The difference in properties of diamond and graphite on the basis of their structures is listed below.
|In diamond, strong three-dimensional networks are formed due to the presence of covalent bonds.||Graphites are formed due to the weak van der Waals force of attraction.|
|Hard in nature||Soft in nature.|
|Since molecules are closely packed they have high density.||Because of the large gap between the molecules, they have low density.|
|Since there is no free carbon atom, the diamond does not conduct electricity.||Because of the presence of free carbon atom in graphite they can conduct electricity.|