Explain the difference in properties of diamond and graphite on the basis of their structures.
(N/A)
| Diamond | Graphite |
|---|---|
| It has a three-dimensional crystalline lattice. | It has a two-dimensional layered structure. |
| Each carbon atom is $sp^{3}$ hybridized and bonded to four other carbon atoms. | Each carbon atom is $sp^{2}$ hybridized and bonded to three other carbon atoms. |
| It consists of a rigid tetrahedral network. | It consists of planar hexagonal rings. |
| The $C-C$ bond length is $154 \, pm$. | The $C-C$ bond length is $141.5 \, pm$. |
| It is extremely hard due to its rigid covalent network. | It is soft and slippery because layers can slide over each other. |
| It is an electrical insulator. | It is a good conductor of electricity due to free electrons. |
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