Identify each solid as molecular, ionic, or atomic. d. I₂(s)

Key Concepts

Molecular Solids

Molecular solids are composed of molecules held together by intermolecular forces such as van der Waals forces, dipole-dipole interactions, or hydrogen bonds. These solids typically have low melting and boiling points compared to ionic or atomic solids. An example is iodine (I2), which forms a molecular solid at room temperature.

Ionic Solids

Ionic solids consist of positively and negatively charged ions held together by strong electrostatic forces known as ionic bonds. These solids generally have high melting and boiling points due to the strength of the ionic interactions. Common examples include sodium chloride (NaCl) and magnesium oxide (MgO).

Atomic Solids

Atomic solids are composed of atoms held together by covalent bonds, metallic bonds, or van der Waals forces. They can be further classified into covalent network solids, like diamond, which have very high melting points, and metallic solids, which conduct electricity and have variable melting points. These solids exhibit unique properties based on their atomic structure.