Explainthe difference in properties of diamond and graphite on the basis oftheir structures.
Explainthe difference in properties of diamond and graphite on the basis oftheir structures.
Diamond
Graphite
It has a crystalline lattice.
It has a layered structure.
In diamond, each carbon atom is sp3 hybridised and is bonded to four other carbon atoms through a σ bond.
In graphite, each carbon atom is sp2 hybridised and is bonded to three other carbon atoms through a σ bond. The fourth electron forms a π 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.
| Diamond | Graphite |
| It has a crystalline lattice. | It has a layered structure. |
| In diamond, each carbon atom is sp3 hybridised and is bonded to four other carbon atoms through a σ bond. | In graphite, each carbon atom is sp2 hybridised and is bonded to three other carbon atoms through a σ bond. The fourth electron forms a π 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. |
