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Draw the two possible Lewis structures of benzene (C_6H_6) in which the six C atoms form a ring structure with alternate single and double bonds. Use the two Lewis structures to explain why the C-C bond distances in benzene are shorter than a C-C single bond but longer than a C=C double bond. (When multiple Lewis structures can be drawn for the same molecular structure, these Lewis structures are called resonance structures.) Optional Exercises (if time permits): Draw the two possible Lewis structures of ozone (O_3). Note that the O-O bond distance in O_3 is shorter than that in H_2O_2 but longer than that in O_2. Why? State your reasoning.
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