🧪 NCERT Class 11 MCQ Quiz Hub

1. Approximate atomic weight of an element is 26.89. If its equivalent weight is 8.9, the exact atomic weight of element would be
26.89
8.9
17.8
26.7

2. The number of moles present in 6 gms of carbon is:
2
0.5
5
1

3. What is the concentration of nitrate ions if equal volumes of 0.1 M AgNO3 and 0.1 M NaCl are mixed together
0.1 N
0.2 M
0.05 M
0.25 M

4. The -ve charged particles is called:
Anion
Cation
Radical
Atom

5. Which is not a unit of pressure:
Bar
N/m²
Kg/m²
Torr

6. What is the normality of a 1 M solution of H3PO4
0.5 N
1.0 N
2.0 N
3.0 N

7. The total number of ions present in 111 g of CaCl2 is
One Mole
Two Mole
Three Mole
Four Mole

8. Which of the following weighs the most?
One g – atom of nitrogen
One mole of water
One mole of sodium
One molecule of H2SO4

9. Under similar conditions of pressure and temperature, 40 ml of slightly moist hydrogen chloride gas is mixed with 20 ml of ammonia gas, the final volume of gas at the same temperature and pressure will be
100 ml
20 ml
40 ml
60 ml

10. An organic compound contains carbon , hydrogen and oxygen. Its elemental analysis gave C, 38.71% and H, 9.67%. The empirical formula of the compound would be
CHO
CH4O
CH3O
CHOC

11. Which of the following cannot give iodometric titrations
Fe3+
Cu2+
Pb2+
Ag+

12. What is the concentration of nitrate ions if equal volumes of 0.1 MAgNO3 and 0.1 M NaCl are mixed together
0.1 M
0.2 M
0.05 M
0.25 M

13. The number of moles present in 6 gms of carbon is:
2
0.5
5

14. The number of moles present in 6 gms of carbon is:
2
0.5
5

15. The number of moles present in 6 gms of carbon is:
2
0.5
5
1

16. Which of the following contains same number of carbon atoms as are in 6.0 g of carbon (C – 12)?
6.0 g Ethane
8.0 g Methane
21.0 g Propane
28.0 g CO

17. The significant figures in 3400 are
2
5
6
4

18. A symbol not only represents the name of the element but also represents
Atomic Mass
Atomic Number
Atomicity
Atomic Volume

19. What is the normality of a 1 M solution of H3PO4
0.5 N
1.0 N
2.0 N
3.0 N

20. The sulphate of a metal M contains 9.87% of M. This sulphate is isomorphous with ZnSO4.7H2O. The atomic weight of M is
40.3
36.3
24.3
11.3

21. The S.I unit of temperature is :
Kelvin
Celsius
Fahrenheit
Centigrade

22. The increasing order (lowest first) for the values of e/m (charge/mass) for
e, p, n, α
n, p, e, α
n, p, α, e
n, α, p, e

23. The ionization enthalpy of hydrogen atom is 1.312 × 106 J mol-1. The energy required to excite the electron in the atom from n = 1 to n = 2 is
8.51 × 105 J mol-1
6.56 × 105 J mol-1
7.56 × 105 J mol-1
9.84 × 105 J mol-1

24. or a given principal level n = 4, the energy of its subshells is in the order
s < p < d < f
s > p > d > f
s < p < f < d
f < p < d < s

25. A gas absorbs a photon of 355 nm and emits at two wavelengths. If one of the emissions is at 680 nm, the other is at:
518 nm
1035 nm
325 nm
743 nm

26. Which of the following statements in relation to the hydrogen atom is correct?
3s orbital is lower in energy than 3p orbital
3p orbital is lower in energy than 3d orbital
3s and 3p orbitals are of lower energy than 3d orbital
3s, 3p and 3d orbitals all have the same energy

27. The magnetic quantum number specifies
Size of orbitals
Shape of orbitals
Orientation of orbitals
Nuclear Stability

28. The electronic configuration of silver atom in ground state is
[Kr]3d104s1
[Xe]4f145d106s1
[Kr]4d105s1
[Kr]4d95s2

29. Which of the following element has least number of electrons in its M-shell?
K
Mn
Ni
Sc

30. Which one of the following sets of ions represents a collection of isoelectronic species? (Atomic nos.: F = 9, Cl = 17, Na = 11, Mg = 12, Al = 13, K = 19, Ca = 20, Sc = 21)
K+, Ca2+, Sc3+, Cl–
Na+, Ca2+ , Sc3+, F–
K+, Cl–, Mg2+, Sc3+
Na+, Mg2+, Al3+, Cl–

