Question

Why ${\mathrm{TiCl}}_2$ Is paramagnetic but ${\mathrm{TiO}}_2$ is diamagnetic?

Answer 1

• In ${\mathrm{TiCl}}_2$ oxidation number of $\mathrm{Ti}$is $+2$.
• Here there is 2 unpaired ${\mathrm{e}}^{-}$ present in the outer orbitals $\left(3{\mathrm{d}}^{2}4{\mathrm{s}}^0\right)$ of ${\mathrm{Ti}}^{+2}$, thus ${\mathrm{TiCl}}_2$ exhibits paramagnetic behavior.
• But, In ${\mathrm{TiO}}_2$, due to the $+4$ oxidation state of $\mathrm{Ti}$, the valence d-orbitals do not contain an unpaired electron $\left(3{\mathrm{d}}^0\right)$.Therefore, it shows diamagnetic properties.