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Question Bank
Of
Chemistry
Probable Questions for AISSCE (Class-XII),
2015-16
Kendriya Vidyalaya Sangathan,
Kolkata Region
Chapter -1-THE SOLID STATE
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1 MARK QUESTIONS:
1. Name a liquefied metal which expands on solidification.
2. How many number of molecules per unit cell which crystallizes in the form of face centred
(monoclinic) lattice with a molecule at each lattice.
3. What is the coordination number of carbon, in diamond ?
4. Name the solid which has weakest intermolecular force ?
5. Arrange the following types of interactions in correct order of their increasing strength :
Covalent, hydrogen bonding, Vander Waals, dipole dipole.
6. Give reason for the appearance of colour in alkali metal halides.
7. Which type of defect occur in Ag Br ?
8. Give one example of doping which produces p-type of semi-conductors.
9. Out of (a) Graphite and (b) Carborundum which one is harder ?
10.How can a material be made amorphous ?
2 /3 MARK QUESTIONS :
1. Give Reason : The energy required to vaporize one mol of copper is smaller than that of energy
required to vaporize 1 mol of diamond.
2.Silver crrystallises with the face- centred cubic unit cell.Each side of this unit cellhas a length of
409 pm .What is the radius of silver atom ? Assumethat the atoms just touch each otheron the
diagonal across face of the unit cell.
3. Give reasons :
(a) Diamond and rhombic Sulphur are covalent solids, but the latter has lower melting points.
(b) Among NaCl and CsCl, CsCl is quite stable.
4.The density of lead is 11.3 g/cm3 and the metal crystallises with fcc unit cell.Estimate the radius
of lead atom .
5. In the mineral spinel; having the formula MgAl2O4 . The oxide ions are arranged in CCP, Mg2+
ions occupy the tetrahedral voids. While Al3+ ions occupy the octahedral voids. (i) What percentage
of tetrahedral voids is occupied by Mg2+ ions ? (ii) What percentage of octahedral voids is
occupied by Al3+ ions ?
6. Give reasons :
(a) Window glass of old building look milky.
b) Window glass of old building is thick at bottom.
(c) CaCl2 will introduce Schottky defect if added to AgCl crystal.
7. Analysis shows that nickel oxide has the formula NiO.98O1.00. What fractions of nickel exist as
Ni2+ and Ni3+ ions ?
8. What type of defect can arise when a solid is heated ? Which physical property is affected by
this and in what way ?
9. (a) What happens when a Ferromagnetic or Ferrimagnetic solid is heated ?
(b) The ions of MgO and NaF all have the same number of electrons and intermolecular distance
are about the same (235 & 215 pm). Why are the melting points are so different (2642 °C & 992
°C) ?
10. (a) If the radius of the Br - ion is 0.182 nm, how large a cation can fit in each of the tetrahedral
hole.
(b) AgI crystallizes in a cubic closed packed ZnS structure. What fraction of tetrahedral site is
occupied by Ag ion ?
(c) At what temp. range, most of the metals becomes super conductors ?
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1. What is the coordination number of each type of ions in a rock-salt type crystal structure?
2. What is a semiconductor? Describe the two main types of semiconductors and explain
mechanisms for their conduction .
3. How would you account for the following?
4. Define the ‘forbidden zone’ of an insulator.
5. Niobium (Nb) crystallises 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 10 mol´ 23 -1)
6. What is the number of atoms in a body-centred cubic unit cell of a crystal?
7 . Which point defect in its crystal unit cells decreases the density of a solid ?
8 .Define the terms ferromagnetism,ferrimagnetism & paramagnetism .
9. Write a feature which will distinguish a metallic solid from an ionic solid.
10. 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 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 )
Chapter-2 SOLUTION
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1 MARK QUESTIONS
1. What is ‘reverse osmosis’?
2 Define an ideal solution and write one of its characteristics.
3. Some liquids on mixing form ‘azeotropes’. What are ‘azeotropes’?
4. What is meant by osmotic pressure?
5. Define mole fraction.
6. Explain Henry’s Law with an example .
7. Define ideal solution .
8. Define Raoult’s Law.
2/3 MARKS QUESTIONS
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 meaning
of 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. Calculate the amount of KCl which must be added to 1 kg of water so that its freezing point is
depressed by 2 K.
6. Differentiate between molality and molarity of a solution. What is the effect of rise in
temperature on molality and molarity of the solution?
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.
someglycerol 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
9. Define the following terms:
(i) Mole fraction
(ii) Isotonic solutions
(iii) Van’t Hoff factor
(iv) Ideal solution
10. 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).
11.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)
12. Define the term osmotic pressure. Describe how the molecular mass of a substance can be
determined by osmotic pressure method.
5 MARK QUESTIONS
1. 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].
2.(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 non-electrolyte,
determine its molar mass.
3.(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.
4(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)
5.(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
6(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)
(Molar mass of glucose = 180 g mol–1)
7 (a) Define the following terms:
(i) Molarity
(ii) Molal elevation constant (Kb)
(b) A solution containing 15 g urea (molar mass = 60 g mol–1) per litre of solution in water has
the same osmotic pressure (isotonic) as a solution of glucose (molar mass = 180 g mol–l) in water.
Calculate the mass of glucose present in one litre of its solution.
8.(a) What type of deviation is shown by a mixture of ethanol and acetone? Give reason.
(b) A solution of glucose (molar mass = 108 g mol–1) in water is labelled as 10% (by mass).
What would be the molality and molarity of the solution? (Density of solution = 1.2 g mL–1)
9.(a) Define the following terms:
(i) Azeotrope
(ii) Osmotic pressure
(iii) Colligative properties
(b) Calculate the molarity of 9.8% (w/w) solution of H2SO4 if the density of the solution is 1.02
g mL–1. (Molar mass of H2SO4 = 98 g mol–1)
.CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1.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)
2.100 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.)
3.Calculate the freezing point depression expected for 0.0711m aqueous solution of Na 2SO4 . If
(Kf for water is 1.86°C mol ).
4. 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)
5.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).
6 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)
7.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.
8. 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?
9.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).
Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.
11. Calculate the mass of compound (molar mass = 256 g mol–1) to be dissolved in 75 g of
benzene to lower its freezing point by 0.48 K (Kf = 5.12 K kg mol–1).
12 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).
13.(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?
14. Define the following terms: i) Mole fraction,ii) Isotonic solution, iii) van’t Hoff factor iv) Ideal
solution v)Raoult’s Law.
15. Find the freezing point of a solution containing 0.520g glucose (C6H12O6) dissolved in 80.2g of
water. Given Kf for water = 1.86 K kg mol-1.
16. Calculate the temperature at which a solution containing 54g glucose (C6H12O6) in 250g of
water will freeze. Given Kf for water = 1.86 K kg mol-1 & molar of glucose is 180g mol-1.
17. Calculate the freezing point depression expected for 0.0711m aq. solution of Na2SO4. If this
solution actually freezes at 0.320 degree Celsius, what would be the value of van’t Hoff factor? Kf
for water = 1.86 K kg mol-1
18. 100mg of a protein is dissolved in just enough water to make 10mL of solution. If this solution
has osmotic pressure of 13.3 mm Hg at 25 degree Celsius ,what is the molar mass of solute?( R =
0.0821 L atm mol-1 K-1, 1atm = 760 mm Hg)
19. A solution of urea in water has a boiling point of 373.128K. Calculate the freezing point of the
same solution. Given Kf for water = 1.86 K kg mol-1 & Kb = 0.52 K kg mol-1.
20. Calculate the amount of sodium chloride which must be added to one kilogram of water so that
the freezing point of water is depressed by 3K. (Kf for water = 1.86 K kg mol-1, Na = 23 & Cl =
35.5)
21. An antifreeze solution is prepared from 222.6 g of ethylene glycol C2H4(OH)2 and 200g of
water. Calculate the molality of the solution. If the density of the solution be 1.072 g mL-1, what
will be the molariry of the solution?
22. A solution prepared by dissolving 8.95 g of a gene fragment in 35.0 mL of water has an
osmotic pressure of 0.335torr at 25 degree Celsius. Assuming gene fragment is non electrolyte
determine its molar mass.
23. 15.0 g of an unknown molecular mass material is dissolved in 450 g of water. The resulting
solution freezes at -0.34degree Celsius. What is the molecular mass of the material? Given Kf for
water = 1.86 K kg mol-1.
