueous solutions: NH3 , RNH2 , R2NH, R3N
6. Give the IUPAC name of H2N – CH2 – C H2 – CH = CH2.
7. Arrange the following compounds in an increasing order of their solubility in
water: C6H5NH2, (C2H5)2NH, C2H5NH2
8. Write the structure of n-methylethanamine.
9. Ethylamine is soluble in water whereas aniline is almost insoluble. Why?
10. Why are diazonium salts of aromatic amines more stable than those of aliphatic
amines?
11.Why is benzene diazonium chloride not stored and is used immediately after its
preparation ?
12.Rearrange the following compounds in an increasing order of their basic
strengths
C6H5NH2 , C6H5N(CH3)2 , (C6H5)2NH and CH3NH2 .
13.Arrange the following compounds in increasing order of solubility in water.
C6H5NH2 , (C6H5)2NH , C2H5NH2
14.Explain why CH3NH2 is stronger base than CH3OH ?
15.Arrange the following compounds in decreasing order of basic strength in gas
phase .
C2H5NH2 , (C2H5)2NH , (C2H5)3N , NH3
16.Aniline does not undergo Friedal craft reaction why ?
17. Convert aniline to O-bromoaniline.
1. Why is alkyl amine more basic than ammonia ?
2. Arrange the following compound in an increasing order of basic strengths in their
aqueous solutions :
NH3, CH3NH2, (CH3)2NH, (CH3)3N
3. Give a chemical test to distinguish between aniline and N-methylaniline.
4. State the reaction taking place when :
Bromine water is added to the aqueous solution of aniline.
5. How is aniline obtained from benzoic acid /
6. What is Hinsberg reagent ?
7. Why is benzene diazonium chloride not stored and used immediately after its
preparation ?
8. Write a chemical reaction in which the iodide ion replaces the diazonium group in a
diazonium salt.
9. Why do amines behave as nucleophiles?
10. Ethylamine is freely soluble in water whereas aniline is only slightly soluble.
11. Why is an alkylamine more basic than ammonia?
12. Arrange the following compounds in an increasing order of their basic strength in
aqueous solutions: NH3 , RNH2 , R2NH, R3N
13. Give the IUPAC name of H2N – CH2 – C H2 – CH = CH2.
14. Arrange the following compounds in an increasing order of their solubility in water:
C6H5NH2, (C2H5)2NH, C2H5NH2
15. Write the structure of n-methylethanamine.
16. Ethylamine is soluble in water whereas aniline is almost insoluble. Why?
17. Why are diazonium salts of aromatic amines more stable than those of aliphatic
amines?
1.Write the structure of N-methyl ethanamine.
2. Why electrophilic substitution takes place more readily in aromatic amines than benzene.
3. Illustrate ammonolysis reaction.
4. Arrange the following in increasing order of basic strength
Aniline, p-nitroaniline and p-toluidine.
6. Why do amines react as nucleophiles?
7. Give a chemical test to distinguish between primary and secondary amine.
8. Write a chemical reaction in which iodide ion displaces diazonium group from a diazonium
salt.
2marks
Convert a. nitrobenzene into phenol b. aniline to chlorobenzene
A. why aniline does not undergo Friedel Crafts reaction?
B. why primary amines cannot be prepared by Gabriel phthalimide reaction.
Illustrate:
a. Sandmeyers reaction
b. Coupling reaction
5. Assign reason for
a. Amines are less acidic than alcohols of comparable molecular masses
1. Aliphatic amines are stronger bases than aromatic amines.
1.
2.
3.
4.
Give the chemical tests to distinguish between the following pairs of compounds:
(i) Ethylamine and Aniline
(ii) Aniline and Benzylamine
2. Identify A and B in each of the following processes:
୒ୟେ୒
ୖୣୢ୳ୡ୲୧୭୬୒୧ /ୌమ
CH3CH2Cl ሱۛۛሮ Aሱۛۛۛۛۛۛۛۛۛۛۛሮ
୒ୟ୒୓మ/ౄిౢ
େ଺ୌହ୒ୌଶ/୓ୌష
(ii) C6H5NH2ሱۛۛۛۛۛۛሮAሱۛۛۛۛۛۛۛۛۛۛሮB
3. Give the chemical tests to distinguish between the following pairs of compounds:
(i) Methylamine and Dimethylamine
(ii) Aniline and N-methylaniline
4. Explain the following giving a reason in each case:
a. Why is an alkylamine more basic than ammonia?
b. Why do primary amines have higher boiling points than the tertiary
amines?
5. Complete the following reaction equations:
a. C6H5NH2 + CHCl3 + KOH (alc) →
b. C6H5N2 Cl + H3PO2 + H2O →
6.Write the chemical equations involved in the following reaction
(i)
Holfmann Bromamide degradation reaction
(ii)
Carbyl amine reaction
7.How will you convert
(i)
Benzoic acid to aniline
(ii)
Aniline to p - nitroaniline
8.Give the chemical equation for the following name reaction
(i) Gabriel pthalimide reaction
(ii) Diazotisation reaction
9.Give chemical test to distinguish between the following compounds
(i) Aniline and ethylamine
(ii) Methyl amine and Dimethyl amine
10.Convert the following
(i) Aniline to Benzyl alcohol
(ii) Methanamine to ethanamine
11.Account the following
(i) Although –NH2group is an o-p directly group nitration of aniline gives alongwith
ortho and para derivatives, metaderivatives also.
(ii) Why diazonium salts of aromatic amines are more stable than those of
aliphatic amines .
1. Identify A and B in each of the following processes :
NaCN
reduction
(i)
CH3CH2Cl
A
Ni/H2
NaNO2/HCl
(ii)
C6H5NH2
B
C6H5NH2
A
OH-
B
2. Give reasons :
(i)
Aniline does not undergo Friedal Craft reaction ?
(ii)
Why primary amines cannot be prepared by Gabriel phthalimide reaction.
3. Complete the following reactions :
(i)
C6H5NH2 + CHCl3 + KOH (alc)
(ii)
C6H5N2Cl + H3PO2 + H2O
4. Illustrate :
(i)
Sandmeyers reaction
(ii)
Coupling reaction
Explain the reaction of aniline with mixture of concentrated nitric and sulphuric acid
6. Give the chemical tests to distinguish between the following pairs of compounds:
(i) Ethylamine and Aniline
(ii) Aniline and Benzylamine
7. Identify A and B in each of the following processes:
୒ୟେ୒
ୖୣୢ୳ୡ୲୧୭୬୒୧ /ୌమ
CH3CH2Cl ሱۛۛሮ A ሱۛۛۛۛۛۛۛۛۛۛۛሮ
୒ୟ୒୓మ/ౄిౢ
େ଺ୌହ୒ୌଶ/୓ୌష
(ii) C6H5NH2 ሱۛۛۛۛۛۛሮ AሱۛۛۛۛۛۛۛۛۛۛሮB
8. Give the chemical tests to distinguish between the following pairs of compounds:
(i) Methylamine and Dimethylamine (ii) Aniline and N-methylaniline
9. Explain the following giving a reason in each case:
a. Why is an alkylamine more basic than ammonia?
b. Why do primary amines have higher boiling points than the tertiary amines?
