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CHEMISTRY
11TH STD.
REVISION SHEET
SEM – 2
1. (a) What is the mass of (i) 1 mole of water (ii) 0.5 mole of CO2 (iii) 2.5 moles of Cl2 ?
(b) How many moles of atoms are contained in : (i) 9.0 g of aluminium (ii) 0.8 g of Iron ?
2. What is the mass in grams of : (i) 6.022  1023 atoms of oxygen ? (ii) 1.0  1023 molecules of H2S ? (iii)
6.022  1023 molecules of oxygen ? (iv) 1.5 moles of H2SO4 ?
3. Calculate the mass of Na2CO3 which will have the same number of molecules as contained in 12.3 g
of MgSO4.7 H2O.
4. What is the mass of carbon present in 0.5 mole of K4 [Fe(CN)6] ?
5. How many molecules approximately do you expect to be present in (i) a small sugar crystal which
weighs 10 mg (ii) one drop of water with 0.05 cc volume ?
6. A sample of NaOH weighing 0.40 g is dissolved in water and the solution is made to 50.0 cm3 in
volumetric flask. What is the molarity of the resulting solution ?
7. Concentrated aqueous sulphuric acid is 98% H2SO4 by mass and has a density of 1.84 g cm-3. What
volume of the concentrated acid is required to make 5.0 litre of 0.500 M H2SO4 solution ?
8. Calculate the percentage of (i) SO42- (ii) H2O in pure crystals of Mohr salt, viz., FeSO4 .
(NH4)2SO4.6H2O.
9. A salt containing water of crystallization gave the following percentage composition :
Mg = 9.76; S = 13.01; O = 26.01 and H2P = 51.22.
10. A chemical compound is found to have the following composition :
C = 19.57% ; Fe = 15.2% N = 22.83%; K = 42.39%
Calculate the empirical formula of the compound. What will be its molecular formula if the
molecular mass of the compound is 368?
11. What mass of slaked lime would be required to decompose completely 4 grams of ammonium
chloride and what would be the mass of each product ? Ca(OH)2 + NH4Cl  CaCl2 + NH3 + H2O.
12. How many moles of methane are required to produce 22g CO2(g) after combustion ?
13. Calculate the mass of iron which will be converted into its oxide (Fe3O4) by the action of 18 g of
steam on it.
14. Give examples of homogeneous mixtures in different physical states (two each).
15. Define element, compound and mixture.
16. Give three main points of difference between a compound and a mixture.
17. Copper oxide obtained by heating copper carbonate or copper nitrate contains copper and oxygen in
the same ratio by mass. Which law is illustrated by this observation ? state the law.
18. Nitrogen forms a number of oxides. Write their formulae and give their names. Giving appropriate
calculations, explain the law that follows from it.
19. N and O combine with H to form NH3 and H2O and they combine with each other to form NO2.
Which law is illustrated ? Explain briefly.
20. What are the postulates of Dalton’s Atomic theory ? How do the laws of chemical combination
follow from it ?
21. What isotope is used as a reference on the atomic scales ? what is one amu or one ‘u’?
22. Why atomic mass is an average value ? Explain with a suitable example.
23. How is mole related to (a) number of atoms/molecules (b) mass of the substance (c) volume of the
gaseous substance ?
24. Define empirical formula and Molecular formula. What is the relationship between them ?
25. Complete the following table :
Particle
Atomic no.
Mass no.
No. of
No. of protons No. of
electrons
neutrons
Sodium atom
11
12
Aluminium
27
10
ion
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CHEMISTRY
Chloride ion
Phosphorus
atom
Cuprous ion
11TH STD.
REVISION SHEET
SEM – 2
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31
18
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15
18
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28
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35
CH : 2 : SEM : 1
26. Find the number of protons, electrons and neutrons in (a) Al3+ (b)
15
8
O 2 .