24. 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 gmol-1) must be dissolved in 65 g of water to lower the
freezing point by 7.5 degree Celsius ? Kf for water = 1.86 K kg mol-1. Assume van’t Hoff factor
for NaCl is 1.87.
25. a) The molecular mass of polymers is determined by osmotic pressure method and not by any
other colligative property method. Give two reasons
b) At 300K, 36 g of glucose (C6H12O6) present per litre in its solution has an osmotic pressure of
4.98 bar. If the osmotic pressure of another glucose solution is 1.52 bar at the same temperature,
calculate the concentration of the other solution.
CHAPTER -3 ELECTROCHEMISTRY
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1 MARK QUESTIONS
1. Define the term molar conductivity. How is it related to conductivity of the related solution?
2. How do metallic and ionic substances differ in conducting electricity?
3.. What is meant by ‘limiting molar conductivity’?
4.Write two advantages of H2 – O2 fuel cell over ordinary cell.
2/3 MARKS QUESTIONS
1. Define conductivity and molar conductivity for the solution of an electrolyte. How do they vary
when the concentration of electrolyte in the solution increases?
2. 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.´
3. 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.
4.Conductivity of 0.00241M acetic acid solution is 7.896 ´10-5 S cm-1. Calculate its molar
conductivity in this solution. If Lm° for acetic acid is 390.5 S cm2 mol-1, what would be its
dissociation constant?
5. The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 W . What
is the cell constant if the conductivity of 0.001 M KCl solution at 298 K is 0.146 ´10-3 S cm-1
6.The conductivity of 0.20 M solution of KCl at 298 K is 0.025 S cm–1. Calculate its molar
Conductivity.
7. State Kohlrausch law of independent migration of ions. Why does the conductivity of a solution
decrease with dilution?
8. (a) Calculate ΔGo for the reaction
Mg(s) + Cu2+(aq)  Mg2+(aq) + Cu(s)
Given: E0cell = 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.
9.A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5.0 ampere
For 20 minutes. What mass of nickel will be deposited at the cathode?
(Given: At. Mass of Ni = 58.7 g mol–1, 1 F = 96500 C mol–1)
10. Express the relation between conductivity and molar conductivity of a solution held in a cell.
11. The molar conductivity of a 1.5M solution of an electrolyte is found to be 138.9 S cm2mol-1.
Calculate the conductivity of the solution.
12. Express the relation among the cell constant, resistance of the solution in the cell and
conductivity of the solution. How is molar conductivity related to its conductivity?
13. What type battery is lead storage battery? Write anode and cathode reactions and the overall
reaction occurring in a lead storage battery, when current is drawn from it.
14 . a) Define molar conductivity of a solution and explain how molar conductivity changes with
change in concentration of solution for a week and a strong electrolyte.
b) The resistance of a conductivity cell containing 0.001M KCl solution at 298K is 1500 ohm.
What is the cell constant, if the conductivity of 0.001M KCl solution at 298K is 0.146 X 10-3 S
cm-1?
15. A voltaic cell is set up at 298K with the following half cells:
Al│Al+3 (0.001M) and Ni│Ni+2 (0.50M). Write the cell reaction and determine the cell
potential. Given:
E0Ni+2/Ni = -0.25V & E0Al+3/Al = -1.66V.
16. Calculate the potential for half-cell containing 0.10M K2Cr2O7(aq.), 0.20M Cr+3(aq.) & 10-4 M
H+(aq.). The half cell reaction is: Cr2O7-2 (aq.) + 14H+(aq.) + 6e- → 2Cr+3 (aq.) + 7H2O(l) and
standard electrode potential is 1.33V
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1. Three conductivity 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 amperes is passed
through them until 1.45 g of silver is deposited at the cathode of cell B. How long did the
urrent flow? What mass of copper and what mass of zinc got deposited in their respective
cells?
2.Calculate the emf of the following cell at 298 K:
Fe (s) | Fe2+ (0.001 M) || H+ (1M) | H2 (g) (1 bar), Pt (s)
(Given Ecello = + 0.44 V)
3.The standard electrode potential (E
G° for the reaction
2
+
2
+
Zn(s) +Cu (aq) -> Zn (aq)+Cu(s)
(1 F = 96500 C mol–1).
4. A voltaic cell is set up 25° C with the following half-cells:
Al | Al3+ (0.0010 M) and Ni | Ni2+ (0.50 M).
Write the equation for the cell reaction that occurs when the cell generates an electric current
and determine the cell potential. (Given : E (Ni /Ni)= 0.25V, E (Al /Al)) =1.66V)
5. Calculate the equilibrium constant for the reaction equilibrium
Fe(s) + Cd2+(aq) l Fe2+(aq) + Cd(s)
Given: Eo (cd / cd2+) = 0.44, Eo (fe / fe2+) = 0.44
6.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.
7. (a) Define the following terms:
(i) Limiting molar conductivity (ii) Fuel cell
(b) Resistance of a conductivity cell filled with 0.1 mol L–1 KCl solution is 100 ohm. If the
resistance of the same cell when filled with 0.02 mol L–1KCl solution is 520 ohm, calculate the
conductivity and molar conductivity of 0.02 mol L–1KCl solution. The conductivity of 0.1 mol L–
1KCl
solution is 1.29 × 10–2 ohm–1 cm–1.
8. (a) State Faraday’s first law of electrolysis. How much charge in terms of Faraday is required for
the reduction of 1 mol of Cu2+ to Cu? (b) Calculate emf of the following cell at 298 K:
Mg(s); Mg 2 +(0.1M)// Cu 2 +(0.01); Cu(s)
[Given Ecello =2.71 V, 1 F=96500 C mol–1 ]
Q9. (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: ENi /Ni2+= –0.25 V, EAl /Al3+= –1.66 V)
Q10. Formulate the galvanic cell in which the following reaction takes place:
Zn(s) + 2Ag+(aq.) → Zn+2 (aq.) + 2Ag(s)
i) Which electrode is negatively charged? ii) Write the reaction taking place at each electrode.
iii) Which are the carriers of current inside the cell?
Q11. The conductivity of a 0.20M solution of KCl at 298K is 0.0248 S cm-1. Calculate its molar
conductivity.
Q12. Explain why electrolysis of NaCl(aq.) gives H2 at cathode and Cl2 at anode. Write the overall
reaction. Given: E0Na+/Na = -2.71V, E0 H2O/H2 = -0.83V, E0Cl2/Cl- = +1.36V & E0 H+/H2O = +1.23V
Q13. State and explain Kohlrausch’s law of independent migration of ions. Write an expression for
the molar conductivity of acetic acid at infinite dilution according to Kohlrausch’s law.
Q14. Two half reactions of an electrochemical cell are given below:
MnO4- (aq.) + 8H+(aq.) + 5e- → Mn+2 (aq.) + 4H2O(l) E0 = +1.51V
Sn+2(aq.) → Sn+4(aq.) + 2e- E0 = -0.15V
Construct the redox equation from these and predict whether the reaction is reactant or product
favoured.
Q15. The chemistry of corrosion of iron is essentially an electrochemical phenomenon. Explain the
reactions occurring during corrosion of iron exposed to atmosphere.
Q16. Calculate the limiting molar conductivity of acetic acid. Given that limiting molar
conductivities of HCl, NaCl & CH3COONa are 426.6, 126.0 & 91.0 S cm2 mol-1 respectively.
Q17. 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 0.10M solution of
zinc nitrate. A voltage of 1.48V is measured for this cell. Use this information to calculate the
concentration of silver nitrate solution. Given: E0Zn+2/Zn = -0.763V & E0Ag+/Ag = +0.80V.
Q18. A copper-silver cell is set up. The copper ion concentration is 0.01M. The concentration of
silver ion is not known. The cell potential was found to be 0.422V. Determine the concentration of
silver ions in the cell. Given: E0Cu+2/Cu = +0.34V & E0Ag+/Ag = +0.80V.
Q19. Conductivity of 0.00241M CH3COOH is 7.896 X 105 S cm-1. Calculate its molar conductivity.
If λ0m for
CH3COOH is 390.5 S cm2 mol-1 , calculate its dissociation constant.
CHAPTER -4 CHEMICAL KINETICS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1 MARK QUESTIONS
Q1Define the following terms giving an example for each:
(i) The order of a reaction (ii) The molecularity of a reaction
Q2.Identify the order of reaction from the following unit for its rate constant:
Q3.Define:
(i) Elementary reaction in a process
(ii) Rate of a reaction.
