Hybridization of Methane (CH₄) - sp3

Introduction

Methane (CH₄) is the simplest organic molecule. Carbon forms four equivalent bonds to hydrogen atoms. But how does carbon, with only 2 unpaired electrons in its ground state, form 4 bonds?

Electron Configuration

Carbon has 4 valence electrons: 2s² 2p². In the ground state, the 2s orbital is full and only 2 of the 3 p orbitals have electrons. That would predict only 2 bonds — but methane has 4.

Atomic Orbitals

The 2s orbital is a sphere. The three 2p orbitals are dumbbells along the x, y, and z axes. They have different shapes and energies.

Orbital Mixing

One s orbital and three p orbitals combine to form four equivalent sp³ hybrid orbitals. Watch them form — the sphere and dumbbells blend into four identical teardrop shapes.

Result

The four sp³ orbitals point toward the corners of a tetrahedron, equally spaced at 109.5° apart. Each orbital has 25% s character and 75% p character.

Bonding

Each sp³ orbital overlaps with a hydrogen 1s orbital to form a sigma (σ) bond. The tetrahedral arrangement minimizes electron repulsion.

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