So4 Lewis Structure !!better!! -

We represent this by drawing all significant resonance structures connected by double-headed arrows, or more commonly, by drawing a single structure with dashed lines or a circle to indicate delocalized bonding, though this is less precise. The above resonance model (using two double bonds) is excellent for explaining formal charge and bond equivalence. However, it violates a subtle but important rule: in the two-double-bond structure, sulfur has 10 electrons around it (four from each of two double bonds and two from each of two single bonds = 4+4+2+2 = 12? Wait, recalc carefully).

Our goal is to distribute these 32 electrons as bonding pairs (lines) and lone pairs (dots) to satisfy the octet rule for as many atoms as possible. so4 lewis structure

The initial structure (Structure A) looks like this: We represent this by drawing all significant resonance

Formal Charge = (Valence electrons) - (Non-bonding electrons) - ½(Bonding electrons) Wait, recalc carefully)