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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

A certain first-row transition metal ion forms many different colored solutions. When four coordination compounds of this metal, each having the same coordination number, are dissolved in water, the colors of the solutions are red, yellow, green, and blue. Further experiments reveal that two of the complex ions are paramagnetic with four unpaired electrons and the other two are diamagnetic. What can be deduced from this information about the four coordination compounds?

Interpretation Introduction

Interpretation: The formation of different colored solutions by a certain first-row transition metal ion and the formation of red, yellow, green, and blue colored solutions on the dissolution of four coordination compounds of the given particular ion in water and the formation of two paramagnetic and the other two diamagnetic complex ions is given. The information deduced about the four coordination compounds is to be stated.

Concept introduction: The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

Explanation

Explanation

During the formation of octahedral compounds, the d -orbital electrons can arrange in two different ways. When the system is low spin, the pairing occurs in the lower energy level and after that electron moves to the high energy level. The opposite occurs in the case of high spin where first both the lower and higher energy levels are singly occupied and after that the pairing of electrons starts. In case of 3d6 complexes, there is no unpaired electron present in the strong-field, while four unpaired electrons are present in weak-field ligand. This is possible for two ions like Fe2+ and Co3+

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