1. Which type of bond is formed by transfer of electrons?
A) Ionic bond
B) Covalent bond
C) Metallic bond
D) Hydrogen bond
Answer: A
Explanation: Ionic bonds form due to complete transfer of electrons from one atom to another.
2. Ionic bond is generally formed between:
A) Metal & Non-metal
B) Metal & Metal
C) Non-metal & Non-metal
D) Noble gases
Answer: A
Explanation: Metals lose electrons, non-metals gain electrons → ionic bond.
3. Which of the following is an example of ionic compound?
A) HCl
B) NaCl
C) H₂O
D) CO₂
Answer: B
Explanation: NaCl is ionic due to transfer of electron from Na to Cl.
4. A covalent bond is formed due to:
A) Transfer of electrons
B) Sharing of electrons
C) Overlapping of orbitals
D) Both B & C
Answer: D
Explanation: Covalent bond is formed by sharing electrons via orbital overlap.
5. Which of the following is a covalent compound?
A) NaCl
B) MgO
C) HCl
D) CaF₂
Answer: C
Explanation: HCl forms covalent bond by sharing electrons.
6. The bond energy is:
A) Energy released in bond formation
B) Energy required to break a bond
C) Energy of atom
D) None of these
Answer: B
Explanation: Bond energy = minimum energy needed to break one mole of bonds.
7. Bond length is:
A) Distance between nuclei of bonded atoms
B) Sum of radii
C) Difference of radii
D) None
Answer: A
Explanation: Bond length is internuclear distance at minimum energy.
8. Bond order in N₂ molecule is:
A) 1
B) 2
C) 3
D) 4
Answer: C
Explanation: N₂ has triple bond → bond order = 3.
9. Higher bond order means:
A) Shorter bond length
B) Higher bond energy
C) Stronger bond
D) All of these
Answer: D
Explanation: Bond order ↑ → bond length ↓, bond energy ↑, strength ↑.
10. Which has highest bond order?
A) O₂
B) O₂⁺
C) O₂⁻
D) O₂²⁻
Answer: B
Explanation: O₂⁺ has bond order 2.5 (highest among these).
11. Which is most stable?
A) N₂
B) O₂
C) F₂
D) Cl₂
Answer: A
Explanation: N₂ has highest bond order (3) → most stable.
12. Ionic compounds are generally:
A) Soluble in non-polar solvents
B) Soluble in polar solvents
C) Insoluble in water
D) Covalent in nature
Answer: B
Explanation: Ionic compounds dissolve in polar solvents like water.
13. Covalent compounds generally have:
A) High melting point
B) Low melting point
C) Metallic properties
D) Conductivity in solid state
Answer: B
Explanation: Covalent compounds have weak intermolecular forces → low melting points.
14. Which has the smallest bond length?
A) N≡N
B) O=O
C) F–F
D) Cl–Cl
Answer: A
Explanation: Triple bond → shortest bond length.
15. Metallic bond theory is explained by:
A) Electron sea model
B) Valence bond theory
C) Hybridization
D) MOT
Answer: A
Explanation: Metallic bonding is explained by free electrons in a sea model.
16. Which has both ionic & covalent bonds?
A) NaCl
B) K₂SO₄
C) NH₄Cl
D) H₂O
Answer: C
Explanation: NH₄Cl has covalent N–H bonds and ionic NH₄⁺Cl⁻ bonding.
17. Bond angle in H₂O is approximately:
A) 180°
B) 120°
C) 109.5°
D) 104.5°
Answer: D
Explanation: Due to 2 lone pairs, bond angle reduces to 104.5°.
18. Bond angle in NH₃ is:
A) 120°
B) 109.5°
C) 107°
D) 90°
Answer: C
Explanation: NH₃ (sp³ hybridised, 1 lone pair) → bond angle 107°.
19. Which has linear geometry?
A) CO₂
B) NH₃
C) H₂O
D) BF₃
Answer: A
Explanation: CO₂ is sp hybridised, linear (180°).
20. Bond angle in BF₃ is:
A) 120°
B) 109.5°
C) 104.5°
D) 90°
Answer: A
Explanation: BF₃ is sp² hybridised → trigonal planar, 120°.
21. Which bond is strongest?
A) Ionic bond
B) Covalent bond
C) Metallic bond
D) Hydrogen bond
Answer: A
Explanation: Ionic bonds are generally strongest due to electrostatic attraction.
