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Chemical Bonding and Molecular Structure CBSE Class 11 MCQ & Practice Questions

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Chemical Bonding and Molecular Structure Revision Guide for CBSE Class 11 Chemistry

Chemical Bonding and Molecular Structure explains why atoms combine and how bonding controls molecular shape, polarity and properties. It is a high-connectivity chapter because its ideas reappear throughout inorganic and organic chemistry.

For CBSE Class 11 Chemistry, combine Lewis structures with VSEPR, hybridisation, valence bond ideas and molecular orbital theory. Practise predicting geometry and magnetic behaviour rather than memorising examples without reasoning.

Important Topics

  • Lewis structures and formal charge
  • VSEPR theory and molecular geometry
  • Hybridisation
  • Bond parameters and polarity
  • Hydrogen bonding
  • Molecular orbital theory

Important Formulae & Relationships

  • Formal charge = valence e− − nonbonding e− − 1/2(bonding e−)
  • Bond order (MOT) = 1/2(Nb − Na)
  • Dipole moment μ = q × r

Use formulas only after checking the required units, sign convention and assumptions for the question.

What to practise in Chemical Bonding and Molecular Structure

Concept Revision

Revise definitions, principles, equations, trends and core ideas from Chemical Bonding and Molecular Structure before attempting MCQs.

Exam-style MCQs

Use chapter-focused multiple-choice practice to improve accuracy, recall and application for CBSE Class 11 Chemistry.

Performance Practice

Attempt ChemNexa tests, review results and return to weak areas for another round of targeted revision.

Top 20 Chemical Bonding and Molecular Structure MCQs with Answers

These public questions are selected from the exact Chemical Bonding and Molecular Structure chapter, screened for topic relevance and deduplicated so repeated versions of the same MCQ are not shown publicly. Use them for quick revision, then sign in to attempt the complete test experience with more questions, results and performance review.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

1. The hybridisation of each carbon atom in ethene is

  • A. sp
  • B. sp²
  • C. sp³
  • D. d²sp³
Answer: B
Explanation: Each carbon forms three sigma bonds and one pi bond, corresponding to sp² hybridisation.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

2. The hybridisation of carbon in CH₄ is

  • A. sp
  • B. sp²
  • C. sp³
  • D. dsp²
Answer: C
Explanation: Four equivalent sigma bonds require sp³ hybridisation.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

3. A double bond consists of

  • A. Two sigma bonds
  • B. One sigma and one pi bond
  • C. Two pi bonds
  • D. One coordinate bond and one pi bond
Answer: B
Explanation: A double bond contains one sigma bond and one pi bond.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

4. The bond order of O₂ is

  • A. 1
  • B. 1.5
  • C. 2
  • D. 2.5
Answer: C
Explanation: Bond order = ½(Nb − Na) = 2 for O₂.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

5. The bond order of O₂⁺ compared with O₂ is

  • A. Lower by 0.5
  • B. Higher by 0.5
  • C. Unchanged
  • D. Zero
Answer: B
Explanation: Removing one electron from an antibonding orbital raises bond order from 2 to 2.5.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

6. The electrovalent bond in NaCl is formed by

  • A. Sharing one electron pair
  • B. Transfer of one electron from Na to Cl
  • C. Transfer of one electron from Cl to Na
  • D. Sharing two electron pairs
Answer: B
Explanation: Sodium loses one electron and chlorine gains it, producing Na⁺ and Cl⁻.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

7. According to Fajan's rules, covalent character increases when

  • A. The cation is large and weakly charged
  • B. The cation is small and highly charged
  • C. The anion is small and non-polarisable
  • D. Both ions are large and singly charged
Answer: B
Explanation: A small highly charged cation strongly polarises the anion, increasing covalent character.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

8. Which chloride has the greatest covalent character?

  • A. NaCl
  • B. MgCl₂
  • C. AlCl₃
  • D. KCl
Answer: C
Explanation: Al³⁺ has high charge density and strongly polarises Cl⁻.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

9. The formal charge on an atom in a Lewis structure is calculated as

  • A. Valence electrons + lone-pair electrons + bond pairs
  • B. Valence electrons − lone-pair electrons − half of bonding electrons
  • C. Atomic number − mass number
  • D. Bond pairs − lone pairs
Answer: B
Explanation: Formal charge = valence electrons − nonbonding electrons − ½(bonding electrons).

