Here's why:

* Intermolecular Forces: Bromine (Br₂) and chlorine (Cl₂) are both diatomic halogens. They experience van der Waals forces, specifically London dispersion forces. These forces arise from temporary fluctuations in electron distribution, creating temporary dipoles.

* Size and Polarizability: Bromine atoms are larger than chlorine atoms. Larger atoms have a greater electron cloud, making them more polarizable. This means that temporary dipoles are stronger and easier to form in bromine compared to chlorine.

* Stronger Intermolecular Forces: Stronger London dispersion forces in bromine result in a higher melting point because more energy is needed to overcome these forces and break the intermolecular bonds.

Melting Points:

* Chlorine (Cl₂): -101.5 °C

* Bromine (Br₂): -7.2 °C