Hybridization
Definition and meaning of Hybridization in chemistry.
Hybridization is the mixing of an atom's atomic orbitals (such as s and p) to form a new set of equivalent hybrid orbitals better suited for bonding. It explains molecular geometries and bond angles that plain, unmixed s and p orbitals could not produce.
In more detail
The main types are sp (linear, 180 degrees), sp2 (trigonal planar, 120 degrees), and sp3 (tetrahedral, 109.5 degrees), with the type determined by the number of sigma-bonding and lone-pair electron domains around the central atom, consistent with VSEPR theory. Hybridization is a bonding model within valence bond theory, not a directly observable property, used to rationalize bond angles and bond strengths. Any p orbitals left unhybridized are available for pi bonding, which is why sp2 carbons can form one pi bond and sp carbons can form two, as in double and triple bonds.
Key facts
| Field | General Chemistry |
|---|---|
| Common types | sp, sp2, sp3 |
| Example molecule | CH4 (sp3) |
| sp3 bond angle | 109.5° |
In methane (CH4), carbon's one 2s and three 2p orbitals combine to form four equivalent sp3 hybrid orbitals. Each overlaps with a hydrogen 1s orbital, giving methane its tetrahedral shape with 109.5 degree bond angles.
Frequently asked questions
Is hybridization something that can be measured directly?
No. Hybridization is a theoretical model within valence bond theory used to explain observed geometries and bond angles; it is not a physically measurable quantity itself.
How is the hybridization of an atom determined?
Count the number of sigma bonds plus lone pairs on the central atom (its electron domains per VSEPR theory); two domains give sp, three give sp2, and four give sp3.