The boiling point of bromine is 59 °c. which of the following best predicts the boiling point of iodine monochloride, a polar compound?
higher than 59 °c because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine.
lower than 59 °c because ionic bonding in bromine is stronger than covalent bonding in iodine monochloride.
lower than 59 °c because dipole-dipole interactions in iodine monochloride are weaker than in bromine.
higher than 59 °c because ionic bonding in iodine monochloride is stronger than h-bonding in bromine.

Higher than 59 °C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine.

Explanation:

Intermolecular forces are broadly classified into four types:

1) Ionic

2) Hydrogen bonding

3) Dipole-dipole

4) London dispersion

The strongest is the ionic interaction while the weakest are the dispersion forces. Bromine () is a non-polar molecule due to the absence of a permanent dipole. The only force of attraction in non-polar molecules are the weak dispersion forces.

In contrast iodine monochloride () is a polar molecule which are held together dipole-dipole forces that are stronger than the London dispersion forces.

Hence, the boiling point of () would be higher than that of  ()