Question

If \(|x|\) represents the difference in maximum oxidation state possible for Mn in its oxide and in its fluoride. Among the following ions, which ions contain unpaired electrons equal to \(|x|\). (A) \(Zn^{2+}\) (B) \(Fe^{2+}\) (C) \(Co^{2+}\) (D) \(V^{2+}\) (E) \(Sc^{3+}\)

• A. A and E
• B. C and D
• C. B and C
• D. B and D

Answer 1

The Correct Option is B

Concept: First determine the difference in the maximum oxidation state of Mn in its oxide and fluoride.
Step 1: Maximum oxidation state of Mn in oxide In \(Mn_2O_7\), \[ Mn^{+7} \] Thus maximum oxidation state in oxide \(= +7\).
Step 2: Maximum oxidation state of Mn in fluoride In \(MnF_4\), \[ Mn^{+4} \] Thus maximum oxidation state in fluoride \(= +4\). \[ |x| = |7 - 4| = 3 \]
Step 3: Find ions having 3 unpaired electrons Write electronic configuration: \[ Zn^{2+} : 3d^{10} \quad \Rightarrow 0 \text{ unpaired electrons} \] \[ Fe^{2+} : 3d^{6} \quad \Rightarrow 4 \text{ unpaired electrons} \] \[ Co^{2+} : 3d^{7} \quad \Rightarrow 3 \text{ unpaired electrons} \] \[ V^{2+} : 3d^{3} \quad \Rightarrow 3 \text{ unpaired electrons} \] \[ Sc^{3+} : 3d^{0} \quad \Rightarrow 0 \text{ unpaired electrons} \]
Step 4: Compare Ions having \(3\) unpaired electrons: \[ Co^{2+} \text{ and } V^{2+} \] Thus the correct pair is: \[ \boxed{C \text{ and } D} \]