C - C bond length in graphite is shorter...

C - C bond length in graphite is shorter than C - C bond length in diamond - Explain.

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In graphite each carbon is in `sp^2` hybridisation and makes three sigma bonds with three neighbouring carbon atoms. Fourth electron forms a `pi` Bond. The electron is delocalised over the whole sheet. Due to this C - C bond length is shorter in graphite. In diamond each carbon is in `sp^3` hybridisation. So every carbon forms four `C - C ` single bonds. `sp^2-sp^2` bond is stronger than `sp^3 -sp^3` bond. Hence C - C bond length in diamond is longer than in graphite.

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C-C bond length in Diamond is

`1.33Å`

`1.54Å`

`1.20Å`

`1.8Å`

The C-C bond lengths in benzene is

`lt C-C` is ethane

`gt C=C` in ethane

`gt C-=C` in ethyne

All the above

What is the C-C bond length (in A^(circ) ) in diamond

1.54

3.34

5.2