So4 -2 Lewis !!better!! -

Every millisecond, the double bonds would hop from one Oxygen to another. Click. Now a different Oxygen has the double bond. Click. Now another.

But there was a problem. When Sulfur tried to share a single pair of electrons with each Oxygen (making four single bonds), he ran out of electrons. He was left with a miserable +4 formal charge, and each Oxygen had a -1 charge. The structure was unstable, like a table with three legs. so4 -2 lewis

And so, ( \text{SO}_4^{2-} ) became the most stable, famous, and well-respected ion in the valley. It was the backbone of gypsum, Epsom salts, and bathtub relaxation. Every millisecond, the double bonds would hop from

In reality, all four Sulfur-Oxygen bonds were —a perfect average between a single and a double bond (called a bond order of 1.5). The negative charge was spread evenly across all four Oxygens. When Sulfur tried to share a single pair

To the other two Oxygens, he gave single bonds but with a heavy heart: "You will carry the negative charge for the team."

"Let's bond!" said Sulfur. "I have six valence electrons of my own. You four each have six. Together, we can form a stable ring of eight."

Suddenly, a wise old floated by. "You have a secret power, Sulfur," it whispered. "You are in Period 3. You can expand your octet. Use your empty 3d orbitals ."