All three of the structures feature covalent bonding.
If you draw a diagram for each, you will note that CIF3 would include C as the central atom with an I and 3 F around it, all with single bonds. Because F is the most electronegative atom, there will be a partial negative charge towards the F opposing I (draw it out and you will see it). Therefore, this is a polar molecule.
For PF3, P will be the central atom. However, you only have 3 F atoms surrounding it, so P would need 2 additional electrons to satisfy its octet. So, drawing the diagram, you will include 3F atoms along with a lone pair around P. The lone pair results in a partial negative charge on the molecule, therefore it is polar.
BF3 may look similar to PF3, but B does not adhere to the octet rule. Thus, if you draw the BF3 diagram, it will include B as the central atom and 3 F's around it, but without a lone pair. Because of its high symmetry, BF3 is non-polar.
