Hybridization of Carbon Dioxide (CO₂) - sp

Q: What is the hybridization of Carbon Dioxide?

Carbon Dioxide (CO₂) is sp hybridized with Linear geometry and 180 degree bond angles.

What is the hybridization of Carbon Dioxide (CO₂)?

The central atom in Carbon Dioxide (CO₂) is sp hybridized. This produces Linear geometry with bond angles of 180 degrees. It has 2 hybrid orbitals and 2 unhybridized p orbitals (pi bond).

Formula	CO₂
Name	Carbon Dioxide
Hybridization	sp
Geometry	Linear
Bond Angle	180°
Hybrid Orbitals	2
Unhybridized p Orbitals	2pᵧ (pi bond), 2pᵩ (pi bond)

Introduction

CO₂ is linear with two C=O double bonds. Carbon only needs 2 σ bonds, so it mixes just 2 orbitals — the most extreme hybridization: sp.

Electron Configuration

Carbon has 4 valence electrons: 2s² 2p². Only one s and one p orbital hybridize. The other two p orbitals stay unhybridized for π bonds.

Atomic Orbitals

The 2s orbital is spherical. The 2pₓ orbital is a dumbbell along the bond axis. The 2pᵧ and 2pᵩ orbitals point perpendicular to the bond axis and remain unhybridized.

Orbital Mixing

One s and one p orbital combine to form two sp hybrids. Two p orbitals are left over for π bonding. Watch just two orbitals blend together.

Result

Two sp orbitals point in opposite directions (180° apart) — linear geometry. Two unhybridized p orbitals remain perpendicular to the bond axis.

Bonding

Each sp orbital forms a σ bond with an oxygen atom. The two unhybridized p orbitals overlap with p orbitals on the oxygens to form two π bonds — giving two C=O double bonds.

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

Visualize Carbon Dioxide's Orbital Mixing in 3D