Benzene is often drawn with alternating C-C (single) and C=C (double) bonds. This drawing implies that the electrons making up each of these double bonds are localized to the two carbons between which they are drawn. If this were the case, we would be able to measure two different lengths for the carbon-carbon bonds in benzene (154 pm and 134 pm).
However, experimental observations suggest a different structure for benzene where the carbon- carbon bond lengths are the same within the molecule, implying that the electrons originally drawn in the double bonds are delocalized among all six the carbons.
Explain how the kinetic energy of the electrons changes when the electrons that would be localized in the C=C bonds are delocalized over all of the carbons in the benzene molecule.
This would lower the kinetic energy because it lowers... View the full answer