What is the hybridization state of the central carbon atom in a methane molecule, and what is the corresponding bond angle between carbon-hydrogen bonds?

💡 Solution & Explanation

In methane, the central carbon atom forms four equivalent single covalent bonds directed toward the corners of a regular tetrahedron. This tetrahedral geometry corresponds to sp3 hybridization of the carbon valence orbitals resulting in bond angles of one hundred nine point five degrees. Alternative options describe trigonal planar or linear geometries typical of double or triple bonds. VSEPR theory explains molecular shapes through electron pair repulsion minimization.