Ionisation energies : The ionisation energies of elements of the first transition series are stated below:

* in kJ mol^-1

         The below stated generalizations can be attained from the ionisation energy values given above in the table.

(i) The ionisation energies of these elements are high and in most of the cases lie between those of s- and p-block elements. This signifies that transition elements are less electropositive than that of s-block elements.

Explanation : Transition metals posses smaller atomic radii and higher nuclear charge in comparison to alkali metals. Both these factors tend to increase ionisation energy, as observed.

(ii) The ionisation energy in any of the transition series increases in nuclear with atomic number; the increase though is not smooth and as sharp as seen in case of the s and p-block elements.

Explanation : The ionisation energy increases because of the increase in nuclear charge with the atomic number at beginning of the series. Slowly, the shielding effect of the added electrons also increases. This shielding effect tends to reduce attraction because of the nuclear charge. These two opposing factors lead to rather gradual increase in the ionisation energies in any of transition series.

(iii) The first ionization energies of the 5d-series of elements are quite higher than those of the 3d and 4d series elements.

Explanation: In 5d-series of the transitions elements, after lanthanum (La), the added electrons moves to the next inner 4f orbitals. The 4f electrons have bad shielding effect. As a result, outermost electrons experience greater nuclear attraction. This leads to the higher ionisation energies for the 5d- series of the transition elements.

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