So4 -2 - Lewis

is the center with two double bonds and two single bonds . The two single-bonded Oxygens carry the negative charges . Sulfur ends up with 12 electrons surrounding it. The Final Form

Because of , those double bonds don't just sit still. They play musical chairs, constantly flipping between all four Oxygen positions. This creates a perfect tetrahedral shape, where every bond is actually equal—a hybrid strength somewhere between a single and a double bond. so4 -2 lewis

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. is the center with two double bonds and two single bonds

Whenever a chemistry student draws ( \textSO_4^2- ), they remember: The Final Form Because of , those double

The geometry of the SO4^2- ion is tetrahedral, with bond angles of approximately 109.5 degrees. This geometry results from the sp3 hybridization of the sulfur atom.

And that is the story of how Sulfur learned to share more than eight, and found peace in the number twelve.