A student investigates the lattice energies and melting points of four crystalline ionic compounds: \(\text{MgO}\), \(\text{CaO}\), \(\text{NaF}\), and \(\text{NaCl}\). The ionic radii of the constituent ions are given in the table below.

Ion	Ionic radius (pm)
\(\text{Mg}^{2+}\)	\(72\)
\(\text{Ca}^{2+}\)	\(100\)
\(\text{Na}^{+}\)	\(102\)
\(\text{F}^{-}\)	\(133\)
\(\text{Cl}^{-}\)	\(181\)
\(\text{O}^{2-}\)	\(140\)

Based on Coulomb's law and the data provided, which of the following correctly ranks the compounds in order of melting point from greatest to least?