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.
To the other two Oxygens, he gave single bonds but with a heavy heart: "You will carry the negative charge for the team."
In the bustling molecular city of , there lived a famous central figure named Sulfur . Sulfur was a bit of an overachiever. While his neighbors, like Oxygen and Hydrogen, were happy with simple bonds, Sulfur wanted to connect with everyone. so4 -2 lewis
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.
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 ." In reality, all four Sulfur-Oxygen bonds were —a
"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."
But the Oxygen atoms were democratic. They didn't like that only two got the "honor" of a double bond. So they did something magical: . Sulfur was a bit of an overachiever
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.