Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 20: Problem 95

Qualitatively draw the crystal field splitting for a trigonal bipyramidal complex ion. (Let the \(z\) axis be perpendicular to the trigonal plane.)

Short Answer

Expert verified
In a trigonal bipyramidal complex, the crystal field splitting diagram consists of three energy levels for the d-orbitals. The highest-energy level is occupied by the \(d_{z^2}\) orbital, followed by the \(d_{x^2-y^2}\) orbital, and the lowest-energy level contains the \(d_{xy}\), \(d_{xz}\), and \(d_{yz}\) orbitals, all having the same energy. The energy difference between the orbital levels represents the crystal field splitting.

Step by step solution

01

Identify the d-orbitals in a trigonal bipyramidal complex

First, we need to know the five d-orbitals in a trigonal bipyramidal complex: \(d_{z^2}\), \(d_{x^2-y^2}\), \(d_{xy}\), \(d_{xz}\), and \(d_{yz}\).
02

Analyze the axial and equatorial ligand's positions

In a trigonal bipyramidal complex, three ligands (A, B, and C) are in the equatorial plane, while the other two ligands (D and E) are in the axial position, perpendicular to the z-axis.
03

Determine the interaction between the ligands and d-orbitals

Now we will analyze how the different d-orbitals interact with the ligands. The \(d_{z^2}\) orbital has a high electron density along the axial ligands (D and E) and will experience a strong repulsion, making it the highest-energy orbital. The \(d_{x^2-y^2}\) orbital has its electron density in between the equatorial ligands (A, B, and C), causing it to experience less repulsion and have lower energy. The \(d_{xy}\), \(d_{xz}\), and \(d_{yz}\) orbitals all have electron density in between both axial and equatorial ligands, experiencing minimum repulsion and forming the lowest-energy group of orbitals.
04

Sketch the crystal field splitting diagram

To draw the crystal field splitting diagram for a trigonal bipyramidal complex, plot the energy (y-axis) against the d-orbitals (x-axis). The highest-energy level will be occupied by the \(d_{z^2}\) orbital, followed by the \(d_{x^2-y^2}\) orbital, and finally, the lowest-energy level will consist of the three orbitals \(d_{xy}\), \(d_{xz}\), and \(d_{yz}\) (all having the same energy). The energy difference between the orbital levels represents the crystal field splitting.

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

Draw geometrical isomers of each of the following complex ions. a. \(\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}^{-}\) b. \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}^{2+}\) c. \(\operatorname{Ir}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\) d. \(\operatorname{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{I}_{2}^{+}\)

The ferrate ion, \(\mathrm{FeO}_{4}^{2-},\) is such a powerful oxidizing agent that in acidic solution, aqueous ammonia is reduced to elemental nitrogen along with the formation of the iron(III) ion. a. What is the oxidation state of iron in \(\mathrm{FeO}_{4}^{2-},\) and what is the electron configuration of iron in this polyatomic ion? b. If \(25.0 \mathrm{mL}\) of a \(0.243 \mathrm{M} \mathrm{FeO}_{4}^{2-}\) solution is allowed to react with \(55.0 \mathrm{mL}\) of \(1.45 \mathrm{M}\) aqueous ammonia, what volume of nitrogen gas can form at \(25^{\circ} \mathrm{C}\) and 1.50 atm?

In which of the following is(are) the electron configuration(s) correct for the species indicated? a. Cu \([\mathrm{Ar}] 4 s^{2} 3 d^{9}\) b. \(\mathrm{Fe}^{3+} \quad[\mathrm{Ar}] 3 d^{5}\) c. Co \([\mathrm{Ar}] 4 s^{2} 3 d^{7}\) d. La \([\mathrm{Ar}] 6 s^{2} 4 f^{1}\) e. \(\mathrm{Pt}^{2+} \quad[\mathrm{Xe}] 4 f^{14} 5 d^{8}\)

Name the following coordination compounds. a. \(\mathrm{Na}_{4}\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) b. \(\mathrm{K}_{2}\left[\mathrm{CoCl}_{4}\right]\) c. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) d. \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\)

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.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

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