Why does sodium chloride have a very high melting point?

Sodium chloride, commonly known as table salt, has a very high melting point primarily due to its giant ionic structure and the strong electrostatic forces that exist between its ions. In sodium chloride, the sodium ions (Na+) and chloride ions (Cl-) are held together in a lattice structure by these strong ionic bonds.

The electrostatic forces of attraction between the oppositely charged ions are substantial, requiring a significant amount of energy to overcome when the salt is heated. As a result, sodium chloride remains solid at high temperatures until sufficient energy is provided to break these interactions.

The other options do not accurately describe the properties of sodium chloride. For instance, weak intermolecular forces would lead to a low melting point, while covalent bonds, which are not present in sodium chloride, are relevant to molecular compounds rather than ionic ones. Moreover, stating that sodium chloride is a liquid at room temperature is incorrect, as it is typically found in solid form under those conditions. Thus, the strong electrostatic forces in its giant ionic structure are the reason for its high melting point.