Final answer:
HCl has a higher boiling point than F2 due to the presence of stronger dipole-dipole attractions in HCl compared to the weaker dispersion forces in F2, resulting in the need for more energy to overcome the IMFs in HCl.
Step-by-step explanation:
The fact that HCl has a higher boiling point than F2 can be adequately explained by the type and strength of intermolecular forces (IMFs) present in these substances. HCl molecules exhibit dipole-dipole attractions due to the significant difference in electronegativity between the hydrogen and chlorine atoms, which creates a dipole moment. On the other hand, F2 is a nonpolar molecule and only exhibits weaker dispersion forces. The dipole-dipole attractions in HCl lead to a higher boiling point (188 K) than F2, whose boiling point is only 85 K. This is a reflection of the stronger IMFs in HCl, which require more energy to overcome during the phase change from liquid to gas.