Chemical Bonding and Molecular Structure — Class 11 MCQs with Answers
Class 11 CBSE Chemistry · Chapter 4
90 practice questions · 30 Easy · 30 Medium · 30 Hard · Updated
Practise the most important Class 11 CBSE Chemistry questions from Chapter 4, "Chemical Bonding and Molecular Structure". You get 9 timed quizzes made from 90 NCERT-based MCQs, with answers and explanations. The questions are split into 30 Easy, 30 Medium and 30 Hard. Warm up on the basics, then move on to the exam-level questions that set top scorers in CBSE & Maharashtra HSC Board exams, JEE Main, MHT-CET, JEE Advanced and NEET UG apart.
To score well in "Chemical Bonding and Molecular Structure", focus on reactions, key concepts and careful numericals. Each MCQ here is timed and uses exam-style marking (+4 correct, −1 wrong, 0 skipped). This trains you to stay accurate under time pressure, as real papers need. Every question has a short explanation, so a wrong answer becomes a quick lesson. It is the fastest way to fix gaps before a test.
Use this chapter for focused revision. Start with the Easy set to check your basics on Chemical Bonding and Molecular Structure, then move to Medium and Hard to practise applying them. Your accuracy, streaks and XP save automatically. This chapter also adds to your overall Class 11 Chemistry mastery score. 14 sample questions are solved in full below, with the answer and a worked explanation. Sign in free to start practising.
Key concepts: Chemical Bonding and Molecular Structure (Class 11 Chemistry)
This chapter explains why atoms combine and what shape the result takes. Starting from Kössel–Lewis and the octet rule, it builds ionic and covalent bonding, Fajans' rules, VSEPR geometry, valence bond theory with hybridisation, and molecular orbital theory, then closes with bond parameters, dipole moment and hydrogen bonding.
- Lewis structures and the octet
- Atoms combine to attain a noble-gas octet by sharing or transferring valence electrons; Lewis dot structures show bonding pairs and lone pairs around each atom.
- Ionic bond
- Formed by electron transfer from a low-IE metal to a high-EA non-metal; its stability is set by lattice enthalpy, rising with charge and smaller ions.
- Covalent bond and parameters
- Shared pairs bind atoms; bond length (internuclear distance) shortens and bond enthalpy grows as bond order rises, so triple bonds are shortest and strongest.
- Coordinate bond
- A covalent bond where both shared electrons come from one atom (donor); once formed it is identical to a normal covalent bond, as in NH₄⁺ and O₃.
Chemical Bonding and Molecular Structure — important questions & MCQs with answers (Class 11 Chemistry)
14 solved questions from this chapter's difficulty levels, each with its answer and explanation. The other 76 are timed and scored when you sign in.
- Q1Easy
NaCl has which type of bond?
A.Ionic✓ CorrectB.CovalentC.MetallicD.HydrogenAnswer: A. Ionic
Explanation: Bond type follows the electronegativity gap: Na (0.9) and Cl (3.0) differ by ~2.1, too large for sharing, so Na transfers an electron to Cl, forming Na⁺Cl⁻ — an ionic bond, not covalent.
- Q2Easy
Hybridisation in BF₃:
A.spB.sp²✓ CorrectC.sp³D.sp³dAnswer: B. sp²
Explanation: Boron in BF₃ has 3 bond pairs and no lone pair, so VSEPR gives sp² hybridisation and a trigonal planar shape with 120° angles. sp³ would need a 4th group or a lone pair, which BF₃ has neither.
- Q3Easy
H₂ molecule is held by:
A.Hydrogen bondB.Ionic bondC.Covalent bond✓ CorrectD.Van der Waals onlyAnswer: C. Covalent bond
Explanation: Identical H atoms have zero electronegativity difference, so neither can pull electrons away from the other; they can only share a pair equally, forming one covalent σ bond, not an ionic one.
- Q4Easy
Shape of NH₃:
A.LinearB.Trigonal planarC.TetrahedralD.Pyramidal✓ CorrectAnswer: D. Pyramidal
Explanation: Nitrogen in NH₃ has 3 bond pairs plus 1 lone pair (5 valence e⁻ used across 3 bonds), giving sp³ hybridisation, but the hidden lone pair makes the molecular shape pyramidal, not trigonal planar.
- Q5Easy
The octet rule states that atoms tend to have:
A.18 electronsB.8 protonsC.2 electrons totalD.8 electrons in valence shell✓ CorrectAnswer: D. 8 electrons in valence shell
Explanation: The octet rule says atoms gain, lose, or share electrons to reach 8 in the valence shell, like Ne's configuration. Picking 18 or 2 confuses period-3 expansion or the He duet with the general rule.
- Q6Easy
CO₂ molecular shape:
A.BentB.Linear✓ CorrectC.TetrahedralD.TrigonalAnswer: B. Linear
Explanation: Carbon in CO₂ has 2 σ bonds and no lone pairs, forcing sp hybridisation and a 180° linear shape. Confusing it with bent SO₂ is the usual slip — SO₂'s sulfur carries a lone pair CO₂'s carbon lacks.
- Q7Medium
Bond order of O₂ from MOT:
A.3B.1C.2✓ CorrectD.2.5Answer: C. 2
Explanation: MO theory gives O₂ 8 bonding electrons (σ2s, σ2p, π2p) and 4 antibonding (σ*2s, π*2p), so bond order = (8−4)/2 = 2, matching the O=O double bond drawn in its Lewis structure.
- Q8Medium
Shape of CH₄:
A.Tetrahedral✓ CorrectB.Square planarC.LinearD.OctahedralAnswer: A. Tetrahedral
Explanation: Carbon's 4 bond pairs in CH₄ with no lone pair give sp³ hybridisation and a tetrahedral shape with 109.5° angles — the ideal geometry for 4 equivalent electron domains and zero lone-pair distortion.
