Calculate the number of unpaired electrons in `Ti^(3+), Mn^(2+)` and calculate the spin only magnetic moment.

Explanation

`Ti^(3+)`
Ti (Z = 22). Electronic configuration [Ar] `3d^(2)4s^(2)`
`Ti^(3+)` - Electronic configuration `[Ar]3d^(1)`
So, the number of unpaired electrons in `Ti^(3+)` is equal to 1.
Spin only magnetic moment of `Ti^(3+) = sqrt(1(1+2)) = sqrt(3) = 1.73 mu_(B)`
`Mn^(2+)`
Mn (Z = 25). Electronic configuration `[Ar] 3d^(5) 4s^(2)`
`Mn^(2+)` - Electronic configuration `[Ar]3d^(5)`
`Mn^(2+)` has 5 unpaired electrons.
Spin only magnetic moment of `Mn^(2+) = sqrt(5(5+2)) = sqrt(35) = 5.91 mu_(B)`