In a methane molecule (CH4), the carbon atom undergoes sp3 hybridization. During sp3 hybridization, one 2s orbital and three 2p orbitals of the carbon atom combine to form four equivalent sp3 hybrid orbitals.

These four sp3 hybrid orbitals are arranged tetrahedrally around the carbon atom, with bond angles of approximately 109.5 degrees between them. Each sp3 hybrid orbital of carbon forms a covalent bond with the 1s orbital of a hydrogen atom, resulting in four C-H bonds of equal length and strength. Therefore, the hybridization of the carbon atom in methane is sp3.