Here's why:

* Intermolecular forces: Bromine (Br₂) and chlorine (Cl₂) are both diatomic halogens. They experience London dispersion forces, which are the weakest type of intermolecular force. However, bromine is a larger molecule than chlorine.

* Larger size, stronger forces: The larger size of bromine means its electron cloud is more polarizable, leading to stronger London dispersion forces. Stronger intermolecular forces require more energy to overcome, resulting in a higher boiling point.

Boiling Points:

* Chlorine (Cl₂): -34.04 °C

* Bromine (Br₂): 58.8 °C

Therefore, bromine has a higher boiling point than chlorine.