10. Complete the following reaction equations:
a. C6H5NH2 + CHCl 3 + KOH (alc) →
b. C6H5N2 Cl + H3PO2 + H2O →
SHORT ANSWER-II(3MARKS)
1. Account for the following observations:
a. pKb for aniline is more than that for methylamine.
b. Methylamine solution in water reacts with ferric chloride solution to give a
precipitate of ferric hydroxide.
c. Aniline does not undergo Friedel-Crafts reaction.
2. Giving an example for each, describe the following reactions:
a. Hofmann’s bromamide reaction
b. A coupling reaction
c. Gabriel phthalimide synthesis.
3. Complete the following reaction equations:
(i)C6H5N2Cl + CH3COCl →
(ii) C2H5NH2 + C6H5SO2Cl →
(iv)
C2H5NH2 + HNO2→
11. How are the following conversions carried out:
(i)
Aniline to nitrobenzene
(ii)
Ethanamine to N-ethylethanamide
(iii)
Chloroethane to propan-1-amine
(iv)
12. In the following cases rearrange the compounds as directed:
a. In an increasing order of basic strength: C6H5NH2 , C6H5N(CH3 ) 2 , (C2H5 )
2 NHand CH3NH2
b. In a decreasing order of basic strength: Aniline, p-nitroaniline and ptoluidine
c. In an increasing order of pKb values: C2H5NH2 , C6H5NHCH3 , ( C2H5 )
2NHand C6H5NH2
8.How would you convert
(i) Aniline to para-bromo aniline. (ii) Aniline to iodobenzene iii) Write chemical
equations for the following conversions
9.Give structures of A, B and C in the following reactions
Fe / HCl
HNO2/ 273K
C6 H5OH
(i)
C6 H5 N O2 --------------------> A --------------------> B --------------------> C
CuCl
H2O / H+
NH3
(ii)
C6 H5 N2 Cl --------------------> A --------------------> B --------------------> C
∆
10.Give reason
(i) Primary amines have higher boiling point than tertiary amine.
(ii) (CH3)2 NH is more basic than (CH3)3N in an aqueous solution.
(iii) Why can’t aromatic primary amines be prepared by Gabriel – Pthalamide
synthesis.
11.An optically active compound (A), C5H11NO on acid hydrolysis gives an acid (B) and
NH3 . When A is treated with Br2 / KOH , a compound (C) is obtained which upon
treatment with HNO2 yields an optically active alcohol (D) and nitrogen gas. The
alcohol gives a positive idoform test. Identify A, B, C and D and write the reaction
involved.
12. How are the following conversion carried out ?
(i) Aniline the fluoro benzene
(ii) Benzene diazonium chloride to Benzene
(iii) Methyl chloride to ethylamine
1. What happens when (write reactions only)
(i)
Nitropropane is treated with LiAlH4.
(ii)
Ethyl isocyanide undergoes hydrolysis
(iii) Benzene diazonium chloride reacts with phenol in basic medium
2. Complete the following reactions :
(i)
C6H5N2Cl + CH3COCl
(ii)
C2H5NH2 + C6H5SO2Cl
(iii) C2H5NH2 + HNO2
3. Give one chemical test to distinguish between the following compounds in the following
pairs :
(i)
Methylamine and dimethylamine
(ii)
Aniline and benzylamine
(iii) Ethylamine and aniline
4. Write short notes on :
(i)
Carbylamine reaction
(ii)
Diazotisation
(iii) Hoffmann’s bromamide reaction
5. State reasons for the following :
(i)
Amines are less acidic than alcohols of comparable molecular masses .
(ii)
Primary amines has higher boiling point than tertiary amines .
(iii) Ethylamine is soluble in water, whereas aniline is not.
4. Account for the following observations:
a. pKb for aniline is more than that for methylamine.
b. Methylamine solution in water reacts with ferric chloride solution to give a
precipitate of ferric hydroxide.
c. Aniline does not undergo Friedel-Crafts reaction.
5. Giving an example for each, describe the following reactions:
a. Hofmann’s bromamide reaction
b. Gatterman reaction
c. A coupling reaction
6. Complete the following reaction equations:
(i)C6H5N2Cl + CH3COCl →
(ii) C2H5NH2 + C6H5SO2Cl →
(iii) C2H5NH2 + HNO2 →
13. How are the following conversions carried out:
(i)
Aniline to nitrobenzene
(ii)
Ethanamine to N-ethylethanamide
Chloroethane to propan-1-amine
(iii)
14. Give one chemical test each to distinguish between the compounds in the following
pairs:
a. Methylamine and dimethylamine
b. Aniline and benzylamine
c. Ethylamine and aniline
15. In the following cases rearrange the compounds as directed:
a. In an increasing order of basic strength: C6H5NH2 , C6H5N(CH3 ) 2 , (C2H5 ) 2 NHand
CH3NH2
b. In a decreasing order of basic strength: Aniline, p-nitroaniline and p-toluidine
c. In an increasing order of pKb values: C2H5NH2 , C6H5NHCH3 , ( C2H5 ) 2 NHand
C6H5NH2
(i)
Explain why an alkylamine is more basic than ammonia.
(ii)
How would you convert
16. (i) Aniline to nitrobenzene (ii) Aniline to iodobenzene?
17. State reasons for the following:
a. pKb value for aniline is more than that for methylamine.
b. Ethylamine is soluble in water whereas aniline is not soluble in water.
c. Primary amines have higher boiling points than tertiary amines
18. Illustrate the following reactions giving a chemical equation in each case:
a. Gabriel phthalimide synthesis
b. A coupling reaction
c. Hoffmann’s bromamide reaction
19. Write chemical equations for the following conversions:
a. Nitrobenzene to benzoic acid
b. Benzyl chloride to 2-phenylethanamine
c. Aniline to benzyl alcohol
State reasons for the following
1. pKB value for aniline is more than that for methylamine.
2. Ethylamine is soluble in water whereas aniline is not soluble in water.
3. Primary amines have higher boiling points than tertiary amines.
Q.2 Give one the chemical test each to distinguish between the compounds in the following pairs
1.Methylamine and dimethylamine.
2.Aniline and benzylamine
3.Ethylamine and aniline.
Q.3 Giving an example for each describe the following reactions
1. Hofmann’s bromamide reaction
2. Gattermann reaction.
3. Coupling reaction.
Q.4 How are the following conversions carried out?
1. Aniline to nitrobenzene.
2. Ethanamine to N-ethylethanamide.
3. Chloroethane to propan -1-amine.
Q5. Give complete reaction in each case.
1. Preparation of ethylamine from acetaldehyde.
2. Preparation of benzonitrile from aniline.
3. Preparation of ethyl isonitrile from ethylamine.
VALUE BASED QUESTION (4 MARKS)
1. Sumit and Amit were asked to make a chemistry project on organic synthesis. They
synthesize benzenediazonium chloride. Sumit asked to Amit to store it and said that
they will synthesize dyes from it next day, but Amit told him they can’t store it and if
they have to synthesize dye from it then it has to be used immediately. Now answer the
following questions:
(a)
Who is right Amit or Sumit? Explain why?
