sp2hübriidorbitaali

sp2hybridization is a concept in chemistry describing the mixing of one s atomic orbital and two p atomic orbitals to form three degenerate sp2 hybrid orbitals. These three sp2 orbitals are oriented in a trigonal planar geometry, lying in a plane with 120-degree angles between them. The remaining unhybridized p orbital is perpendicular to this plane.

This type of hybridization is commonly observed in atoms that form double bonds, such as in alkenes. For example, in ethylene (C2H4), each carbon atom undergoes sp2 hybridization. Two sp2 orbitals from each carbon atom overlap to form a sigma bond between them. The remaining two sp2 orbitals on each carbon atom overlap with the s orbitals of hydrogen atoms to form carbon-hydrogen sigma bonds. The unhybridized p orbitals on adjacent carbon atoms then overlap side-by-side, forming a pi bond, which is characteristic of the double bond.

The sp2 hybridization model helps explain the planar structure and bond angles observed in molecules like benzene, where all carbon atoms are sp2 hybridized and form a hexagonal ring with delocalized pi electrons. It is a fundamental concept for understanding molecular geometry, bonding, and reactivity in organic chemistry and other fields. The formation of sp2 hybrid orbitals results in stronger sigma bonds compared to those formed by unhybridized orbitals due to better overlap.