Q4.Distinguish between ‘rate expression’ and ‘rate constant’ of a reaction
Q5.. Define the following terms:
(i) Pseudo first order reaction
(ii) Half life period of reaction (t1/2)
L mol–1s–1
2/3 MARK QUESTIONS
Q1. 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?
Q2. 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.
Q3. 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?
Q4.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)
Q5.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?
Q6.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.
Q7.For a first order reaction, show that time required for 99% completion is twice the time
Required for the completion of 90% of reaction.
Q8.(a) For a reaction A + B P, the rate law is given by,
r =k[A]1/ 2 [B]2 .
What is the order of this reaction?
(b) A first order reaction is found to have a rate constant k = 5.5 × 10–14 s–1. Find the
half life of the reaction.
Q9.The rate of a reaction becomes four times when the temperature changes from 293 K to 313 K.
Calculate the energy of activation (Ea) of the reaction assuming that it does not change with
temperature.
[R = 8.314 JK–1 mol–1, log 4 = 0.6021]
Q10. Define half-life of a reaction. Write the expression of half-life for
(i) zero order reaction and
(ii) first order reaction.
Q11. Define order of a reaction.
Q12. A reaction is of second order with respect to a reactant. How is the rate affected if the
concentration of the reactant is i) doubled ii) reduced to half.
Q13. The decomposition of NH3 on a platinum surface is a zero order reaction. What are the rates
of production of N2 & H2 if k = 2.5 X 10-4 Ms-1.
Q14.List the factors on which the rate of chemical reaction depends.
Q15. A first order reaction has a rate constant of 0.00510 min-1. If we begin with 0.10M
concentration of the reactant, how much of the reactant will remain after 3.0 h?
Q16. The half life for radioactive decay of 14C is 5730 yr. An archaeological artifact containing
wood had only 80% of the 14C found in a living tree. Estimate the age of the sample.
Q17. Define activation energy.
5 MARK QUESTIONS
Q1. (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 togetherdoubled?
(b) The rate constant k of a reaction increases four fold 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)
Q2.(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
artefact has only 80% of the 14 C activity found in fresh wood. Calculate the age of the artifact
Q3.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.
Q4. 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?
Q5(a) Explain the following terms:
(i) Rate of a reaction
(ii) Activation energy of a reaction
(b) The decomposition of phosphine, PH3, proceeds according to the following equation:
4PH3(g) P4(g) + 6H2(g)
It is found that the 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 is required for 3/4th of PH3 to decompose?
(ii) What fraction of the original sample of PH3 remains behind after 1 minute
Q6.(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 reaction, assuming that it does not change with
temperature. (R = 8.314 J K–1 mol–1)
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
Q1. 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?
Q2.. 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?
Q3.The thermal decomposition of HCO2H is a first order reaction with a rate constant of
2.4 × 10–3 s–1 at a certain temperature. Calculate how long will it take for three-fourths of
initial quantity of HCO2H to decompose. (log 0.25 = – 0.6021)
Q4. 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?
Q5 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?
760 mm Hg = 1 atm.)
Q6. The following data were obtained during the first order thermal decomposition of SO2Cl2 at a
constant volume:
SO2Cl2 SO2(g) + Cl2(g)
Experiment
Time/second–1
1
0
2
100
Calculate the rate constant.
(Given: log 4 = 0.6021, log 2 = 0.3010)
Total pressure/atm
0.4
0.7
Q7.(a) Express clearly what you understand by ‘rate expression’ and ‘rate constant’ of a reaction.
(b) Nitrogen pentoxide decomposes according to the equation
2N2O5 (g) 4NO2 (g) +O2 (g)
This first order reaction was allowed to proceed at 40°C and the data given below were
collected:
[N2O5](M)
Time (min)
0.400
0.00
0.289
20.00
0.209
40.00
0.151
60.00
0.109
80.00
(i) Calculate the rate constant for the reaction. Include units with your answer.
(ii) Calculate the initial rate of reaction.
(iii) After how many minutes will [N2O5] be equal to 0.350 M?
Q8. (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 t1/2
for this reaction. (Given log 1.428 = 0.1548
Q9.. For a certain chemical reaction variation in the concentration vs time is given
Y
Log[R]
t(S)
X
For this reaction write /draw
(i)
What is the order of the reaction?
(ii)
What are the units of rate constant K
(i)
Give the relationship between K and t1/2
(ii)
What does the slope of the above line indicate?
Draw the plot of log [Ro]/[R] vs time t(s)
Q10. For a certain chemical reaction
A +2B
2C+D
The experimentally obtained information is tabulated below.
Exp
[A]o (molL-1) [B]o (molL-1)
Initial rate of reaction (molL-1S1)
1
0.30
0.30
0.096
2
0.60
0.30
0.384
3
0.30
0.60
0.192
4
0.60
0.60
0.768
For this reaction
Derive the order of reaction w.r.t both the reactants A and B.
(i)
Write the rate law.
(ii)
Calculate the value of rate constant K.
(iii) Write the expression for the rate of reaction in terms of A and C.
Q11. The rate for a zero order reaction in A is 0.0030 mol L-1 s-1. How long will it take for the
initial concentration of A to fall from 0.10M to 0.075M?
Q12. A first order reaction takes 40 min for 30% completion. Calculate its half life.
Q13. Derive the expression for half life of a first order reaction.
Q14. The reaction: 4PH3(g) → P4 (g) + 6H2(g) was found to follow the rate law as: Rate = k[PH3]
with a half life of 37.9s. at 120 degree Celsius. Calculate i) Time required for 3/4th of PH3 to
decompose. ii) Fraction of the original sample of PH3 left out after 1 min.
Q1 5. A first order reaction is 15% complete in 20min. How long will it take to be 60% completed?
Q1 6. The rate of a reaction becomes double when temperature increases from 298K to 308K.
Calculate Ea
Q17. The rate of a reaction becomes four times when temperature increases from 300K to 320K.
Calculate Ea
Q18. What is the effect of temperature on the rate constant of a reaction? How can this effect be
expressed quantitatively?
Q19. The rate constants for a reaction at two different temperatures are found to be as follows:
k1 = 2.15 X 10-8 L mol-1 s-1 at 650K, k2 = 2.39 X 10-7 L mol-1 s-1 at 700K Calculate Ea for this
reaction.
CHAPTER -5 SURFACE CHEMISTRY
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1
Why is adsorption always exothermic?
2
Why does the sky appear blue?
3
Which has higher enthalpy of adsorption---physisorption or chemisorption?
4
Give an example of shape selective catalysis.
5
Define—
i)Electrophoresis
ii)Peptisation
iii)aerosol
iv)Tyndall effect
v)associated colloids
vi) shape selective catalysis
6
Write any three differences between physisorption and chemisorption
How does physisorption and chemisorption vary with temperature?
7
What are the characteristics of the following colloids?Give an example of each.
i)multimolecular colloids
ii) lyophobic sols
iii)macromolecular colloids
8
What are emulsions?Name the two different types of emulsions.
Give an example of each type.
9
What are lyophilic and lyophobic sols ?Give one example of each type.Which of these sols
can be
easily coagulated on the addition of small amount of electrolytes?
10 Explain what is observed
(i) When a beam of light is passed through a colloidal sol.
(ii) An electrolyte, NaCl is added to hydrated ferric oxide sol.
(iii) Electric current is passed through a colloidal sol?
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1
What causes Brownian movement in a colloidal solution?
2
What is the sign of ∆𝐻 and ∆𝑆 when a gas is adsorbed by an adsorbent.
3
A delta is formed at the meeting point of sea and river water.Why?
4
Why is a Cottrell smoke precipitator fitted at the mouth of chimneys?
5
When AgNO3 solution is added to KI solution,the resulting colloid particles of AgI sol are
positively charged.Why?
6
What happens when hydrated ferric oxide sol is mixed with As2S3 sol?
7
8
9
10
11
12
13
14
15
16
What are the dispersed phase and dispersion medium in i) milk and ii) smoke?
Define—
i)Coagulation
ii)micelle
iii)collodion
iv)Zeta potential
v)Dialysis
vi)enzyme
vii)adsorption
viii)Hardy Schluze rule
viii)alcosol
viii) desorption
What is the difference between a colloidal solution and an emulsion?What is the role of
emulsifier in forming emulsion?
