---
title: "In an aqueous redox experiment, iron metal ( \\(\\text{Fe}\\)) is oxidized in two successive steps, first forming the pale green \\(\\text{Fe}^{2+}\\) ion and subsequently forming the yellow-brown \\(\\text{Fe}^{3+}\\) ion. Which of the following represents the ground-state electron configuration of the \\(\\text{Fe}^{3+}\\) ion?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/123445/"
date_modified: "2026-09-28T11:59:43+00:00"
---

# In an aqueous redox experiment, iron metal (
\(\text{Fe}\)) is oxidized in two successive steps, first forming the pale green \(\text{Fe}^{2+}\) ion and subsequently forming the yellow-brown \(\text{Fe}^{3+}\) ion. Which of the following represents the ground-state electron configuration of the \(\text{Fe}^{3+}\) ion?

In an aqueous redox experiment, iron metal (
\(\text{Fe}\)) is oxidized in two successive steps, first forming the pale green \(\text{Fe}^{2+}\) ion and subsequently forming the yellow-brown \(\text{Fe}^{3+}\) ion. Which of the following represents the ground-state electron configuration of the \(\text{Fe}^{3+}\) ion?

- **A.** \([\text{Ar}]\, 3d^5\)
- **B.** \([\text{Ar}]\, 4s^2\, 3d^3\)
- **C.** \([\text{Ar}]\, 4s^1\, 3d^4\)
- **D.** \([\text{Ar}]\, 3d^6\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123445/*