Question

Magnetic Moment of \( \text{Mn}^{2+} \) is:

Hint:

The magnetic moment depends on the number of unpaired electrons, calculated using \( \mu = \sqrt{n(n+2)} \, \text{BM} \), where \( n \) is the number of unpaired electrons.

Answer 1

Step 1: Determine the number of unpaired electrons. The electronic configuration of \( \text{Mn}^{2+} \) is: \[ \text{[Ar]} \, 3d^5 \] This indicates 5 unpaired electrons in the \( 3d \) subshell. Step 2: Use the formula for magnetic moment. The magnetic moment \( \mu \) is given by: \[ \mu = \sqrt{n(n+2)} \, \text{BM}, \] where \( n \) is the number of unpaired electrons. \[ \mu = \sqrt{5(5+2)} = \sqrt{35} = 5.9 \, \text{BM}. \] Hence, the magnetic moment of \( \text{Mn}^{2+} \) is 5.9 BM.