What is an adsorption isotherm?Describe Freundlich adsorption isotherm.
Explain how the phenomenon of adsorption finds application in the following processesi)production of vaccum
ii)heterogeneous catalysis
iii)Froth floatation process
What is meant by coagulation of colloidal solution?Describe any three methods by which
coagulation of hydrophobic sols can be carried out.
What is meant by activity and selectivity of a catalyst?Give examples with reactions.
Name the two types of catalysis reaction.Give an example of each type with the chemical
reaction involved.
Classify colloids where the dispersion medium is water.State their characteristics and write
an example of each of these classes.
Which one of the following electrolyes is most effective for the coagulation of hydrated
ferric oxide sol and why?
NaCl ,Na2SO4 ,Na3PO4
CHAPTER -6 GENERAL PRINCIPLES AND
PROCESSES OF ISOLATION OF ELEMENTS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1
2
3
4
5
6
7
8
9
10
Name the method used for the refining of each of the following metals--i)Zirconium ii) copper metal iii)Nickel metal
Out of C and CO,which is a better reducing agent in the lower temperature range in the blast
furnace to extract iron from iron oxide?
Name the method of refining to obtain silicon of high purity.
Copper matte is charged into a silica lined converter in the extraction of copper.What is the
role of silica lining here?
Which solution is used for the leaching of silver metal in the presence of air in the metallurgy
of silver?
Describe the principle controlling each of the following processes—
i)zone refining of metals
ii)electrolytic refining of metals.
iii)vapour phase refining of metals.
Describe the principle of each of the following processes—
i)preparation of cast iron from pig iron
ii) preparation of pure alumina from bauxite ore
Name one chief ore each of copper and aluminium.Name the method used for the
concentration of these two ores.
Name the principal ore of aluminium.Explain the significance of leaching in the extraction of
aluminium.
Differentiate between---i)calcination and roasting ii)mineral and ore
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1
2
3
4
5
6
7
8
How is copper extracted from a low grade ore of it?
How is wrought iron different from steel?
What is the composition of copper matte?
Write the principle behind hydraulic washing.
What is meant by the term ‘pyrometallurgy’?
Why is froth floatation process selected for the concentration of sulphide ores?
What is the role of CO in the extraction of iron?
Which form of iron is the purest form of commercial iron?
9
10
11
12
13
What type of ores are concentrated by magnetic separation method?
Which solution is used for the leaching of silver metal in the presence of air in the
metallurgy of silver?
Describe the role of the following—
i)Iodine in the extraction of Titanium
ii) Zinc in the extraction of silver
How is chemical reduction different from electrolytic reduction?Name a metal each which
is obtained by i)electrolytic reduction ii) chemical reduction
Describe the principle involved in each of the following processes--i)Mond’s process for refining of nickel
ii)Column chromatography for purification of rare elements.
CHAPTER -7 p-BLOCK ELEMENTS
GROUP 15 ELEMENTS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1
2
3
4
5
6
QUESTIONS BASED ON REACTIONS-Write the chemical equation involved in the preparation of H3PO3
How does ammonia react with a solution of Cu2+?
Write the reaction of thermal decomposition of sodium azide.
What happens when PCl5 is heated?
Write a chemical reaction to show that all bonds in PCl 5 are not equivalent
Complete the following reactions--i)Ca3P2 + H2O
ii)H3PO3 is heated
iii)NH3 + NaOCl 
iv)P4 +NaOH +H2O
v)I2+HNO3(conc.)
vi)P4 +SO2Cl2
vii)Cu + HNO3(dilute)
viii)HgCl2 +PH3
OTHER QUESTIONS--
7
Give reasons for the following-------Nitrogen is chemically less reactive than phosphorus.
----NH3 is basic while BiH3 is only feebly basic.
---- nitrogen shows catenation properties less than phosphorus
----the bond angle in PH3 is lesser than in NH3
----NO2 dimerises easily to N2O4
---- nitrogen does not form pentahalides although it shows +5 oxidation state
----BiH3 is a stronger reducing agent than SbH3
----(CH3)3P=O exists but (CH3)3N=O does not
----nitrogen is not much reactive at room temperature
8
9
10
11
12
Which allotrope of phosphorus is reactive and why?
What is the basicity of H3PO3 and why?
What is the covalence of nitrogen in N2O5?
What is the oxidation number of phosphorus in H3PO2?
Draw the structures of---PCl5 ,H4P2O7,N2O5
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1
Give reasons for the following-------NH3 forms hydrogen bond but PH3 does not
----- R3P=O exists but R3N=O does not
----H3PO2 acts as a monobasic acid
----Ammonia has greater affinity for protons than phosphine
---- PCl5 behaves as an ionic compound in the solid state
----Bi(V) is a stronger oxidizing agent than Sb(V)
----the basic character of the hydrides of group 15 elements decreases with
increasing atomic numbers
----in the structure of HNO3 molecule,the N—O bond is shorter than the N--OH
bond
---- all the P—Cl bonds in PCl5 are not equivalent
----NF3 is an exothermic compound but NCl 3 is not
----the N—O bond is in NO2- is shorter than the N—O bond in NO3----the bond angles(O—N—O) are not of the same value in NO2- and NO2+
---- H3PO2is a stronger reducing agent than H3PO3
----- PCl5 can act as an oxidizing agent but not as a reducing agent
2
3
Which one of PCl4+ and PCl4- is not likely to exist and why?
How is ammonia manufactured industrially?Draw flow chart for the manufacture of
ammonia.Give any two uses of it.
Draw the structures of—(HPO3)3 ,white and red phosphorus
4
GROUP 16 ELEMENTS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1
QUESTIONS BASED ON REACTIONS-Complete the following reactions--i)O3 +I- +H2O
ii)C +H2SO4(conc)
iii)SO2 +NaOH
iv)CaF2 + H2SO4(conc)
v)SO3 + H2O
vi) SO3 +H2SO4
OTHER QUESTIONS
2
Give reasons for the following-------sulphur has greater tendency for catenation than oxygen in the same group
----the electron gain enthalpy with negative sign for oxygen(-141kJ/mol)is
numerically
less than that for sulphur(-200 kJ/mol)
----sulphur in vapour state exhibits paramagnetism
----OF6 compound is not known
----H2S is less acidic than H2Te
----oxygen is a gas but sulphur is a solid
----all the bonds in SF4 are not equivalent
3
Draw the structures of—H2SO5 ,S8 ,SO32-, SF4 , O3 , H2S2O7 , H2S2O8 , H2SO4 , H2SO3 ,
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1
Give reasons for the following-------all the bonds in SF4 are not equivalent
---- SF4 is easily hydrolysed but SF6 is not easily hydrolysed
----there is a large difference between the melting and boiling points of oxygen and
sulphur
----supersonic jet aeroplanes are responsible for the depletion of ozone layer
----SF6 is kinetically an inert substance
2
3
4
5
6
Of PH3 and H2S ,which is more acidic and why?
Predict the shape and asked angle (90o or more or less)in SO32- and the angle O-S-O
What happens when Sulphur dioxide is passed into aqueous solution of Fe(111) salt?
Why does O3 act as a powerful oxidizing agent?
Write the conditions to maximize the yield of H2SO4 by contact process.
GROUP 17 ELEMENTS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1
QUESTIONS BASED ON REACTIONS—
Complete the following reactions--i)Cl2 + NaOH(cold and dilute)
ii)I2 +H2O +Cl2
iii) Cl2+ F2(excess)
iv) Cl2 + NaOH(hot and conc)
v) F2 + H2O
2
3
4
5
6
Give reasons for the following----
----Fluorine does not exhibit positive oxidation state
----bond dissociation energy of F2 is less than that of Cl2
----HCl is stronger acid than HF in aqueous medium
----Iron dissolves in HCl to form FeCl2 but not FeCl3
------HF has higher boiling point than HCl
----electron gain enthalpy with negative sign for fluorine is less than that of chlorine
----interhalogens are more reactive than halogens
----acidic character increases from HF to HI
----ICl is more reactive than I2
Mention all the oxidation states exhibited by chlorine in its compounds
Predict the shape and asked angle (90o or more or less)in ClF3and the angle F-Cl-F
Arrange the following in increasing order of their acidic strength
HCl , HBr , HI , HF
Draw the structures of— BrF3 , NF3 , HClO4 , ClF3
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1
Give reasons for the following-------pentahalides of a metal are more covalent than trihalides
----F2 is most reactive of all the four common halogens
----despite having greater polarity,HF boils at a lower temperature than H2O
----ClF3 molecule has a T shaped structure and not a trigonal planar one .
