AS LEVEL CHEMISTRY / REVISION NOTE
Orbital Hybridization
A high-yield guide to how atomic orbitals combine, why molecular shapes form, and how to identify sp, sp², and sp³ hybridization with confidence.
Atomic orbitals Sigma bonding Molecular geometry
Focus: electron domains → hybrid orbitals → shape
MOLECULAR MODE: ACTIVE
01 / CORE IDEA
What is hybridization?
Hybridization is the mixing of atomic orbitals on the same atom to form a new set of equivalent hybrid orbitals. These orbitals point in specific directions, allowing atoms to form strong sigma bonds and predictable shapes.
03 / REFERENCE TABLE
The three essential hybridization patterns
TYPE 01
sp hybridization
1 s orbital + 1 p orbital → 2 sp orbitals
Electron-pair geometry: linear
Bond angle: 180°
Example: carbon in ethyne, C₂H₂.
TYPE 02
sp² hybridization
1 s orbital + 2 p orbitals → 3 sp² orbitals
Electron-pair geometry: trigonal planar
Bond angle: 120°
Example: each carbon in ethene, C₂H₄.
TYPE 03
sp³ hybridization
1 s orbital + 3 p orbitals → 4 sp³ orbitals
Electron-pair geometry: tetrahedral
Bond angle: 109.5°
Example: carbon in methane, CH₄.
04 / WORKED EXAMPLES
Read the structure, identify the hybridization
BeCl₂ Two bonding regions around Be sp; linear; 180°
BF₃ Three bonding regions around B sp²; trigonal planar; 120°
CH₄ Four bonding regions around C sp³; tetrahedral; 109.5°
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