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For 7th edition 6A.15 and 6.5, the questions ask you to draw the structures of SO2 and SO3 respectively. I thought having all of the oxygens with double bonds would be the most stable structure, providing the lowest formal charges. However, the answers show SO2 with 1 double and 1 single bond, and SO3 with 1 double bond and 2 single bonds. Why is this?
The book might be referring to a sulfite (SO3 -2) ion, where having one double bond and two single bonds would account for the -2 charge on the molecule. I'm not really sure about the SO2 because I'm pretty sure sulfur dioxide is supposed to be neutral.
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