Practicing Success
What is the current order of spin-only magnetic moment (in B.M.) of \(Mn^{2+}, Cr^{2+}\) and \(V^{2+}\)? |
\(Mn^{2+} > V^{2+} > Cr^{2+}\) \(V^{2+} > Cr^{2+} > Mn^{2+}\) \(Mn^{2+} > Cr^{2+} > V^{2+}\) \(Cr^{2+} > V^{2+} > Mn^{2+}\) |
\(Mn^{2+} > Cr^{2+} > V^{2+}\) |
The correct answer is option 3. \(Mn^{2+} > Cr^{2+} > V^{2+}\) The spin-only magnetic moment of a transition metal ion can be calculated using the formula: \(\mu_{\text{spin-only}} = \sqrt{n(n+2)} \, \text{B.M.} \) where \( n \) is the number of unpaired electrons. Let us determine the number of unpaired electrons for each ion: \(Mn^{2+}\) (Manganese ion) Atomic number of Mn: 25 Electronic configuration of Mn: \([Ar] 3d^5 4s^2\) For \(Mn^{2+}\): Remove \(2\) electrons from \(4s\), giving \([Ar] 3d^5\) Number of unpaired electrons: 5 Spin-only magnetic moment: \(\mu = \sqrt{5(5+2)} = \sqrt{35} \approx 5.92 \, \text{B.M.}\) \(Cr^{2+}\) (Chromium ion) Atomic number of Cr: 24 Electronic configuration of Cr: \([Ar] 3d^5 4s^1\) For \(Cr^{2+}\): Remove \(2\) electrons, one from \(4s\) and one from \(3d\), giving \([Ar] 3d^4\) Number of unpaired electrons: 4 Spin-only magnetic moment: \(\mu = \sqrt{4(4+2)} = \sqrt{24} \approx 4.90 \, \text{B.M.}\) \(V^{2+}\) (Vanadium ion) Atomic number of V: 23 Electronic configuration of V: \([Ar] 3d^3 4s^2\) For \(V^{2+}\): Remove \(2\) electrons from \(4s\), giving \([Ar] 3d^3\) Number of unpaired electrons: 3 Spin-only magnetic moment: \(\mu = \sqrt{3(3+2)} = \sqrt{15} \approx 3.87 \, \text{B.M.}\) Therefore, the order is: \(Mn^{2+} > Cr^{2+} > V^{2+}\) |