27. The elements P (atomic weight 39) and Q (atomic weight 80) contain 20 and 45 neutrons respectively
in their nucleus. Give their electronic arrangements separately.
28. The Vividh Bharati station of All India Ratio, Delhi broadcasts at a frequency of 1368 kHz
(kilohertz). Calculate the wavelength of the electromagnetic radiation emitted by the transmitter.
Which part of the electromagnetic spectrum does it belong to ?
29. The wavelength range of the visible spectrum extends from violet (400 nm) to red (750 nm). Express
these wavelengths in frequencies (Hz) (1 nm = 10-9 m)
30. The threshold frequency v0 for a metal is 7.0  10114 s-1. Calculate the kinetic energy of an electron
emitted when radiation of frequency v = 1.0  1015 s-1 hits this metal.
31. Sodium street lamp gives off a characteristic yellow light of wavelength 588 nm. Calculate the
energy per mole (in kJ/mol) of these protons.
32. Calculate the frequency and the wavelength of the radiation in nanometers emitted when an
electron in the hydrogen atom jumps from third orbit to the ground state. In which region of the
electromagnetic spectrum will this line lie ? (Rydberg constant = 109, 677 cm-1)
33. Calculate the wavelength of the spectral line in Lyman series corresponding to n2 = 3.
34. If the energy difference between two electronic states is 214.68 kJ mol-1 Calculate the frequency of
light emitted when an electron drops from the higher to the lower state. Planck’s constant,
h = 39.79  10-14 kJ sec mol-1.
35. Applying Bohr’s model when electron in H atom comes from n = 4 to n = 2, calculate the wavelength
of the line. In this process, write whether energy is released or absorbed. Also write the range of
radiation (RH = 2.18  10-18 J, h = 6.63  10-34 J)
36. Calculate the momentum of a particle which has a de Broglie wavelength of 1 Å or 0.1 nm. (h = 6.6 
10-34 kg m2 s-1).
37. The kinetic energy of an energy of an electron is 5  10-5 eV (electron volts). Calculate the wavelength
of the wave associated with the electron. The mass of the electron may be taken as 10-30 kg.
38. A tennis ball of mass 6.0  10-2 kg is moving with a speed of 62 ms-1. Calculate the wavelength
associated with this moving tennis ball. Will the movement of this ball exhibit a wave character ?
Explain.
39. Calculate the ration between the wavelength of an electron and a proton if the proton is moving
with half the velocity of electron (Mass of proton = 1.67  10-27 kg and mass of electron = 9.11  10-31
kg)
40. The approximate mass of an electron is 10-27 g. Calculate the uncertainty in its velocity if the
uncertainty in its position were of the order of 10-11 m (h = 6.6 10-34 kg m2 sec-1).
41. Calculate the product of uncertainty in position and velocity for an electron of mass 9.1 10-31 kg
according to Heisenberg uncertainty principle.
42. What is the minimum uncertainty in the position of a bullet of mass 5g that is known to have a
speed somewhere between 5550,00000 and 550,00001 m s-1 ?
43. Write the correct orbital notations for each of the following sets of quantum numbers :
(i) n = 1, l = 0, m = 0; (ii) n = 2, l = 1, m = -1; and (iii) n = 3, l = 2, m = +1
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CHEMISTRY
11TH STD.
REVISION SHEET
SEM – 2
44. Which of the following sets of quantum numbers are not possible ?
(i) n = 3, l = 2, m = 0, s = -1/2
(ii)
n = 3, l = 2, m = -2, s = -1/2
(iii) n = 3, l = 3, m = -3, s = +1/2
(iv)
