In the diagram attached, the 3 resonance structures of arenium ion bonded to H electrophile are shown.I labelled the carbon atoms in one of the structures for convenience. From the diagram, the A and B carbons, and D and E carbons, have a double bond between them for two of the resonance structures; whereas the B and C carbons, and C and D carbons, have a double bond between them for only one of the resonance structures. From this can we safely assume that in the resonance hybrid, the bond between the A and B carbons, and D and E carbons have a high percentage of double bond character; compared to the bond between the B and C carbons, and C and D carbons, which have a higher percentage of single bond character? Also since the bond between A and B carbons (also between C and D carbons) are double bonds for 2 of the 3 resonance structures can we say that in the resonance hybrid, the charge between the A and B carbons is (2/3)(2) (as the single bond remains fixed and the 2 electrons of double bond become delocalized)? And that each of the carbon atoms has a charge of -(2/3).