Why is the H–F bond much stronger than the H–I bond?
Correct answer C. H–F is shorter and more polar, so the attraction between atoms is greater
Topic / 39 questions
Chemical Bonding MCQs
Chemical Bonding MCQs are multiple-choice questions on how atoms join to form molecules, covering VSEPR theory, hybridisation, sigma and pi bonds, dipole moment, polarity and bond energy. They follow the MDCAT chemistry curriculum, and every question on MCQs360 shows its correct answer instantly so you can check shapes and bond counts as you practise.
- Gases 40
- Liquids 40
- Solids 40
- Chemical Equilibrium 40
- Reaction Kinetics 40
- Thermochemistry and Energetics 40
- Electrochemistry 40
- Fundamental Concepts of Chemistry 40
- Atomic Structure 39
- Chemical Bonding 39
- Alcohols and Phenols 38
- Industrial Chemistry 37
- Aldehydes and Ketones 37
- Alkyl Halides 37
- s- and p-Block Elements 37
- Chemistry of Hydrocarbons 36
- Fundamental Principles of Organic Chemistry 36
- Carboxylic Acids 36
- Transition Elements 35
- Macromolecules 35
Charges of ±1.6 × 10⁻¹⁹ C are separated by 1.0 × 10⁻¹⁰ m. What is the dipole moment (1 D = 3.34 × 10⁻³⁰ C m)?
Correct answer D. 4.8 D
Which molecule is polar?
Correct answer D. CHCl₃
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NH₃ and NF₃ are both pyramidal. Why does NH₃ have a much larger dipole moment than NF₃?
Correct answer D. In NH₃ the lone pair moment adds to the bond moments, while in NF₃ it opposes them
How many sigma and pi bonds are present in a benzene molecule, C₆H₆ (Kekulé structure)?
Correct answer D. 12 sigma and 3 pi
How is a sigma (σ) bond formed?
Correct answer A. By head-on (end-to-end) overlap of orbitals along the internuclear axis
According to VSEPR theory, which order of electron-pair repulsion is correct?
Correct answer D. Lone pair–lone pair > lone pair–bond pair > bond pair–bond pair
What is the shape and bond angle of the methane molecule, CH₄?
Correct answer B. Tetrahedral, 109.5°
What is the shape of the sulphur dioxide molecule, SO₂?
Correct answer C. Bent (angular)
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What is the shape of the carbonate ion, CO₃²⁻?
Correct answer B. Trigonal planar
What is the shape of the ammonium ion, NH₄⁺?
Correct answer A. Tetrahedral
What is the hybridisation of the carbon atom in carbon dioxide, CO₂?
Correct answer D. sp
What is the hybridisation of the oxygen atom in a water molecule?
Correct answer B. sp³
What is the percentage s-character of an sp² hybrid orbital?
Correct answer A. 33.3%
Which order of carbon-carbon bond energies is correct?
Correct answer A. C≡C > C=C > C–C
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What is the shape of the hydronium ion, H₃O⁺?
Correct answer D. Trigonal pyramidal
Which of the following molecules is linear?
Correct answer A. BeCl₂
What is the hybridisation of carbon atoms in graphite?
Correct answer C. sp²
The enthalpy change for CH₄(g) → C(g) + 4H(g) is +1664 kJ mol⁻¹. What is the average C–H bond energy?
Correct answer C. 416 kJ mol⁻¹
Which bond is the strongest?
Correct answer B. H–F
About Chemical Bonding MCQs
Shape questions ask you to apply VSEPR theory and hybridisation to molecules such as NH₃, H₂O, BF₃, PCl₅ and SF₆, giving the shape, bond angle and hybridisation of the central atom. Carbon hybridisation in compounds and allotropes such as graphite also appears, along with counting sigma and pi bonds in ethene, ethyne and carbon dioxide. Other questions cover how sigma and pi bonds form, bond energy and bond strength, the order of single, double and triple bond energies, and average bond energies from atomisation data. Dipole moment questions test its unit, the debye, molecular polarity and calculating percentage ionic character from observed and theoretical dipole moments.
Key facts to remember
- VSEPR theory: electron pairs around a central atom repel one another, with lone pair–lone pair > lone pair–bond pair > bond pair–bond pair repulsion.
- NH₃ is trigonal pyramidal (about 107°) and H₂O is bent (about 104.5°); both have an sp³ hybridised central atom.
- sp, sp² and sp³ hybridisation give linear (180°), trigonal planar (120°) and tetrahedral (109.5°) arrangements; PCl₅ (sp³d) is trigonal bipyramidal and SF₆ (sp³d²) is octahedral.
- A sigma bond forms by head-on overlap of orbitals and a pi bond by sideways overlap of parallel p orbitals; a double bond is one σ and one π, and a triple bond is one σ and two π.
- Dipole moment μ = q × d and is measured in debye, where 1 D = 3.34 × 10⁻³⁰ C m.
- Carbon–carbon bond energy increases in the order C–C < C=C < C≡C.
Exams that include Chemical Bonding MCQs
Pakistan
- MDCAT
- ECAT
- NUMS
- AKU
- FSc boards
India
- NEET
- JEE Main
Bangladesh
- HSC
- Medical Admission Test
How to prepare for Chemical Bonding MCQs
- Count bond pairs and lone pairs around the central atom first, then name the shape and hybridisation.
- Learn a short table of shapes from AB₂ to AB₆, including the lone-pair versions such as AB₃E and AB₂E₂.
- To count sigma and pi bonds, remember every single bond is σ and each extra bond in a double or triple bond is π.
- Revise how symmetry cancels bond dipoles, which explains why CO₂ and BF₃ are non-polar.
Frequently asked questions
What does the MDCAT syllabus include in Chemical Bonding?
The PMDC MDCAT curriculum for Chemical Bonding covers VSEPR theory and the shapes of molecules, sigma and pi bonds, hybridisation, dipole moment, molecular polarity and ionic character, and bond energy and bond strength. Shapes and hybridisation of common molecules are the most frequently tested parts.
Which exams ask Chemical Bonding MCQs?
Chemical bonding is one of the most tested chemistry topics in MDCAT, ECAT, NUMS and AKU entry tests and FSc board papers in Pakistan. It is also a core chapter for NEET and JEE Main in India and HSC and medical admission tests in Bangladesh.
Why is CO₂ non-polar although its C=O bonds are polar?
Carbon dioxide is linear, so its two C=O bond dipoles are equal in size and point in opposite directions. They cancel each other out, giving the molecule a net dipole moment of zero even though each bond is polar.
Last reviewed October 2026