22. Which molecule has polar covalent bond?
A) H₂
B) Cl₂
C) HCl
D) O₂
Answer: C
Explanation: H–Cl bond is polar due to electronegativity difference.
23. Which molecule has non-polar covalent bond?
A) HCl
B) H₂O
C) F₂
D) NH₃
Answer: C
Explanation: F₂ has equal sharing (same atoms) → non-polar.
24. Lattice energy of ionic compounds depends on:
A) Size of ions
B) Charge of ions
C) Distance between ions
D) All of these
Answer: D
Explanation: Lattice energy ∝ q₁q₂ / r.
25. Which has highest lattice energy?
A) NaCl
B) MgO
C) KCl
D) CaO
Answer: B
Explanation: Mg²⁺O²⁻ has highest charges → highest lattice energy.
26. The VSEPR theory is used to predict:
A) Bond energy
B) Bond order
C) Shape of molecules
D) Lattice energy
Answer: C
Explanation: VSEPR theory predicts molecular geometry based on repulsion between electron pairs.
27. According to VSEPR theory, shape of BeCl₂ is:
A) Linear
B) Bent
C) Trigonal planar
D) Tetrahedral
Answer: A
Explanation: BeCl₂ has 2 bond pairs, no lone pairs → linear (180°).
28. Shape of BF₃ is:
A) Linear
B) Trigonal planar
C) Tetrahedral
D) Pyramidal
Answer: B
Explanation: BF₃ is sp² hybridised, 120° bond angle → trigonal planar.
29. The shape of CH₄ molecule is:
A) Trigonal planar
B) Square planar
C) Tetrahedral
D) Linear
Answer: C
Explanation: CH₄ is sp³ hybridised, tetrahedral (109.5°).
30. Hybridisation of carbon in CH₄ is:
A) sp
B) sp²
C) sp³
D) dsp²
Answer: C
Explanation: CH₄ has 4 sigma bonds → sp³ hybridisation.
31. The shape of NH₃ molecule is:
A) Linear
B) Trigonal planar
C) Pyramidal
D) Tetrahedral
Answer: C
Explanation: NH₃ has sp³ hybridisation, one lone pair → pyramidal (107°).
32. The shape of H₂O molecule is:
A) Linear
B) Bent
C) Tetrahedral
D) Trigonal planar
Answer: B
Explanation: H₂O has sp³ hybridisation, two lone pairs → bent (104.5°).
33. Which has trigonal bipyramidal geometry?
A) PCl₅
B) SF₆
C) ClF₃
D) XeF₂
Answer: A
Explanation: PCl₅ is sp³d hybridised → trigonal bipyramidal.
34. Which has octahedral geometry?
A) PCl₅
B) SF₆
C) XeF₂
D) IF₃
Answer: B
Explanation: SF₆ is sp³d² hybridised → octahedral.
35. Hybridisation of Xe in XeF₂ is:
A) sp³
B) sp³d
C) sp³d²
D) sp³d³
Answer: B
Explanation: XeF₂ → sp³d hybridisation, linear shape.
36. Shape of ClF₃ is:
A) Linear
B) T-shaped
C) Trigonal planar
D) Octahedral
Answer: B
Explanation: ClF₃ has sp³d hybridisation with 2 lone pairs → T-shaped.
37. Hybridisation in SF₄ is:
A) sp³
B) sp³d
C) sp³d²
D) sp³d³
Answer: B
Explanation: SF₄ is sp³d hybridised, seesaw shape.
38. Shape of SF₄ is:
A) Linear
B) Seesaw
C) Square planar
D) T-shaped
Answer: B
Explanation: SF₄ (sp³d) has one lone pair → seesaw geometry.
39. In XeF₄, the geometry is:
A) Square planar
B) Octahedral
C) Tetrahedral
D) Trigonal bipyramidal
Answer: A
Explanation: XeF₄ has sp³d² hybridisation with 2 lone pairs → square planar.
40. Which molecule has square pyramidal shape?
A) XeF₂
B) XeF₄
C) IF₅
D) SF₆
Answer: C
Explanation: IF₅ is sp³d² hybridised with one lone pair → square pyramidal.
41. The shape of XeF₆ is:
A) Octahedral
B) Distorted octahedral
C) Square planar
D) Trigonal bipyramidal
Answer: B
Explanation: XeF₆ is sp³d³ hybridised with one lone pair → distorted octahedral.
42. Which of the following is non-linear?
A) CO₂
B) BeCl₂
C) H₂O
D) C₂H₂
Answer: C
Explanation: H₂O has bent shape, others are linear.