(b)
Which is more stable aryl or alkyl diazinium salt? Explain.
(c)
Write values associated with the suggestion of Amit.
2. Ethanamine to N-ethylethanamide.
3. Chloroethane to propan -1-amine.
Q5. Give complete reaction in each case.
1. Preparation of ethylamine from acetaldehyde.
2. Preparation of benzonitrile from aniline.
3. Preparation of ethyl isonitrile from ethylamine.
BIOMOLECULES(CH-14)
SECTION-A (ONE MARK)
1marks
1.Name polysaccharide which is stored in the liver of animals.
2. What structural feature is required for a carbohydrate to behave as reducing sugar?
3. How many asymmetric carbon atoms are present in D (+) glucose?
4. Name the enantiomer of D-glucose.
5. Give the significance of (+)-sign in the name D-(+)-glucose
2marks
1. What are anomers. Give the structures of two anomers of glucose.
2.Write the hydrolysed products of
(i) maltose (ii) cellulose.
3. What are vitamins? How are they classified?
4. (i) Why is sucrose called a reducing sugar?
(ii) Give the type of glycosidic linkage present in sucrose.
5. Classify the following as monosaccharides or oligosaccharides.
(i) Ribose (ii) Maltose
(iii) Galactose (iv) Lactose
1. What are anomers ? Give one example.
2. Write the constituents of sucrose.
3. Write the constituents of maltose.
4. Which of the two constituents of starch is water soluble ?
5. Name two components of α-glucose which constitute starch.
6. What are three types of RNA molecules which perform different functions.
7. Of the two bases named below, which one is present in RNA and which one is present in
DNA ? Thymine, Uracil
1.
2.
3.
4.
5.
6.
7.
What is meant by reducing sugar ?
What type of bonding occurs in β-pleated structure of protein ?
Name the protein present in milk. What type of protein is it ?
Why must vitamin c be supplied regularly in diet ?
Name two essential amino acids.
Under what conditions glucose is converted to gluconic and saccharic acid ?
Name the deficiency diseases resulting from lack of vitamin A and E in the diet.
8. What is glycosidic linkage ?
9. Why is cellulose not digested in human body ?
10. Where does the water present in the egg go after boiling the egg ?
1. What are disaccharides? Give an example.
2. What are reducing sugars? Give one example.
3. What are monosaccharides?
4. Name the deficiency diseases resulting from lack of vitamins A and E in the diet.
5. Write the full forms of DNA and RNA
6.How do you explain the presence of all the six carbon atoms in glucose in a straight
chain.
7.What is meant by ‘reducing sugars ’?
8.What are the products of hydrolysis of sucrose?
9.What happens when glucose is treated with bromine water?
10.What happens when glucose reacts with nitric acid?
11.Glucose on reaction with HI Gives n-hexane. What dose it suggest about the
structure of glucose?
12.What type of bonding occurs in bita-pleated structure of proteins ?
13.Deficiency of which vitamin causes rickets?
14 eficiency of which vitamins causes scurvy?
1.What are disaccharides? Give an example.
1. What are reducing sugars? Give one example.
2. What are monosaccharides?
3. What are the products of hydrolysis of sucrose?
4. What happens when glucose is treated with bromine water?
5. What happens when glucose reacts with nitric acid?
6. Name the bases present in RNA. Which one of these in not present in DNA?
7. What are three types of RNA molecules which perform different functions?
8. What type of bonding helps in stabilising the a-helix structure of proteins?
9. What is a glycosidic linkage?
10. Write the name of linkage joining two amino acids.
11. What is glycosidic linkage?
12. Why are carbohydrates generally optically active?
13. What is meant by biocatalysts?
14. B-complex is often prescribed vitamin. What is complex about it and write its
usefulness.
15. Name the location where protein synthesis occurs in our body.
2marks
1. Explain
a) Polypeptide.
b) Enzymes.
2. Write the main structural diffrence between DNA and RNA of the four bases, name those which
are common to both DNA and RNA.
3. What is meant by denaturation of proteins?
4. What are essential and non-essential amino acids? Give one example of each type.
5. Mention the type of linkages responsible for the formation of
a) Primary structure of protiens.
b) Cross linking of polypeptide chains.
1. Explain what is meant by the following :
(a) peptide linkage
(b) pyranose structure of glucose
2. What are essential and non-essential amino-acids ? Give two examples of each type.
3. Differentiate between globular and fibrous proteins.
4. Describe what you understand by primary and secondary structure of proteins
5. Answer the following :
(a) What type of linkage is responsible for the primary structure of proteins ?
(b) Name the location where protein synthesis occurs in our body ?
6. Name two fat soluble vitamins, their sources and the diseases caused due to their
deficiency in diet.
7. Name the four bases present in DNA. Which one of these is not present in RNA ?
8. Write the reactions involved when D-glucose is treated with following reagents :
(a) HCN
(b) Br2 water
9. What is essentially the difference between α–glucose and β–glucose ? What is meant by
pyranose structure of glucose ?
10. Write three such behavior of glucose which can not be explained by an open chain structure
of glucose molecule. What alternative structure has been proposed for the glucose molecule
?
11. Define enzymes. How do enzymes differ from ordinary chemical catalysts ?
12. Comment on the specificity of enzyme action. What is the most important reason for their
specificity
13. What is the difference between a nucleoside and a nucleotide
14. (a) Write the structure of the product obtained when glucose is oxidized with nitric acid.
1. Name the bases present in RNA. Which one of these is not present in DNA ?
2. Name two water soluble vitamins, their sources and the diseases caused due to their
deficiency in diet.
3. Answer the following :
(i)
What type of linkage is responsible for the primary structure of proteins ?
(ii)
Name the location where protein synthesis occurs in our body.
4. Give reasons for the following statements :
(i)
Amino acids are amphoteric in nature.
(ii)
Amino acids have comparatively higher melting points than the corresponding
haloacids.
5. What is meant by denaturation of proteins ?
1. Define the following terms in relation to proteins:
Peptide linkage (ii) Denaturation
2. List the reactions of glucose which cannot be explained by its open chain
structure.
3. Explain what is meant by (i) a peptide linkage (ii) a glycosidic linkage
4. Name two water soluble vitamins, their sources and the diseases caused due to
their deficiency in diet.
5. Name the four bases present in DNA. Which one of these is not present in RNA?
6. Name two fat soluble vitamins, their sources and the diseases caused due to
their deficiency in diet.
7. What are the following substances? (i) Invert sugar (ii) Polypeptides
8. State what the following are and how they differ from each other: (i) a nucleotide,
and (ii) a nucleoside
9. Name the products of hydrolysis of sucrose. Why is sucrose not a reducing
sugar?
10. What are essential and non-essential amino acids in human food? Give one
example of each type.
11. What is essentially the difference between a-form of glucose and b-form of
glucose? Explain.
