So4 -2 Lewis -

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

If Sulfur followed the rules perfectly, it would form four with the Oxygens. This gives everyone an octet, but it leaves Sulfur with a hefty formal charge. In nature, molecules prefer to be "relaxed," and high formal charges are stressful. The "Hypervalent" Twist so4 -2 lewis

The sulfur atom is the central atom, and the four oxygen atoms are bonded to it. We start by drawing single bonds between the sulfur atom and each of the four oxygen atoms. This uses 8 electrons (2 electrons per bond). The remaining electrons are 32 - 8 = 24. To the other two Oxygens, he gave single

charge. Sulfur is a Period 3 element, meaning it can have an . The "Hypervalent" Twist The sulfur atom is the

is commonly represented as:

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.