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Chemical Bonding MCQ and Answer
1. Sharing or transfer of electrons from one atom to the other to attain stable octet configuration follows _______
a) Duet rule
b) Triplet rule
c) Octet rule
d) Septet rule
Answer: Octet rule
2. Which of the following molecule doesn’t involve covalent bond?
a) H2O
b) CCl4
c) NaCl
d) O2
Answer: NaCl
3. Calculate the formal charge of C in CH4.
a) 4
b) 1
c) -4
d) 0
Answer: 0
4. Which of the following doesn’t follow octet rule?
a) CH4
b) CCl4
c) HCl
d) NO2
Answer: NO2
5. Atoms obtain octet configuration when linked with other atoms. This is said by _________
a) Lewis
b) Kossel
c) Langmuir
d) Sidgwick
Answer: Lewis
6. Find out the correct Lewis symbol for the atom carbon among the following options.
a) .C:
b) :C.
c) :C:
d) .C.
Answer: :C:
7. Ionic bonds easily form when electron when ionization energy of the metallic atom is _____ comparatively.
a) negative
b) constant
c) more
d) less
Answer: less
8. What is the energy that is released upon the formation of an ionic compound known as?
a) Ionization energy
b) Lattice energy
c) Electron gain enthalpy
d) Electropositivity
Answer: Lattice energy
9. What’s the amount of lattice energy of NaCl?
a) 788 KJ mol-1
b) 688 KJ mol-1
c) 588 KJ mol-1
d) 488 KJ mol-1
Answer: 788 KJ mol-1
10. Which of the following molecule’s formation doesn’t include ionic bond?
a) LiCl
b) MgO
c) SnCl4
d) H2O
Answer: H2O
11. Ionic bond formation depends on the arrangement of __________
a) molecule
b) atom
c) lattice
d) kernal
Answer: lattice
12. A chemical bond formation that involves the complete transfer of electrons between atoms is
a) ionic bond
b) covalent bond
c) metallic bond
d) partial covalent bond
Answer: ionic bond
13. Formation of a compound through ionic bond ______ the ionization energy of the metal ion.
a) does not depends on
b) depend on
c) is independent regarding
d) may or may not depend on
Answer: depend on
14. The bond enthalpy of H2O and OH are 502 KJ mol-1 and 427 KKJ mol-1. Then what is the average bond enthalpy?
a) 502 KJ mol-1
b) 464.5 KJ mol-1
c) 427 KJ mol-1
d) 75 KJ mol-1
Answer: b
15. What is the bond order of CO?
a) 3
b) 2
c) 1
d) 4
Answer: a
16. All the __________ species(molecules and ions) have the same bond order.
a) isotopic
b) isoelectronic
c) isobaric
d) isoneutronic
Answer: b
17. Which of the following molecules may have a dipole movement?
a) N2
b) CH4
c) BeF2
d) H2O
Answer: d
18. Which of the following cannot be used to measure bond lengths?
a) Spectroscopy
b) X-ray diffraction
c) Electron diffraction
d) Young’s Double-slit method
Answer: d
19. The covalent radius in a chlorine molecule and van der Waal’s radius between chlorine molecules respectively can be ________ & _________
