Periodic Table & Chemical Bonding
Periodicity, ionic and covalent bonding, VSEPR, hybridisation, and coordination compounds
Key Concepts
- Atomic radius decreases across a period and increases down a group
- Ionisation energy and electronegativity rise across a period
- Ionic bonding (electron transfer) vs covalent bonding (electron sharing)
- VSEPR and hybridisation (sp, sp², sp³) predict molecular geometry
- Coordination compounds: crystal field theory and isomerism
Important Formulae
| Bond order (MOT) | BO = (N_b − N_a)/2 |
| Formal charge | FC = V − N − B/2 |
| Dipole moment | μ = q × d |
| Effective nuclear charge | Z_eff = Z − σ |
Quick Tips
- Lone pairs repel more than bonding pairs, reducing bond angles (H₂O 104.5°, NH₃ 107°).
- Bond order of 0 means the molecule does not exist (e.g. He₂).
- Half-filled and fully-filled orbitals give extra stability (Cr, Cu exceptions).
Sample Practice Questions
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The molecular shape of methane (CH₄) is:
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Answer: Tetrahedral
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The most electronegative element in the periodic table is:
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Answer: Fluorine
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Across a period (left to right), the atomic radius generally:
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Answer: Decreases
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The bond order of the oxygen molecule (O₂) according to molecular orbital theory is:
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Answer: 2
Practice Questions
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What are the key concepts in Periodic Table & Chemical Bonding for JEE?
Atomic radius decreases across a period and increases down a group; Ionisation energy and electronegativity rise across a period; Ionic bonding (electron transfer) vs covalent bonding (electron sharing); VSEPR and hybridisation (sp, sp², sp³) predict molecular geometry; Coordination compounds: crystal field theory and isomerism.
Which formulae are important for Periodic Table & Chemical Bonding in JEE?
Bond order (MOT): BO = (N_b − N_a)/2; Formal charge: FC = V − N − B/2; Dipole moment: μ = q × d; Effective nuclear charge: Z_eff = Z − σ.
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