Magnetic moment of `[MnCl_(4)]^(2-)` is 5.92 BM. Explain.

Explanation

`mu=5.92=sqrt(n(n+2)), therefore n=5.` Thus `Mn^(2+)` has 5 unpaired electrons in the complex ion. So electronic configuration of `Mn^(2+)=3d^(5)(=d^(1)d^(1)d^(1)d^(1)d^(1))`. This shows that `Mn^(2+)` is `sp^(3)` hybridised rather than `dsp^(2)` and hence the complex has a tetrahedral structure.