a) 99pm, 198pm
b) 198pm, 99pm
c) 198pm, 198pm
d) 99pm, 99m
Answer: a
20. What are the units of measuring the bond angle?
a) meters
b) kilograms
c) degree
d) mole
Answer: c
21. How many orbitals are included in sp3d hybridization?
a) 5
b) 4
c) 3
d) 6
Answer: 5
22. A double bond is made up of __________
a) Two sigma bonds
b) Two pi bonds
c) One sigma and one pi bond
d) Two sigmas and one pi bond
Answer: One sigma and one pi bond
23. Which of the following molecules geometry is true?
a) BrF5 – Triagonal pyramidal
b) ClF3 – T-shape
c) PCl5 – See-saw
d) SF4 – Triagonal bipyramidal
Answer: ClF3 – T-shape
24. What is the shape of water?
a) Triagonal
b) Triagonal bipyramidal
c) Bent
d) Square planar
Answer: Bent
25. The angle between two bonds in a linear molecule is _______
a) 108°
b) 180°
c) 74.5°
d) 90°
Answer: 180°
26. Which of the following is correct regarding repulsive interaction?
a) Lone pair-Lone pair is greater than Lone pair-Bond pair is greater than Bond pair-Bond pair
b) Lone pair-Lone pair is less than Lone pair-Bond pair is less than Bond pair-Bond pair
c) Lone pair-Bond pair is greater than Lone pair-Lone pair is greater than Bond pair-Bond pair
d) Lone pair-Lone pair is greater than Lone pair-Bond pair is less than Bond pair-Bond pair
Answer: Lone pair-Lone pair is greater than Lone pair-Bond pair is greater than Bond pair-Bond pair
27. The shape of the molecule depends on the _______
a) adjacent atom
b) valence electrons
c) surroundings
d) atmosphere
Answer: valence electrons
28. Which type of bond is present between hydrogens in hydrogen molecule?
a) Sigma bond
b) Pi bond
c) Ionic bond
d) Metallic bond
Answer: Sigma bond
29. The pi-bond involves __________
a) axial overlapping
b) side-wise overlapping
c) end to end type of overlapping
d) head-on overlapping
Answer: side-wise overlapping
30. A __________ overlap doesn’t result in the formation of a bond.
a) positive
b) negative
c) zero
d) rational
Answer: zero
31. A positive overlap is same as ________
a) out-phase overlap
b) negative overlap
c) zero overlap
d) in-phase overlap
Answer: in-phase overlap
32. Which of the following is not a homonuclear diatomic molecule?
a) H2
b) N2
c) O2
d) HCl
Answer: HCl
33. What is the electronic configuration of carbon in it’s excited state?
a) 1s22s22p4
b) 1s22s22p3
c) 1s22s22p5
d) 1s22s12p4
Answer: 1s22s22p3
34. The bond enthalpy of ___________ molecule is 435.8 kJ mol-1.
a) Hydrogen
b) Oxygen
c) Nitrogen
d) Helium
Answer: Hydrogen
35. The strength of covalent ___________ extent of overlapping of orbitals.
a) may be or may not be related
b) is independent on
c) is dependent on
d) is not related to
Answer: is dependent on
36. What is the bond angle of H-C-H in methane molecule?
a) 104.5°
b) 109.5°
c) 108°
d) 120°
Answer: 109.5°
37. What do you think is the number of sigma bonds in an ethene molecule?
a) 6
b) 7
c) 4
d) 5
Answer: 5
38. Mention the types of orbitals that undergo hybridization in order to get octahedral geometry?
a) s-orbital only
b) s-orbital and p-orbital
c) s-orbital, p-orbital, and d-orbital
d) d-orbital and p-orbital
Answer: s-orbital, p-orbital, and d-orbital
39. What is the geometry of PCl5 molecule?
a) Square pyramidal
b) V-shape
c) Trigonal bipyramidal
d) Tetrahedral
Answer: Trigonal bipyramidal
40. Which of the following statement is true regarding hybrid orbitals?
a) The amount of orbitals formed after the hybridization is not equal to the number of orbitals before hybridization
b) The hybrid orbitals don’t have equal energy
c) They can form more stable bonds than the pure orbitals
d) Hybridization doesn’t indicate geometry
Answer: They can form more stable bonds than the pure orbitals
41. Who introduced the concept of hybridization?
a) Pauling
b) London
c) Sidgwick
d) Alexander
Answer: Pauling
42. The phenomenon of forming completely new atomic orbitals by intermixing them is known as
a) Allocation
b) Hybridization
c) Chemical bond formation
d) Electron configuration
Answer: Hybridization
43. Which of the bonding orbital has greater energy comparatively?
a) Both Bonding molecular orbital and Anti-bonding molecular orbital have the same energy
b) The energy of Bonding molecular orbital and Anti-bonding molecular orbital depends on the situation
c) Bonding molecular orbital
d) Anti-bonding molecular orbital
Answer: Anti-bonding molecular orbital
44. Take NA as the number of Anti-bonding molecular orbitals and NB as the number of Bonding molecular orbitals. The molecule is stable when NA ____________ NB.