n = 3, l = 1, m = 0, s = +1/2
45. Which of the following orbitals are not possible ?
7s, 2d, 3f and 1p
46. Give the electronic configurations of : (i) Scandium (at.no.21), and (ii) Chromium (at. No. 24).
47. Write the electronic configurations of the elements : Chlorine and Phosphorus.
48. Give the electronic configurations of the ions : (i) H-1 (ii) Na+ (iii) N-1 (iv) N2+
49. Name the elements that correspond to each of the given electronic configurations. Write down their
atomic numbers also. (i) 1s2 2s2 2p2
(ii) 1s2 2s2 2p6 3s2 3p1 (iii) 1s2 2s2 2p6 3s2 3p6
50. Correct the following electronic configurations of the elements in the ground state :
(i) 1s2 2s1 2px2 2py2 2pz2 3s2 3px1
(ii)
1s2 2s1 2py2 2py2 2pz1
(iii) 1s2 2s2 2p6 3s2 3p6 3d5
(iv)
1s2 2s2 2p6 3s2 3p6 3d4 4s2
51. Which of the following quantum numbers for orbitals in hydrogen atom has a greater energy for
electrons ?
(i) n = 3, l = 2 and m = +1
(ii)
n = 3, l = 2 and m = -1
52. How can you say that electron is a universal constituent of all atoms ?
53. Give experiments to show that (i) Cathode rays carry negative charge (ii) Cathode rays consist of
material particles.
54. How was proton discovered ?
55. How can you say that nucleus is small in size but heavy in mass ?
56. Define wavelength, frequency, wave number and velocity of a wave. How are they inter-related ?
57. What is Planck’s Quantum Theory ?
58. Explain the dual character of light radiations.
59. How is the atomic spectra of hydrogen obtained ? what are the different series of lines present in it ?
In which regions do they lie ?
60. What is Rydberg formula ? How does it help to calculate the wave numbers of different series of
lines of the hydrogen spectra ?
61. What was the drawback of Rutherford’s model of atom ?
62. How does Bohr model explain the line spectrum of hydrogen ?
63. Outline the weaknesses of Bohr’s model of atom.
64. State de Broglie relationship. For what purpose is it used ?
65. Derive de Broglie equation for microscopic particles.
66. State Heisenberg’s uncertainty principle. Give its mathematical expression >
67. Explain why it is impossible to measure simultaneously the position and the velocity of a fast
moving small body like an electron.
68. How are the quantum numbers related to each other ?
69. Define pauli exclusion principle. Why it is called exclusion principle ?
70. In an atom, the first shell may contain upto 2 electrons, the second shell upto 8 the third upto 18 and
the fourth shell upto 32 electrons. Explain this arrangement in terms of quantum numbers.
71. Draw the shapes of d-orbitals.
72. State and explain ‘’aufbau principle’.
73. State Hund’s rule and its importance in filling the orbitals in various energy levels; take atomic
number 17 as an example.
74. State Hund’s rule of maximum multiplicity. How is it used for the distribution of electrons in
nitrogen (At. No. 7) and fluorine (At.no. 9) atoms ?
75. Write the sequence in which electrons fill the various energy sub-shells in an unexcited atom.
76. Why do some atoms possess exceptional electrtonic configuration ? Explain with suitable example.
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CHEMISTRY
11TH STD.
REVISION SHEET
SEM – 2
77. Write electronic configurations of atoms of Cr (at.no. 24) and Cu (at.no.29). Show the orientations of
electron spins by arrow heads.
78. List the main features of the “quantum mechanical model of atom”.
79. (i) Calculate the number of electrons which will together weigh one gram.
(ii) Calculate the mass and charge of one mole of electrons.
80. (a) The Vividh Bharati station of All India Radio, Delhi broadcasts at a frequency of 1368 kHz
(kilohertz). Calculate the wavelength of the electromagnetic radiation emitted by the transmitter.
Which part of the electromagnetic spectrum does it belong to ?
(b) A 100 watt bulb emits monochromatic light of wavelength 400 nm. Calculate the number of
photons emitted per second by the bulb.
(c) What is the number of photons of light with a wavelength of 4000 pm that provide 1 J energy ?
