Hybridisation explains how atomic orbitals blend to create new shapes that support bonding. This module helps you understand how hybrid orbitals determine molecular geometry and why geometry shapes chemical behaviour.

You begin by exploring how s and p orbitals combine to form sp, sp², and sp³ hybrids. Clear diagrams help you visualise how these orbitals orient themselves in space, linear for sp, trigonal planar for sp², and tetrahedral for sp³. These shapes become the foundation for predicting molecular structure.

You then explore how geometry influences polarity, reactivity, and physical properties. Bond angles, electron pair repulsion, and orbital overlap all contribute to how molecules behave in reactions and how they interact with light, solvents, and other molecules.

Real‑world examples from methane to carbon dioxide to benzene show how hybridisation explains stability, shape, and reactivity.

By the end, hybridisation feels like the architectural language of chemistry, a way of understanding how atoms build the structures that shape matter.

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