There are four carbon atoms and ten hydrogen atoms in butane. Each carbon atom undergoes sp3 hybridisation, resulting in the formation of four equivalent sp3 hybrid orbitals. These sp3 orbitals overlap with the 1s orbitals of hydrogen atoms to form ten C-H sigma bonds.
However, there is no hybridisation in the carbon-carbon bond. The carbon-carbon bond in butane is formed by the overlap of two sp3 orbitals, one from each carbon atom. This type of bond is known as a sigma bond and is the strongest type of covalent bond.
Therefore, butane does not contain any pure or hybridised orbitals.
