---
title: "A student investigates periodic trends and compiles the valence electron configurations and first ionization energies for phosphorus and sulfur, shown in the table below.  | Element | Valence Electron Configuration | First Ionization Energy (\\(\\text{kJ/mol}\\)) | | :— | :— | :— | | \\(\\text{P}\\) | \\(3s^2 3p^3\\) | \\(1012\\) | | \\(\\text{S}\\) | \\(3s^2 3p^4\\) | \\(1000\\) |  Which of the following statements correctly identifies the element from which an electron is more easily removed and provides the valid chemical reasoning?"
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url: "https://nerd-notes.com/ubq/119613/"
date_modified: "2026-08-21T08:11:47+00:00"
---

# A student investigates periodic trends and compiles the valence electron configurations and first ionization energies for phosphorus and sulfur, shown in the table below.

| Element | Valence Electron Configuration | First Ionization Energy (\(\text{kJ/mol}\)) |
| :— | :— | :— |
| \(\text{P}\) | \(3s^2 3p^3\) | \(1012\) |
| \(\text{S}\) | \(3s^2 3p^4\) | \(1000\) |

Which of the following statements correctly identifies the element from which an electron is more easily removed and provides the valid chemical reasoning?

A student investigates periodic trends and compiles the valence electron configurations and first ionization energies for phosphorus and sulfur, shown in the table below.

| Element | Valence Electron Configuration | First Ionization Energy (\(\text{kJ/mol}\)) |
| :--- | :--- | :--- |
| \(\text{P}\) | \(3s^2 3p^3\) | \(1012\) |
| \(\text{S}\) | \(3s^2 3p^4\) | \(1000\) |

Which of the following statements correctly identifies the element from which an electron is more easily removed and provides the valid chemical reasoning?

- **A.** \(\text{P}\) loses an electron more easily than \(\text{S}\) because the \(3p\) electrons in \(\text{P}\) experience a smaller effective nuclear charge than the \(3p\) electrons in \(\text{S}\).
- **B.** \(\text{P}\) loses an electron more easily than \(\text{S}\) because the half-filled \(3p\) subshell in \(\text{P}\) creates greater electron-electron repulsion among valence electrons.
- **C.** \(\text{S}\) loses an electron more easily than \(\text{P}\) because the electron removed from \(\text{S}\) comes from a paired \(3p\) orbital, where electron-electron repulsion lowers the energy required for removal.
- **D.** \(\text{S}\) loses an electron more easily than \(\text{P}\) because the valence electrons in \(\text{S}\) occupy a higher principal energy level than the valence electrons in \(\text{P}\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119613/*