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