----interhalogen compounds are strong oxidizing agents
----the acidic strength decreases in the order HCl >H2S >PH3
----Fluorine forms the the largest number of interhalogen compounds amongst the
halogens
2
3
4
5
Why does fluorine not play the role of central atom in interhalogen compounds?
Name two poisonous gases which can be prepared from chlorine gas.
Which neutral molecule would be isoelectronic with ClO-?
How are interhalogen compounds formed?What general compositions can be assigned to
them?
GROUP 18 ELEMENTS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1
QUESTIONS BASED ON REACTIONS—
Complete the following reactions--i)XeF6 +H2O(excess)
ii)PtF6 +Xe 
iii)XeF2 +PF5
iv)XeF4 +O2F2
v)XeF4 +SbF5
vi)XeF2 +H2O
2
Give reasons for the following----
3
4
5
----The majority of known noble gas compounds are those of xenon
----noble gases have very low boiling points
----XeF2 has a straight linear structure and not a bent angular structure
Which noble gas is used in filling balloons for meteorological observations?
What happens when XeF6 is hydrolysed?
Draw the structures of-----XeF4 , XeO3 , XeF2 , XeF6 XeOF4
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1
2
3
Give reasons for the following-------Helium forms no real compound
----Helium is used in diving equipments
What inspired N Bartlett for carrying out reaction between Xe and PtF6?
Predict the shape and asked angle (90o or more or less)in XeF2and the angle F—Xe---F
CHAPTER -8 THE d- AND f -BLOCK
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1 MARK QUESTIONS
Q. 1. What is the equivalent wt. of KMnO4 in : (a) Acidic Medium (b) Neutral Medium (c) In
alkaline Medium
Q. 2. K2PtCl6 is well known compound and corresponding Ni4+ Salt is unknown ? Whereas
Ni+2 is more stable than Pt+2
Q. 3. Sc3+ is more stable than Sc2+ .
Q. 4. Why KMnO4 is bright in colour ?
Q. 5. Why gold, Pt are dissolved in aqua Regia ?
Q. 6. CrO is basic but Cr2O3 is amphoteric ?
Q. 7. In the titration of Fe2+ ions with KMnO4 in acidic medium, why dil. H2SO4 is used
and not dil. HCl.
Q. 8. (a) The E° value for Ce4+/Ce3+ is 1.74 Volt.
(b) K2Cr2O7 is used as Primary Standard in volumetric analysis.
Q. 9. (a) Although Cu+ has configuration 3 d10 4 s0 (stable) and Cu2+ has configuration 3 d9
(unstable configuration) still Cu2+ compounds are more stable than Cu+ .
(b) Titanium (IV) is more stable than Ti (III) or Ti (II).
Q. 10. The actinoids exhibit more number of oxidation states Why ? Give their common
oxidation states.
Q. 11. (a) Give reason CrO3 is an acid anhydride.
(b) Give the structure of CrO5
Q. 12. A well known orange crystalline compound (A) when burnt impart violet colour to
flame. (A) on treating (B) and conc. H2SO4 gives red gas (C) which gives red yellow solution
(D) with alkaline water. (D) on treating with acetic acid and lead acetate gives yellow p. pt.
(E). (B) sublimes on heating. Also on heating (B) with NaOH gas (F) is formed which gives
white fumes with HCl. What are (A) to (F) ?
Q. 13. Why is Cr2+ reducing and Mn3+ oxidising when both have d4 configuration ?
Q. 14. (a) In MnO4 – ion all the bonds formed between Mn and Oxygen are covalent. Give
reason.
(b) Beside + 3 oxidation state Terbium Tb also shows + 4 oxidation state. (Atomic no. = 65)
Q. 15. (a) Highest manganese flouride is MnF4 whereas the highest oxide is Mn2O7 .
(b) Copper cannot liberate H2 from dil acids . Why ?
Q.16 A metal which is strongly attracted by a magnet is attacked slowly by the HCl liberating
a gas and producing a blue solution. The addition of water to this solution causes it to turn
pink.Identify the metal
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
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 . 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) K2MnO4from pyrolusite ore.
3. Compare actinoids and lanthanoids with reference to their :
(i) electronic configurations of atoms
(ii) oxidation states of elements
Iii ) general chemical reactivity of elements
4. 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+)
5. 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)
6. 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.
7). 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.
8) (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 Mn2+/Mn value for manganese is much more than expected from the trend for
other elements in the series.
9. 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.
There is a greater range of oxidation states among the actinoids than lanthanoids .
10. 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
 CHAPTER -9 CO-ORDINATION COMPOUNDS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1 MARK & 2 MARKS QUESTIONS
Q. 1. A cationic complex has two isomers A & B. Each has one Co3+, five NH3 ,
one Br--- and one SO4 2- . A gives a white precipitate with BaCl2 solution while B
gives a yellow precipitate with AgNO3 solution.
(a) What are the possible structures of the complexes A and B ?
(b) Will the two complexes have same colour ?
Q. 2. FeSO4 solution mixed with (NH4 ) 2SO4 solution in 1 : 1 molar ratio gives
the test of Fe2+ ion but CuSO4 solution mixed with aqueous ammonia in 1 : 4
molar ratio does not give the test of Cu2+ ion. Explain why ?
Q. 3. If to an aqueous solution of CuSO4 in two tubes, we add ammonia
solution in one tube and HCl (aq) to the other tube, how will the colour of the
solutions change ? Explain with the help of reaction.
Q. 4. A, B and C are three complexes of Chromioum with the empirical formula
H12O6Cl3Cr. All the three complexes have Cl and H2O molecules as the ligands.
Complex A does not react with conc. H2SO4 . Complexes B and C lose 6.75% and
13.5% of their original weight respectively on heating with conc. H2SO4 .
Identify A, B and C.
Q.5 Compare the following complexes with respect to structural shapes of
units,magnetic behaviour & hybrid orbitals involved in units:
Q. 6. Write the name, stereochemistry & magnetic behaviour of the following:
(At. Nos. Mn = 25, Co = 27, Ni = 28)
Q. 7. How t2g and eg orbitals are formed in an octahedral complex ?
Q. 8. Explain the reason behind a colour of some gem stone with the help of
example.
Q. 9. How many EDTA lethylendiamine tetra acetic acid) molecules are
required to make an octahedral complex with a Ca2+ ion.
Q. 10. What is the hybridisation of central metal ion and shape of Wilkinson’s
catalyst ?
Q. 11. Which vitamin is a complex compound of cobalt ?
Q. 12. Write the IUPAC name of [CO (NH3 ) 4 Br2] 2 [ZnCl4 ].
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1. Name the following coordination compounds according to IUPAC system of
nomenclature:
(i) [Co(NH3)4 (H2O) Cl]Cl2
[CrCl2(en)2]Cl, (en = ethane –1, 2 – diamine)
2. Give an example of linkage isomerism
3. Give an example of coordination isomerism.
4. Describe the shape and magnetic behaviour of following complexes:
5. Explain the following cases giving appropriate reasons:
(i) Nickel does not form low spin octahedral complexes.
(ii) The -complexes are known for the transition metals only.
Co2+ is easily oxidised to Co3+ in the presence of a strong ligand.
6. Write the name, the state of hybridization, the shape and the magnetic
behaviour of the following
complexes:
[CoCl4]2–, [Ni(CN)4]2–, [Cr(H2O)2(C2O4)2]–
(Atomic number: Co = 27, Ni = 28, Cr = 24)
7. (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?
(c) Why is CO a stronger ligand than NH3 in complexes?
8. (a) Write the formulae for the following coordination compounds:
(i) Tetraammineaquachloridocobalt (III) chloride
(ii) Potassiumtetracyanonickelate (II)
(b) Write the hybridisation of the complex [NiCl4]2–. (Atomic number of Ni =
28)
9. Which of the following is more stable complex and why? [Co(NH3)6]3+ and
[Co(en)3]3+
10. (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+?
(en = ethane-1,2-diamine)
(iii) Why is [NiCl4]2– paramagnetic but [Ni(CO)4] is diamagnetic?
(At nos.: Cr = 24, Co = 27, Ni = 28)
CHAPTER -10 HALOALKANES & HALOARENES
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
ONE MARK QUESTIONS
1.Identify the chiral molecule in the following pair
2.Draw the structure of 2-Bromopentane.
