d. S₂O₈²⁻ (peroxydisulfate ion)
1. Lewis Structure: 24 electron pairs (12 from each sulfur and 6 from each of the four oxygens, plus 2 extra electrons from the 2- charge). One peroxo bond between the two oxygen atoms and one single bond each with the two sulfur atoms. Each sulfur atom forms two double bonds with adjacent oxygen atoms.
2. Molecular structure: For each sulfur atom, there are four bonding groups. Electron geometry is tetrahedral, molecular geometry is tetrahedral, with bond angles close to \(109.5^{\circ}\).
3. Hybrid orbitals: For each sulfur, the hybridization state is sp³ due to four electron groups.
e. SO₃²⁻ (sulfite ion)
1. Lewis Structure: 26 electron pairs (6 from sulfur and 6 from each of the three oxygens, plus 2 extra electrons from the 2- charge). Sulfur forms one double bond and two single bonds with the three oxygen atoms, and each oxygen has three lone pairs.
2. Molecular structure: Sulfur has four electron groups (3 bonding, 1 lone pair). Electron geometry is tetrahedral, molecular geometry is trigonal pyramidal, bond angles slightly less than \(109.5^{\circ}\).
3. Hybrid orbitals: Sulfur's hybridization state is sp³ due to four electron groups.
f. SO₄²⁻ (sulfate ion)
1. Lewis Structure: 32 electron pairs (6 from sulfur, 6 from each of the four oxygens, plus 2 extra electrons from the 2- charge). Sulfur forms double bonds with each of the four oxygen atoms, and each oxygen has two lone pairs.
2. Molecular structure: Sulfur has four electron groups (all bonding), electron geometry is tetrahedral, molecular geometry is tetrahedral, bond angles close to \(109.5^{\circ}\).
3. Hybrid orbitals: Sulfur's hybridization state is sp³ due to four electron groups.
g. SF₂
1. Lewis Structure: 14 electron pairs (6 from sulfur, 7 from each of the two fluorines). Sulfur forms single bonds with each fluorine and has three lone pairs.
2. Molecular structure: Sulfur has five electron groups (2 bonding, 3 lone pairs), electron geometry is trigonal bipyramidal, molecular geometry is bent/V-shaped, bond angles less than \(109.5^{\circ}\).
3. Hybrid orbitals: Sulfur's hybridization state is sp³ᵈ due to five electron groups.
h. SF₄
1. Lewis Structure: 20 electron pairs (6 from sulfur, 7 from each of the four fluorines). Sulfur forms single bonds with each fluorine and has two lone pairs.
2. Molecular structure: Sulfur has six electron groups (4 bonding, 2 lone pairs), electron geometry is octahedral, molecular geometry is square planar, bond angles \(90^{\circ}\) and \(180^{\circ}\).
3. Hybrid orbitals: Sulfur's hybridization state is sp³ᵈ² due to six electron groups.
i. SF₆
1. Lewis Structure: 48 electron pairs (6 from sulfur, 7 from each of the six fluorines). Sulfur forms single bonds with each fluorine.
2. Molecular structure: Sulfur has six electron groups (all bonding), electron geometry is octahedral, molecular geometry is octahedral, bond angles \(90^{\circ}\) and \(180^{\circ}\).
3. Hybrid orbitals: Sulfur's hybridization state is sp³ᵈ² due to six electron groups.
j. F₃S-SF
1. Lewis Structure: 22 electron pairs (12 from each sulfur, 7 from each of the four fluorines). Each sulfur forms single bonds with three fluorine atoms and a single bond between the two sulfur atoms.
2. Molecular structure: Each sulfur has four electron groups (3 bonding, 1 lone pair), electron geometry is tetrahedral, molecular geometry is trigonal pyramidal, bond angles slightly less than \(109.5^{\circ}\).
3. Hybrid orbitals: Sulfur's hybridization state is sp³ for each sulfur atom due to four electron groups.
k. SF₅⁺
1. Lewis Structure: 34 electron pairs (6 from sulfur, 7 from each of the five fluorines, minus 1 electron due to the +1 charge). Sulfur forms single bonds with each of the fluorine atoms.
2. Molecular structure: Sulfur has five electron groups (all bonding), electron geometry is trigonal bipyramidal, molecular geometry is trigonal bipyramidal, bond angles \(120^{\circ}\) and \(90^{\circ}\).
3. Hybrid orbitals: Sulfur's hybridization state is sp³ᵈ due to five electron groups.
