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) $\mathrm{SO}_{2} \mathrm{~F}$, (b) $\mathrm{MgF}_{2}$, (c) $W$,
(d) $\mathrm{Pb},(\mathrm{e}) \mathrm{PF}_{5}$

Key Concepts

Molecular Solids

Molecular solids are composed of discrete molecules that are held together in the solid state by relatively weak intermolecular forces such as London dispersion forces, dipole–dipole interactions, or hydrogen bonds. These forces result in materials that generally have low melting points compared to ionic or covalent network solids and are often soft or volatile.

Ionic Solids

Ionic solids consist of a regular lattice of positive and negative ions arranged in a repeating pattern. The strong ionic bonds between these oppositely charged ions result in high melting and boiling points, significant hardness, and brittleness. Their properties are dictated by the electrostatic forces that hold the ions together.

Covalent Network Solids

Covalent network solids are characterized by a continuous network of covalent bonds that extend throughout the material. This interconnected bonding structure results in very high melting points, exceptional hardness, and low electrical conductivity in the solid state. Their strength and stability come from the robust covalent association between atoms over large distances.

Metallic Solids

Metallic solids are formed by metal atoms that are bonded together by a 'sea' of delocalized electrons, which allows the metals to conduct electricity and heat efficiently. This type of bonding provides flexibility (malleability and ductility), high thermal and electrical conductivity, and often a shiny, reflective appearance.

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