Chemistry · Class 11 · Chapter 4
Chemical Bonding and Molecular Structure
12 lessons 109 min 1 simulations 9 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.
What the exam asks
NEET repeatedly asks for the shape and hybridisation of a given species (including expanded-octet molecules like SF₄, ClF₃, XeF₂ and XeF₄), bond order and magnetic behaviour from MO theory, which molecules have zero dipole moment, and comparisons of bond angle or bond length. Students lose marks by ignoring lone pairs when naming shapes, by using the wrong MO energy order for O₂ versus N₂, and by confusing electron geometry with molecular shape.
Lessons
12 lessons · 109 min
1Kössel-Lewis approach and the octet ruleNCERT § "Kössel-Lewis Approach to Chemical Bonding"9 min2Ionic bonding and lattice enthalpyNCERT § "Ionic or Electrovalent Bond"9 min3Bond parameters: length, angle, enthalpy and orderNCERT § "Bond Parameters"7 min4Resonance structuresNCERT § "Resonance Structures"7 min5Polarity of bonds and dipole momentNCERT § "Polarity of Bonds"9 min6VSEPR theory and molecular shapesNCERT § "The Valence Shell Electron Pair Repulsion (VSEPR) Theory"11 min 1 sim7Valence bond theory and orbital overlapNCERT § "Valence Bond Theory"9 min8HybridisationNCERT § "Hybridisation"8 min9Molecular orbital theoryNCERT § "Molecular Orbital Theory"8 min10Homonuclear diatomic moleculesNCERT § "Bonding in Some Homonuclear Diatomic Molecules"8 min11Hydrogen bondingNCERT § "Hydrogen Bonding"10 min12Chapter reviewMust-know facts, traps and formulas14 min