43. Hybridisation of C in C₂H₂ is:
A) sp³
B) sp²
C) sp
D) dsp²
Answer: C
Explanation: C in acetylene (C₂H₂) is sp hybridised (linear).
44. Hybridisation of C in C₂H₄ is:
A) sp³
B) sp²
C) sp
D) dsp²
Answer: B
Explanation: Ethene has double bond → sp² hybridisation.
45. Hybridisation of C in C₂H₆ is:
A) sp³
B) sp²
C) sp
D) dsp²
Answer: A
Explanation: Ethane has only single bonds → sp³ hybridisation.
46. The bond angle in sp³ hybridisation (ideal) is:
A) 90°
B) 109.5°
C) 120°
D) 180°
Answer: B
Explanation: sp³ → tetrahedral → 109.5°.
47. The bond angle in sp² hybridisation is:
A) 90°
B) 109.5°
C) 120°
D) 180°
Answer: C
Explanation: sp² → trigonal planar → 120°.
48. The bond angle in sp hybridisation is:
A) 90°
B) 109.5°
C) 120°
D) 180°
Answer: D
Explanation: sp → linear → 180°.
49. In NH₄⁺ ion, the hybridisation of N is:
A) sp²
B) sp³
C) sp³d
D) sp³d²
Answer: B
Explanation: NH₄⁺ has 4 sigma bonds, no lone pairs → sp³ hybridisation.
50. Which of the following is trigonal pyramidal?
A) BF₃
B) NH₃
C) CH₄
D) CO₂
Answer: B
Explanation: NH₃ has sp³ hybridisation with one lone pair → trigonal pyramidal.
51. Valence Bond Theory (VBT) explains bond formation by:
A) Sharing of electrons
B) Transfer of electrons
C) Overlap of atomic orbitals
D) Lattice formation
Answer: C
Explanation: VBT states that covalent bonds are formed by overlapping of atomic orbitals containing unpaired electrons.
52. The overlapping of orbitals along the internuclear axis forms:
A) π-bond
B) σ-bond
C) Ionic bond
D) Metallic bond
Answer: B
Explanation: End-to-end overlap → sigma (σ) bond.
53. Sidewise overlap of orbitals forms:
A) σ-bond
B) π-bond
C) Ionic bond
D) Hydrogen bond
Answer: B
Explanation: Side-by-side overlap → pi (π) bond.
54. Which bond is stronger?
A) σ-bond
B) π-bond
C) Both equal
D) None
Answer: A
Explanation: σ-bond is stronger due to greater overlap.
55. A double bond contains:
A) 1 σ + 1 π
B) 2 σ
C) 1 σ only
D) 2 π
Answer: A
Explanation: Double bond = 1 sigma + 1 pi.
56. A triple bond contains:
A) 1 σ + 1 π
B) 1 σ + 2 π
C) 2 σ + 1 π
D) 3 σ
Answer: B
Explanation: Triple bond = 1 sigma + 2 pi.
57. In Molecular Orbital Theory (MOT), molecular orbitals are formed by:
A) Mixing of nuclei
B) Mixing of atomic orbitals
C) Overlap of sigma bonds
D) Overlap of pi bonds
Answer: B
Explanation: MOT states molecular orbitals are linear combinations of atomic orbitals (LCAO).
58. Which is true for bonding molecular orbital (BMO)?
A) Higher energy than atomic orbital
B) Lower energy than atomic orbital
C) Destabilising
D) Anti-symmetric
Answer: B
Explanation: BMO has lower energy than atomic orbitals → stabilising.
59. Which is true for antibonding molecular orbital?
A) Higher energy
B) Lower energy
C) Stabilising
D) Increases bond order
Answer: A
Explanation: Antibonding orbitals have higher energy → destabilising.
60. Bond order (MOT) =
A) ½ (Nb – Na)
B) ½ (Na – Nb)
C) Nb + Na
D) Nb / Na
Answer: A
Explanation: Bond order = ½ (no. of bonding electrons – no. of antibonding electrons).
61. In H₂ molecule, bond order is:
A) 0
B) 1
C) 2
D) 3
Answer: B
Explanation: H₂ → 2 bonding e⁻, 0 antibonding e⁻ → (2–0)/2 = 1.
62. In He₂ molecule, bond order is:
A) 0
B) 1
C) 2
D) 3
Answer: A
Explanation: He₂ → 2 bonding e⁻, 2 antibonding e⁻ → (2–2)/2 = 0 (unstable).