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

10. The shape of BeCl₂ in the gaseous state is

  • A. Bent
  • B. Linear
  • C. Trigonal planar
  • D. Tetrahedral
Answer: B
Explanation: Two bond pairs and no lone pairs give a linear shape.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

11. The shape of BF₃ is

  • A. Trigonal planar
  • B. Trigonal pyramidal
  • C. Bent
  • D. Tetrahedral
Answer: A
Explanation: Three bond pairs and no lone pairs give trigonal planar geometry.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

12. The shape of NH₃ is

  • A. Trigonal planar
  • B. Trigonal pyramidal
  • C. Tetrahedral
  • D. Bent
Answer: B
Explanation: Three bond pairs and one lone pair give trigonal pyramidal molecular shape.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

13. The shape of H₂O is

  • A. Linear
  • B. Bent
  • C. Trigonal planar
  • D. Tetrahedral
Answer: B
Explanation: Two bond pairs and two lone pairs on oxygen produce a bent shape.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

14. The bond angle in CH₄ is approximately

  • A. 90°
  • B. 104.5°
  • C. 109.5°
  • D. 120°
Answer: C
Explanation: Methane has tetrahedral geometry with bond angle 109.5°.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

15. The H–N–H bond angle in NH₃ is smaller than the tetrahedral angle because

  • A. N–H bonds are ionic
  • B. Lone pair–bond pair repulsion exceeds bond pair–bond pair repulsion
  • C. Nitrogen has no lone pair
  • D. Hydrogen atoms repel less than electrons
Answer: B
Explanation: The lone pair compresses the bond angle from 109.5° to about 107°.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

16. The H–O–H bond angle is about

  • A. 90°
  • B. 104.5°
  • C. 107°
  • D. 120°
Answer: B
Explanation: Two lone pairs on oxygen compress the bond angle to about 104.5°.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

17. The hybridisation of each carbon atom in ethyne is

  • A. sp
  • B. sp²
  • C. sp³
  • D. dsp³
Answer: A
Explanation: Each carbon has two regions of electron density and is sp hybridised.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

18. A triple bond consists of

  • A. Three sigma bonds
  • B. Two sigma and one pi bond
  • C. One sigma and two pi bonds
  • D. Three pi bonds
Answer: C
Explanation: A triple bond contains one sigma and two pi bonds.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

19. Which molecule is paramagnetic according to molecular orbital theory?

  • A. N₂
  • B. O₂
  • C. F₂
  • D. H₂
Answer: B
Explanation: O₂ has two unpaired electrons in antibonding π* orbitals.

CBSE Class 11 Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

20. Hydrogen bonding is strongest when hydrogen is bonded to

  • A. Sulfur
  • B. Nitrogen, oxygen or fluorine
  • C. Carbon only
  • D. Chlorine only
Answer: B
Explanation: Highly electronegative, small N, O and F atoms permit strong hydrogen bonding.

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Chemical Bonding and Molecular Structure Practice Tests

Chemical Bonding and Molecular Structure Frequently Asked Questions

What should I master first in Chemical Bonding?

Start with Lewis structures, electron-pair counting and VSEPR. These make geometry and hybridisation questions much easier.

Why is molecular orbital theory important?

It explains bond order and magnetic behaviour, including cases that simple Lewis structures cannot describe adequately.

How can I avoid geometry mistakes?

Count electron domains around the central atom, distinguish electron-pair geometry from molecular shape, and then account for lone-pair repulsions.

Continue with another chapter to build connected concepts and strengthen your overall Chemistry preparation.

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