sp² hybridization

sp² hybridization combines one s orbital and two p orbitals into three equivalent coplanar hybrid orbitals, leaving one unhybridized p orbital. The arrangement supports trigonal planar bonding and π bonding.

sp² hybrid orbital: An orbital formed by mixing one s orbital with two p orbitals, oriented within a common plane. These three equivalent orbitals make the arrangement’s in-plane σ bonds.
Atomic orbital: A quantum-mechanical description of an electron state associated with an atom. Hybridization combines atomic orbitals on a single atom.
Ethene: The simplest alkene, with formula C₂H₄ and a carbon–carbon double bond. Each carbon uses sp² orbitals for σ bonds and an unhybridized p orbital for the π bond.
sp hybridization: A bonding arrangement formed by mixing one s orbital with one p orbital, leaving two unhybridized p orbitals. It produces two linear hybrid directions rather than three coplanar ones.
Trigonal planar molecular geometry: A molecular shape with three bonded atoms arranged around a central atom in one plane, about 120° apart. The three hybrid orbitals point toward the vertices of this characteristic geometry.
s orbital: An atomic orbital with spherical angular symmetry around the nucleus. One s orbital contributes to the three sp² hybrids.
Benzene: A six-carbon aromatic molecule with formula C₆H₆ and a delocalized π-electron system. Its ring carbons are approximately trigonal planar and sp²-hybridized.
sp³ hybridization: A bonding arrangement formed by mixing one s orbital with three p orbitals into four hybrid orbitals. Its four hybrid directions contrast with the three planar directions of sp².
Sigma bond: A covalent bond formed by orbitals overlapping along the axis between two nuclei. End-on overlap of sp² orbitals commonly forms the arrangement’s in-plane bonds.
p orbital: An atomic orbital with two lobes oriented along a spatial axis. Two p orbitals mix, while a third can remain unhybridized.

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