O || O⁻─S─O⁻ || O

Net charge = (+2) + 4×(–1) = –2 (correct total), but having a +2 on sulfur is unfavorable.

Net charge = (+1) + 3×(–1) + 0 = –2 → better but not optimal.

Each single bond uses 2 electrons. With four bonds, we have used .*Remaining: 24 electrons. 3. Distribute Remaining Electrons

In the basic octet-only version, Sulfur has a formal charge of and each Oxygen has -1 . Because Sulfur is in Period 3, it can expand its octet to reduce these charges.