So4 -2 Lewis ((new)) -

is commonly represented as:

And so, ( \textSO_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. 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. is commonly represented as: And so, ( \textSO_4^2-

If you calculate the formal charges for the "octet-only" version, sulfur has a +2positive 2 charge and each oxygen has a -1negative 1 When Sulfur tried to share a single pair

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

The two double-bonded oxygens have a charge of , the two single-bonded oxygens have a charge of -1negative 1 , and the sulfur is . This adds up to the total ionic charge of -2negative 2 5. Determine Molecular Geometry