So4 -2 Lewis ~repack~ Site

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

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.

He summoned two of the Oxygen atoms. "You two," he said, "will share double bonds with me." so4 -2 lewis

One day, Sulfur decided to host the biggest gathering in the valley. He sent invitations to four Oxygen atoms.

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. Every millisecond, the double bonds would hop from

Sulfur’s eyes lit up. "Of course!"

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. It was the backbone of gypsum, Epsom salts,

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