6A.15(b) - Lewis structure for SO2 and SO2Cl-
Posted: Sun Jul 28, 2019 11:59 am
We are asked to draw the lewis structure for for Cl-, SO2, and their product. In the answer manual, S02 has S bonded to the first oxygen with a double bond, but to the second oxygen with only a single bond, and then a lone pair. Why would this be the case rather than 2 double bonds, which would minimize formal charge? Similarly, for the product, the answer manual shows S double bonded to one oxygen, but single bonded to O and Cl with a lone pair. Why wouldn't S have double bonds with everything to minimize formal charge? S should have an expanded octet, so I don't see why 6 bonds should be a problem.