Final answer:
ICl will have a higher boiling point than Br₂ because it is a polar molecule with dipole-dipole attractions in addition to London dispersion forces, which require more energy to overcome compared to the only dispersion forces present in nonpolar Br₂.
Step-by-step explanation:
Predicting the higher boiling point between ICl and Br₂ involves understanding the intermolecular forces at play. ICl and Br₂ have similar molar masses but differ in polarity. ICl is a polar molecule which means it has a net dipole due to an unequal distribution of electrons.
This gives rise to dipole-dipole attractions in addition to the London dispersion forces which Br₂ (a nonpolar molecule) solely relies on. Dipole-dipole interactions are generally stronger than dispersion forces, leading to a higher boiling point for ICl. Hence, ICl will have the higher boiling point compared to Br₂, which does not have dipole-dipole attractions.