Chemistry
Chemistry
Problem
Draw two different Lewis formulas for , one of which obeys the octet rule for all its atoms, the other of which has an octet for S expanded to 12 electrons. Use formal charges to determine which is the preferred structure.Intuitive explanation
The key insight is that sulfur can accommodate more than 8 electrons using d-orbitals, giving you two valid Lewis structures to compare. The first uses only single and double bonds to satisfy the octet rule for sulfur; the second distributes negative charge across oxygen atoms by adding extra S–O double bonds, expanding sulfur's valence shell to 12 electrons. Formal charges reveal which structure minimizes charge separation and places negative charge on the most electronegative atoms—that's your preferred form.
Intuitive explanation
The key insight is that sulfur can accommodate more than 8 electrons using d-orbitals, giving you two valid Lewis structures to compare. The first uses only single and double bonds to satisfy the octet rule for sulfur; the second distributes negative charge across oxygen atoms by adding extra S–O double bonds, expanding sulfur's valence shell to 12 electrons. Formal charges reveal which structure minimizes charge separation and places negative charge on the most electronegative atoms—that's your preferred form.