Final answer:
Each carbon atom in the H3C—CH3 molecule (ethane) is sp3 hybridized, forming four sigma bonds in a tetrahedral arrangement using sp3 hybrid orbitals.
Step-by-step explanation:
The molecule in question is H3C—CH3, commonly known as ethane. In ethane, each carbon atom is sp3 hybridized. This hybridization occurs when one s orbital mixes with three p orbitals to form four equivalent sp3 hybrid orbitals. In ethane, each carbon forms single bonds with three hydrogen atoms and one single bond with another carbon atom. Each of these single bonds is formed by the overlap of one sp3 hybrid orbital from the carbon atom with the s orbital of a hydrogen atom, which is referred to as a sp3-s bond.
The sp3 hybridization allows for the formation of four sigma bonds arranged in a tetrahedral geometry around each carbon atom. Every hybrid orbital contributes one electron to the bond, resulting in a stable configuration for the ethane molecule.