12. Describe what you understand by primary structure and secondary structure of
proteins
13. Explain what is meant by the following:(i) peptide linkage(ii) pyranose structure of
glucose
14. Write the main structural difference between DNA and RNA. Of the four bases,
name those which are common to both DNA and RNA.
15. Write the reactions involved when D-glucose is treated with the following
reagents:(i) HI (ii) H2NOH
16. Give an example each of the following;
(i) Reducing sugar
(ii) Non-reducing sugar
17.Name the vitamins whose deficiency are responsible for (i)night blindness (ii) poor
coagulation of blood .
18.What is difference between amylase and amylopectin?
19.State what the following and how they differ from each other
(ii) a nucleotide, and
(ii) a nucleoside
20. Describe the following terms in reference to proteins:
(i) Primary structure
(ii) Denaturation
1. Define the following terms in relation to proteins:
Peptide linkage (ii) Denaturation
2. List the reactions of glucose which cannot be explained by its open chain structure.
3. Explain what is meant by (i) a peptide linkage (ii) a glycosidic linkage
4. Name two water soluble vitamins, their sources and the diseases caused due to their
deficiency in diet.
5. Name the four bases present in DNA. Which one of these is not present in RNA?
6. Name two fat soluble vitamins, their sources and the diseases caused due to their
deficiency in diet.
7. What are the following substances? (i) Invert sugar (ii) Polypeptides
8. State what the following are and how they differ from each other: (i) a nucleotide, and
(ii) a nucleoside
9. Name the products of hydrolysis of sucrose. Why is sucrose not a reducing sugar?
10. What are essential and non-essential amino acids in human food? Give one example
of each type.
11. What is essentially the difference between a-form of glucose and b-form of glucose?
Explain.
12. Describe what you understand by primary structure and secondary structure of
proteins
13. Explain what is meant by the following:(i) peptide linkage(ii) pyranose structure of
glucose
14. Write the main structural difference between DNA and RNA. Of the four bases, name
those which are common to both DNA and RNA.
15. Write the reactions involved when D-glucose is treated with the following reagents:(i)
HI (ii) H2NOH
SECTION-C (THREE MARKS)
1. Define the following terms :
(a) Glycosidic linkage
(b) Invert sugar
(c)
Oligosaccharides
2. What is glycogen ? How is different from starch ? How is starch structurally different from
cellulose ?
3. Define the following terms :
(a) Anomers
(b) Denaturation of proteins (c) Essential amino
acids
4. Define the following terms as related to proteins :
(a) Peptide linkage
(b) Primary structure
(c) Denaturation
5. Define the following terms :
(a) Polysaccharides
(b) Amino acids
(c) Enzymes
6. (a) Deficiency of which vitamin causes scurvy ?
(b) What type of linkage is responsible for the formation of proteins ?
(c) Write the product formed when glucose is treated with HI ?
7. (a) Deficiency of which vitamin causes rickets ?
(b) Give example for each of fibrous protein and globular protein
(c) Write the product formed on reaction of D-glucose with Br2 water.
8. Define the following terms :
(a) Invert sugar
(b) Vitamins
(c) Nucleoside
9. Define the following terms :
(a) Nucleotide
(b) Anomers
(c) Essential amino acids
10. (a) Deficiency of which vitamin causes night-blindness ?
(b) Name the base that found in nucleotide of RNA only.
(c) Glucose on reaction with HI gives n-hexane. What does it suggest about the structure of
glucose ?
1. Define the following giving one example of each :
(i)
Zwitter ion
(ii)
Glycosidic linkage
2. What happens when D-glucose is treated with the following reagents ?
(i)
HI
(ii)
Bromine water
(iii) HNO3
3. Name the major classes of carbohydrates and give an example of each of these classes.
4. Define the following terms :
(i)
Co-enzymes
(ii)
Mutation in biomolecules
(iii) Nucleotides
5. Answer the following questions :
(i)
How are proteins related to amino acids ?
(ii)
How are oligopeptides different from polypeptides ?
(iii)
When is a protein said to be denatured ?
1. What happens when D-glucose is treated with the following reagents?
(i) HNO3
(ii) Bromine water (iii) HI Indicate the products formed.
2. State clearly what are known as nucleosides and nucleotides.
3. Amino acids may be acidic, alkaline or neutral. How does this happen? What are
essential and non-essential amino acids? Name one of each type.
4. Differentiate between fibrous proteins and globular proteins. What is meant by
the denaturation of a protein
5. Mention three such facts/reactions about glucose which cannot be explained by
its open end structure. What is meant by pyranose structure of glucose?
6. What is glycogen? How is it different from starch? How is starch structurally
different from cellulose?
7. What happens when D-glucose is treated with the following reagents?
(ii) Bromine water
(iii) HI Indicate the products formed.
(i) HNO3
8. State clearly what are known as nucleosides and nucleotides.
9. Amino acids may be acidic, alkaline or neutral. How does this happen? What are
essential and non-essential amino acids? Name one of each type.
10. Differentiate between fibrous proteins and globular proteins. What is meant by the
denaturation of a protein
11. Mention three such facts/reactions about glucose which cannot be explained by its
open end structure. What is meant by pyranose structure of glucose?
12. What is glycogen? How is it different from starch? How is starch structurally different
from cellulose?
VALUE BASED QUESTION (4 MARKS)
1. After watching a programme on TV about the adverse effects of junk food and soft
drinks on the health of school children, Sonali, a student of Class XII, discussed the issue
with the school principal. Principal immediately instructed the canteen contractor to
replace the fast food with the fibre and vitamins rich food like sprouts, salad, fruits, etc.
This decision was welcomed by the parents and the students.
After reading the above passage, answer the following questions:
(a) What values are expressed by Sonali and the Principal of the school?
(b) Give two examples of water-soluble vitamins
2. Shanti, a domestic helper of Mrs. Anuradha, fainted while mopping the floor. Mrs.
Anuradha immediately took her to the nearby hospital where she was diagnosed to be
severely ‘anaemic’. The doctor prescribed an iron rich diet and multivitamins
supplement to her. Mrs. Anuradha supported her financially to get the medicines. After
a month, Shanti was diagnosed to be normal.
After reading the above passage, answer the following questions:
(i) What values are displayed by Mrs. Anuradha?
(ii) Name the vitamin whose deficiency causes ‘pernicious anaemia’.
(iii) Give an example of a water soluble vitamin.
3. After watching a programme on TV about the adverse effects of junk food and
soft drinks on the health of school children, Sonali, a student of Class XII,
discussed the issue with the school principal. Principal immediately instructed the
canteen contractor to replace the fast food with the fibre and vitamins rich food
like sprouts, salad, fruits, etc. This decision was welcomed by the parents and
the students.
After reading the above passage, answer the following questions:
(a) What values are expressed by Sonali and the Principal of the school?
(b) Give two examples of water-soluble vitamins
2. Glucose occurs freely in nature as well as in combined from. It is present in sweet
fruits and honey. Ripe Grapes also sontain glucose in large amount. Glucon-D is instant
source of energy. Starch gets hydrolysed into glucose I out body Glucose is stored in
the form of glycogen.
