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

Explanation

`mu=sqrt(n(n+2))BM, mu=5.92` BM means n=5, i.e., 5 unpaired electrons. `Mn^(2+)=3d^(5)4s^(0)4p^(0)`. To form `[MnCl_(4)]^(2-)`, hybridisation will be `sp^(3)`. Hence, the structure will be tetrahedral.