Chemistry - Complete d-block Question with Solution | TestHub

Electronic configuration of the given elements are

$\text{Mn}\to 1{\text{s}}^{2}2{\text{s}}^{2}2{\text{p}}^{6}3{\text{s}}^{2}3{\text{p}}^{6}3{\text{d}}^{5}4{\text{s}}^2$

$\text{Cr}\to 1{\text{s}}^{2}2{\text{s}}^{2}2{\text{p}}^{6}3{\text{s}}^{2}3{\text{p}}^{6}3{\text{d}}^{5}4{\text{s}}^1$

$\text{Ti}\to 1{\text{s}}^{2}2{\text{s}}^{2}2{\text{p}}^{6}3{\text{s}}^{2}3{\text{p}}^{6}3{\text{d}}^{2}4{\text{s}}^2$

$\text{V}\to 1{\text{s}}^{2}2{\text{s}}^{2}2{\text{p}}^{6}3{\text{s}}^{2}3{\text{p}}^{6}3{\text{d}}^{3}4{\text{s}}^2$

In general, ionization potential ( both 1^stand 2^nd) increases form left to right across the period due to increase in effective nuclear charge. On this basis, the second IP values should exhibit the trend :

Mn > Cr > V > Ti

But the actual observed order is :

Cr > Mn > V > Ti

Practically, only chromium is exceptional and rest others show the normal trend. This exceptional behaviour of chromium is due to the stable configuration ( 3d⁵) that it achieves after the loss of first electron.