Answer
Polar: IF5, PCl3, IF
Non-polar: XeF6, SiCl4, CSe2
Step-by-step explanation
XeF6 should be non-polar because its molecular geometry is octahedral.
SiCl4 is a non-polar compound because of its linear and symmetrical shape.
IF5 is polar in nature. The molecule has a bent-shaped geometrical structure because of lone pair and bond pair repulsion as per VSEPR theory due to which there occurs an imbalance in charge distribution across the molecule.
PCl3 is a polar molecule because of its tetrahedral geometrical shape having a lone pair on the Phosphorus atom and the difference between the electronegativity of Chlorine(3.16) and Phosphorus(2.19) atoms resulting in unequal sharing of electrons and developing positive and negative poles across the molecule making it a polar molecule.
IF is a polar covalent molecule. Fluorine is more electronegative than iodine due to which dipole moment is generated that makes the IF a polar molecule.
CSe2 is non-polar molecule. This is because the molecular geometry of CSe2 is linear with symmetric charge distribution on the central atom.