The C - C bond length in benzene lies between | vedclass

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(A) Due to the delocalization of $\pi$ electrons,benzene exhibits resonance.
This resonance leads to the formation of hybrid structures where all $C

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Resonance

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(A) Due to the delocalization of $\pi$ electrons,benzene exhibits resonance.
This resonance leads to the formation of hybrid structures where all $C - C$ bonds have partial double bond character.
Consequently,the bond length is intermediate between a pure single bond $(1.54 \ \mathring{A})$ and a pure double bond $(1.34 \ \mathring{A})$.

The $C - C$ bond length in benzene lies between a single and a double bond. The reason is:

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