Final answer:
HCl has a higher boiling point than F2 because it has a strong dipole moment, leading to higher dipole-dipole attractions compared to the weaker dispersion forces in nonpolar F2.
Step-by-step explanation:
HCl has a higher boiling point than F2 primarily because HCl is a polar molecule with a strong dipole moment, and thus it experiences more significant dipole-dipole interactions. In contrast, F2 is a nonpolar molecule and only experiences relatively weaker London dispersion forces. The intermolecular forces are crucial for determining the boiling points of substances as they indicate how easily molecules can be separated from one another to transition into a gas phase. As HCl molecules have a higher dipole-dipole attraction, they require more energy to be separated, which results in a higher boiling point compared to F2, where the dispersion forces are weaker.
The boiling point of a substance is determined by the strength of the intermolecular forces (IMFs) between its molecules. In the case of HCl and F₂, HCl has a higher boiling point than F₂ because it has a stronger dipole moment, which leads to stronger dipole-dipole attractions between its molecules. The dipole-dipole interactions in HCl molecules are sufficient to cause them to stick together and form a liquid at room temperature, while the weaker dispersion forces in F₂ molecules are not. This is why HCl is a liquid at room temperature, while F₂ is a gas.