Final answer:
SO₂ and HCl both exhibit polar interactions, with dipole-dipole forces being the significant intermolecular force, due to their difference in electronegativity between atoms and molecular shape allowing for a net dipole moment.
Step-by-step explanation:
The student has asked which of the given substances has polar interactions (dipole–dipole forces) between molecules. Among the options provided, SO2 and HCl are examples of molecules that exhibit dipole-dipole interactions. The molecule of SO2 is polar because it has a bent shape and a difference in electronegativity between the sulfur and oxygen atoms that creates a dipole. Similarly, HCl is polar because of the difference in electronegativity between the hydrogen and chlorine atoms.
Regarding the example provided, CHCl3 is a polar molecule due to the difference in electronegativity between chlorine and carbon/hydrogen, and the molecular geometry allowing for an overall dipole moment. On the other hand, CCl4 is nonpolar because, despite the polar C-Cl bonds, the molecule's symmetrical tetrahedral shape allows the bond polarities to cancel out each other, resulting in no net dipole moment.
Thus, out of the options provided, SO2 and HCl have polar interactions due to their polar nature, which leads to dipole-dipole forces between their molecules.