Question

An explanation of why an ionic bond is solid at room temperature?

Answer 1

Well, an ionic compound is usually a solid at room temperature... not an ionic bond.

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Common examples are `"NaCl"` and `"Na"_2"CO"_3` (what are their common names?), with melting points of `801^@ "C"` and `851^@ "C"` respectively.

Their high melting points are due to strong interatomic ion-ion interactions in a three-dimensional lattice structure... These forces are due to the interaction of one ion with many other counterions, and depend on both size and charge (charge being a more significant factor).

Obviously `25^@ "C"`, approximately room temperature, is much less than either of these melting points.

As a result, these substances cannot melt... having less than enough thermal energy to melt, they must be less energetic than liquids. Therefore, they must be solids.

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Can you propose an ionic compound with a melting point higher than `"NaCl"` and `"Na"_2"CO"_3`?