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Chemical Bonding & Molecular Structure WBJEE MCQs

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Chemical Bonding and Molecular Structure Revision Guide for WBJEE 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 WBJEE 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 WBJEE 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.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

1. The molecular geometry of BF3 is

  • A. Bent
  • B. Trigonal planar
  • C. Tetrahedral
  • D. Pyramidal
Answer: B
Explanation: Three bonding domains around B give trigonal planar geometry.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

2. The molecular geometry of CH4 is

  • A. Tetrahedral
  • B. Square planar
  • C. Trigonal planar
  • D. Pyramidal
Answer: A
Explanation: Four bonding pairs around carbon arrange tetrahedrally.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

3. The molecular geometry of NH3 is

  • A. Trigonal planar
  • B. Tetrahedral molecular geometry
  • C. Linear
  • D. Trigonal pyramidal
Answer: D
Explanation: NH3 has three bonds and one lone pair; its molecular geometry is pyramidal.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

4. The molecular geometry of H2O is

  • A. Trigonal planar
  • B. Tetrahedral
  • C. Bent
  • D. Linear
Answer: C
Explanation: Two bonds and two lone pairs on O give a bent molecular geometry.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

5. The hybridisation of carbon in methane is

  • A. sp
  • B. dsp2
  • C. sp3
  • D. sp2
Answer: C
Explanation: Four equivalent sigma bonds arise from sp3 hybrid orbitals.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

6. Sigma bonds are formed by

  • A. Electron transfer
  • B. Head-on overlap
  • C. Sidewise overlap only
  • D. No orbital overlap
Answer: B
Explanation: Sigma bonding results from overlap along the internuclear axis.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

7. The bond order of O2 according to MO theory is

  • A. 2
  • B. 1
  • C. 2.5
  • D. 3
Answer: A
Explanation: Bond order=(bonding-antibonding electrons)/2=2.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

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

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

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

9. The bond order of N2 is

  • A. 2.5
  • B. 3
  • C. 2
  • D. 1
Answer: B
Explanation: N2 has a triple bond and MO bond order 3.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

10. A molecule is stable in simple MO theory when its bond order is

  • A. Always zero
  • B. Negative only
  • C. Exactly -1
  • D. Greater than zero
Answer: D
Explanation: Positive bond order indicates net bonding stabilisation.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

11. Bonding concept check

  • A. Linear
  • B. Trigonal pyramidal
  • C. Trigonal planar
  • D. Tetrahedral molecular geometry
Answer: B
Explanation: NH3 has three bonds and one lone pair; its molecular geometry is pyramidal.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

12. WBJEE advanced

  • A. Trigonal planar
  • B. Tetrahedral molecular geometry
  • C. Linear
  • D. Trigonal pyramidal
Answer: D
Explanation: NH3 has three bonds and one lone pair; its molecular geometry is pyramidal.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

13. An ionic bond is formed primarily by

  • A. Hydrogen bonding
  • B. Electrostatic attraction between oppositely charged ions
  • C. Sharing one electron pair equally
  • D. Overlap of two p orbitals only
Answer: B
Explanation: Electron transfer produces ions held by Coulombic attraction.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

14. A covalent bond is formed by

  • A. Sharing of electron pair(s)
  • B. Complete electron transfer only
  • C. Attraction of nuclei without electrons
  • D. Neutron exchange
Answer: A
Explanation: Covalent bonding involves shared electron density.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

15. A coordinate covalent bond has the shared pair supplied by

  • A. Both atoms equally, one electron each
  • B. A neutron
  • C. A proton
  • D. One atom
Answer: D
Explanation: Both electrons in a coordinate bond originate from one donor atom.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

16. The shape of BeCl2 in the gaseous monomeric state is

  • A. Trigonal planar
  • B. Tetrahedral
  • C. Linear
  • D. Bent
Answer: C
Explanation: Be has two bonding domains and no lone pair; VSEPR gives linear geometry.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

17. The approximate bond angle in CH4 is

  • A. 90°
  • B. 109.5°
  • C. 120°
  • D. 180°
Answer: B
Explanation: Ideal tetrahedral bond angle is about 109.5°.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

18. The H-N-H bond angle in NH3 is smaller than tetrahedral mainly because

  • A. Lone-pair-bond-pair repulsion is stronger than bond-pair-bond-pair repulsion
  • B. N has no lone pair
  • C. NH3 is planar
  • D. Hydrogen is highly electronegative
Answer: A
Explanation: The lone pair compresses H-N-H angles.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

19. The H-O-H bond angle is smaller than H-N-H mainly because H2O has

  • A. No lone pairs
  • B. A triple bond
  • C. sp hybridisation
  • D. Two lone pairs on the central atom
Answer: D
Explanation: Two lone pairs exert stronger cumulative repulsion.

WBJEE Chemistry · Chemical Bonding and Molecular Structure · Very Very Hard

20. The hybridisation of carbon in ethene is

  • A. d2sp3
  • B. sp2
  • C. sp3
  • D. sp
Answer: B
Explanation: Each alkene carbon is approximately trigonal planar and sp2 hybridised.

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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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