Question

Explain how the bonding in bromine leads to the observed melting point (266 K).

a) Bromine molecules are held together by covalent bonds, and the weak van der Waals forces result in a low melting point.
b) Bromine forms ionic bonds with other elements, leading to a high melting point.
c) Bromine exhibits metallic bonding, causing a moderate melting point.
d) Bromine undergoes hydrogen bonding, contributing to the observed melting point.

Answer 1

The bonding in bromine molecules is due to nonpolar covalent bonds, which result in weak dispersion forces and a low melting point. Therefore, option a) is correct.

Step-by-step explanation:

The melting point of bromine, which is 266 K, is explained by the bonding in bromine molecules. Bromine exists as diatomic molecules held together by nonpolar covalent bonds. These bonds result in weak intermolecular forces, specifically dispersion forces, which are the only forces acting between bromine molecules. Dispersion forces are weaker than other types of intermolecular forces, such as ionic or metallic bonding, which lead to high melting points. Therefore, option a) is the correct choice to explain the observed low melting point of bromine.