Identify each solid as molecular, ionic, or atomic. b. CO₂(s)

Verified step by step guidance

1. Identify the type of bonding present in the solid CO₂.
2. Recognize that CO₂ is composed of nonmetal atoms (carbon and oxygen).
3. Understand that CO₂ forms covalent bonds between carbon and oxygen atoms.
4. Recall that molecular solids are composed of molecules held together by intermolecular forces.
5. Conclude that CO₂(s) is a molecular solid because it consists of CO₂ molecules held together by weak intermolecular forces.

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 solid carbon dioxide (CO2), which forms when gas is cooled and solidifies into a molecular structure.

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 categorized into covalent network solids, like diamond, which have very high melting points, and metallic solids, which conduct electricity and have variable melting points. Atomic solids are characterized by their strong bonding and structural integrity.