---
title: "The complete photoelectron spectrum of a sample of neutral sulfur atoms in the gas phase is shown below.  Which of the following statements correctly compares the peak corresponding to the \\(2p\\) subshell with the peak corresponding to the \\(3p\\) subshell?"
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url: "https://nerd-notes.com/ubq/119650/"
date_modified: "2026-08-21T08:11:55+00:00"
---

# The complete photoelectron spectrum of a sample of neutral sulfur atoms in the gas phase is shown below.

Which of the following statements correctly compares the peak corresponding to the \(2p\) subshell with the peak corresponding to the \(3p\) subshell?

The complete photoelectron spectrum of a sample of neutral sulfur atoms in the gas phase is shown below.

Which of the following statements correctly compares the peak corresponding to the \(2p\) subshell with the peak corresponding to the \(3p\) subshell?

![A photoelectron spectrum plotted on Cartesian axes. The horizontal axis is labeled 'Binding Energy (\(\text{MJ/mol}\))' with a logarithmic-style decreasing scale from left to right, marked with values \(1000\), \(100\), \(10\), and \(1.0\). The vertical axis is labeled 'Relative Number of Electrons' with evenly spaced tick marks from \(0\) to \(6\). The spectrum displays five distinct vertical peaks representing the subshells of sulfur: the first peak on the far left at approximately \(247\text{ MJ/mol}\) has a relative height of \(2\); the second peak at approximately \(23\text{ MJ/mol}\) has a relative height of \(2\); the third peak at approximately \(16\text{ MJ/mol}\) has a relative height of \(6\); the fourth peak at approximately \(2.0\text{ MJ/mol}\) has a relative height of \(2\); and the fifth peak on the far right at approximately \(1.0\text{ MJ/mol}\) has a relative height of \(4\). No other peaks, gridlines, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787299915-Z01O0A.jpg)

- **A.** The \(2p\) peak is shorter than the \(3p\) peak, and the \(2p\) electrons have a lower binding energy because the \(2p\) subshell contains fewer unpaired electrons.
- **B.** The \(2p\) peak is taller than the \(3p\) peak, and the \(2p\) electrons have a higher binding energy because they are in an energy level closer to the nucleus and experience less shielding.
- **C.** The \(2p\) peak is taller than the \(3p\) peak, and the \(2p\) electrons have a lower binding energy because greater electron-electron repulsions in the filled subshell make them easier to remove.
- **D.** The \(2p\) peak is shorter than the \(3p\) peak, and the \(2p\) electrons have a higher binding energy because the \(2p\) electrons occupy a larger spatial volume with lower electron density.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119650/*