63. Bond order of O₂ molecule is:
A) 1
B) 2
C) 3
D) 2.5
Answer: B
Explanation: O₂ → bond order = 2 (paramagnetic).
64. O₂ molecule is:
A) Diamagnetic
B) Paramagnetic
C) Ferromagnetic
D) None
Answer: B
Explanation: O₂ has 2 unpaired electrons in π orbitals → paramagnetic.*
65. Bond order of O₂⁺ is:
A) 1.5
B) 2
C) 2.5
D) 3
Answer: C
Explanation: O₂⁺ → one electron removed from antibonding → bond order 2.5.
66. Bond order of O₂⁻ is:
A) 1.5
B) 2
C) 2.5
D) 3
Answer: A
Explanation: O₂⁻ → one electron added to antibonding orbital → bond order 1.5.
67. Which is diamagnetic?
A) O₂
B) O₂⁺
C) O₂²⁻
D) B₂
Answer: C
Explanation: O₂²⁻ has paired electrons → diamagnetic.
68. Bond order of N₂ is:
A) 1
B) 2
C) 3
D) 4
Answer: C
Explanation: N₂ bond order = 3 (triple bond, very stable).
69. Bond order of N₂⁺ is:
A) 2
B) 2.5
C) 3
D) 3.5
Answer: B
Explanation: N₂⁺ loses one electron from bonding orbital → bond order 2.5.
70. Which molecule is paramagnetic according to MOT?
A) N₂
B) O₂
C) CO₂
D) H₂O
Answer: B
Explanation: O₂ is paramagnetic (2 unpaired electrons).
71. The increasing bond order in O₂ species is:
A) O₂ < O₂⁺ < O₂²⁻
B) O₂²⁻ < O₂ < O₂⁺
C) O₂ < O₂²⁻ < O₂⁺
D) O₂⁺ < O₂ < O₂²⁻
Answer: B
Explanation: Bond order: O₂²⁻ (1) < O₂ (2) < O₂⁺ (2.5).
72. According to MOT, which species is least stable?
A) N₂
B) O₂
C) He₂
D) CO
Answer: C
Explanation: He₂ bond order = 0 → unstable.
73. In B₂ molecule, magnetic property is:
A) Diamagnetic
B) Paramagnetic
C) Ferromagnetic
D) None
Answer: B
Explanation: B₂ has 2 unpaired electrons in π orbitals → paramagnetic.
74. CO molecule is isoelectronic with:
A) N₂
B) O₂
C) F₂
D) Ne₂
Answer: A
Explanation: CO (14 e⁻) is isoelectronic with N₂ (14 e⁻).
75. Which has highest bond energy?
A) O₂
B) N₂
C) F₂
D) Cl₂
Answer: B
Explanation: N₂ has bond order 3 (triple bond) → highest bond energy.
76. Resonance in molecules occurs due to:
A) Rapid interconversion of isomers
B) Delocalization of electrons
C) Vibrations of nuclei
D) Hybridization of orbitals
Answer: B
Explanation: Resonance represents electron delocalization across different positions without actual movement of atoms.
77. The resonance energy of benzene is approximately:
A) 36 kcal/mol
B) 50 kcal/mol
C) 100 kcal/mol
D) 10 kcal/mol
Answer: A
Explanation: Benzene is more stable than expected due to resonance energy (~36 kcal/mol).
78. Which ion shows resonance?
A) NH₄⁺
B) CO₃²⁻
C) Na⁺
D) Cl⁻
Answer: B
Explanation: Carbonate ion has delocalized π-electrons across three oxygen atoms.
79. The most stable resonance structure is the one with:
A) Maximum number of covalent bonds
B) Least formal charge
C) Negative charge on more electronegative atom
D) All of the above
Answer: D
Explanation: Stability depends on bond maximization, proper charge placement, and minimal separation.
80. In resonance, the actual structure of a molecule is:
A) One of the resonance forms
B) A mixture of resonance forms
C) An intermediate hybrid
D) Rapidly interchanging isomers
Answer: C
Explanation: The real structure is a resonance hybrid, more stable than any single canonical form.
81. Which of the following molecules has resonance?
A) SO₂
B) NH₃
C) H₂O
D) CH₄
Answer: A
Explanation: SO₂ has multiple resonance structures with delocalized π-bonds.
82. Hydrogen bonding is strongest in:
A) H₂S
B) H₂Se
C) H₂O
D) H₂Te
Answer: C
Explanation: Due to high electronegativity and small size of oxygen, H₂O shows strong H-bonding.
