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
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Lattice energy of an ionic compound depends on:
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Answer: Charge and size of ions
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Bond order from MO theory = :
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Answer: (Bonding e⁻ − Antibonding e⁻) / 2
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The shape of PCl₅ is:
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Answer: Trigonal bipyramidal
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Hybridization of carbon in CH₄ is:
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Answer: sp³
Practice Questions
Practice 20 randomly selected NEET questions on Chemical Bonding. Answers are revealed after each question.
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What are the key concepts in Chemical Bonding for NEET?
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.
Which formulae are important for Chemical Bonding in NEET?
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.
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