Chemistry · Class 11 · Chapter 4

Chemical Bonding and Molecular Structure

12 lessons121 min5 simulations9 practice questions

This chapter explains why atoms join and what shapes the resulting molecules take. It moves from the octet-based Kössel-Lewis picture, through ionic bonding and bond parameters, to three models of covalent bonding: VSEPR for shapes, valence bond theory with hybridisation, and molecular orbital theory for bond order and magnetism. It closes with hydrogen bonding, which ties structure to physical properties.

Also called: chemical bonding · VSEPR theory · hybridisation · molecular orbital theory

Start

Lessons

12 lessons · 121 min

01Kössel-Lewis approach and the octet ruleNCERT § "Kössel-Lewis Approach to Chemical Bonding"9 min 02Ionic bonding and lattice enthalpyNCERT § "Ionic or Electrovalent Bond"9 min 03Bond parameters: length, angle, enthalpy and orderNCERT § "Bond Parameters"7 min 04Resonance structuresNCERT § "Resonance Structures"10 min1 sim 05Polarity of bonds and dipole momentNCERT § "Polarity of Bonds"12 min1 sim 06VSEPR theory and molecular shapesNCERT § "The Valence Shell Electron Pair Repulsion (VSEPR) Theory"11 min1 sim 07Valence bond theory and orbital overlapNCERT § "Valence Bond Theory"9 min 08HybridisationNCERT § "Hybridisation"11 min1 sim 09Molecular orbital theoryNCERT § "Molecular Orbital Theory"8 min 10Homonuclear diatomic moleculesNCERT § "Bonding in Some Homonuclear Diatomic Molecules"11 min1 sim 11Hydrogen bondingNCERT § "Hydrogen Bonding"10 min 12Chapter reviewMust-know facts, traps and formulas14 min

Simulations

5 in this chapter

Resonance: one real structureIn: Resonance structures Add up the bond dipolesIn: Polarity of bonds and dipole moment VSEPR: build a molecule's shapeIn: VSEPR theory and molecular shapes Mixing orbitals into hybridsIn: Hybridisation Fill a molecular orbital diagramIn: Homonuclear diatomic molecules