So4 -2 Lewis Structure [top]

While the structure calculated in Section 3.3 shows two double bonds, resonance theory dictates that the double bond character is evenly distributed. There are six equivalent resonance structures where the double bonds rotate among the four oxygen atoms.

Net charge = 0 + 0 + (–1) + (–1) = –2 – perfect. so4 -2 lewis structure

To reach the most stable state, move one lone pair from two different Oxygen atoms to form with the Sulfur. Result: Sulfur has two double bonds and two single bonds . Final Structure Summary While the structure calculated in Section 3

To draw the Lewis structure for the sulfate ion ( SO42−cap S cap O sub 4 raised to the 2 minus power To reach the most stable state, move one

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.

In the intermediate structure (all single bonds):