A student compares the photoelectron spectroscopy (PES) data for gaseous phosphorus (ex\text{P}ex) and sulfur (ex\text{S}ex) atoms. The table below lists the valence electron configuration and the binding energy corresponding to the lowest-energy peak in the spectrum for each element.

Element	Valence electron configuration	Lowest binding energy peak (\(\text{MJ/mol}\))
\(\text{P}\)	\(3s^2 3p^3\)	\(1.01\)
\(\text{S}\)	\(3s^2 3p^4\)	\(1.00\)

Which of the following statements best explains why the lowest binding energy peak for \(\text{S}\) occurs at a lower energy than that for \(\text{P}\)?