81. When electromagnetic radiation of wavelength 300 nm falls on the surface of sodium, electrons are
emitted with a kinetic energy of 1.68 × 105 J mol-1. What is the minimum energy needed to remove an
electron from sodium ? what is the maximum wavelength that will cause a photoelectron to be
emitted ?
82. Which of the following relate to wave nature of light or particle nature or both ?
(a) Interference (b) Diffraction
(c)
Photoelectric effect (d) Black body radiation
(e) Planck’s equation, E = hv (f) Einstein equation. E = mc2
83. (a) Which transition between Bohr orbits corresponds to third line in the Balmer series of the
hydrogen spectrum.
(b) To which orbit the electron in the hydrogen atom will jump on absorbing 12.1 Ev of energy ?
84. How much energy is required to ionize a hydrogen atom if the electron occupies n = 5 orbit ?
Compare your answer with the ionization energy of hydrogen atom (energy required to remove the
electron from n = 1orbit)
85. Show that the circumference of the Bohr orbit for hydrogen atom is an integral multiple of the de
Broglie wavelength associated with the electron moving around the orbit.
86. (a) A molecule of O2 and that of SO2 travel with the same velocity. What is the ratio of their
wavelengths ?
(b) The mass of an electron is 9.1 × 10-31 kg. If its K.E. is 3.0 10-25 J, Calculate its wavelength.
CH : 3 : Sem - 1
87. Write the names and atomic numbers of the following elements :
(i) The fourth alkali metal
(ii) The third alkaline earth metal
(iii) The fifth element of the first transition series
(iv) The first inner transition element and
(v) The sixth noble gas.
88. The outer electronic configuration of some elements are given below :
(i) 3s2 3p3 (ii) 3d5 4s1 (iii) 3s2 3p6 4s2 (iv) 5d1 6s2 (v) 4f1 5d1 6s2
State to which block of the periodic table each of these elements belongs.
89. An element ‘X’ with atomic number 112 has recently been discovered. Predict its electronic
configuration and suggest the group in which this element would be placed.
90. Arrange the following elements in the increasing order of metallic character : B, Al, Mg, K.
91. Which one of the following pairs would have a large size ? Explain.
(i) K or K+
(ii)
Br or Br(iii)
O2- or F(iv)
Li+ or Na+
+
2+
(v) P or As
(vi)
Na or Mg
92. Arrange the following in order of increasing radii ?
(i) I, I+, I(ii)
C, N, Si, P
(iii)
O2-, N+3, S2-, F2nd Floor, Rajcastle, Near Kalpataru, Ellora Park, Baroda – 390007 Ph: +91-265-3053166
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CHEMISTRY
11TH STD.
REVISION SHEET
SEM – 2
93. Arrange the following in the order of increasing ionization enthalpy :
(i) 1 s2 2s2 2p6 3s2 (ii)
1s2 2s2 2p6 3s1 (iii)
1s2 2s2 2p6
(iv)
1s2 2s2 2p6
(v)
1s2 2s2
2p3
94. Which of the following pairs of elements would you expect to have lower first ionization enthalpy ?
Explain.
(i) Cl or F
(ii)
Cl or S
(iii) K or Ar
(iv) Kr or Xe.
95. Arrange the elements with the following electronic configuration in order of increasing electron gain
enthalpy.
(i) 1s2 2s2 2p5
(ii)
1s2+ 2s2 2p4
(iii)
1s2 2s2 2p3
(iv)
1s2 2s2 2p6 2s2 3p4
96. The electron gain enthalpies of halogens decrease in the order F > Cl > Br > I. Comment upon the
statement.
97. State the modern periodic law. What are the main features of the long form of the periodic table ?
98. Explain briefly ‘Groups’ and ‘periods’. ‘Transition’ and ‘normal’ elements in the long form of the
periodic table.
99. On the basis of electronic configurations, justify that the second and third periods contains 8
elements each, 4th and 5th periods contain 18 elements each and 6th period contains 32 elements.
