The number of paramagnetic metal complex species among $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+},\left[\mathrm{Co}\left(\mathrm{C}_2 \mathrm{O}_4\right)_3\right]^{3-}$, $\left[\mathrm{MnCl}_6\right]^{3-},\left[\mathrm{Mn}(\mathrm{CN})_6\right]^{3-},\left[\mathrm{CoF}_6\right]^{3-},\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-}$ and $\left[\mathrm{FeF}_6\right]^{3-}$ with same number of unpaired electrons is __________.
Answer (integer)
2
Solution
<p>To determine which metal complexes are paramagnetic and have the same number of unpaired electrons, let's analyze each one:</p>
<p><strong>$[\mathrm{Co}(\mathrm{NH}_3)_6]^{3+}$:</strong></p>
<p><p>Cobalt ion: $\mathrm{Co}^{3+}$</p></p>
<p><p>Electron configuration: $3d^6$</p></p>
<p><p>Orbital occupancy: $\mathrm{t}_{2g}^{2,2,2}$ $\mathrm{e}_{g}^{0,0}$</p></p>
<p><p>Magnetic property: Diamagnetic (unpaired electrons = 0)</p></p>
<p><strong>$[\mathrm{Co}(\mathrm{C}_2 \mathrm{O}_4)_3]^{3-}$:</strong></p>
<p><p>Cobalt ion: $\mathrm{Co}^{3+}$</p></p>
<p><p>Electron configuration: $3d^6$</p></p>
<p><p>Orbital occupancy: $\mathrm{t}_{2g}^{2,2,2}$ $\mathrm{e}_{g}^{0,0}$</p></p>
<p><p>Magnetic property: Diamagnetic (unpaired electrons = 0)</p></p>
<p><strong>$[\mathrm{MnCl}_6]^{3-}$:</strong></p>
<p><p>Manganese ion: $\mathrm{Mn}^{3+}$</p></p>
<p><p>Electron configuration: $3d^4$</p></p>
<p><p>Orbital occupancy: $\mathrm{t}_{2g}^{1,1,1}$ $\mathrm{e}_{g}^{1,0}$</p></p>
<p><p>Magnetic property: Paramagnetic (unpaired electrons = 4)</p></p>
<p><strong>$[\mathrm{Mn}(\mathrm{CN})_6]^{3-}$:</strong></p>
<p><p>Manganese ion: $\mathrm{Mn}^{3+}$</p></p>
<p><p>Electron configuration: $3d^4$</p></p>
<p><p>Orbital occupancy: $\mathrm{t}_{2g}^{2,1,1}$ $\mathrm{e}_{g}^{0,0}$</p></p>
<p><p>Magnetic property: Paramagnetic (unpaired electrons = 2)</p></p>
<p><strong>$[\mathrm{CoF}_6]^{3-}$:</strong></p>
<p><p>Cobalt ion: $\mathrm{Co}^{3+}$</p></p>
<p><p>Electron configuration: $3d^6$</p></p>
<p><p>Orbital occupancy: $\mathrm{t}_{2g}^{2,1,1}$ $\mathrm{e}_{g}^{1,1}$</p></p>
<p><p>Magnetic property: Paramagnetic (unpaired electrons = 4)</p></p>
<p><strong>$[\mathrm{Fe}(\mathrm{CN})_6]^{3-}$:</strong></p>
<p><p>Iron ion: $\mathrm{Fe}^{3+}$</p></p>
<p><p>Electron configuration: $3d^5$</p></p>
<p><p>Orbital occupancy: $\mathrm{t}_{2g}^{2,2,1}$ $\mathrm{e}_{g}^{0,0}$</p></p>
<p><p>Magnetic property: Paramagnetic (unpaired electrons = 1)</p></p>
<p><strong>$[\mathrm{FeF}_6]^{3-}$:</strong></p>
<p><p>Iron ion: $\mathrm{Fe}^{3+}$</p></p>
<p><p>Electron configuration: $3d^5$</p></p>
<p><p>Orbital occupancy: $\mathrm{t}_{2g}^{1,1,1}$ $\mathrm{e}_{g}^{1,1}$</p></p>
<p><p>Magnetic property: Paramagnetic (unpaired electrons = 5)</p></p>
<p>From this analysis, the paramagnetic complexes having the same number of unpaired electrons (4 unpaired electrons) are:</p>
<p><p>$[\mathrm{MnCl}_6]^{3-}$</p></p>
<p><p>$[\mathrm{CoF}_6]^{3-}$</p></p>
<p>These two complexes show the same paramagnetic property, each with 4 unpaired electrons.</p>
About this question
Subject: Chemistry · Chapter: Coordination Compounds · Topic: Ligands and Coordination Number
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