Final answer:
The correct answer is option b. The correct Lewis structure indicates a trigonal planar electron-pair geometry around sulfur with sp² hybridization and 120-degree bond angles. Option b is the correct answer.
Step-by-step explanation:
To determine the correct option for the hybridization and bond angles of a molecule with an F-S-F bond, we consider the number of electron regions around the central sulfur atom. If sulfur has five regions of electron density, as in SF4, the hybridization would be sp³d, with bond angles of 90 and 120 degrees. However, with only two bonds and one lone pair, as the question suggests, the electron-pair geometry is trigonal planar, and the hybridization of the sulfur atom is sp². The geometry of the sp² hybrid orbitals is also trigonal planar with bond angles of 120 degrees.
Looking at various sulfur compounds helps clarify this concept. For instance, SO2, which has a structure similar to the one implied in the question, has sp² hybridization and exhibits a trigonal planar shape with 120-degree angles. On the other hand, SO4 with four regions of electron density, indicates sp³ hybridization, and H2S, with bent geometry due to two lone pairs, suggests sp³ hybridization but with smaller bond angles due to less effective hybridization on the larger sulfur atom.
Therefore, the correct answer is option b. Hybridization =sp². Angle 120.