Hybridization is a model used to explain how atomic orbitals mix to form new orbitals that allow atoms to create stable molecular structures. Although hybridization is a theoretical concept rather than a physical phenomenon you can directly observe, it provides an elegant way to explain molecular shapes, bond angles, and bonding patterns. In IB Chemistry hybridization is essential for analyzing bonding in carbon compounds and predicting molecular geometry using VSEPR theory.
What Is Hybridization?
Hybridization is the mixing of atomic orbitals (s and p orbitals) on an atom to form new, equivalent hybrid orbitals that are used to form covalent bonds.
The goal of hybridization is to match orbital geometry with molecular geometry so that atoms can bond efficiently.
Hybrid orbitals:
- Have equal energy
- Point in specific directions
- Maximize orbital overlap
- Explain bond angles and shapes
Hybridization occurs primarily in covalently bonded molecules.
Why Hybridization Happens
Atoms form stable molecules by maximizing orbital overlap.
However, unhybridized s and p orbitals do not always align with the observed shapes of molecules.
For example:
- Carbon has 2s and 2p orbitals
- But methane (CH₄) has four identical bonds and a tetrahedral shape
- Hybridization explains this by mixing one s and three p orbitals → sp³ orbitals
Hybridization aligns theory with actual molecular geometry.
Types of Hybridization in IB Chemistry
IB Chemistry focuses on three main types:
1. sp³ Hybridization (Tetrahedral)
How It Forms
One s orbital mixes with three p orbitals:
