Identify the 'best' Lewis structure based on the guidelines presented in this class. The formal charges have been omitted. O: :0-S-O: .O: 0=s-8: :6-s=0 B :O: :040: :: C Option D is best because none of the oxygen atoms have a formal charge. O: =s=0 || :O: Option C is best because every atom is following the octet rule. D Option A is best because the double bonds are opposite each other so there will be less electron repulsion. Options A and B are best because they have only 2 atoms with formal charge, and the extra electrons are located on the most electronegative atoms.