Question

the complete photoelectron spectrum of an element is given above. which of the following electron configurations is consistent with the spectrum?
a (1s^{2}2s^{2}2p^{1})
b (1s^{2}2s^{2}2p^{6}3s^{2}3p^{1})
c (1s^{2}2s^{2}2p^{6}3s^{2}3p^{6})
the photoelectron spectrum for the element nitrogen is represented above. which of the following best explains how the spectrum is consistent with the electron - shell model of the atom?
a the leftmost peak represents the valence electrons.
b the two peaks at the right represent a total of three electrons.
c the electrons in the 1s sub - level have the smallest binding energy.
d the electrons in the 2p sub - level have the smallest binding energy.

Explanation:

Step1: Analyze photoelectron spectrum peaks

In a photoelectron spectrum, the binding - energy and relative number of electrons in each sub - level are shown. The peaks with higher binding energy correspond to electrons closer to the nucleus.

Step2: Evaluate electron configurations for first question

For the first question, we know that the number of peaks and their relative intensities in the photoelectron spectrum should match the electron configuration. The electron configuration $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$ has electrons in $1s$, $2s$, $2p$, $3s$, and $3p$ sub - levels, which can account for the peaks in the spectrum.

Step3: Evaluate statements for second question

For the second question, the electrons in the $1s$ sub - level are closest to the nucleus and have the highest binding energy. The electrons in the outermost sub - level (valence electrons) have the smallest binding energy. The two peaks at the right represent the valence electrons.

Answer:

First question: B. $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$
Second question: D. The electrons in the $2p$ sublevel have the smallest binding energy.