Final answer:
The bond dipole in one P-F bond in PF₅ has uniform polarity, but due to PF₅'s trigonal bipyramidal geometry, the bond dipoles cancel out, resulting in a nonpolar molecule.
Step-by-step explanation:
The geometry of the bond dipole for one P-F bond in the PF5 molecule is such that the polarities of individual P-F bonds are of identical magnitude. However, due to the highly symmetrical trigonal bipyramidal geometry of the molecule, the bond dipoles cancel each other out, resulting in a molecule with an overall dipole moment of zero. Each fluorine atom is positioned at the vertices of a pyramid with one fluorine at the apex and the other four fluorines at the base forming a square. With no lone pair repulsions, we do not expect any bond angles to deviate from the ideal, and the PF5 molecule maintains its nonpolar character despite the polarity of the individual P-F bonds.