Sodium chloride melts at 1074 K, while magnesium oxide melts at 3125 K. Both have identical structures. Why is there such a difference in their melting points?

The difference in melting points is due to the ionic nature of the compounds. Sodium chloride has weaker ionic bonds, resulting in a lower melting point. Magnesium oxide has stronger ionic bonds, leading to a higher melting point.

Explanation:

The difference in melting points between sodium chloride and magnesium oxide can be attributed to the ionic nature of the compounds.

Sodium chloride consists of positive sodium ions (Na+) and negative chloride ions (Cl-) arranged in a crystalline lattice structure. When heated, the strong ionic bonds between the ions need to be broken, requiring less energy compared to magnesium oxide.

On the other hand, magnesium oxide contains both positive magnesium ions (Mg2+) and negative oxide ions (O2-) also arranged in a crystalline lattice structure. However, the ionic bonds in magnesium oxide are stronger compared to those in sodium chloride, resulting in a higher melting point.

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