A student compares the thermodynamic and structural properties of four crystalline solids at \(298\text{ K}\), as summarized in the table below.

Compound	Cation	Anion	Internuclear distance (\(\text{pm}\))	Lattice energy (\(\text{kJ/mol}\))
\(\text{NaF}\)	\(\text{Na}^+\)	\(\text{F}^-\)	\(235\)	\(923\)
\(\text{NaCl}\)	\(\text{Na}^+\)	\(\text{Cl}^-\)	\(283\)	\(786\)
\(\text{CaO}\)	\(\text{Ca}^{2+}\)	\(\text{O}^{2-}\)	\(240\)	\(3414\)
\(\text{MgO}\)	\(\text{Mg}^{2+}\)	\(\text{O}^{2-}\)	\(212\)	\(3791\)

Based on the data in the table and Coulomb's law, which of the following best explains why the lattice energy of \(\text{CaO}\) is approximately four times greater than the lattice energy of \(\text{NaF}\)?