The reason for diamagnetic nature of [Co(NH 3 ) 6 3 + ] and paramagnetic nature of [CoF 6 3- ] should be determined. Concept introduction: A transition metal cation has no outer s- electrons available for bonding, rather the inner d -electrons (in case of 3d transition metal elements) are available for making coordinate bonds with the ligands. Electrons are distributed in the five d- orbitals according to Hund’s rule which results in a maximum number of unpaired electrons.The abbreviated electronic configuration of an element depicts the electronic configuration of the elements which represents the noble gas configuration.

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Chapter 19, Problem 40QAP

Interpretation Introduction

Interpretation: The reason for diamagnetic nature of [Co(NH3)63+] and paramagnetic nature of [CoF63-] should be determined.

Concept introduction: A transition metal cation has no outer s- electrons available for bonding, rather the inner d -electrons (in case of 3d transition metal elements) are available for making coordinate bonds with the ligands. Electrons are distributed in the five d- orbitals according to Hund’s rule which results in a maximum number of unpaired electrons.The abbreviated electronic configuration of an element depicts the electronic configuration of the elements which represents the noble gas configuration.

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