a) is greater than
b) is equal to
c) is less than
d) is greater than or equal to
Answer: is less than
45. What’s the bond order of Oxygen?
a) 3
b) 2
c) 1
d) 0
Answer: 2
46. What do you think is the relationship between bond order and bond length?
a) Directly proportional
b) Indirectly proportional
c) No relation
d) Cannot predict
Answer: Indirectly proportional
47. Which of the following molecule is not true about paramagnetic molecules?
a) Attracted by the magnetic field
b) A molecular orbital is singly occupied
c) An example is oxygen molecule
d) Repelled by the magnetic field
Answer: Repelled by the magnetic field
48. Combination of two atomic orbitals results in the formation of two molecular orbitals namely
a) one bonding and one non-bonding orbital
b) two bonding orbitals
c) two non-bonding orbitals
d) two bonding and non-bonding orbitals
Answer: one bonding and one non-bonding orbital
49. Stability increases, as the energy ___________
a) increases
b) doesn’t change
c) decreases
d) increases and then decreases
Answer: decreases
50. What is the electronic configuration of the carbon atom?
a) 1s22s22p2
b) σ1s2σ*1s2σ2s2σ*2s2π2px2π2py2
c) 1s22s22p1
d) σ1s2σ*1s σ2s2π2px2π2py2
Answer: 1s22s22p2
51. The electronic configurations of molecules change when the number of electrons is ________
a) 10
b) 20
c) 17
d) 14
Answer: 14
52. Which of the following is true regarding nitrogen molecule.
a) Diamagnetic
b) Paramagnetic
c) Bond order is 2
d) Total number of electrons in the molecule is 13
Answer: Diamagnetic
53. H2, N2, O2 and Li2 are ______________
a) heteronuclear diatomic molecules
b) heteronuclear triatomic molecules
c) homonuclear diatomic molecules
d) homonuclear triatomic molecules
Answer: homonuclear diatomic molecules
54. What is the total number of electrons in the Chlorine molecule?
a) 17
b) 34
c) 18
d) 16
Answer: 34
55. What is the electronic configuration of hydrogen molecule?
a) σ1s2
b) σ1s1
c) σ1s
d) σ*1s
Answer: σ1s2
56. What is the condition, for a molecule do not exist?
a) NA = NB
b) NA > NB
c) NA < NB
d) NA >/< NB
Answer: NA = NB
57. Which of the following molecule doesn’t exist?
a) O2
b) H2
c) He2
d) N2
Answer: H2
58. Water molecules contain _____________ hydrogen bond/s.
a) intermolecular
b) intramolecular
c) both intermolecular and intramolecular
d) neither intermolecular nor intramolecular
Answer: intermolecular
59. The magnitude of the H-bonding depends on the ___________ of the compound.
a) surroundings
b) system
c) atmosphere
d) physical state
Answer: physical state
60. Which of the following molecule can form a hydrogen bond with hydrogen?
a) Sodium
b) Oxygen
c) Aluminum
d) Rubidium
Answer: Oxygen
61. Which of the following molecules doesn’t involve hydrogen bond formation?
a) H2O
b) O-nitrophenol
c) NaCl
d) HF
Answer: NaCl
62. Alcohol and HF molecule contains __________ & _____________ hydrogen bonds.
a) intramolecular, intermolecular
b) intermolecular, intermolecular
c) intermolecular, intramolecular
d) intramolecular, intramolecular
Answer: intermolecular, intermolecular
63. Nitrogen, fluorine and oxygen are ___________ in nature.
a) electronegative
b) electropositive
c) metallic
d) semi-metallic
Answer: electronegative
64. Which bond acts like a bridge two molecules formed by a covalent bond?
a) Covalent bond
b) Ionic bond
c) Hydrogen bond
d) Metallic bond
Answer: Hydrogen bond
65. A molecule named o-nitrophenol consists of ______________hydrogen bond/s.
a) intermolecular
b) intramolecular
c) both intermolecular and intramolecular
d) neither intermolecular nor intramolecular
Answer: intramolecular