So4 Lewis Structure -

Valence = 6. Non-bonding = 6 (three lone pairs). Bonding = 2 (one single bond). (FC = 6 - 6 - ½(2) = 6 - 6 - 1 = -1)

Now the formal charges are: S (0), two O’s (0), and two O’s (-1). Sum = (0 + 0 + (-1) + (-1) = -2). This is much better! But can we do even better? so4 lewis structure

Before drawing any bonds, we must calculate the total number of valence electrons available. This is the currency of all Lewis structures. Valence = 6

Each has FC = 0 (as calculated above).

The resulting "best" structure features and two single bonds . Final Formal Charges: Double-bonded Oxygens: 0 (FC = 6 - 6 - ½(2) =

Let’s recount the electrons around sulfur in Structure B:

Connect each oxygen to the sulfur with a single bond (a line representing 2 electrons). This uses up (4 \text bonds \times 2 \text electrons = 8) electrons.