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Titanium shows magnetic moment of 1.73 B...

Titanium shows magnetic moment of `1.73 B.M.` in its compounds. What is the oxidation number of `Ti` in the compound?

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The correct Answer is:
3
Magnetic moment `mu = sqrt(n(n+2))` BM
`1.73 = sqrt(n(n+2)), therefore n=1`, it has one unpaired electron hence electronic configuration is `[Ar]3d^(1)` and electronic configuration for Z=22 is `[Ar]3d^(2)4s^(2)`. Hence charge on Ti is `+3`.
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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?

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