100. Elements A, B, C and D have atomic numbers 12, 19, 29 and 36 respectively. On the basis of
electronic configuration write to which group of the periodic table each element belongs.
101. Name the four blocks into which the elements of the periodic table has been classified. Why are
they named so ? List the groups of periodic table belonging to each block.
102. What do you understand by ‘Representative elements’ ? Name the groups whose elements are
called representative elements.
103. What are the transition elements ? why are they so called ? Name the different transition series.
104. Which elements are called inner transition elements ? Name the different inner transition series.
Why are they so named ?
105. Describe the main characteristics of s, p, d and f-block elements.
106. Name different blocks of elements in the periodic table. Give the general electronic configuration of
each block.
107. What do you understand by periodic properties of elements ? Name any three such properties.
108. What is meant by atomic and ionic radii ? Explain giving reasons why the size of Cl-0 ion is bigger
than that of Cl atom whereas size of Na+ ion is smaller than that of Na Atom ?
109. What do you understand by the term successive ionization enthalpies ? explain why second
ionization enthalpy is always greater than the first ionization enthalpy ?
110. If we consider ionization enthalpies of elements in the second period from Li to Ne, they ordinarily
increase by Be and N have higher ionization ehthalpies than B and O respectively which succeed
them. Why is it so ?
111. Write main points of difference between electronegativity and electron gain enthalpy.
112. The valence of representative elements is either equal to the number of the valence electrons or
eight minus this number. What is the basis of this rule ?
113. Write the general electronic configuration of s-, p-, d- and f-block elements.
114. Considering the atomic number and position in the periodic table, arrange the following elements
in the increasing order of metallic character : Si, Be, Mg, Na, P.
115. How would you explain the fact that the first ionization enthalpy of sodium is lower than that of
magnesium but its second ionization enthalpy is higher than that of magnesium ?
116. Would you expect the second electron gain enthalpy of O as positive, more negative or less
negative than the first ? Justify your answer.
117. Predict the formula of the stable binary compounds that would be formed by the combination of
the following pairs of elements.
(i) Magnesium and nitrogen
(ii)
Silicon and oxygen (iii)
Element 71 and fluorine.
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CHEMISTRY
11TH STD.
REVISION SHEET
SEM – 2
CH : 2 : STATES OF MATTER
118. A certain mass of a gas occupies 39 mL at 760 mm pressure. What volume would it occupy if the
pressure is raised to 780 mm provided that temperature remains constant ?
119. A bulb ‘X’ of unknown volume containing a gas at one atmospheric pressure is connected to an
evacuated bulb of 0.5 litre capacity through a stop-cock. On opening the stop-cock, the pressure in
the whole system after some time was found to have a constant value of 570 mm at the same
temperature. What is the volume of the bulb X ?
120. 300 mL of oxygen gas at - 10C are heated to 10C. what is the new volume if pressure remains
constant ?
121. 25 dm3 of ammonia at 283 K are heated until its volume is 30 dm3. To what temperature must it
have been raised to accomplish the change ?
122. A gas cylinder containing cooking gas can withstand a pressure of 14.9 atmospheres. The pressure
gause of the cylinder indicates 12 atmosphere at 27C. Due to sudden fire in the building, the
temperature starts rising. At what temperature the cylinder will explode ?
123. One litre flask containing vapours of methyl alcohol (Mol mass 32) at a pressure of 1 atm. And 25C
was evacuated till the final pressure was 10-3 mm. How many molecules of methyl alcohol were left
in the flask ?
124. Temperature at the foot of a mountain is 30C and pressure is 760 mm whereas at the top of the
mountain these are 0C and 710 mm. Compare the densities of the air at the foot and at the top of
the mountain.
