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

Explanation

The magnetic moment may be expressed as
`sqrt(n(n+2))` = 5.92
`n(n+2) = (5.92)^(2)=35`
`n^(2)+2n-35 = 0` or `n=((-2)+-sqrt(4-4(-35)))/2=((-2)+-sqrt(144))/2 = (-2+12)/2=10/2=5`
No. Of the unpaired electrons = 5
In order to have five unpaired electrons in the d-orbitals. `Mn^(2+)` ion in the complex must be `sp^(3+)` hybridised which imples that no 3d orbital is involved in the hybridisation.