Explain the difference in properties of diamond and graphite on the basis of their structures.

 Diamond Graphite It has a crystalline lattice. It has a layered structure. In diamond, each carbon atom is ${\mathrm{sp}}^{3}$ hybridized and is bonded to four other carbon atoms through a $\mathrm{\sigma }$ bond. In graphite, each carbon is ${\mathrm{sp}}^{2}$ hybridized and is bonded to three other carbon atoms through a $\mathrm{\sigma }$ bond. The fourth electron forms a n bond. It is made up of tetrahedral units. It has a planar geometry. The C-C bond length in diamond is 154 pm. The C-C bond length in graphite is 141.5 pm. It has a rigid covalent bond network which is difficult to break. It is quite soft and its layers can be separated easily. It acts as an electrical Insulator. It is a good conductor of electricity.