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Class XI · Chemistry

Chemical Bonding and Molecular Structure: NEET MCQ practice

441 practice questions on Chemical Bonding and Molecular Structure, each with an explanation. Practise them chapter by chapter in the GyaanLoop app.

441

Practice questions

198

Easy

233

Medium

10

Hard

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What Chemical Bonding and Molecular Structure covers

Topics in the NEET (UG) 2026–27 syllabus for this chapter.

  • Kossel-Lewis approach to chemical bond formation, ionic and covalent bonds
  • Ionic bonding, factors affecting lattice energy
  • Covalent bonding, electronegativity, Fajan's rule, dipole moment, VSEPR theory and shapes of molecules
  • Valence bond theory, hybridization involving s, p and d orbitals, resonance
  • Molecular orbital theory- LCAOs, bonding/antibonding orbitals, bond order, bond length, bond energy
  • Elementary idea of metallic bonding, hydrogen bonding and its applications

Sample questions on Chemical Bonding and Molecular Structure

Try each one, then open the answer and explanation.

Question 1 · Practice question

Which option is incorrect among the following for the given property?

  1. A.Dipole moment (HF > HCI > HBr > HI)
  2. B.Bond length (HI > HBr > HCI > HF)
  3. C.Acidic strength (HI > HBr > HCI > HF)
  4. D.Thermal stability (HF
Show answer

Answer: D. Thermal stability (HF

Thermal stability of hydrogen halides decreases down the group: HF is the most stable due to strong H–F bond, while HI is least stable. The given option suggests the opposite trend, making it incorrect. The other trends (dipole moment decreasing, bond length increasing, acidity increasing down the group) are all correct facts from NCERT.

Question 2 · Practice question

In the MOT of F₂ molecule, number of electrons occupying antibonding orbitals are

  1. A.8
  2. B.9
  3. C.7
  4. D.5
Show answer

Answer: A. 8

The F₂ molecule has a total of 18 electrons (each F atom has 9). In its molecular orbital configuration, the antibonding orbitals occupied are σ*1s², σ*2s², π*2px², and π*2py², summing to 8 antibonding electrons. This gives a bond order of 1 (Bond Order = (10 bonding electrons − 8 antibonding electrons)/2 = 1). Distractors like 9 or 7 arise from miscounting or incorrect MO filling.

Question 3 · Practice question

The shape of trimethyl amine is:

  1. A.Octahedral
  2. B.Tetrahedral
  3. C.Bent shape
  4. D.Pyramidal
Show answer

Answer: D. Pyramidal

Trimethyl amine (N(CH₃)₃) has a nitrogen atom with three bonded methyl groups and one lone pair, giving it a trigonal pyramidal shape, which is simply 'pyramidal'. Tetrahedral would require four bonds without a lone pair (like methane), but the lone pair makes it pyramidal.

Question 4 · Practice question

Which of the following compounds shows maximum hydrogen bonding?

  1. A.HF
  2. B.H₂O
  3. C.NH
  4. D.CH₃OH
Show answer

Answer: B. H₂O

Water (H₂O) shows the maximum hydrogen bonding because each molecule can form up to four hydrogen bonds (two via its H atoms and two via lone pairs on oxygen), leading to an extensive 3D network. HF also has strong hydrogen bonds, but fewer per molecule, while NH₃ and CH₃OH have fewer hydrogen bonds per molecule overall.

Question 5 · Practice question

Hydrogen bond between two atoms is formed due to

  1. A.Displacement of electrons towards more electronegative atom resulting in fractional positive chargeon hydrogen
  2. B.Displacement of electrons towards hydrogenatom resulting in a polar molecule
  3. C.Formation of a bond between hydrogen atoms of one molecule and the other
  4. D.Existence of an attractive force which binds hydrogen atoms together.
Show answer

Answer: A. Displacement of electrons towards more electronegative atom resulting in fractional positive chargeon hydrogen

Hydrogen bonding forms when hydrogen is attached to a highly electronegative atom (like F, O, N), causing electron density to shift toward that atom. This leaves hydrogen with a partial positive charge (δ⁺), which can attract a lone pair on another electronegative atom. Option B is wrong because electrons move away from hydrogen, not toward it; option C incorrectly suggests hydrogen–hydrogen bonding, and option D is too vague without explaining the origin of the force.

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