Sulfur is the central atom. There are 6 + 2×7 = 20 electrons, and 4 of them are used to make 2 bonds. The two fluorines take 6 lone pairs, and the remaining four electrons go to the sulfur:

The central atom has a steric number of 4 – two atoms and two lone pairs. The **electron geometry, **therefore**, is tetrahedral**, and the **molecular geometry is bent**.

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Steric number 4 corresponds to *sp ^{3}*-hybridization where the idealized bond angles are 109.5

^{o}. Because the groups on the central atom are not identical, the bond angles differ from the idealized values.

There is a debate that the sulfur is *sp*^{2}-hybridized and the lone pairs are in p orbitals and angles are close to 90^{o} (92^{o}). This contradicts the VSEPR theory, and your final reference should be your instructor.

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