(i)What is meant by D in Glucon-D ?
(ii) What will happen if we have high amount of glocuse in our blood?
(iii) How will you test glucose in urine of diabetic patients?
(iv) How often people suffering from type I diabetes, should perform test for
diabetes? How will it help?
3.Shanti, a domestic helper of Mrs. Anuradha, fainted while mopping the floor. Mrs.
Anuradha immediately took her to the nearby hospital where she was diagnosed to be
severely ‘anaemic’. The doctor prescribed an iron rich diet and multivitamins
supplement to her. Mrs. Anuradha supported her financially to get the medicines. After a
month, Shanti was diagnosed to be normal.
After reading the above passage, answer the following questions:
(i) What values are displayed by Mrs. Anuradha?
(ii) Name the vitamin whose deficiency causes ‘pernicious anaemia’.
(iii)Give an example of a water soluble vitamin.
4.Amino acids contain amino(-NH2)group and carboxyl(-COOH) group. These are
monomes of proteins. Proteins occur in every part of body and from the fundamental
basis of structure and functions of life. They are also required for growth and
maintenance of body.
(i) what are essential amino acids? Why should these be part of our died?
(ii) What are the chieg sources of proteins? Why should children take proteins?
(iii) Name a disease caused by deficiency of amino acids. What is its causes?
(iv) What balues are possessed by children taking milk, fruits, pulses regularly?
POLYMERS(CH-15)
1mark
1.
2.
3.
4.
Write the monomers used for the preparation of Nylon – 66.
Name the monomer unit of polymer Dacron
1. Give an example of elastomers.
2. Is (CH2-CH)n a homopolymer or a copolymer?
5. Which of the following is a natural polymer?
Buna-S, Proteins, PVC
6. 4. Write the names of monomer of the following polymer:
[C
(CH2)5
N] n
O
H
7. 5. Give one example of condensation polymer.
8. 6. Is (CH2
CH) n a homopolymer or a copolymer?
Cl
1.
2.
3.
4.
5.
Define the term ‘homopolymerisation’ giving an example.
Give an example of elastomers.
What does the part 6, 6 mean in the name nylon-6, 6 ?
What is the difference between Buna-N and Buna-S.
What are biodegradable polymers ?
1.
2.
3.
4.
Define the term ‘polymerisation’.
Give an example of elastomers.
What does the part ‘6, 6’ mean in the name nylon-6,6?
What is the primary structural feature necessary for a molecule to make it
useful in a condensation polymerisation reaction
5. Write the name and structure of the monomer of each of the following
polymers:
(i) Neoprene
ii) Buna-S
(iii) Teflon
6. What is meant by ‘copolymerisation’?
7. What are biodegradable polymers?
8. Define the term ‘homopolymerisation’ giving an example.
1.Distinguish between homopolymers andf copolymers
2. What are biodegradable polymers?
3. Write the name of monomers of neoprene.
4. Write the monomers of Buna-N.
5. Write the structure and one use of each of the polymers:a) PVC b) Urea-formaldehyde resin
c) Bakelite
1. Give example of a natural polyamide which is an important constituent of diet.
2. Classify polythene and bakelite as thermosetting plastics or thermoplastics.
3. Among fibres, elstomers and thermosetting polymers, which one has strongest
4.
5.
6.
7.
8.
9.
10.
11.
intermolecular forces of attraction?
Define the term ‘polymerisation’.
Give an example of elastomers.
What does the part ‘6, 6’ mean in the name nylon-6,6?
What is the primary structural feature necessary for a molecule to make it useful in a
condensation polymerisation reaction
Write the name and structure of the monomer of each of the following polymers:
(i) Neoprene (ii) Buna-S
(iii) Teflon
What is meant by ‘copolymerisation’?
What are biodegradable polymers?
Define the term ‘homopolymerisation’ giving an example.
2marks
1. Write the monomers used for the preparation of Nylon – 66.
2.When phenol is treated with formaldehyde,an industrially important polymer is
formed. Name the polymer and mention its uses
3.How will you prepare Nylon-6,6 [
4. Classify the following in to homopolymer or Co – polymer. Nylon – 6, HDPE
5. What is Vulcanisation? How does it modify the properties of rubber?
1. What is a biodegradable polymer? Give an example of biodegradable aliphatic polyester.
2. How does vulcanisation change the character of natural rubber?
b) Why are the numbers 6, 6 and 6 put in the names of nylon-6, 6 and nylon 6?
3. Define thermoplastic and thermosetting polymers with example.
4. Write the structure of repeating monomeric unit of
a) Dacron b) Neoprene c) PVC d) Teflon.
5. Distinguish between homopolymers and copolymers with examples.
1. How can you differentiate between addition and condensation polymers?
2. Write the structures of the monomers of the following polymers:
[a]PVC
[b]Polypropene
3. Discuss the main purpose of vulcanization of rubber.
4. [a] how does vulcanisation change the properties of natural rubber?
[b]Why the nos. 6,6 and 6 put in the names of nylon 6,6 and nylon6?
5. Differentiate between molecular structures and behaviors of thermoplastic and thermosetting
polymers. Give
one example of each type.
6. What is the repeating unit in the condensation polymer obtained by combining
HO2CCH2CH2CO2H(succinic acid)and H2NCH2CH2NH2(ethylene diamine)?
7. Write the names and structures of the monomers of the following polymers:
[a]Bakelite
[b] Polythene
8. Draw the structure of the monomer for each of the following polymers:
[a]Nylon-6
[b]Polypropene
1. Draw the molecular structure of the monomers of
(i)
PVC
(ii)
Teflon
2. What is the repeating unit in the condensation polymer obtained by combining
HO2CCH2CH2CO2H (succinic acid) and H2NCH2CH2NH2 (ethylenediamine ?
3. (a) How does vulcanisation change the character of natural rubber ?
(b)What is the role of benzoyl peroxide in addition polymerisation of alkenes ?
4. How is Dacron obtained from ethylene glycol and terephthalic acid ?
5. What is a biodegradable polymer ? Give an example of a biodegradable aliphatic
polyster.
1. Draw the structures of the monomers of the following polymers: (i) Teflon (ii)
Polythene
2. What is the repeating unit in the condensation polymer obtained by combining
HO2CCH2CH2CO2H(succinic acid) and H2NCH2CH2NH2 (ethylene diamine).
3. Differentiate between molecular structures and behaviours of thermoplastic and
thermosetting polymers. Give one example of each type.
4. Differentiate between condensation and addition polymerisations. Give one
example each of the resulting polymers.
5. State reasons for the following occurrences:
(i) Soaps do not do the cleansing in hard water.
(ii) Synthetic detergents are preferred to soaps in washing machines.
6. Mention two important uses of each of the following :(i) Bakelite(ii) Nylon-6
7. Which polymer is obtained when free radical polymerisation of chloroprene
occurs? Write the structure of the polymer thus obtained.
8. What is a biodegradable polymer? Give an example of a biodegradable aliphatic
polyester.
