Hybridization of Formaldehyde (CH₂O) - sp2

Q: What is the hybridization of Formaldehyde?

Formaldehyde (CH₂O) is sp2 hybridized with Trigonal Planar geometry and 120 degree bond angles.

What is the hybridization of Formaldehyde (CH₂O)?

The central atom in Formaldehyde (CH₂O) is sp2 hybridized. This produces Trigonal Planar geometry with bond angles of 120 degrees. It has 3 hybrid orbitals and 1 unhybridized p orbital (pi bond).

Formula	CH₂O
Name	Formaldehyde
Hybridization	sp2
Geometry	Trigonal Planar
Bond Angle	120°
Hybrid Orbitals	3
Unhybridized p Orbitals	2pᵩ (pi bond)

Introduction

Formaldehyde (CH₂O) has a C=O double bond and two C–H single bonds. Carbon is sp² hybridized, just like in ethene, but here the double bond is to oxygen.

Electron Configuration

Carbon has 4 valence electrons: 2s² 2p². Three orbitals hybridize for the σ framework, and one p orbital remains for the π bond with oxygen.

Atomic Orbitals

The 2s orbital is spherical. Two p orbitals (pₓ and pᵧ) join the hybridization. The pᵩ orbital stays unhybridized, perpendicular to the molecular plane.

Orbital Mixing

One s and two p orbitals mix into three sp² hybrids. The unhybridized p orbital remains ready for π bonding. Watch the mixing happen.

Result

Three sp² orbitals in a trigonal planar arrangement (~120°). One points toward oxygen, two toward hydrogen atoms. The leftover p orbital is perpendicular to this plane.

Bonding

Each sp² orbital forms a σ bond. The unhybridized p orbital on carbon overlaps with a p orbital on oxygen to form the π bond, completing the C=O double bond.

Interactive hybridization explorer with step-by-step orbital mixing animations for 8 molecules.

Visualize Formaldehyde's Orbital Mixing in 3D