The successive ionization energies for gaseous sodium atoms are shown in the table below.

Ionization	Process	Ionization energy \(\left(\text{kJ/mol}\right)\)
First \(\left(IE_1\right)\)	\(\text{Na(g)} \rightarrow \text{Na}^+\text{(g)} + e^-\)	\(496\)
Second \(\left(IE_2\right)\)	\(\text{Na}^+\text{(g)} \rightarrow \text{Na}^{2+}\text{(g)} + e^-\)	\(4562\)
Third \(\left(IE_3\right)\)	\(\text{Na}^{2+}\text{(g)} \rightarrow \text{Na}^{3+}\text{(g)} + e^-\)	\(6910\)

Which of the following statements best accounts for why the second ionization energy of \(\text{Na}\) is nearly ten times greater than its first ionization energy?