Free Chemical Bonding MCQs with Answers
964 Chemical Bonding MCQs from Chemistry, each with the correct answer and a written explanation of why it is correct. Free and unlimited, with no account needed.
Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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Read the Chemical Bonding notesFree MDCAT chapter notes with key terms964 questions · page 29 of 49
- A. The bond angle between CH₃ and C is 120°
- B. The bond angle between C and O is 180°
- C. The bond angle between C-C-C is 109.5° and between C-O-C is ~109.5°
- D. The bond angle between CH₃ and C is 90°
Explanation: The carbon atoms in the tertiary-butyl group are sp³ hybridized, leading to tetrahedral geometry with bond angles of approximately 109.5°.
Correct answer: The bond angle between C-C-C is 109.5° and between C-O-C is ~109.5°- A. HCl
- B. NH₄⁺
- C. NaCl
- D. O₂
Explanation: In NH₄⁺, the N-H bond formed by donation of a lone pair from NH₃ to H⁺ is a coordinate covalent bond.
Correct answer: NH₄⁺- A. 90°
- B. 107°
- C. 120°
- D. 180°
Explanation: NH₃ has three bonding pairs and one lone pair, resulting in a trigonal pyramidal geometry with a bond angle of ~107°.
Correct answer: 107°- A. CH₄
- B. C₆H₆ (benzene)
- C. H₂O
- D. NH₃
Explanation: Benzene has a ring structure with π-electrons delocalized over the six carbon atoms, forming resonance structures.
Correct answer: C₆H₆ (benzene)- A. -717 kJ/mol
- B. -437 kJ/mol
- C. -349 kJ/mol
- D. -243 kJ/mol
Explanation: Born-Haber cycle: ΔH = ΔH + IE + (1/2)D - EA - U. -437 = 89 + 419 + (243/2) - 349 - U. U ≈ -717 kJ/mol.
Correct answer: -717 kJ/mol- A. SF₆
- B. XeF₄
- C. BF₃
- D. CH₄
Explanation: XeF₄ has four bonding pairs and two lone pairs, arranged in a square planar geometry per VSEPR theory.
Correct answer: XeF₄- A. A bonding electron pair
- B. A non-bonding electron pair on nitrogen
- C. A shared electron pair between hydrogen atoms
- D. A free proton
Explanation: The lone pair on nitrogen in NH₃ is a non-bonding pair, responsible for the trigonal pyramidal shape and bond angle reduction.
Correct answer: A non-bonding electron pair on nitrogen- A. sp
- B. sp²
- C. sp³
- D. sp³d
Explanation: The carbon forms four sigma bonds with hydrogen; diagram labels show all bonds are equivalent → tetrahedral geometry → sp³ hybridization.
Correct answer: sp³- A. Lone pairs repel bonding pairs
- B. Hydrogen's electronegativity
- C. Lone pairs have no effect
- D. Oxygen's sp² hybridization
Explanation: Oxygen in H₂O has two lone pairs, which repel the O-H bonds more strongly than bonding pairs repel each other.
Correct answer: Lone pairs repel bonding pairs- A. A
- B. B
- C. C
- D. D
Explanation: Boron in BCl₃ has 3 bonded pairs and no lone pairs. The electron pairs repel each other equally, arranging themselves far apart in a…
Correct answer: C- A. 4 σ, 1 π
- B. 5 σ, 2 π
- C. 5 σ, 1 π
- D. 4 σ, 2 π
Explanation: Each C-H bond = 1 σ → 4 σ bonds. C=C double bond = 1 σ + 1 π → add 1 σ + 1 π. Total = 5 σ + 1 π.
Correct answer: 5 σ, 1 π- A. CO₂
- B. SO₂
- C. Both
- D. None
Explanation: CO₂ is a linear molecule, so the two C=O bond dipoles point in opposite directions and cancel each other, making CO₂ nonpolar.
Correct answer: CO₂- A. Equal to single bond
- B. Equal to double bond
- C. Average of single and double bond
- D. Cannot be determined
Explanation: In molecules with delocalized electrons, such as benzene, the electrons are shared across multiple atoms, resulting in resonance…
Correct answer: Average of single and double bond- A. sp²
- B. sp³
- C. sp³d
- D. sp³d²
Explanation: ICl₃ has three bonding pairs and two lone pairs (five electron domains), requiring sp³d hybridization.
Correct answer: sp³d- A. A & B only
- B. C & D only
- C. Only C
- D. Only D
Explanation: S is the least electronegative, and thus, H - S has the least polarity.
Correct answer: Only C- A. 90°
- B. 104.5°
- C. 120°
- D. 109.5°
Explanation: A molecule with three bonding pairs and no lone pairs around the central atom adopts a trigonal planar geometry.
Correct answer: 120°- A. I1 < I2
- B. I1 > I2
- C. I1 = I2
- D. None of the above
Explanation: The magnesium and sodium atoms have roughly the same size. What differs is the effective nuclear charge, which is +1 for Na and +2 for Mg.
Correct answer: I1 < I2- A. H2O can form more hydrogen bonds
- B. HF has stronger hydrogen bonds.
- C. H2O has a higher molecular weight.
- D. HF is a polar molecule.
Explanation: Water (H2O) has a higher boiling point than hydrogen fluoride (HF) because, despite both forming hydrogen bonds, water's tetrahedral shape…
Correct answer: H2O can form more hydrogen bonds- A. 5 sigma and 5 pi
- B. 7 sigma and 3 pi
- C. 8 sigma and 2 pi
- D. 6 sigma and 4 pi
Explanation: The number of sigma and pi-bonds in 1-butene 3-yne are 7 sigma and 3 pi. It has one C=C double bond which contains one pi bond.
Correct answer: 7 sigma and 3 pi- A. 102°
- B. 107.5⁰
- C. 120⁰
- D. 190.5⁰
Explanation: The bond angle in the tetrahedral CH 4 molecule is 109.5°. The replacement of one of the bonded electron pairs with a lone pair compresses…
Correct answer: 107.5⁰