3.Write the IUPAC name of (CH3)2CHCH(Cl)CH3
4.Write the IUPAC name of
5.What happens when CH3Br is treated with KCN
6. What happens when Ethyl chloride is treated with aquous KOH?
7.Write the IUPAC name of
8.Which compound in the following pair undergoes faster SN1 reaction?
9.Write the IUPAC name of the following compound
10.Write the IUPAC name of the following
11. Write the IUPAC name of the following
12.Write the IUPAC name of (CH3)3CCH2Br
13.Write the IUPAC name of CH2=CHCH2Br
14.Draw the structure of 1,4-Dibromobut-2-ene.
15. Draw the structure of 2-chloro-3-methylpentane.
16.Which will react faster in SN2 displacement 1-Bromopentane or 2-Bromopentane and why?
17. Draw the structure of 4-tert-butyl-3-iodoheptane.
18. Write the IUPAC name of( CH3)3CCH2Cl
19. Draw the structure of 1-chloro-4-ethylcyclohexane.
20. Draw the structure of4-Bromo-3-methylpent-2-ene
21.Complete the following chemical equation
22. Write the IUPAC name of
TWO MARK QUESTIONS
1.Write the mechanism of the following reaction
2.i) which of the alkyl halides from the following pair is chiral and undergoes faster SN2 reaction
ii)Out of SN1 and SN2, which occurs with a) inversion of configuration
b)racemisation?
3.Draw the structure of major monohalo product of each of the following reactions
4.Write chemical equation when
i)ethyl chloride is treated with aquous KOH
ii)chlorobenzene is treated with CH3COCl in the presernce of anhy.AlCl3.
5.i)Which alkyl halide out of the following would you expect to react faster by SN2 mechanism and
why?
ii)racemisation occurs in SN1 reactions and why?
6. Draw the structure of
i)p-bromochlorobenzene
ii)1-Chloro-4-methylcyclohexane
7. Draw the structure of
i)4-tert-butyl-3-iodoheptane
ii)4-Bromo-3-methylpent-2-ene
8. Write the IUPAC name of
i)CH2=CHCH2Br
ii)(CCl3)3CCl
9.Chlorobenzene is less reactive towards a nucleophilic substitution reaction.Give two reasons for
the same
10. Account for the following
i)Alkyl halides though polar are immiscible in water.
ii)Grignard reagent should be prepared under anhydrous conditions
11. Which of the following would you expect to react faster by SN2 mechanism and
why?
12. Which out of the following reacts faster by SN1 mechanism and why?
13. Which of the following would you expect to react faster by SN2 mechanism with –OH and why?
i)CH3Br or CH3I
ii)(CH3)3CCl or CH3Cl
THREE MARK QUESTIONS
1. i)Why are haloalkanes more reactive than haloarenes towards nucleophiles?
ii) Which of the following would you expect to react faster by SN1 mechanism and why?
2. i) Which of the following would you expect to react faster by SN2 mechanism
a)CH3Br or CH3I
b) (CH3)3CCl or CH3Cl
ii)Write the product of the following reaction
3.Explain the following
i)The dipole moment of chlorobenzene is lower than that of cyclohexylchloride
ii)alkyl halides ,though polar are immiscible with water
iii) Grignard reagent should be prepared under anhydrous conditions
4. Answer the following
i)what is meant by a chirality of a compound?Give an example.
ii)Which of the following compound is more easily hydrolysed by KOH and why?
CH3CHClCH2CH3
or CH3CH2CH2CH2Cl
iii)Which one undergoes SN2 substitution faster and why?
5.How would you differentiate between SN1 and SN2 mechanism.Give one example of each.
6. Explain the following
i) the dipole moment of chlorobenzene lower than that of cyclohexylchloride
ii) alkyl halides ,though polar are immiscible with water
iii)in the pair (CH3)3-Cl and CH3Cl, CH3Cl will react faster in SN2 reaction with –OH?
7. Explain the following
i)p-Dichlorobenzene has higher M.P. than those of o-and m-isomers.
ii)Haloarenes are less reactive than haloalkanes towards nucleophilic substitution reaction.
iii)The treatment of alkyl chloride with aquous KOH leads to the formation of alcohol but in the
presence of alcoholic KOH,alkene is the major product.
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
ONE MARK QUESTIONS
1.Write the IUPAC name of the following compound
2.How methyl bromide be preferentially converted to methyl isocyanide ?
3.What happens when Bromine attacks
4.Draw the structure of 2-(2-bromophenyl)butane.
5. Draw the structure of 2-(2-chlorophenyl)-1-iodooctane.
6. Draw the structure of 1-Bromo-4-sec-butyl-2-methylbenzene
7. Draw the structure of 3-(4-chlorophenyl)-2-methylpropane.
8. Write the IUPAC name of
9.A solution of KOH hydrolyses CH3CHClCH2CH3 and CH3CH2CH2CH2Cl.Which one of these is more
easily
Hydrolysed?
10. Write the IUPAC name of
11.Write the chemical reaction in which iodide ion replaces diazonium group in a diazonium salt.
12. Write the IUPAC name of
TWO MARK QUESTIONS
1.Account for the following
i)The C-Cl bond length in chlorobenzene is less than that in CH3Cl
ii)Chloroform is stored in closed dark color bottles.
2.Complete the following reactions
3. Write the mechanism of the following reaction
4.Give reason for the following
i)The order of reactivity of haloalkanes is RI>RBr>RCl
ii)Neopentyl chloride ,(CH3)3C-CH3Cl does not follow SN2 mechanism
5.Complete the following ractions
6.Discuss the mechanism of SN1 mechanism of haloalkanes.
THREE MARK QUESTIONS
1. i)Draw the structure of major monohalo product in each of the following cases
ii) Which of the following would you expect to react faster by SN2 mechanism
a)CH3Br or CH3I
b) (CH3)3CCl or CH3Cl
2. Account for the following
i)Ethyl iodide undergoes SN2 reaction faster than ethyl bromide.
ii)
iii) The C--X bond length in halobenzene is less than that in CH3-X
3. Although chlorine is an electron withdrawing group,yet it is ortho,para directing in electrophilic
aromatic substitution reaction.Explain why?
4. Answer the following
i)Haloalkanes easily dissolve in organic solvents .Why?
ii)What is meant by a racemic mixture?Give an example.
iii)Of the two bromo derivatives C6H5CH(CH3)Br and (C6H5)CH(C6H5)Br,which one is more
reactive in SN1 substitution and why?
5.Rearrange the following in order of reactivity towards SN2 reaction
i)2-Bromo-2-methylbutane , 1-Bromopentane , 2-Bromopentane
ii) 1-Bromo-3-methylbutane , 2-Bromo-2-methylpropane , 3-Bromo-2-methylbutane
iii) 1-Bromobutane , 1-Bromo-2,2-Dimethylpropane , 1-Bromo-2-methylbutane ,
1-Bromo-3-methylbutane
6. i)Write the mechanism of the following reaction
ii)Why is the dipole moment of chlorobenzene lower than that of cyclohexylchloride
7. i)Write a chemical test to distinguish between
a)chlorobenzene and benzyl chloride
b)Chloroform and carbon tetrachloride
ii) why is methyl chloride hydrolised more easily than chlorobenzene?
8.Complete the following reaction
9.i)State one use each of DDT and iodoform
ii) Which of the following would you expect to react faster by SN2 mechanism and why
a) 1-Bromopentane , 2-Bromopentane
b) 1-Bromo-2-methylbutane , 2-Bromo-2-methylbutane
CHAPTER -11 ALCOHOLS,PHENOLS & ETHERS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1.
2.
3.
4.
5.
6.
How would you distinguish between propan-1-ol & propan-2-ol ?
Write down the mechanism of dehydration of ethanol to ethene.
Write down reaction representing Reimer - Tiemann Reaction
How would distinguish between PhOH & PhCH2OH ?
Write down the mechanism of dehydration of ethanol to diethylether.
Arrange pentan-1-ol, n-butane, pentanal, & ethoxyethane in the increasing order of
their boiling points with reason.
7. Write down reaction representing Kolbe’s Reaction & preparation of aspirin.
8. Why C-OH bond length in phenol is shorter than that in alcohols?
9
10
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1. Write down the IUPAC name of Me3CCH2OH & EtOPh
2. Arrange phenol, para-nitrophenol & para-cresol in the increasing order of their pka values,
along with reason.