9. Arrange the following polymers in increasing order of their intermolecular forces:
(a) Nylon-6,6, Buna-S, Polythene
(b) PVC, Nylon-6, Neoprene
10.Explain the term copolymeristation and give two examples.
11. Draw the molecular structures of the monomers of
(i) PVC
(i) Teflon
12. Draw the structures of the monomers of the following polymers:
(i) Bakelite
(ii) Nylon-6
13. Differentiate between condensation and addition polymeristations. Give one
example each of the resulting polymers.
14. Distinguish between homopolymers and copolymers and give an example of each
class.
15. What are biodegradable polymers? Give two examples
. Write the structure of following polymers and also give their main uses :
(a) Polystyrene (ii) Melamine - formaldehyde resin.
2. Draw the structures of the monomers of the following polymers: (i) Teflon (ii) Polythene
3. What is the repeating unit in the condensation polymer obtained by combining
HO2CCH2CH2CO2H(succinic acid) and H2NCH2CH2NH2 (ethylene diamine).
4. Differentiate between molecular structures and behaviours of thermoplastic and
thermosetting polymers. Give one example of each type.
5. Differentiate between condensation and addition polymerisations. Give one example
each of the resulting polymers.
6. State reasons for the following occurrences:
(i) Soaps do not do the cleansing in hard water.
(ii) Synthetic detergents are preferred to soaps in washing machines.
7. Draw the molecular structures of the monomers of (i) PVC (ii) Teflon
8. Draw the structures of the monomers of the following polymers: (i) Bakelite (ii) Nylon
9. Mention two important uses of each of the following
:(i) Bakelite(ii) Nylon-6
10. Which polymer is obtained when free radical polymerisation of chloroprene occurs?
Write the structure of the polymer thus obtained.
11. What is a biodegradable polymer? Give an example of a biodegradable aliphatic
polyester.
12. Arrange the following polymers in increasing order of their intermolecular forces:
(a) Nylon-6,6, Buna-S, Polythene
(b) PVC, Nylon-6, Neoprene
SECTION-C (THREE MARKS)
1.Write the names and structures of monomers of the following polymers:
[a]Buna-S
[b] Neoprene
[c]Nylon-6,6.
2. Explain the following terms giving a suitable example of each:
[a] Elastomer
[b] Condensation polymers [c]Addition polymers
3. Give one example each of:
[a] Addition polymers
[b] Copolymers
[c]Condensation polymers
1. Explain the following terms giving a suitable example for each ;
(i)
Elastomers
(ii)
Condensation polymers
(iii) Addition polymers
2. What are addition polymers ? How are the two types of addition polymers differ from
each other ? Give example of each type.
3. Write the chemical equation for the synthesis of
(i)
Terylene
(ii)
Neoprene
(iii) Teflon
4. Identify The four groups into which the polymers are classified on the basis of magnitude
of intermolecular forces present in them ? To which group or groups do polythene and
Bakelite belong ?
5. Write the monomers of Nylon-6, Dacron and PHBV. Give their uses also.
1. Write the names and structure of the monomers of the following polymers:
i)Dacron (ii)Buna-s (iii)Orlon
2. Draw the structures of the monomers of the following materials: (i) PVC (ii)
Teflon (iii) Neoprene iii) Buna-S
2. Give one example each of (i) addition polymers, (ii) condensation polymers, (iii)
copolymers
3. Identify the four groups into which the polymers are classified on the basis of the
magnitude of intermolecular forces present in them. To which group or groups do
polythene and bakelite belong?
4. What are addition polymers? How are the two types of addition polymers
different from each other?Give one example of each type.
5. Explain the following terms giving a suitable example for each:
a. Elastomers (ii) Condensation polymersv(iii) Addition polymers
6. Write the monomer of Nylon-6.and PHBV. Give their uses.
7. 38. Explain the following terms giving a suitable example for each:
(i) Elastomers
(ii) Condenstation polymers
(iii) Addition polymers
8. Write the name and structure of the monomers of the following polymers:
(i) Buna-S
(ii) Dacron
(iii) Neoprene
9. Mention two important use of each of the following polymers:
(i) Bakelite
(ii) Nylon 6,6
(iii) PVC
10. Write chemical equation for the synthesis of
(i) terylene
(ii) neoprene
(iii) Teflon
11. Giving one Example each of
(i) addition polymers,
(ii) condensation polymers,
(iii) copolymers.
12. Write the (i) structure and (ii) one use of each of the following polymers:
(a) PVC
(b) Urea-formaldehyde resin
(c) Bakelite
VALUE BASED QUESTION (4 MARKS)
1. Government had banned use of polythene bags in Delhi. Shopkeepers hae started
using bags mede up of biodegradable paper which are ecofriendly. Some small
shopkeepers are still using polythene bags but these are thinner and colourless.
(i) Why should we ban polythene? What values are possessed by people, not
using polythene and use biodegradable materials for bags?
(ii) Why are polythene bags made thinner and colourless? How can we manage
them?
(iii) What is/are monomer(s) of polythene? Is it homo-or co-polymer?
2. Cotton has become most popular these days. Synthetic fibers like terylene, terecot
and nylon have been outdated, Natural fibres are better than synthetic fibres.
(i) Why are cotton fibers preferred over synthetic fibers? Which polymer is used
cotton?
(ii) Why should synthetic fibres not used in kitchen?
(iii) What are semi-synthetic polymers? Give its use and example.
(iv) What are the uses of polymers in consumer products? What are the values
possessed by people using bio-degradable plastics?
3.After the ban on plastic bags, students of one school decided to make the people
aware of the harmful effects of plastic bags on environment and Yamuna River. They
organized rally by joininghands with other schools and distributed paper bags to
vegetable vendors, shopkeepers and departmentas stores. All students pledged not to
use polythene bags in future to save Yamuna River.
(i) What values are shown by the student?
(ii) What are biodegradable polymers? Give one example.
(iii) Is Polythene a condensation or an addition polymer?
13. Write the names and structure of the monomers of the following polymers:
14. Buna-S (ii) Neoprene (iii) Nylon-6
15. Write the structures of the monomers of the following polymers : (i) PVC (ii)
Polypropene
16. Draw the structures of the monomers of the following materials: (i) PVC (ii) Teflon (iii)
Neoprene
17. Give one example each of (i) addition polymers, (ii) condensation polymers, (iii)
copolymers
18. Identify the four groups into which the polymers are classified on the basis of the
magnitude of intermolecular forces present in them. To which group or groups do
polythene and bakelite belong?
19. Write the structure of the monomer of each of the following polymers:
(i) Polyvinyl chloride (ii) Teflon
(iii) Bakelite.
20. Write the names and structures of the monomers of the following polymers:
(i) Buna-S(ii) Dacron(iii) Neoprene
21. What are addition polymers? How are the two types of addition polymers different from
each other?Give one example of each type.
22. Explain the following terms giving a suitable example for each:
a. Elastomers (ii) Condensation polymersv(iii) Addition polymers
1. Write chemical equation for the synthesis of
a) Neoprene b) Glyptal c) PTFE
2. What is the primary structure feature necessary for a molecule to make it useful in a
condensation polymerisation reaction?
