Why are ionic compounds typically solid at room temperature?

Why are ionic compounds typically solid at room temperature?

• A. Because they are always liquids at room temperature.
• B. Because they form covalent bonds.
• C. Because strong electrostatic attractions between oppositely charged ions give high melting points.
• D. Because they have weak interparticle forces.

Answer: (C)

The main idea is that strong electrostatic attractions between oppositely charged ions create a crystal lattice that takes a lot of energy to break apart. In an ionic solid, every ion is held in place by numerous strong Coulomb forces from neighboring ions throughout the lattice. To melt the substance, you must supply enough energy to overcome these attractions for many ions at once, which means a high melting point. At room temperature, the thermal energy available to the particles is not enough to overcome those forces, so ionic compounds stay solid. The other statements aren’t correct because ionic solids aren’t formed by covalent bonds, they aren’t inherently liquids at room temperature, and the forces between ions in the lattice are not weak.

The main idea is that strong electrostatic attractions between oppositely charged ions create a crystal lattice that takes a lot of energy to break apart. In an ionic solid, every ion is held in place by numerous strong Coulomb forces from neighboring ions throughout the lattice. To melt the substance, you must supply enough energy to overcome these attractions for many ions at once, which means a high melting point. At room temperature, the thermal energy available to the particles is not enough to overcome those forces, so ionic compounds stay solid. The other statements aren’t correct because ionic solids aren’t formed by covalent bonds, they aren’t inherently liquids at room temperature, and the forces between ions in the lattice are not weak.