Final answer:
Chlorine has weaker intermolecular forces at room temperature than sulfur. Chlorine is a gas while sulfur is a solid, pointing to sulfur having stronger dispersion forces.
Step-by-step explanation:
Among sulfur and chlorine, chlorine demonstrates relatively weaker intermolecular forces at room temperature compared to sulfur. This is due to the fact that chlorine (Cl₂) exists as a diatomic molecule and is a gas at room temperature, indicating weaker dispersion forces. On the other hand, sulfur typically exists in the form of S₈ molecules, which are solid at room temperature, suggesting stronger intermolecular forces are in play. The larger and heavier a molecule, the greater the number of electrons and the stronger the dispersion forces it can exhibit. Thus, sulfur's solid state at room temperature reflects the presence of stronger dispersion forces compared to the gaseous state of chlorine at the same temperature.