31. In the ground state, an element has 13 electrons in its M-shell. The element is_____.
Copper
Chromium
Nickel
Iron

32. The electrons of the same orbitals can be distinguished by
Principal quantum number
Azimuthal quantum number
Spin quantum number
Magnetic quantum number

33. Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers, l = 1 and 2 are, respectively:
12 and 4
12 and 5
16 and 4
16 and 5

34. A body of mass 10 mg is moving with a velocity of 100 ms-1. The wavelength of de-Broglie wave associated with it would be (Note: h = 6.63 × 10-34 Js)
6.63 × 10-37 m
6.63 × 10-31 m
6.63 × 10-34 m
6.63 × 10-35 m

35. The ionization enthalpy of hydrogen atom is 1.312 × 106 J mol-1. The energy required to excite the electron in the atom from n = 1 to n = 2 is
8.51 × 105 J mol-1
6.56 × 105 J mol-1
7.56 × 105 J mol-1
9.84 × 105 J mol-1

36. In Hydrogen atom, energy of first excited state is – 3.4 eV. Then find out KE of same orbit of Hydrogen atom
3.4 eV
6.8 eV
-13.6 eV
+13.6 eV

37. Which of the following sets of quantum numbers represents the highest energy of an atom?
n = 3, l = 0, m = 0, s = + 12
n = 3, l = 1, m = 1, s = + 12
n = 3, l = 2, m = 1, s = + 12
n = 4, l = 0, m = 0, s = + 12

38. In the Bohrs model of the hydrogen atom, the ratio of the kinetic energy to the total energy of the electron in a quantum state n is:
1
2
-1
-2

39. Which of the following statements does not form a part of Bohrs model of hydrogen atom?
Energy of the electrons in the orbit is quantised
The electron in the orbit nearest the nucleus has the lowest energy
Electrons revolve in different orbits around the nucleus
The position and velocity of the electrons in the orbit cannot be determined simultaneously

40. Which of the following statements in relation to the hydrogen atom is correct?
3s orbital is lower in energy than 3p orbital
3s, 3p and 3d orbitals all have the same energy
s and 3p orbitals are of lower energy than 3d orbital3
3s, 3p and 3d orbitals all have the same energy

41. A sub-shell with n = 6 , l = 2 can accommodate a maximum of
12 electrons
36 electrons
10 electrons
72 electrons

42. The chemistry of lithium is very similar to that of magnesium even though they are placed in different groups. Its reason is:
Both are found together in nature
Both have nearly the same size
Both have similar electronic configuration
The ratio of their charge and size (i.e. charge density) is nearly the same

43. The element with atomic number 35 belongs to
d – Block
f – Block
p – Block
s – Block

44. The correct order of first ionization potential among following elements, Be, B, C, N and O is
B < Be < C < O < N
B < Be < C < N < O
Be < B < C < N < O
Be < B < C < O < N

45. Representative elements are those which belong to
p and d – Block
s and d – Block
s and p – Block
s and f – Block

46. Which of the following properties generally decreases along a period?
Ionization Energy
Metallic Character
Electron Affinity
Valency

47. On the Paulings electronegativity scale the element next to F is
N
Cl
O
Ne

48. The group number, number of valence electrons, and valency of an element with the atomic number 15, respectively, are
16, 5 and 2
15, 5 and 3
16, 6 and 3
15, 6 and 2

49. Which of the following oxides is amphoteric in character?
SnO2
CO2
SiO2
CaO

50. In the modern periodic table, the period indicates the value of:
Atomic Number
Atomic Mass
Principal Quantum Number
Azimuthal Quantum Number

51. In the long form of the periodic table, the valence shell electronic configuration of 5s²5p4 corresponds to the element present in:
Group 16 and period 6
Group 17 and period 6
Group 16 and period 5
Group 17 and period 5

52. Arrange S, O and Se in ascending order of electron affinity
Se < S < O
Se < O < S
S < O < Se
S < Se < O

53. In the modern periodic table , the period indicates the value of:
Atomic Number
Atomic Mass
Principal Quantum Number
Azimuthal Quantum Number

54. The electronic configuration of an element is 1s², 2s² 2p6, 3s² 3p³. What is the atomic number of the element which is just below the above element in the periodic table
31
34
33
49

