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Chemical Bonding

Ionic, covalent, metallic bonds, VSEPR, hybridisation

Key Concepts
  • Ionic bonding: transfer of electrons; forms between metal and non-metal
  • Covalent bonding: sharing of electrons; VSEPR predicts geometry
  • Hybridisation: sp (linear), sp² (trigonal planar), sp³ (tetrahedral)
  • Molecular orbital theory: bonding and antibonding orbitals
  • Hydrogen bonding: strong dipole–dipole involving N, O, or F
Important Formulae
Bond order (MO theory) BO = (bonding e⁻ − antibonding e⁻) / 2
Formal charge FC = V − N − B/2 (V=valence e⁻, N=non-bonding, B=bonding)
Dipole moment μ = q × d
Quick Tips
  • Lone pairs cause greater repulsion than bonding pairs — they reduce bond angle (H₂O: 104.5°, NH₃: 107°).
  • Bond order > 0 means stable molecule; BO = 0 means molecule does not exist (e.g. He₂).
  • Resonance structures: actual bond lengths are intermediate; benzene is the classic example.
Sample Practice Questions

  1. The geometry of BF₃ (no lone pairs on B) is:

    • Tetrahedral
    • Trigonal planar
    • Linear
    • Pyramidal
    Show answer

    Answer: Trigonal planar

  2. The hybridization of nitrogen in NH₃ is:

    • sp
    • sp²
    • sp³
    • sp³d
    Show answer

    Answer: sp³

  3. Hybridization of carbon in CH₄ is:

    • sp
    • sp²
    • sp³
    • dsp²
    Show answer

    Answer: sp³

  4. Resonance structures of ozone (O₃) show:

    • Fixed single bond
    • Fixed double bond
    • Delocalized electrons
    • No bonds
    Show answer

    Answer: Delocalized electrons

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Practice Questions

Practice 20 randomly selected NEET questions on Chemical Bonding. Answers are revealed after each question.

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