Based only on their formulas, classify each of the following...

Based only on their formulas, classify each of the following in the solid state as a molecular, ionic, covalent (network), or metallic solid: (a) $\mathrm{Au}$, (b) $\mathrm{NO}_{2}$, (c) $\mathrm{CaF}_{2},(\mathrm{~d}) \mathrm{SF}_{4}$, (e) $\mathrm{C}_{\text {diamond }}$.

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Key Concepts

Metallic Solids

Metallic solids are made up of metal atoms that share a ‘sea’ of delocalized electrons, which enables the formation of metal bonds. This bonding mechanism imparts properties such as ductility, malleability, electrical conductivity, and thermal conductivity to the solid.

Covalent Network Solids

Covalent network solids are formed when atoms are linked by an extensive network of covalent bonds throughout the entire structure. This arrangement leads to extremely hard materials with very high melting points, as seen in substances that require significant energy to disrupt the continuous bonding network.

Ionic Solids

Ionic solids are composed of a lattice of positively and negatively charged ions that are bonded together by strong electrostatic forces. This arrangement creates materials with high lattice energies, high melting points, and characteristic brittleness.

Molecular Solids

Molecular solids consist of individual molecules that are held together in the solid state by relatively weak intermolecular forces such as van der Waals forces, dipole–dipole interactions, or hydrogen bonds. Such solids generally feature low melting points and are less rigid compared to other solid types.

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