The hybridization state of carbon in methane (CH4) is sp3.
Methane's central carbon atom forms four sigma bonds with four hydrogen atoms. To accommodate these four bonds, the carbon atom undergoes sp3 hybridization. This process involves mixing one s orbital and three p orbitals to create four new, equivalent sp3 hybrid orbitals.
Here's a breakdown:
- Atomic Orbitals Involved: One 2s orbital and three 2p orbitals of carbon.
- Hybridization Process: The 2s and 2p orbitals mix to form four sp3 hybrid orbitals.
- Geometry: These four sp3 hybrid orbitals arrange themselves in a tetrahedral geometry around the carbon atom, minimizing electron repulsion. Each sp3 orbital then forms a sigma bond with a 1s orbital of a hydrogen atom.
- Bond Angle: The bond angle in methane is approximately 109.5 degrees, consistent with perfect tetrahedral geometry.
The sp3 hybridization explains methane's stable tetrahedral structure and its ability to form strong covalent bonds with four hydrogen atoms.
