AP Chemistry: 1.6 Photoelectron Spectroscopy – Exam Style questions with Answer- MCQ

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Question

 

The complete photoelectron spectrum of an element is given above. Which labeled peak corresponds to the is electrons and why?

A  Peak X , because 1s electrons are the easiest to remove from the atom.
B Peak X , because 1s electrons have the strongest attractions to the nucleus.
C  Peak Y , because electrons in the 1s sublevel are the farthest from the nucleus.
D  Peak Y, because there are fewer electrons in an s sublevel than in a p sublevel.
▶️Answer/Explanation

Ans: B Greater binding energies correlate to stronger attractions to the nucleus.

Question

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?

A The spectrum shows an odd number electrons.

B The spectrum shows a single electron in the 2p subshell.

C The spectrum shows equal numbers of electrons in the first and second electron shells.

D  The spectrum shows three electrons with the same binding energy in the second electron shell.

▶️Answer/Explanation

Ans:B The spectrum is consistent with the electron configuration for boron: \(1s^22^s2^2p^1\). The leftmost peak represents the two electrons in the filled 1s subshell. The two peaks on the right represent the two  electrons in the filled 2s subshell and the single electron in the 2p subshell.

Question

The complete photoelectron spectrum of the element carbon is represented above. Which of the following best explains how the spectrum is consistent with the electron shell model of the atom?

A  The spectrum shows four electrons in the inner electron shell.

B  The spectrum shows equal numbers of electrons in the three occupied electron subshells.

C  The spectrum shows that all the electrons in the valence shell have the same binding energy.

D  The spectrum shows more electrons in the inner electron shell than in the outer electron shell.
▶️Answer/Explanation

Ans: B The peak on the left represents two 1s electrons, and the two peaks on the right represent two 2s electrons and two 2p electrons, respectively.

Question

A sample containing atoms of C and F was analyzed using x-ray photoelectron spectroscopy. The portion of the spectrum showing the Is peaks for atoms of the two elements is shown above. Which of the following correctly identifies the 1s peak for the F atoms and provides an appropriate explanation?

(A) Peak X, because F has a smaller first ionization energy than C has.

(B) Peak X, because F has a greater nuclear charge than C has.

(C) Peak Y, because F is more electronegative than C is.

(D) Peak Y, because F has a smaller atomic radius than Ĉ has.

▶️Answer/Explanation

Ans:B

Question

The photoelectron spectra of the 1s electrons of two isoelectronic species, \(Ca^{2+}\) and Ar, are shown above. Which of the following correctly identifies the species associated with peak X and provides a valid justification?
(A) Ar, because it has completely filled energy levels
(B) Ar, because its radius is smaller than the radius of \(Ca^{2+}\)
(C) \(Ca^{2+}\), because its nuclear mass is greater than that of Ar
(D)\( Ca^{2+}\), because its nucleus has two more protons than the nucleus of Ar has

▶️Answer/Explanation

Ans:C

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