/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 30 Consider an octahedral complex \... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 24: Problem 30

Consider an octahedral complex \(\mathrm{MA}_{3} \mathrm{~B}_{3}\). How many geometric isomers are expected for this compound? Will any of the isomers be optically active? If so, which ones?

Short Answer

Expert verified
There are two geometric isomers expected for the octahedral complex MA3B3: the fac isomer and the mer isomer. However, neither of these isomers will be optically active, as both possess planes of symmetry in their structures.

Step by step solution

01

Understand the Octahedral complex structure

An octahedral complex has six ligands surrounding the central metal atom. In this case, we have three A ligands and three B ligands. The arrangement of these ligands gives rise to different geometric isomers.
02

Draw the possible geometric isomers of the octahedral complex MA3B3

There are two possibilities for the arrangement of A and B ligands around the central metal atom: 1. All three A ligands can occupy a facial position (in a triangular face of the octahedron), while the B ligands occupy positions opposite to each A ligand, with two of them on the same face. This arrangement is called the fac isomer. 2. The second possibility is that A and B ligands can be in a meridional position with each A ligand having one B ligand occupying positions trans to it (also known as mer isomer).
03

Determine optical activity for each geometric isomer

To check for optical activity, we need to look for a plane of symmetry in the two isomers. If there is a plane of symmetry, the complex is not optically active. In the fac isomer, there are three planes of symmetry: Each plane passes through the central metal atom and is perpendicular to one of the triangular faces. Therefore, the fac isomer is NOT optically active. In the mer isomer, there is a single plane of symmetry: This plane passes through the central metal atom, dividing it into two equal halves. Because of this plane of symmetry, the mer isomer is also NOT optically active. So, in conclusion:
04

Summarize the results

There are two possible geometric isomers for the complex MA3B3: the fac isomer and the mer isomer. Neither of these isomers is optically active, as both have planes of symmetry.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

Suppose that a transition-metal ion was in a lattice in which it was in contact with just two nearby anions, located on opposite sides of the metal. Diagram the splitting of the metal \(d\) orbitals that would result from such a crystal field. Assuming a strong field, how many unpaired electrons would you expect for a metal ion with six \(d\) electrons? (Hint: Consider the linear axis to be the z-axis).

Pyridine \(\left(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}\right)\), abbreviated py, is the following molecule: (a) Why is pyridine referred to as a monodentate ligand? (b) Consider the following equilibrium reaction: \(\left[\mathrm{Ru}(\mathrm{py})_{4}(\mathrm{bipy})\right]^{2+}+2 \mathrm{py} \rightleftharpoons\left[\mathrm{Ru}(\mathrm{py})_{6}\right]^{2+}+\) bipy What would you predict for themagnitude of the equilibrium constant for this equilibrium? Explain the basis for your answer.

The complexes \(\left[\mathrm{V}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) and \(\left[\mathrm{VF}_{6}\right]^{3-}\) are both known. (a) Draw the \(d\) -orbital energy-level diagram for \(\mathrm{V}(\mathrm{III})\) octahedral complexes. (b) What gives rise to the colors of these complexes? (c) Which of the two complexes would you expect to absorb light of higher energy? Explain.

In crystal-field theory, ligands are modeled as if they are point negative charges. What is the basis of this assumption, and how does it relate to the nature of metalligand bonds?

(a) A complex absorbs light with wavelength of \(530 \mathrm{~nm}\). Do you expect it to have color? (b) A solution of a compound appears green. Does this observation necessarily mean that all colors of visible light other than green are absorbed by the solution? Explain. (c) What information is usually presented in a visible absorption spectrum of a compound? (d) What energy is associated with the absorption at \(530 \mathrm{~nm}\) in \(\mathrm{kJ} / \mathrm{mol}\) ?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Reactions

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.