Paramagnetism is a property due to the presence of unpaired electrons. In case of transition metals, as they contain unpaired electrons in the (n-1)d orbitals, most of the transition metal ions and their compounds are paramagnetic. Paramagnetism increases with increases in number of unpaired electrons. Magnetic moment is calculated from `'"Spin only formula"'` viz.
`mu = sqrt(n(n+2)) B.M. n = no`. of unpaired electrons
Similarly the colour of the compounds of transition metals may be attributed to the presence of incomplete (n-1)d subshell. When an electron from a lower energy of d-orbital is excited to a higher energy d-orbital, the energy of excitation corresponding to the frequency of light absorbed. This frequency generally lies in the visible region. The colour observed correponds to complementary colour of the light absorbed. The frequency of the light absorbed is determined by the nature of the ligand.
Titanium shows magnetic moment of `1.7 BM` in its compound. What is the oxidation state of titanium in the compound?

Options

A. `+2`
B. `+1`
C. `+3`
D. `+4`

Answer

C

Explanation

`mu = 113` i.e. one unpaired electron, `Ti(E.C.) = [Ar]^(18)3d^(2),4s^(2)`, so it will lose three electrons to have one unpaired electron and thus the oxidation state of titanium is +3.