3. Complete the reaction : ? + ? → Me3COMe
PhCH2OPh + HI → ? + ?
4. How would you convert phenol to acetophenone & methanol to anisole?
5. Write down the IUPAC names of PhCH=CHC(Me2)OH & MeO-isoPr
6. Complete the reaction PhOH + O2 → ?
Me3COH + Cu (573K) → ?
7. How would you convert cumene to phenol & acetaldehyde to iso-propylalcohol?
8.
9
CHAPTER -12 ALDEHYDES,KETONES & ACIDS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1
2
3
4
5
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
6
7
8
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.
9
Give chemical tests to distinguish between:
(i) Acetaldehyde and benzaldehyde
(ii) Propanone and propanol.
10
(a) Illustrate the following name reactions:
(i) Hell–Volhard–Zelinsky reaction
(ii) Wolff–Kishner reduction reaction
. W Which acid of each pair shown here would you expect to be stronger ?
11
(i) CH2CO2H or FCH2CO2H
(ii) FCH2CO2H or ClCH2CO2H
(iii) FCH2CH2CH2CO2H or CH3 —CHF — CH2CO2H
(iv) F3C—
—COOH or H3C— —COOH
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1
2
3
4
5
6
7
. (a) An organic compound contains 69.77% carbon, 11.63% hydrogen and the rest is
oxygen. Themolecular 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 the organic compound.
(b) State reasons for the following:
(i) Monochloroethanoic acid has a higher pKavalue than dichloroethanoic acid.
(ii) Ethanoic acid is a weaker acid than benzoic acid.
How will you convert cyclohexanol into cyclohexanone?
How will you convert Ethyl benzene into Benzoic acid?
Arrange
8 the following carbonyl compounds in increasing order of their reactivity in nucleophilic
addition reactions.
(i) Ethanal, Propanal, Propanone, Butanone
(ii) Benzalidehyde, p-Tolualdehyde, p-Nitrobenzaldehyde, Acetophenone.
G 9 Give names of the reagents to bring about the following transformation.
(i) Hexan-1-ol to hexanal,
(ii) cyclohexanol to cyclohexanone
(iii) p-Fluorotoluene to p-fluorobenzaldehyde,
(iv) Ethanenitrile to ethanol,
(v) Allyl alcohol to propenal, and (vi) But-2-ene to ethanol.
CHAPTER -13 AMINES
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
ONE MARK QUESTIONS
1 Arrange the following compounds in an increasing order of their solubility in water.
C6H5NH2, (C2H5)2NH , C2H5NH2
2 Which of the two is more basic and why ?
Aniline and p-Methylaniline
3 Which of the two is more basic and why ?
CH3NH2 or NH3
4 Which of the two is more basic and why ?
CH3NH2 or aniline
5 Arrange in Increasing order of basic strength.
C6H5NH2 ,C6H5NHCH3, C6H5 CH2NH2
6 Arrange in increasing order of basic strength in aqueous solution.
NH3,CH3NH2,(CH3)2NH,(CH3)3N
7 Draw the structure of prop-2-en-1-amine
8 Draw the structure of N-Methylethanamine.
10 draw the structure of2-Aminotoluene
11 Write the IUPAC name.
12 Arrange in decreasing order of basic strength in aqueous solution.
NH3,CH3NH2,(CH3)2NH,(CH3)3N
13 Write one reaction that can be used as a test of primary amines.
14 Give a chemical test to distinguish between ethylamine and aniline.
15 Give a chemical test to distinguish between N-methyl aniline and aniline.
16 Why electrophylic substitution takes place more readily in aromatic amines than benzene?
17 Why does NH3 acts as a Lewis base?
TWO MARK QUESTIONS
1. (i) Arrange the following compounds in increasing order of their basic strength:
C6H5NH2,C6H5N(CH3)2,(C2H5)2NH and CH3NH2
(ii) ) Arrange the following compounds in decreasing order of pkb values:
C2H5NH2, C6H5NHCH3, (C2H5)2NH and C6H5NH2.
2 . Give a chemical test to distinguish between :
(i)
Ehylamine and Aniline.
(ii)
Aniline and Benzylamine.
3. Explain the following reactions :
(i)
Gabriel pthalimide reaction.
(ii)
Coupling reaction.
4. Give a chemical test to distinguish between :
(i)
Ethylamine and Aniline.
(ii)
Ethylamine and dimethylamine.
5 .Describe the following giving the relevant chemical equation in each case:
(i)
Carbylamine reaction.
(ii)
Hofmann bromamide reaction.
6. How will you convert :
(i) nitrobenzene into aniline?
(ii) aniline to iodobenzene ?
7. Illustrate the following with an example of reaction in each case :
(i) Sandmeyer’s reaction.
(ii) Coupling reaction.
8. How will you convert :
(i) nitrobenzene into phenol ?
(ii) aniline to chlorobenzene ?
9 . How will you convert :
i) Methylamine to iodometane ?
(ii) Chlorobenzene to p- chloroaniline ?
10 .Write equation for
i) Gabriel phthalimide synthesis
ii)Hoffman bromamide reaction
11. Give a chemical test to distinguish between :
(i)
Aniline and N- methylaniline
ii)Ethylamine and dimethylamine.
12.Illustrate the following
i)Acetylation
ii) Gabriel phthalimide synthesis
13. Assign reason
i)Amine are less acidic than alcohols of comparable molecular masses
ii)Aliphatic amines are stronger bases than aromatic amines
14.Convert the following
i)Aniline to nitrobenzene
ii)Ethanamine to N-ethyl ethanamide
THREE MARK QUETIONS
15. Idenitify A,B and C in the following
i)CH3Br
KCN
ii)CH3COOH
--- A (LAH)-- B
NH3,∆
HNO2/273K--- C
--A ---- Br2,KOH---
16.How will you convert
i)Nitrobenzene to aniline
ii)Ethanoic acid to Methanamine
iii)Aniline to N-phenylethanamide
16.Accout for the following
i) aniline does not undergo Friedel Craft reaction
ii)Ethyl amine is soluble in water but aniline is not
iii)pKb of methyl amine is less than that of aniline
B CHCl3,NaOH-----C
17. Complete the
following reactions
18.Write the main products of the following
19.State reason
i)pKb of aniline is more than that of methyl amine
ii) Ethyl amine is soluble in water but aniline is not
iii)Primary amines have higher B.P. than tertiary amines
20. Give chemical test to distinguish between
i)Methylamine and dimethylamine.
i) Aniline and Benzylamine
iii) Ethylamine and aniline
21. Complete the following equations :
i)
C6H5N2Cl + C6H5NH2

ii) C6H5N2Cl + CH3CH2OH

iii) RNH2 + CHCl3 + KOH

22.Give example to describe the following
i)Hoffman Bromamide
ii)coupling reaction
iii)Gatterman reaction
23. Complete the following equations :
C6H5NH2 + CH3COCl

ii) C6H5NH2 + C6H5SO2Cl

i)
iii) C6H5NH2 + HNO2

24.Carry out the following conversions
i) Benzene dizonium chloride to Nitrobenzene
ii)Aniline to Benzene diazonium chloride
iii)Ethylamine to methylamine
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
ONE MARK QUESTIONS
1 Out of CH3NH2 and (CH3)3N, which one has higher boiling point ?
2. Write the IUPAC
name.
3. Rearrange the following in an increasing order of their basic strength.
C6H5NH2,C6H5N(CH3)2,(C2H5)2NH and CH3NH2
4. Write the IUPAC name.NH2CH2CH2CH=CH2
5. Write a chemical equation to illustrate the ammonolysis reaction.
6 Rearrange the following compounds in increasing order of their basic strength:
Aniline,p-nitroaninline and p-toulidine.
7. Write a chemical reaction in which iodide ion displaces diazonium group from a diazonium salt.
8. Account metyl amine in water reacts with ferric chloride to give a precipitate of with ferric
hydroxide.
TWO MARK QUESTIONS
1. Complete the following equations :
(i)
C6H5N2Cl + H3PO2 + H2O
(ii) C6H5NH2. + Br2 (aq)


2. Account for the following :
(i) diazomium salts ofaromatic amines are more stable than those of aliphatic amines.
(ii) Amines are more basic than alcohols of comparable molecular masses.