3. Identify the four groups into which the polymers are classified on the basis of the magnitude of
intermolecular forces present in them? To which group or groups do polythene and bakelite belong?
1
2
3
CHEMISTRY IN EVERYDAY LIFE-(CH-16)
1 MARK QUESTIONS
A detergent is a soap without soap. Justify
Allosteric sites of enzymes play animportant role in drug-enzyme inhibition.
Illustrate.
Same substances can act as antiseptic as well as disinfectant by varying the
concentration. Suggest example.
What are antifertility drugs? Give one example.
Differentiate between antiseptic and disinfectant
4
5
1. Name a substance which can be used as an antiseptic as well as
disinfectant.
2. What is tincture of iodine?
3. What is meant by narrow spectrum antibiotics?
4. Write the name of an antacid which is often used as a medicine.
5. Name the sweetening agent used in the preparation of sweets for
diabetic patients.
6. Which one of the following drugs is an antibiotic?
Morphine, Equanil, Chloramphenicol, Aspirin
7. Define antihistamine with an example.
8. What is meant by the term’ broad spectrum antibiotics’? Explain.
1.
2.
3.
4.
5.
6.
7.
Write the name of an antacid which is often used as medicine.
What type of drug phenacetin is ?
Name two narcotics which are used as analgesics ?
Why is ethanol added to soap ?
Why should not medicines be taken without consulting doctors ?
What are main constituents of dettol ?
Name the sweetening agent used in the preparation of sweet for a
diabetic patient.
8. Which class of drugs is used in sleeping pills ?
9. What is a soft soap ?
10.
What is meant by ‘narrow spectrum antibiotics’ ?
1.
2.
3.
Name a substance that can be used as an antiseptic as well as a
disinfectant
What is understood by ‘chemotherapy’?
What is tincture of iodine?
Write the name of an antacid which is often used as a medicine.
5. What is meant by the ‘broad spectrum antibiotics’?
6. What is meant by ‘narrow spectrum antibiotics’?
7. What is meant by a ‘broad spectrum antibiotic’?
8. What are main constituents of dettol?
9. Write the name of an antacid which is often used as medicine.
10. Define tranquilizers
11. Why is ethanol added to soap?
12. What are antiseptics?
13. What are drug targets?
14. Name drug which prevents histamines interaction with the
receptors of stomach wall?
15. What is the function of antidepressant drugs?
16. What is allosteric sites?
17. Which forces are involved in holding the drugs to the drugs to the
active site of enzymes?
1. Define the term chemotherapy?
2. Why do we require artificial sweetening agents?
3. What are main constituent of Dettol?
4. What type drug phenaticinis?
5. Name the drugs that are used to control allergy?
6. Why is the use of aspartame limited to cold food and drinks?
7. What are tranquilizers? Give an example?
8. What type of drug chloramphenicol?
9. Why is biothional is added to the toilet soap?
10.
What are food preservatives?
1. Name the main constituent of dettol.
2. What is tincture of iodine?
3. Define and give example of tranquilizer.
4. Why is the use of sweetner aspartame limited to cold foods and
drinks?
5. What is mean by 'narrow spectrum antibiotics’?
4.
SECTION-B (TWO MARKS)
1. What are food preservatives? Name 2 such substances.
2. What are the following substances? Give 1 example of each
[a] Tranquilizers
[b] Synthetic detergents.
3. Explain the cleansing action of soaps. Why do soaps do not work in
hard water?
4. Explain the following types of substances with one suitable example
for each case:
[a]Cationic detergents
[b] Analgesics
5. What are biodegradable and non biodegradable detergents? Give one
example of each.
6. How do antiseptics differ from disinfectants? Give one example of
each.
1. State the reason in each of the following cases :
(i) Soap do not work well in hard water.
(ii) Synthetic detergent are better than soaps.
2. Explain the following terms with an example for each :
(i) Antifertility drugs
(ii) Antibiotics
3. Name a broad spectrum antibiotics and state two disease for which
it is prescribed.
4. Why is paracetamol preferred over aspirin ?
5. Explain the cleansing action of soap.
1. What are biodegradable and non-biodegradable detergents? Give
one example of each class.
2. Why do soaps not function in hard water, for washing clothes?
How are synthetic detergents better than soaps for this purpose?
3. What are artificial sweetening agents? Give two examples.
4. Explain the cleaning action of soap. Why do soaps not work in
hard water?
5. What is meant by ‘narrow spectrum antibiotics’? give one
example.
6. State the reason in each of the following cases:
(i) Soaps do not work well in hard water.
(ii) Synthetic detergents are better than soaps.
7.Explain the following terms giving an example of each:
(i) Antacids
(ii) Sweetening agents
8. Explain the following terms with an example for each:
(i) Antifertility drugs
(ii) Antibiotics
9.Mention one important use of each of the following:
(i) Equanil
(ii) Sucralose
1.
2.
3.
4.
5.
Why do soaps not work in hard water?
Give the differences between cationic and anionic detergents.
Why do we require artificial sweetening agents?
What are antiseptics? Give an example.
What is broad spectrum antibiotics?
1. Mention one important use of the following-(i) Equanil
(ii)Sucrolose
2. Define the following and give one example- (i)Antipyretics (ii)
Antibiotics
3. Name the medicines used for the treatment of the following- (i)
Tuberculosis (ii) Typhoid
4. What are tincture of iodine?
5. What is artificial sweetening agent? Give two examples?
6. How are synthetic detergents better than soaps?
7. What are sulpha drugs? Give two examples?
8. What forces are involved in holding the active sites of the
enzymes?
9. Describe the following giving an example in each case- (i) Edible
colours (ii) Antifertility drugs
10.
Give two examples of organic compounds used as
antiseptics?
11.
What are biodegradable and non-biodegradable detergents?
Give one example of each class.
12.
Why do soaps not function in hard water, for washing
clothes? How are synthetic detergents better than soaps for this
purpose?
13.
What are artificial sweetening agents? Give two examples.
14.
Explain the cleaning action of soap. Why do soaps not work
in hard water?
1. Explain Antacids, sweetening agents.
2. Define Broad spectrum antibiotic.
3. How drugs prevent the attachment of natural substrate on active
site of an enzyme.
4. Mention one important use of
a) Equanil b) Sucralose.
5. What are anionic detergents?
How are they prepared?
Write their two main uses.
SECTION-C (THREE MARKS)
1. Answer the following questions:
[a]Why is use of aspartame limited to cold food and drinks?
[b]Soaps do not work in hard water.
[c]Why is bithional added to soap?
2. Describe the following giving 1 example of each:
[a]Detergents
[b] Food preservatives
[c] Antacids
3. Explain the following terms with 1 suitable example of each.
[a] A sweetening agent for diabetic patients. [b] Enzymes
[c]Analgesics
4. Explain the following terms giving 1example of each type.
[a]Antacids
[b] Disinfectants
[c] Enzymes
]
1. (a) Differentiate between disinfectant and an antiseptic. Give one
example of each.
