The photoelectron spectrum for the element boron is represented above. Which of the following best explains how the spectrum is consistent with the electron shell model of the atom? The spectrum shows an odd number electrons. A The spectrum shows a single electron in the 2p subshell. B The spectrum shows equal numbers of electrons in the first and second electron shells. C The spectrum shows three electrons with the same binding energy in the second electron shell.

Explanation:

The figure attached is representation of the photoelectron spectrum for the element boron, which is the missing part of the question.

There are three peaks. Each peak represents one subshell: 1s, 2s, and 2p.

Indeed, Boron has 5 electrons: 2 in the subshell 1s, 2 in the subshell 2s and one in the subshell 2p.

The first peak, the peak to the left of the diagram, is as high as the second peak, meaining there are the same relative number of electrons in the 1s and 2s subshells.

The third peak, the one to the right of the diagram is half as high as the other two peaks, there are half electrons in the 2p subshell as in the 1s and 2s subshells.

Since Boron has five electrons, the photoelectrum spectrum shows that there are two electrons in the 1s subshell,  two electrons in the 2s subshell, and a single electron in the 2p subshell.

Then, as for the answer choices:

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