3. . How will you convert :
i) Ethylamine to ethanoic acid ?
(ii) aniline to benzonitrile ?
4.i)Why aniline does not undergo Friedel Craft reaction?
ii)Why can pimary aromatic amines not be prepared by Gabriel phthalimide synthesis?
5.Idenitify A and B in the following
i)CH3CH2l
ii)C6H5NH2
NaCN
--- A (reduction Ni/H2 )-- B
NaNO2/HCl --A ---- C6H5NH2/OH---
B
6.Arrange the following
C6H5NH2 ,(C2H5)2NH, C2H5NH2, ,(C2H5)3N
i)in increasing order of basic strength in water
ii) in increasing order of basic strength in gas phase
7.Write the reaction and reaction conditions for the following conversions
i)benzene dizonium chloride to nitrobenzene
ii)Aniline to benzene dizonium chloride
THREE MARK QUETIONS
1.Accout for the following
i)Primary amines have higher B.P. than tertiary amines
ii) aniline does not undergo Friedel Craft reaction
iii),(CH3)2NH is more basic than (CH3)3N in an aquous medium
OR
Idenitify A,B and C in the following
i) C6H5NO2
ii)CH3CN
Sn + HCl
H2O,H+
----A
- A
NaNO2/HCl
NH3,∆
--B
H2O
--
C
--B ---- Br2,KOH---
C
2.Write the main products of the following
3. . Idenitify A,B and C in the following
i) C6H5NO2
Sn + HCl
----A
NaNO2/HCl
--B
ii) C6H5N2+Cl- ----CuCN- AH2O,H+- B
H2O
--
NH3,∆
4.Write equations for the following conversions
i)Nitrobenzene to benzoic acid
ii)Benzyl chloride to 2-phenylethanamine
iii)Aniline to benzyl chloride
--
C
C
5.Complete the following
i)RCONH2 -----LiAlH4,H2O-
ii)
C6H5N2Cl + H3PO2 + H2O
iii) C6H5NH2. + Br2 (aq)


6.a)Write one chemical reaction for each
i)carbylamines reaction
ii)Acetylation reaction
b)Write structure of N,N- ethylmethylethanamide
7.How will you carry out the following conversions
i) Aniline to Nitrobenzene to benzoic acid
ii) ethanamine to N-Ethylethanamide
iii)Chloroethane to propan-1-amine
CHAPTER -14 BIOMOLECULES
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1. Define the following terms in relation to proteins:
(i) Peptide linkage (ii) Denaturation (iii) Primary structure
2. Explain what is meant by
(i)a glycosidic linkage (ii) Invert sugar (iii) Polypeptides
3. Name the products of hydrolysis of sucrose. Why is sucrose not a reducing
sugar?
4. List the reactions of glucose which cannot be explained by its open chain
structure.
5. Write the differences between (i) DNA and RNA(ii) α-form of glucose and βform of glucose.
6. Name two water soluble vitamins, state their sources and the diseases caused
due to their deficiency in diet.
7. Draw the pyranose structure of αD(+) glucose.
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1. What are essential and non-essential amino acids in human food? Give one
example of each type.
2. What are disaccharides? Give an example.
3. Name two fat soluble vitamins, their sources and the diseases caused due to
their deficiency in diet.
4. What are three types of RNA molecules which perform different functions?
5. Differentiate between (i) amilose and amilopectin (ii) Globular and fibrous proteins
(iii) α-helix and β- pleated sheet structures of proteins.
6.
What happens when glucose is reacted with (i) HI (ii) Br 2 water (iii) HNO3
7. Amino acids may be acidic, alkaline or neutral. How does this happen?
8. Define:- (i) Secondary structure of proteins (ii) Phosphodiesteric linkage.
9. 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.
CHAPTER -15 POLYMERS
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1. Write the names and structure of the monomers of the following polymers:
(i) Buna-S (ii) Neoprene (iii) Nylon-6
2. Differentiate between molecular structures and behaviours of thermoplastic and
thermosetting polymers. Give one example of each type.
3. What is a biodegradable polymer? Give an example of a biodegradable aliphatic
polyester.
4. What does ‘6, 6’ indicate in the name nylon-6,6?
5. Write the names and structure of the monomers of the following polymers:
(i) PVC(ii) Polypropene (iii) Teflon
6. Write the names and structure of the monomers of the following polymers:
(i) Bakelite (ii) Polythene.(iii) Nylon-6, 6
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1. Define the term ‘polymerisation’
2. Give an example of elastomers.
3.What is the repeating unit in the condensation polymer obtained by combining
HO2CCH2CH2CO2H (succinic acid) and H2NCH2CH2NH2 (ethylene diamine).
4.Give one example each of
(i) addition polymers, (ii) condensation polymers,(iii) copolymers
5. 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?
6. Mention two important uses of each of the following:
(i) Bakelite(ii) Nylon-6
7. Is –(CH2—CH)– n a homopolymer or a copolymer?
|
Cl
8.Write the names and structures of the monomers of the following polymers :
(i)
Glyptal (ii) PHBV
9. 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. To
make the awareness more impactful, they organised rally by joining hands with
other schools and distributed paper bags to vegetable vendors, shopkeepers and
departmental stores. All students pledged not to use polythene bags in future to save
Yamuna River.
After reading the above passage, answer the following questions:
(i) What values are shown by the students?
(ii) What are biodegradable polymers? Give one example.
(iii) Is polythene a condensation or an addition polymer?
Which of the following is a natural polymer?
Buna-S, Proteins, PVC
Write the name of monomers used for getting the following polymers:
(i) Bakelite (ii) Neoprene
CHAPTER -16 CHEMISTRY IN EVERYDAY LIFE
CATEGORY-I QUESTIONS REPEATED AT LEAST 3 OR MORE TIMES
1. Explain the following types of substance with one suitable example, for each
case: (i) Cationic detergents (ii) Food preservatives (iii) Analgesics
2. How do antiseptics differ from disinfectants? Name a substance that can be used
as an antiseptic as well as a disinfectant.
3. Why is use of aspartame limited to cold foods and soft drinks?
4. Why is bithional added to soap?
5. What class of drug is Ranitidine?
6. Explain the following types of substance with one suitable example, for each
case: (i) Non-ionic detergents (ii)Disinfectants (iii) ) Antacids
Explain the following types of substance with one suitable example, for each case: (i) )
Tranquillisers (ii) antiseptics (iii) antibiotics.
CATEGORY –II QUESTIONS REPEATED ONCE OR TWICE
1. What are biodegradable and non-biodegradable detergents? Give one
example of each class.
2. Name a substance that can be used as an antiseptic as well as a disinfectant.
3. What is understood by ‘chemotherapy’?
4. 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
5. If water contains dissolved Ca2+ ions, out of soaps and synthetic
detergents, which will you use for cleaning clothes?
Which of the following is an antiseptic?
0.2% phenol, 1% phenol.
6. On the occasion of World Health Day, Dr. Satpal organised a ‘health camp’ for the poor
farmers living in a nearby village. After check-up, he was shocked to see that most of the farmers
suffered from cancer due to regular exposure to pesticides and many were diabetic. They
distributed free medicines to them. Dr. Satpal immediately reported the matter to the National
Human Rights Commission (NHRC). On the suggestions of NHRC, the government decided to
provide medical care, financial assistance, setting up of super-speciality hospitals for treatment
and prevention of the deadly disease in the affected villages all over India.
(i) Write the values shown by (a) Dr. Satpal (b) NHRC
(ii) What type of analgesics are chiefly used for the relief of pains of terminal cancer?
(iii) Give an example of artificial sweetener that could have been recommended to diabetic
patients.
7. Mr. Roy, the principal of one reputed school organized a seminar in which he invited parents
and principals to discuss the serious issue of diabetes and depression in students. They all resolved
this issue by strictly banning junk food in schools and introducing healthy snacks and drinks like
soup, lassi, milk, etc. in school canteens. They also decided to make compulsory half an hour of
daily physical activities for the students in the morning assembly. After six months, Mr. Roy
conducted the health survey in most of the schools and discovered a tremendous improvement in
the health of the students.
After reading the above passage, answer the following questions :
(i) What are the values (at least two) displayed by Mr. Roy ?
(ii) As a student, how can you spread awareness about this issue ?
(iii) What are tranquilizers ? Give an example.
(iv) Why is use of aspartame limited to cold foods and drinks ?