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There are no double bonds in benzene.

In a benzene molecule, every carbon is attached to another two carbon atoms and to a hydrogen atom. Then there is a free p-orbital to every carbon atom. All of these over lap to form delocalized orbitals. It is experimentally proved that C-C bond distance in benzene are all the same and liebetween the actual lengths of a C-C bond and a C=C bond.

In the valence bond description of bonding there is resonance between two principal forms, each has 3 double bonds. The net effect of the resonance is very similar to the molecular orbital approach above.

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