How do the carbon atoms in diamond bond?

In a diamond, each carbon atom forms four covalent bonds with other carbon atoms in a tetrahedral structure.

In more detail, diamond is an allotrope of carbon, meaning it is one of the different forms in which carbon can exist. In a diamond, each carbon atom is covalently bonded to four other carbon atoms. These bonds are incredibly strong and are arranged in a tetrahedral structure, which means that the bonds are spread out in three dimensions. This arrangement results in a rigid, lattice-like structure that gives diamond its renowned hardness.

The carbon atoms in a diamond are all sp3 hybridised. This means that one 2s orbital and three 2p orbitals in the carbon atom have merged to form four new equivalent orbitals. These orbitals are then used to form the four covalent bonds with other carbon atoms. The bonds are evenly distributed around the carbon atom, creating the tetrahedral structure.

The strength of these covalent bonds and the rigid structure they form are what make diamonds so hard and durable. It's also why diamonds have such a high melting point and are excellent conductors of heat. However, diamonds do not conduct electricity because all of the electrons are involved in the covalent bonds and there are no free electrons to carry an electric charge.

In summary, the carbon atoms in a diamond are bonded together through strong covalent bonds in a tetrahedral structure. This structure, along with the sp3 hybridisation of the carbon atoms, gives diamond its unique properties.