What is the hybridisation of carbon in diamond?

sp³

The hybridization of carbon in diamond is 3. sp³.

In sp³ hybridization, one s orbital and three p orbitals combine to form four equivalent sp³ hybrid orbitals. These orbitals are arranged tetrahedrally around the carbon atom. In diamond, each carbon atom is bonded to four other carbon atoms by single covalent bonds. The sp³ hybrid orbitals on each carbon atom overlap with the sp3 hybrid orbitals on the other four carbon atoms to form these bonds.

The sp² hybridization has three equivalent sp² hybrid orbitals and one p orbital. The sp² hybrid orbitals are arranged in a trigonal planar configuration. In graphite, each carbon atom is bonded to three other carbon atoms by single covalent bonds. The sp² hybrid orbitals on each carbon atom overlap with the sp² hybrid orbitals on the other three carbon atoms to form these bonds. The p orbital on each carbon atom overlaps with a p orbital on an adjacent carbon atom to form a pi bond.

The sp hybridization has one sp hybrid orbital and one p orbital. The sp hybrid orbital is linear. In acetylene, each carbon atom is bonded to one other carbon atom by a triple bond. The sp hybrid orbital on each carbon atom overlaps with the sp hybrid orbital on the other carbon atom to form a sigma bond. The p orbitals on each carbon atom overlap to form two pi bonds.

The sp³d hybridization has four sp³d hybrid orbitals and one d orbital. The sp³d hybrid orbitals are arranged in a trigonal bi-pyramidal configuration. This hybridization is rarely seen in carbon compounds.

Therefore, the hybridization of carbon in diamonds is sp³.