Final answer:
The correct Lewis structure for SO3²- involves sulfur with one double bond and two single bonds to oxygen, with two oxygen atoms carrying a negative charge each.
Step-by-step explanation:
The correct Lewis structures for the compound SO3²- (sulfite ion) involves sulfur (S) with one double bond and two single bonds to three oxygen (O) atoms. Each of the oxygens with a single bond carries a negative charge. Considering formal charges, to get the most stable structure, you should distribute the electrons in such a way that the sulfur has an expanded octet and the formal charges on the atoms are minimized. This will result in the sulfur atom having a formal charge of 0, and two oxygens with single bonds each will have a formal charge of -1, while the oxygen with the double bond will have a formal charge of 0. Each oxygen atom, as well as the sulfur atom, will satisfy the octet rule, and there will be lone pairs on the oxygen atoms accordingly.