The number of unpaired electrons responsible for the paramagnetic nature of the following complex species are respectively :
[Fe(CN)6]3−, [FeF6]3−, [CoF6]3−, [Mn(CN)6]3−
Solution
<p>The number of unpaired electrons responsible for the paramagnetic nature of each complex species is calculated as follows:</p>
<p><strong>Complex</strong>: $[Fe(CN)_6]^{3-}$ </p>
<p><p><strong>Ion</strong>: $Fe^{3+}$</p></p>
<p><p><strong>Electronic Configuration</strong>: $3d^5$</p></p>
<p><p><strong>Orbital Population</strong>: </p>
<p><p>$t_{2g}^{2,2,1}$</p></p>
<p><p>$e_g^{0,0}$</p></p></p>
<p><p><strong>Unpaired Electrons</strong>: 1</p></p>
<p><strong>Complex</strong>: $[FeF_6]^{3-}$ </p>
<p><p><strong>Ion</strong>: $Fe^{3+}$</p></p>
<p><p><strong>Electronic Configuration</strong>: $3d^5$</p></p>
<p><p><strong>Orbital Population</strong>: </p>
<p><p>$t_{2g}^{1,1,1}$</p></p>
<p><p>$e_g^{1,1}$</p></p></p>
<p><p><strong>Unpaired Electrons</strong>: 5</p></p>
<p><strong>Complex</strong>: $[CoF_6]^{3-}$ </p>
<p><p><strong>Ion</strong>: $Co^{3+}$</p></p>
<p><p><strong>Electronic Configuration</strong>: $3d^6$</p></p>
<p><p><strong>Orbital Population</strong>: </p>
<p><p>$t_{2g}^{2,1,1}$</p></p>
<p><p>$e_g^{1,0}$</p></p></p>
<p><p><strong>Unpaired Electrons</strong>: 4</p></p>
<p><strong>Complex</strong>: $[Mn(CN)_6]^{3-}$ </p>
<p><p><strong>Ion</strong>: $Mn^{3+}$</p></p>
<p><p><strong>Electronic Configuration</strong>: $3d^4$</p></p>
<p><p><strong>Orbital Population</strong>: </p>
<p><p>$t_{2g}^{2,1,1}$</p></p>
<p><p>$e_g^{0,0}$</p></p></p>
<p><p><strong>Unpaired Electrons</strong>: 2</p></p>
<p>Each complex's paramagnetic nature is due to the specific number of unpaired electrons as indicated above.</p>
About this question
Subject: Chemistry · Chapter: Coordination Compounds · Topic: Ligands and Coordination Number
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