Friday, August 5, 2011
Why is the boiling point of NaCl higher than that of MgCl2?
Shouldn't it be the other way round? According to Coulomb's law, MgCl2 should have a higher boiling point than NaCl as Mg2+ ion is smaller and has a higher charge than Na+ ion. Isn't the magnitude of lattice energy directly related to its melting/boiling point?
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