Final answer:
The bond dipole geometry for one PF bond in PF5 is trigonal bipyramidal. PF5, designated as AX5, has five nuclei and no lone pairs, resulting in a symmetrical trigonal bipyramidal shape with zero net dipole moment.
Step-by-step explanation:
The geometry of the bond dipole for one PF bond in the PF5 molecule is trigonal bipyramidal. This is because PF5 has five nuclei around the central phosphorus atom and no lone pairs of electrons. The molecule is designated as AX5 where all electron groups are bonding pairs, which leads to no lone pair repulsions and expectations of ideal bond angles. This molecular geometry of PF5 is indeed trigonal bipyramidal, consistent with the overall symmetry of the molecule where each P-F bond dipoles are arranged such that they cancel out, giving PF5 a zero net dipole moment.