Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 26: Problem 16

Give reasons for the following: (a) \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) is pale coloured. (b) Anhydrous \(\mathrm{CuSO}_{4}\) is white but \(\mathrm{CuSO}_{A} .5 \mathrm{H}_{2} \mathrm{O}\) is blue in colour.

Short Answer

Expert verified
a) Mn hydration complex is pale as its electron configuration prevents absorption of light from the visible region. b) Anhydrous \(\mathrm{CuSO}_{4}\) is white but becomes blue when hydrated due to energy level shifts in copper cations with water ligands, reflecting blue light.

Step by step solution

01

Reason for pale color of Mn complex

This type of complex shows pale colour because the transition of electron is not taking place. The oxidation state of Mn in the complex \( \left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) is \(+2\). In \(Mn^{+2}\) , the electronic configuration is \(3d^{5}\) which is half filled. As there is no vacant d-orbital available for the transition of electrons from one orbital to another, the \(Mn^{+2}\) ion does not absorb any light from the visible region and hence appears to be pale or colorless.
02

Reason for color change in Copper Sulphate

Anhydrous Copper Sulphate (\(\mathrm{CuSO}_{4}\)) is white in color because it doesn't have any water molecules attached to it. When it hydrates to form \(\mathrm{CuSO}_{4} .5 \mathrm{H}_{2} \mathrm{O}\), copper cations in the complex [\(Cu(H2O)4]^{2+}\) interact with the water ligands to cause a shift in the d-orbitals' energy levels, hence absorbing light in the red region and reflecting the complementary blue light. Therefore, hydrated Copper Sulphate appears blue.

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

Discuss the theory of the following methods used for the measurement of magnetic susceptibility: (a) Faraday's method (b) Evan's method

Determine the \(\Delta_{0}\) values for \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) and \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) if \(0\left({ }^{3} A_{2 g} \rightarrow{ }^{3} T_{2 g}\right)\) is \(8700 \mathrm{~cm}^{-1}\) and \(\cup\left({ }^{4} T_{1 g} \rightarrow{ }^{4} T_{2 g}\right)\) is \(8000 \mathrm{~cm}^{-1}\). Also draw Orgel diagrams for these complexes.

What are Orgel diagrams? Discuss their utility in case of coordination complexes.

What is the origin of diamagnetism and paramagnetism? Discuss the effect of temperature on diamagnetic and paramagnetic susceptibility.

What is the difference between \(L-S\) coupling and \(j-j\) coupling? Discuss the significance of both schemes.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

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.

Sign-up for free