In graphite, each carbon atom is bonded to three other carbon atoms-

In graphite, each carbon atom is covalently bonded to three other carbon atoms. This bonding occurs through sp2 hybridization, where one s and two p orbitals combine to form three hybridized orbitals. These orbitals are arranged in a trigonal planar geometry, resulting in the carbon atoms being positioned in the same plane. This arrangement forms a two-dimensional sheet composed of a hexagonal array of six-membered carbon rings. These individual layers, often referred to as graphene, are held together by weak out-of-plane van der Waals forces, allowing them to slide over one another [2]. Unlike diamond, which forms a three-dimensional tetrahedral lattice by bonding to four carbon atoms, graphite's planar hexagonal structure is responsible for its unique properties such as high in-plane conductivity and lubricity [1].

Sources

1. [2] https://www.sciencedirect.com/science/article/abs/pii/S0927025615004000
2. [1] https://www.nature.com/articles/s41467-025-64971-1