The 'spin only' magnetic moment of Ti in a given compound is `1.73` BM. The oxidation state and configuration of Ti in the compound are --------- respectively.

Options

A. `+1, 4s^(2) 3d^(1)`
B. `+3, 3d^(1)`
C. `+2, 4s^(1)`
D. `+4, 3d^(1)`

Answer

B

Explanation

According to 'spin-=only' formula, we have
`mu = sqrt(n(n+2))` BM
`1.73 BM = sqrt(n(n+2))` BM
Squaring both the sides, we have
`3.0 = n(n+2) = n^(2) + 2n`
`n^(2) + 2n - 3 = 0 implies n = 1`
This implies that Ti in the given compounds haws one unpaired electron. Ground state configuration of Ti atom is `3d^(2) 4s^(2)` :

Since electrons are lost first form 4s, Ti will have one unpaired electron only in the oxidation state `(+3)`, leading to the configuration `3d^(1)`.