Chemistry - Complete d-block Question with Solution | TestHub

${\mathrm{Mg}}^{2+}=1{\mathrm{s}}^2,2{\mathrm{s}}^2,2{\mathrm{p}}^6$ (No unpaired electrons) ${\mathrm{Ti}}^{3+}=1{\mathrm{s}}^2,2{\mathrm{s}}^2,2{\mathrm{p}}^6,3{\mathrm{s}}^2,3{\mathrm{p}}^6,4{\mathrm{s}}^0,3{\mathrm{d}}^1$ (One unpaired electrons) ${\mathrm{V}}^{3+}=1{\mathrm{s}}^2,2{\mathrm{s}}^2,2{\mathrm{p}}^6,3{\mathrm{s}}^2,3{\mathrm{p}}^6,4{\mathrm{s}}^0,3{\mathrm{d}}^2$ (Two unpaired electrons) ${\mathrm{Fe}}^{2+}=1{\mathrm{s}}^2,2{\mathrm{s}}^2,2{\mathrm{p}}^6,3{\mathrm{s}}^2,3{\mathrm{p}}^6,4{\mathrm{s}}^0,3{\mathrm{d}}^6$ (Four unpaired electrons) $\therefore {\mathrm{Fe}}^{2+}$ has highest number of unpaired electrons.