55. The reduction in atomic size with increase in atomic number is a characteristic of elements of-
d−block
f−block
Radioactive series
High atomic masses

56. The number of elements in the 5th period of the periodic table is
3
9
8
18

57. The electronic configuration of halogen is
ns² np6
ns² np3
ns² np5
ns²

58. Which of the following forms the most stable gaseous negative ion?
F
Cl
Br
I

59. On the Paulings electro negativity scale the element next to F is
N
Cl
O
Ne

60. The element californium belongs to a family of :
Alkali metal family
Actinide series
Alkali earthl family
Lanthanide series

61. Increasing order of electro negativity is
Bi < P < S < Cl
P < Bi < S < Cl
S < Bi < P < Cl
Cl < S < Bi < P

62. The bond length between hybridised carbon atom and other carbon atom is minimum in
Propane
Butane
Propene
Propyne

63. The bond length between hybridised carbon atom and other carbon atom is minimum in
Propane
Butane
Propene
Propyne

64. The number of nodal planes present in s × s antibonding orbitals is
1
2
0
3

65. The hybrid state of sulphur in SO2 molecule is
sp²
sp³
sp
sp³d

66. Which one of the following does not have sp² hybridised carbon?
sp²
sp³
sp
sp³d

67. Which one of the following does not have sp² hybridised carbon?
Acetone
Acetic acid
Acetonitrile
Acetamide

68. Which of the following will have the lowest boiling point?
2-MethylButane
2-MethylPropane
2,2-Dimethylpropane
n-Pentane

69. Among the following the maximum covalent character is shown by the compound
MgCl2
FeCl2
SnCl2
AlCl3

70. Among the following mixtures, dipole-dipole as the major interaction, is present in
benzene and ethanol
KCl and water
acetonitrile and acetone
benzene and carbon tetrachloride

71. The value of n in the molecular formula BenAl2Si6O18 is
3
5
7
9

72. Which of the following types of hybridisation leads to three dimensional geometry of bonds around the carbon atom?
sp
sp²
sp³
None of these

73. An atom of an element A has three electrons in its outermost orbit and that of B has six electrons in its outermost orbit. The formula of the compound between these two will be
A3B6
A2B3
A3B2
A2B

74. The maximum number of hydrogen bonds that a molecule of water can have is
1
2
3
4

75. The number of types of bonds between two carbon atoms in calcium carbide is
Two sigma, two pi
One sigma, two pi
One sigma, one pi
Two sigma, one pi

76. Based on lattice enthalpy and other considerations which one the following alkali metals chlorides is expected to have the higher melting point?
RbCl
KCl
NaCl
LiCl

77. Dipole-induced dipole interactions are present in which of the following pairs?
H2O and alcohol
Cl2 and CCl4
HCl and He atoms
SiF4 and He atoms

78. The structure of IF7 is
Pentagonal bipyramid
Square pyramid
Trigonal bipyramid
Octahedral

79. The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing order of the polarizing power of the cationic species, K+,Ca++, Mg2+, Be2+?
Ca2+ < Mg2+ < Be+ < K+
Mg2+ < Be2+ < K+ < Ca2+
Be2+ < K+ < Ca2+ < Mg2+
K+ < Ca2+ < Mg2+ < Be2+

80. The species having pyramidal shape is
SO3
BrF3
SiO32-
OSF2

81. The outer orbitals of C in ethene molecule can be considered to be hybridized to give three equivalent sp² orbitals. The total number of sigma (s) and pi (p) bonds in ethene molecule is
1 sigma (s) and 2 pi (p) bonds
3 sigma (s) and 2 pi (p) bonds
4 sigma (s) and 1 pi (p) bonds
5 sigma (s) and 1 pi (p) bonds

82. Which of the following is a linear molecule?
ClO2
CO2
NO2
SO2

83. The vapour pressure of water at 300 K in a closed container is 0.4 atm. If the volume of container is doubled, its vapour pressure at 300 K will be
0.8 atm
0.2 atm
0.4 atm
0.6 atm

84. Name the liquid with higher vapour pressure in the following pairs:(a) Alcohol, glycerine (b) Petrol, kerosene (c) mercury, water.
Alcohol, Water, Petrol
Petrol, Water, Alcohol
Alcohol, Petrol, Water
None of these

85. The rate of diffusion methane is twice that of X. The molecular mass of X is
64.0
32.0
40
80