Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 26

Give three examples of first-row transition metal (Sc to \(\mathrm{Cu}\) ) ions whose electron configurations are represented by the argon core.

Short Answer

Expert verified
The three examples of first-row transition metal ions whose electron configurations are represented by the argon core are: \(Cr^{3+}\), \(Mn^{2+}\) and \(Fe^{3+}\) .

Step by step solution

01

Understand Electron Configuration

First-row transition metals are elements defined between Scandium (Sc) and Copper (Cu) on the periodic table. These metals share the electron configuration of Argon (Ar), which has configuration 1s² 2s² 2p⁶ 3s² 3p⁶. That is why the electrons in the inner orbitals (1s, 2s, 2p, 3s and 3p) are called core electrons.
02

Identify possible ions

The three possible ions belonging to first-row transition metals between Scandium and Copper, which can have the same electron configuration as an Argon core, can be identified. They can be identified by considering the ionization state of the metal, which should result in the same configuration as Argon. These ions can only be \(Cr^{3+}\), \(Mn^{2+}\) and \(Fe^{3+}\) since for them loss of some external electrons leads to Argon core configuration.
03

Confirm electron configuration

Confirm that each of these ions indeed matches the Argon core configuration. For the electron configuration of \(Cr^{3+}\), three electrons are lost from the \(4s^{1}3d^{5}\) configuration of Chromium, resulting in the neutral Argon electronic structure. Similarly, for \(Mn^{2+}\), two electrons are lost from the \(4s^{2}3d^{5}\) configuration of Manganese, and for \(Fe^{3+}\), three electrons are lost from the \(4s^{2}3d^{6}\) configuration of Iron, both resulting in the neutral Argon electronic structure.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Compare the physical and chemical properties of metals and nonmetals.

In each of the following pairs, indicate which one of the two species is smaller: (a) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-},\) (b) Na or \(\mathrm{Na}^{+}\), (c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-},\) (d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+},\) (e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\).

Arrange the elements in each of these groups in order of increasing electron affinity: (a) \(\mathrm{Li}, \mathrm{Na}, \mathrm{K}\) (b) \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I}\)

Explain which of these anions is larger, and why: \(\mathrm{Se}^{2-}\) or \(\mathrm{Te}^{2-}\)

A neutral atom of a certain element has 17 electrons. Without consulting a periodic table, (a) write the ground-state electron configuration of the element, (b) classify the element, (c) determine whether the atoms of this element are diamagnetic or paramagnetic.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free