For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. a. \(\mathrm{SO}_{2}\) b. \(\mathrm{SO}_{3}\) c. d. e. \(\mathrm{SO}_{3}^{2-}\) i. \(\mathrm{SF}_{6}\) f. \(\mathrm{SO}_{4}^{2-}\) j. \(\mathrm{F}_{3} \mathrm{~S}-\mathrm{SF}\) g. \(\mathrm{SF}_{2}\) \(\mathbf{k} . \mathrm{SF}_{5}{ }^{+}\) h. \(\mathrm{SF}_{4}\)

To find the total number of valence electrons, we need to count the individual valence electrons for each atom: Sulfur (S) has 6 valence electrons, and Oxygen (O) has 6 valence electrons. Total valence electrons in \(\mathrm{SO}_{2}\) = (1 * 6) + (2 * 6) = 18

Place S at the center as the central atom with two O atoms connected by single bonds: O-S-O Distribute the remaining 14 electrons as lone pairs, with each O atom having 3 lone pairs.

\(\mathrm{SO}_{2}\) has a bent molecular geometry due to the presence of 1 lone pair on S. The bond angle between the O-S-O is approximately 120°.

Sulfur uses three orbitals (one for each bond and one for the lone pair) in the molecule. Thus, Sulfur's hybridization is \(\mathrm{sp^{2}}\) for \(\mathrm{SO}_{2}\). Repeat the same steps for the remaining molecules/ions: b. \(\mathrm{SO}_{3}\) Lewis Structure: O=S=O (with a double bond to each O) Molecular Structure: Trigonal planar Hybrid Orbitals: \(\mathrm{sp^{2}}\) c. \(\mathrm{SO}_{3}^{2-}\) Lewis Structure: O=S-O (1 double bond, one single bond, sulfur has 1 lone pair) Molecular Structure: Bent Hybrid Orbitals: \(\mathrm{sp^{2}}\) i. \(\mathrm{SF}_{6}\) Lewis Structure: F-S-F (no lone pairs on Sulfur) Molecular Structure: Octahedral Hybrid Orbitals: \(\mathrm{sp^{3}d^{2}}\) f. \(\mathrm{SO}_{4}^{2-}\) Lewis Structure: O=S=O (with a double bond to each O) Molecular Structure: Tetrahedral Hybrid Orbitals: \(\mathrm{sp^{3}}\) j. \(\mathrm{F}_{3} \mathrm{~S}-\mathrm{SF}\) Lewis Structure: F-S-F (with 1 lone pair on Sulfur) Molecular Structure: T-shape Hybrid Orbitals: \(\mathrm{sp^{3}d}\) g. \(\mathrm{SF}_{2}\) Lewis Structure: F-S-F (with 2 lone pairs on Sulfur) Molecular Structure: Bent Hybrid Orbitals: \(\mathrm{sp^{3}}\) k. \(\mathrm{SF}_{5}{ }^{+}\) Lewis Structure: F-S-F (with no lone pairs on Sulfur) Molecular Structure: Trigonal bipyramidal Hybrid Orbitals: \(\mathrm{sp^{3}d}\) h. \(\mathrm{SF}_{4}\) Lewis Structure: F-S-F (with 1 lone pair on Sulfur) Molecular Structure: See-saw shape Hybrid Orbitals: \(\mathrm{sp^{3}d}\)