Final answer:
The statement is true; diatomic chlorine has weaker intermolecular forces than diatomic bromine because the larger and heavier bromine atoms exhibit stronger London dispersion forces.
Step-by-step explanation:
The statement that diatomic chlorine has weaker intermolecular forces than diatomic bromine is true. This is because intermolecular forces, specifically London dispersion forces, are generally stronger in larger and heavier atoms due to their greater polarizability. Since bromine atoms are larger and heavier than chlorine atoms, the dispersion forces in Br₂ are stronger than those in Cl₂. This results in bromine being a liquid at room temperature, whereas chlorine is a gas under the same conditions. The trend of increasing strength of London dispersion forces and higher boiling points as one moves down the halogen group from fluorine to iodine illustrates this principle.