Final answer:
The Lewis structures and molecular geometries for PF5 and PF6- are trigonal bipyramidal and octahedral, respectively. POF3 has a tetrahedral shape with a P=O double bond and P-F single bonds.
Step-by-step explanation:
The question asks to draw the Lewis structures and describe the geometry of various phosphorus fluoride compounds and a phosphorus oxyfluoride compound.
For PF4, while this specific formula is incorrect as it does not match any known stable phosphorus fluoride compound, we can assume it to be a typo for PF3 or PF5.
For PF5, the electron pair geometry is trigonal bipyramidal, with a molecular structure that is also trigonal bipyramidal. Each equatorial P-F bond is 120° apart and each axial P-F bond is 90° from equatorial bonds.
For PF6-, it has an octahedral electron pair geometry with an octahedral molecular structure; all P-F bonds are 90° apart.
For POF3, the Lewis structure should include a double bond between phosphorus and oxygen, and three single bonds from phosphorus to each fluorine, resulting in a tetrahedral shape with slightly less than 109.5° between bonds due to the difference in electron pair repulsion between the P=O double bond and the P-F single bonds.