In photoelectron spectroscopy (PES), which of the following statements best explains why the peak corresponding to the $1s$ electrons of oxygen occurs at a higher binding energy than that of nitrogen?

A) Nitrogen has a smaller atomic radius, allowing its valence electrons to shield the $1s$ electrons more effectively from the nucleus.

B) Oxygen has paired electrons in its $2p$ subshell, which repels the inner core electrons and forces the $1s$ electrons to higher energy.

C) Oxygen has a greater nuclear charge, resulting in a stronger electrostatic attraction between the nucleus and its $1s$ electrons.

D) Nitrogen has a half-filled $2p$ subshell, which provides anomalous overall stability that lowers the ionization energy of all core electrons.

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Chemistry · Atomic Structure · Chemistry · Electrons in Atoms

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