Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure – Revision Notes

Bonding in this chapter splits into ionic bonds, formed by electron transfer, and covalent bonds governed by the octet rule, with VSEPR theory then used to predict molecular shape. Hybridization states such as sp³ for tetrahedral geometry and molecular orbital theory’s bond order calculation round out the picture, alongside hydrogen bonding’s effect on water’s boiling point.

Last Updated: September 23, 2026

Bond Types

• Ionic: electron transfer.
• Covalent: electron sharing; octet rule.

Shape and Hybridization

• VSEPR theory predicts shape via electron pair repulsion.
• sp (linear), sp² (trigonal planar), sp³ (tetrahedral).

Molecular Orbital Theory

• Bond order=½(bonding−antibonding electrons).

Hydrogen Bonding

• Between H (bonded to N/O/F) and an electronegative atom; explains water’s high boiling point.

One-Line Summary

Chemical bonding theories (ionic, covalent, VSEPR, hybridization, and molecular orbital theory) explain how and why atoms combine, and predict the shape, stability, and properties of the resulting molecules.

Frequently Asked Questions

What is the difference between ionic and covalent bonding?
An ionic bond forms through the complete transfer of electrons between atoms, usually a metal and a non-metal, creating oppositely charged ions that attract each other, while a covalent bond forms through the mutual sharing of electron pairs.

How does VSEPR theory help predict the shape of a molecule?
The Valence Shell Electron Pair Repulsion theory predicts molecular shape based on the idea that electron pairs around a central atom arrange themselves as far apart as possible to minimise repulsion.

Written by Satish

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