hybridization

chemistry

Written by

The Information Architects of Encyclopaedia Britannica

Last updated

June 29, 2026

Quick Summary

Hybridization in chemistry is a concept that explains how atomic orbitals within an atom mix to form new, equivalent hybrid orbitals. This mixing allows atoms, particularly carbon, to form stronger and more stable covalent bonds.1

For example, a carbon atom has one 2s orbital and three 2p orbitals. When these hybridize, they form four equivalent sp³ hybrid orbitals. These orbitals are oriented towards the corners of a tetrahedron, enabling carbon to form four identical single bonds, as seen in methane (CH₄).1

Another type of hybridization is sp², where one 2s orbital and two 2p orbitals combine to form three sp² hybrid orbitals arranged in a triangular plane. The remaining unhybridized 2p orbital can form a pi bond. This type of hybridization is observed in ethylene (C₂H₄) and results in a planar molecule with a double bond. Hybridization is a key concept in valence bond theory, helping to explain molecular geometry and bonding patterns.1

Summary created from Britannica articles using AI. AI can make mistakes, so verify using Britannica articles.

8 Britannica Sources

Ask Britannica AI about this topic

Britannica doesn't have a full article on this topic, so we've curated a list of our relevant coverage.

boron group element
Salts of M2+ ions
The boron orbitals are hybridized to either the sp² (when boron forms bonds with three other atoms, for example, in borazine) or the sp³ (when boron forms bonds with four atoms, as in metal borohydrides) configuration (see chemical bonding: Valence bond theory: Hybridization).
Read More
The boron orbitals are hybridized to either the sp² (when boron forms bonds with three other atoms, for example, in borazine) or the sp³ (when boron forms bonds with four atoms, as in metal borohydrides) configuration (see chemical bonding: Valence bond theory: Hybridization).
Read More

carbonium ion
Classification.
…in an sp² state of hybridization—that is, three electrons of the carbon atom occupy orbitals formed by the combination (hybridization) of three ordinary orbitals, one denoted s and two, p. All three orbitals lie in one plane; thus, the cationic centre of the molecule formed by bonding the carbon atom…
Read More
…in an sp² state of hybridization—that is, three electrons of the carbon atom occupy orbitals formed by the combination (hybridization) of three ordinary orbitals, one denoted s and two, p. All three orbitals lie in one plane; thus, the cationic centre of the molecule formed by bonding the carbon atom…
Read More

chemical bonding
Hybridization
The discussion is not yet complete, however. If this description of carbon were taken at face value, it would appear that, whereas three of the CH bonds in methane are formed from carbon 2p orbitals, one is formed from a carbon 2s orbital. It…
Read More
The discussion is not yet complete, however. If this description of carbon were taken at face value, it would appear that, whereas three of the CH bonds in methane are formed from carbon 2p orbitals, one is formed from a carbon 2s orbital. It…
Read More