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Sodium chloride (SO-dee-um KLOR-ide) is an important table salt and is also used in a number of industrial processes. It is a colorless to white powder or crystalline solid with no odor and a characteristic salty taste. It is somewhat hygroscopic and easily absorbs moisture from the air.
Unlike some ionic compounds, the ions in sodium chloride are organized in cubic form. Each sodium ion is surrounded by six chloride ions of opposite charge. These alternating spheres of ions create a stable crystal lattice that is difficult to disrupt.
To melt this giant ionic lattice, a lot of energy must be overcome. This is because the strong electrostatic attractions between the ions must be overcome to allow the atoms within the solid to displace each other.
Why do some ionic compounds have a higher melting point than others?
The difference in the bonds that hold the ions together makes a big difference to the melting point. Sodium chloride has ionic bonds which make it require more energy to melt than metals with covalent bonds.
Another ionic compound that has a high melting point is KCl. KCl has the same structure as NaCl at 1 bar but transitions to the simple cubic B2 structure at a lower pressure. This results in a steepening of the melting curve.