- Q9Medium
Paramagnetic molecule among these:
A.N₂B.O₂✓ CorrectC.F₂D.H₂Answer: B. O₂
Explanation: O₂'s MO configuration places 2 electrons singly in the degenerate π*2p orbitals by Hund's rule, leaving them unpaired, which makes O₂ paramagnetic — unlike N₂, F₂, and H₂, whose electrons pair up.
- Q10Medium
Shape of H₂O:
A.LinearB.TetrahedralC.Bent / V-shaped✓ CorrectD.Trigonal planarAnswer: C. Bent / V-shaped
Explanation: Oxygen in H₂O has 4 electron domains (2 bond pairs + 2 lone pairs, tetrahedral electron geometry), but the 2 lone pairs push the H–O–H angle down to ~104.5°, giving a bent, V-shaped molecular shape.
- Q11Medium
Among NH₃, NF₃, the dipole moment of NH₃ is greater because:
A.NF₃ is non-polarB.F is less electronegativeC.Lone pair and N–H dipoles add✓ CorrectD.Sizes are equalAnswer: C. Lone pair and N–H dipoles add
Explanation: In NH₃ the N lone-pair dipole points the same way as the 3 N–H bond dipoles, so they reinforce. In NF₃ the more electronegative F pulls bond dipoles toward itself, opposing the lone pair and partly cancelling it.
- Q12Hard
Polar molecule among these:
A.H₂O✓ CorrectB.CO₂C.CH₄D.BF₃Answer: A. H₂O
Explanation: H₂O is bent (2 lone pairs on O), so its 2 O–H bond dipoles don't cancel, giving a net dipole. CO₂, CH₄, and BF₃ are symmetric (linear, tetrahedral, trigonal planar) with identical bonds, so theirs cancel to zero.
- Q13Hard
Hybridisation of carbon in C₂H₄ (ethene):
A.spB.sp²✓ CorrectC.sp³D.sp³dAnswer: B. sp²
Explanation: Each carbon in H₂C=CH₂ forms 3 σ bonds (2 to H, 1 to C) plus 1 π bond from an unhybridised p-orbital, needing only 3 hybrid orbitals — sp². The leftover p-orbital handles the π bond of the C=C double bond.
- Q14Hard
Highest bond order among O₂, O₂⁺, O₂⁻, O₂²⁻:
A.O₂²⁻B.O₂C.O₂⁻D.O₂⁺✓ CorrectAnswer: D. O₂⁺
Explanation: MO bond orders here are O₂²⁻ = 1, O₂ = 2, O₂⁻ = 1.5, and O₂⁺ = 2.5 — each electron removed from a filled π*2p orbital raises the bond order, so O₂⁺, having lost an electron from neutral O₂, ranks highest.
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Start this chapter free →Chemical Bonding and Molecular Structure — FAQs
What are the key concepts in Class 11 Chemistry Chemical Bonding and Molecular Structure?+
This chapter explains why atoms combine and what shape the result takes. Starting from Kössel–Lewis and the octet rule, it builds ionic and covalent bonding, Fajans' rules, VSEPR geometry, valence bond theory with hybridisation, and molecular orbital theory, then closes with bond parameters, dipole moment and hydrogen bonding. Key ideas include Lewis structures and the octet, Ionic bond, Covalent bond and parameters, Coordinate bond.
What does Class 11 Chemistry Chapter 4 (Chemical Bonding and Molecular Structure) cover on XamBaaz?+
It has 90 NCERT-based MCQs on "Chemical Bonding and Molecular Structure": 30 Easy, 30 Medium and 30 Hard. Together they make 9 timed quizzes, and you never get the same set twice. Every question has an instant explanation. They help you prepare for CBSE & Maharashtra HSC Board exams, JEE Main, MHT-CET, JEE Advanced and NEET UG.
Are these "Chemical Bonding and Molecular Structure" questions free to practise?+
Yes. Sign in with Google to practise "Chemical Bonding and Molecular Structure" free. Full unlimited access is ₹999/year on a launch offer until 1 December 2026. No chapter is charged separately.
How should I revise "Chemical Bonding and Molecular Structure" for the exam?+
Start with the Easy quiz to check your basics, then try Medium and Hard to practise applying them. There are 9 timed quizzes on this chapter, so you can come back for a fresh set instead of one you have seen. Read each explanation, retry the questions you miss, and track your accuracy until it stays high.
Are these "Chemical Bonding and Molecular Structure" MCQs available with answers?+
Yes. 14 sample questions are shown here in full, each with the correct option and a step-by-step "Why" explanation. Sign in free with Google to start practising, with instant scoring.
Is there negative marking in the "Chemical Bonding and Molecular Structure" quizzes?+
Yes. The timed quizzes use exam-style marking: +4 for a right answer, −1 for a wrong one and 0 for a skip, the same negative marking as JEE Main, JEE Advanced and NEET UG. MHT-CET and CBSE board papers have no negative marking. Our mocks for those are scored their way.
What are the important questions from Chemical Bonding and Molecular Structure (Class 11 Chemistry)?+
The questions that matter most test Lewis structures and the octet, Ionic bond, Covalent bond and parameters, Coordinate bond. This page shows 14 solved important MCQs with answers and explanations; all 90 questions on the chapter are available as timed quizzes once you sign in.
Is there an online quiz for Chemical Bonding and Molecular Structure?+
Yes — Class 11 Chemistry Chemical Bonding and Molecular Structure has timed online quizzes at Easy, Medium and Hard levels, with instant scoring and a worked explanation on every question. The first quiz on the chapter is free.