Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 21: Problem 18

What is the maximum number of unpaired \(d\) electrons that an octahedral transition metal complex ion can have? Predict a compound that would have this number of unpaired electrons.

Short Answer

Expert verified
The maximum number of unpaired \(d\) electrons in an octahedral transition metal complex ion is 5. A compound that exhibits this property is \(\text{Mn}(\text{H}_2\text{O})_6^{2+}\).

Step by step solution

01

Review the electron configuration of transition metals

Transition metals have electron configurations that follow the general pattern: \([\text{previous noble gas}] \ \text{ns}^{2}\text{nl}^{x}\), where \(x\) is the number of electrons in \(d\) orbitals. In the case of transition metals, the \(d\) orbital can hold up to 10 electrons.
02

Analyze the electron configuration in the octahedral complex ions

An octahedral complex ion consists of a central metal atom surrounded by six ligands. The ligands approach the central metal along the \(x\), \(y\), and \(z\) axes. In an octahedral complex, the \(d\) orbitals split into two groups: \(t_{2g}\) (lower energy) and \(e_g\) (higher energy). The \(t_{2g}\) set contains the \(d_{xy}\), \(d_{xz}\), and \(d_{yz}\) orbitals; the \(e_g\) set contains the \(d_{x^2 - y^2}\) and \(d_{z^2}\) orbitals.
03

Understand the maximum number of unpaired electrons in an octahedral complex ion

In an octahedral complex ion, the ligands cause a splitting of the \(d\) orbitals' energy levels. As a result, the \(t_{2g}\) orbitals are filled before the \(e_g\) orbitals. For maximum unpaired \(d\) electrons, we would want a transition metal that has five valence \(d\) electrons. These five electrons will fill the \(t_{2g}\) orbitals with three unpaired electrons and \(e_g\) orbitals with two unpaired electrons.
04

Predict a compound with the maximum number of unpaired electrons

Manganese (Mn) in its \(+2\) oxidation state has the electron configuration: \([\text{Ar}]\ 3d^5\). Therefore, when formed as an octahedral complex ion, for example, as \(\text{Mn}(\text{H}_2\text{O})_6^{2+}\), it will have the maximum number of unpaired \(d\) electrons, which are 5. So, the maximum number of unpaired \(d\) electrons in an octahedral transition metal complex ion is 5, and \(\text{Mn}(\text{H}_2\text{O})_6^{2+}\) is a compound that exhibits this property.

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

When an aqueous solution of KCN is added to a solution containing \(\mathrm{Ni}^{2+}\) ions, a precipitate forms, which redissolves on addition of more \(\mathrm{KCN}\) solution. Write reactions describing what happens in this solution. [Hint: \(\mathrm{CN}^{-}\) is a Bronsted-Lowry base \(\left(K_{\mathrm{b}} \approx 10^{-5}\right)\) and a Lewis base.]

Which is more likely to be paramagnetic, \(\mathrm{Fe}(\mathrm{CN})_{6}^{4-}\) or \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}\) ? Explain.

Draw all the geometrical isomers of \(\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{BrCl}^{+1}\) . Which of these isomers also have an optical isomer? Draw the various isomers.

Sketch a d-orbital energy diagram for the following. a. a linear complex ion with ligands on the \(x\) axis b. a linear complex ion with ligands on the \(y\) axis

Consider the complex ions $\mathrm{Co}\left(\mathrm{NH}_{3}\right) 6^{3+}, \mathrm{Co}(\mathrm{CN})_{6}^{3-},\( and \)\mathrm{CoF}_{6}^{3-} .$ The wavelengths of absorbed electromagnetic radiation for these compounds (in no specific order) are \(770 \mathrm{nm},\) \(440 \mathrm{nm},\) and 290 $\mathrm{nm} .$ Match the complex ion to the wave- length of absorbed electromagnetic radiation.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear 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