(b)What is tincture of iodine and what is it used for?
2. What are anionic detergents? How are they prepared? Write
their two main uses.
3.
Explain the following types of substances with one suitable
example, for each case:
(i) Cationic detergents
(ii) Food preservatives
(iii) Analgesics
4. What are biodegradable and non-biodegradable detergents ? Give
one example of each.
5. Mention the action of following on human body
(i) Bromopheniranine
(ii) Aspirin
Equanil
SHORT ANSWER-II(3MARKS)
1. What are the following substances? Give one example of each
type. (i) Antacid (ii) Nonionic detergents (iii) Antiseptics
2. What are the following substances? Give one example of each of
them.
(i) Cationic detergents
(ii) Antioxidant (iii) Sweetening
agents
3. What are analgesic medicines? How are they classified and when
are they commonly recommended for use?
4. Explain the following terms with an example for each:
(i) Antibiotics (ii) Antiseptics (iii) Analgesics
5. How do antiseptics differ from disinfectants? Name a substance
that can be used as an antiseptic as well as a disinfectant
6. Describe the following giving one example for each:
(i) Detergents (ii) Food preservatives (iii) Antacids
7. Explain the following terms with one suitable example for each:
(i) A sweetening agent for diabetic patients. (ii) Enzymes (iii)
Analgesics
8. Answer the following questions :
(i) Why do soaps not work in hard water ?
(ii) What are the main constituents of dettol?
(iii) How do antiseptics differ from disinfectants
9. (a) Which one of the following is a food preservative?
Equanil, Morphine, Sodium benzoate
(b) Why is bithional added to soap?
(c) Which class of drugs is used in sleeping pills?
10.
(i) What class of drug is Ranitidine?
(ii) If water contains dissolved Ca2+ ions, out of soaps and
synthetic detergents, which will you use be for cleaning clothes?
(v) Which of the following is an antiseptic? 0.2% phenol, 1%
phenol
11. Mention the action of following on human body
(iii) Bromopheniranine
(iv) Aspirin
(v) Equanil
1.
What is the difference between narcotics and non-narcotics
analgesics?
2.
Explain the cleansing action of soaps.
3.
Account for the following:(a). Some builders are added to soap.
(b). Soaps are biodegradable whereas detergents are nonbiodegradable.
(c). Ethanol is added to soaps.
4.
5.
Give an example of :(a). antipyretics (b). Anti fertility drug (c). analgesics
What are fillers? What role do they play in soap?
1. What are barbiturates? To which class of drugs do they belong?
Give two examples.
2. What is the use of –
(i) Benadryl (ii) sodium benzoate (iii) Progesterone
3. Identify the type of drug(i) Ofloxacin (ii) Aspirin (iii) Cimetidine
4. Describe the following with suitable example(i) Disinfectant (ii) Analgesics
(ii) Broad spectrum antibiotics
5. Explain the following types of substance with one suitable
example, for each case:
(i) Cationic detergents (ii) Food preservatives (iii) Analgesics
6. How do antisepitcs differ from disinfectants? Give one example of
each type.
7. What are the following substances? Give one example of each
type. (i) Antacid (ii) Nonionic detergents (iii) Antiseptics
8. What are the following substances? Give one example of each of
them.
(i) Cationic detergents
(ii) Antioxidant (iii) Sweetening
agents
9. What are analgesic medicines? How are they classified and when
are they commonly recommended for use?
10.
Explain the following terms with an example for each:
(i) Antibiotics (ii) Antiseptics (iii) Analgesics
11.
How do antiseptics differ from disinfectants? Name a
substance that can be used as an antiseptic as well as a disinfectant
12.
Describe the following giving one example for each:
(i) Detergents (ii) Food preservatives (iii) Antacids
13.
Explain the following terms with one suitable example for
each:
(i) A sweetening agent for diabetic patients. (ii) Enzymes (iii)
Analgesics
14.
Answer the following questions :
(i) Why do soaps not work in hard water ?
(ii) What are the main constituents of dettol?
(iii) How do antiseptics differ from disinfectants
15.
(a) Which one of the following is a food preservative?
Equanil, Morphine, Sodium benzoate
(b) Why is bithional added to soap?
(c) Which class of drugs is used in sleeping pills?
16.
(i) What class of drug is Ranitidine?
(ii) If water contains dissolved Ca2+ ions, out of soaps and
synthetic detergents, which will you use be for cleaning clothes?
(iii) Which of the following is an antiseptic? 0.2% phenol, 1%
phenol
I
Explain with example
1. A sweetening agent for diabetic patients
2. Enzymes
3. Analgesics
II Explain
1. Food preservatives
2. Broad spectrum antibiotics
3. Ant fertility drugs
III Mention the action of following on Human Body
1. Bromopheniramine
2. Aspirin
3. Equanil
Value Based Questions [4 Marks]
Ishita a class XII student, read the composition of the detergent
which their housemaid was using for washing clothes. She found
that besides the cleansing agent, the other ingredient of the
detergent was polyphosphates. She told her mother about the
pollution that detergents causes to our rivers.
After reading the above, answer the following.
(a). What values are expressed by Ishita?
(b). What are the cleansing agents usually present in domestic
detergents?
(c). Why does polyphosphates added to detergents?
VALUE BASED QUESTION (4 MARKS)
Mr. Naresh works in a multi-national company. He is stressed due to his
hectic schedule. Mr. Amit, his friend, comes to know that he has started
taking sleeping pills without consulting the doctor.
VALUE BASED QUESTION (4 MARKS)
1. In India, large number of people take spicy food and chat etc. , which
contain a lot of acid. Excess of acid in the stomach causes irriation and
pain. Antacids are commonly used for neutralization of excess of acids.
(i) Why is sodium hydrogencarbonate,
(ii) Why are mental hydroxides better than sodium
hydrogencarbonate? Do these treat that cause of hyperacidity?
(iii) which is the best drug to cure the cause of hyperacidity?
(iv) What are the values possessed by people not taking junk food?
2.Synthetic detergents are cleansing agents which have all the properties
of soap but which actually do not contain any soap. These can be used in
both hard as esll hard water. Some of the detaegents give foam even in
ice-cold water.
(i) What type of detergents are used in toothpaste?
(ii) Which type of detergents have germicidal properties and are
used hair conditioners?
(iii) Liquid dishwashing detergents are of which type?
(iv) What is the main problem in using detergents?
(v) What is the solution to above problem? How can we save our
environment
3.Mr. Naresh works in a multi-national company. He is stressed due to
his hectic schedule. Mr. Amit, his friend, comes to know that he has
started taking sleeping pills without consulting the doctor. Mr. Amit
requests Naresh to stop this practice and takes him to a Yoga centre.
With regular Yoga sessions, Mr. Naresh is now a happy and relaxed
man.
After reading the above passage, answer the following questions:
(i) Write the values shown by Mr. Amit.
(ii) Which class of drugs is used in sleeping pills?
(iii) Why is it not advisable to take sleeping pills without
consultation with the doctor?