125. Calculate the number of moles of hydrogen gas present in 500 cm3 of the gas taken at 300K and
760mm pressure. If this sample of hydrogen is found to have a mass equal to 4.09 10-2g, calculate
the molar mass of hydrogen.
126. A large flask fitted with a stop-cock is evacuated and weighed; its mass is found to be 134.567 g. it
is then filled to a pressure of 735 mm at 31C with a gas of unknown molecular mass and then
reweighed; its mass is 137.456 g. the flask is then filled with water and weighed again; its mass is
now 1067.9g assuming that the gas is ideal, calculate the molar mass of the gas.
127. 200 mL of hydrogen and 250mL of nitrogen each measured at 15C and 760 mm pressure are put
together in a 500 mL flask. What will be the final pressure of the mixture at 15C ?
128. Two vessels of capacities 1.5 litres and 2.0 litres containing hydrogen at 750 mm pressure and
oxygen at 100 mm pressure respectively are connected to each other through a valve. What will be
the final pressure of the gaseous mixture assuming that temperature remains constant ?
129. Calculate the molar mass of an unknown gas which diffuses 1.117 times faster than oxygen gas
through the same aperture under the same conditions of temperature and pressure.
130. Uranium isotopes have been separated by taking advantage of the different rates of diffusion of the
two forms of uranium hexafluoride, one containing U-238 isotope and the other containing U-235.
What are the relative rates of diffusion of these two molecules under ideal conditions ?
131. A small quantity of gaseous NH3 and HBr are introduced simultaneously into the opposite ends of
an open tube which is one metre long. Calculate the distance of the white solid NH4Br formed from
the end which was used to introduce NH3.
132. Calculate the pressure exerted by 10.2 g of NH3 in a 3.0 dm3 vessel at 25C (a) using ideal gas
equation (b) using van der walls equation. The van der waals constants are : a = 4.17 dm6 atm mol-2,
b = 0.0371dm3 mol-1.
133. Define Boyle’s law. How is it represented mathematically ?
134. What type of curves are obtained when at constant temperature, we plot
(i) P vs 1/V
(ii)
PV vs P
(iii)
V vs P
135. Define Charles law. Give its mathematical formulae.
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CHEMISTRY
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REVISION SHEET
SEM – 2
136. Define Absolute zero. Can this temperature be attained in actual practice ? Give reason for your
answer.
137. Derive the relationship between pressure, temperature and density of a gas (i.e. M = d RT/P)
138. Define Dalton’s law of partial pressures. Using this law, how is the pressure of dry gas determined?
139. Define Graham’s law of diffusion.
140. What is compressibility factor ? What is its value for ‘an ideal gas’ ? How does it help to understand
the extent of deviation of a gas from ideal behaviour ?
141. Why do real gases show deviation from ideal behaviour ? Write van der Waals equation for n
moles of a gas.
142. What are the units of van der Waals constants ‘a’ and ‘b’ ? what is their significance ?
143. Define vapour pressure, boiling point and heat of vaporization.
144. What is difference between boiling and evaporation ?
145. Explain the effect of temperature on the following :
(i) Surface tension
(ii)
viscosity
(iii)
Vapour pressure
(iv)
Density.
146. Which type of intermolecular forces exist among the following molecules ?
(i) H2S molecules (ii) H2O molecules (iii) Cl2 and CCl4 molecules (iv) SiH4 molecules
(v) Helium atoms (vi) He atoms and HCl molecules.
147. A balloon filled with an ideal gas is taken from the surface of the sea deep to a depth of 100m. what
will be its volume in terms of its original volume ?
148. Through the two ends of a glass tube of length 200 cm, hydrogen chloride gas and ammonia are
allowed to enter. At what distance ammonium chloride will first appear ?
149. (a) what is boyle temperature ?
(b)Compressibility factor, Z of a gas is given as Z =
pV
(i) what is the value of Z for an ideal gas ?
nRT
(ii) for real gas what will be the effect on value of Z above Boyle’s temperature ?
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