83. Hydrogen bonding leads to:
A) Higher boiling points
B) Higher viscosity
C) Higher surface tension
D) All of the above
Answer: D
Explanation: H-bonding creates strong intermolecular forces, increasing these physical properties.
84. Which of the following exhibits intramolecular hydrogen bonding?
A) o-nitrophenol
B) p-nitrophenol
C) m-nitrophenol
D) Phenol
Answer: A
Explanation: o-Nitrophenol has intramolecular H-bonding between –OH and –NO₂ group.
85. Which of the following exhibits intermolecular hydrogen bonding?
A) o-nitrophenol
B) p-nitrophenol
C) Both A and B
D) None
Answer: B
Explanation: p-Nitrophenol molecules form H-bonds with neighboring molecules.
86. Ice floats on water due to:
A) Lower density of ice because of H-bonding
B) Higher density of ice because of H-bonding
C) Presence of covalent bonds
D) Resonance in H₂O
Answer: A
Explanation: H-bonding in ice creates an open lattice structure, lowering density.
87. Which of the following molecules shows resonance stabilization?
A) CH₂=CH₂
B) CH₃–CH₃
C) C₆H₆
D) CH₄
Answer: C
Explanation: Benzene has delocalized π-electrons and resonance stabilization.
88. Which type of hydrogen bond is stronger?
A) Intermolecular
B) Intramolecular
C) Both equal
D) None
Answer: A
Explanation: Intermolecular H-bonds generally lead to higher stability and stronger interactions.
89. Which factor is not essential for hydrogen bonding?
A) High electronegativity
B) Small size of atom
C) Presence of lone pairs
D) High atomic mass
Answer: D
Explanation: Atomic mass doesn’t influence hydrogen bonding; electronegativity and size do.
90. Which of the following shows hydrogen bonding in liquid state?
A) HF
B) NH₃
C) H₂O
D) All of these
Answer: D
Explanation: HF, NH₃, and H₂O all form intermolecular hydrogen bonds in liquid state.
91. The abnormal high boiling point of water is due to:
A) Ionic bonding
B) Covalent bonding
C) Hydrogen bonding
D) van der Waals forces
Answer: C
Explanation: Strong hydrogen bonds between water molecules increase its boiling point.
92. Which of the following molecules does not show resonance?
A) O₃
B) NO₂⁻
C) H₂O
D) CO₃²⁻
Answer: C
Explanation: Water has localized bonds, no delocalization of electrons.
93. Which of the following molecules shows extensive hydrogen bonding leading to dimer formation?
A) Acetic acid
B) Methanol
C) Phenol
D) Ammonia
Answer: A
Explanation: Acetic acid forms strong dimeric structures via intermolecular H-bonds.
94. Hydrogen bonding is absent in:
A) HCl
B) HF
C) NH₃
D) H₂O
Answer: A
Explanation: Chlorine is large and less electronegative, so HCl does not form H-bonds.
95. Which of the following explains the planarity of benzene?
A) Hybridization
B) Resonance
C) Hydrogen bonding
D) Ionic nature
Answer: B
Explanation: Delocalized π-electrons in resonance enforce planarity in benzene.
96. Which bond order indicates resonance stabilization?
A) 1
B) 1.33
C) 2
D) 3
Answer: B
Explanation: Bond orders like 1.33 (e.g., CO₃²⁻, NO₃⁻) arise due to resonance.
97. The anomalous high viscosity of glycerol is due to:
A) Ionic bonding
B) Extensive hydrogen bonding
C) Resonance
D) van der Waals forces
Answer: B
Explanation: Glycerol has three –OH groups, forming multiple H-bonds → high viscosity.
98. The bond angle in water decreases from tetrahedral angle due to:
A) Resonance
B) Lone pair–bond pair repulsion and H-bonding
C) Hydrogen bonding only
D) Ionic bonding
Answer: B
Explanation: Strong lone pair repulsions reduce bond angle to ~104.5°.
99. Which of the following molecules exhibits both resonance and hydrogen bonding?
A) Benzene
B) Acetic acid
C) Methane
D) Ethylene
Answer: B
Explanation: Acetic acid has resonance in –COOH and hydrogen bonding between molecules.
100. Which property of DNA structure is due to hydrogen bonding?
A) Double helix stability
B) Base pairing specificity
C) Complementary strand binding
D) All of the above
Answer: D
Explanation: H-bonding between bases stabilizes double helix and ensures specific base pairing.