Question

The spin only magnetic moment of Mn\(^{2+}\) ion is:

• A. 4.901 BM
• B. 5.916 BM
• C. 3.873 BM
• D. 2.846 BM

Hint:

The magnetic moment is calculated using the number of unpaired electrons in the ion.

Answer 1

The Correct Option is B

Step 1: Understand the formula for magnetic moment.
The magnetic moment for a transition metal ion is given by the formula: \[ \mu = \sqrt{n(n+2)} \, \text{BM} \] where \( n \) is the number of unpaired electrons. For Mn\(^{2+}\), the electron configuration is \( [Ar] 3d^5 \), so there are 5 unpaired electrons. Substituting into the formula: \[ \mu = \sqrt{5(5+2)} = \sqrt{35} = 5.916 \, \text{BM} \] Thus, the correct answer is (B).