For each compound, draw the Lewis structure, determine the geometry using VSEPR theory, determine whether the molecule is polar, identify the hybridization of all interior atoms, and make a sketch of the molecule according to valence bond theory showing orbital overlap: a. COF2 (carbon is the central atom) b. S2Cl2 (ClSSCl) c. SF4.

Verified step by step guidance

1. Step 1: Draw the Lewis structure for each compound. For COF2, place carbon in the center with single bonds to each fluorine and a double bond to oxygen. For S2Cl2, arrange the atoms as Cl-S-S-Cl with single bonds. For SF4, place sulfur in the center with single bonds to each fluorine.
2. Step 2: Use VSEPR theory to determine the geometry of each molecule. For COF2, the geometry is trigonal planar. For S2Cl2, the geometry is bent or V-shaped around each sulfur. For SF4, the geometry is seesaw.
3. Step 3: Determine the polarity of each molecule. COF2 is polar due to the difference in electronegativity between carbon, oxygen, and fluorine. S2Cl2 is nonpolar as the dipoles cancel out. SF4 is polar due to the asymmetrical shape.
4. Step 4: Identify the hybridization of all interior atoms. In COF2, carbon is sp2 hybridized. In S2Cl2, each sulfur is sp3 hybridized. In SF4, sulfur is sp3d hybridized.
5. Step 5: Sketch each molecule according to valence bond theory, showing orbital overlap. For COF2, show sp2 hybrid orbitals on carbon overlapping with p orbitals on oxygen and fluorine. For S2Cl2, show sp3 hybrid orbitals on sulfur overlapping with p orbitals on chlorine. For SF4, show sp3d hybrid orbitals on sulfur overlapping with p orbitals on fluorine.