Lanthanide contraction

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Lanthanide contraction is a term used in chemistry to describe different but closely related concepts associated with smaller than expected atomic radii of the elements in the lanthanide series (atomic number 58 to 71).

1 Cause
2 Effects
3 Chemical behavior of the lanthanides
4 Influence on the post-lanthanides
5 External references

[edit] Cause

In single electron atoms, average separation of an electron from the nucleus is determined by the subshell it belongs to and it decreases with increasing charge on the nucleus which in turn leads to a decrease in atomic radius. In multi-electron atoms, the decrease in radius brought about by increase in nuclear charge is partially offset by electrostatic repulsion among electrons. Particularly, a "shielding effect" operates. ie., as electrons are added in outer shells, electrons already present shield the outer electrons from nuclear charge making them see a lower effective charge on the nucleus. The shielding effect exerted by the inner electrons decreases in order s > p > d > f. Usually in a period as a particular subshell is filled up, atomic radii go on decreasing. This effect is particularly pronounced in case of lanthanides as their 4f subshells are being filled across the period and they are least able to shield outer (5th and 6th) shell electrons. Thus the shielding effect is least able to counter decrease in radii due to increasing nuclear charge. This leads to "Lanthanide contraction". Radius drops from 1.020 Ångström in case of Cerium(III) to 0.861 Ångström in case of Lutetium(III).

[edit] Effects

As a result of the increased attraction of the outer shell electrons across the lanthanide period, the following effects are observed. Each of these effects is sometimes referred to as the lanthanide contraction:

The atomic radii of the lanthanides are smaller than would normally be expected.

The ionic radii of the lanthanides decrease from 1.17 Ångström La³⁺ to 1.00 Ångström Lu³⁺ in the lanthanide period.

The third row of d block elements have only marginally larger atomic radii than the second transition series.

The radii of the elements following the lanthanides is smaller than would be expected if there were no f-transition metals.

[edit] Chemical behavior of the lanthanides

Since the outer shells of the lanthanides do not change within the group, their chemical behaviour is very similar. The differing atomic and ionic radii does affect their chemistry, however. Without the lanthanide contraction a chemical separation of lanthanides would be extremely difficult. However, this contraction makes the chemical separation of period 5 and period 6 transition metals of the same group rather difficult.

[edit] Influence on the post-lanthanides

All elements following the lanthanides in the periodic table are influenced by the lanthanide contraction. The period 6 elements have very similar radii compared with the elements of the period 5 elements in the same group.

For example, the atomic radii of the metal zirconium, Zr, (a period 5 element) is 1.59 Ångström and that of hafnium, Hf, (a period 6 element) is 1.56 Ångström. The ionic radius of Zr⁴⁺ is 0.79 Ångström and that of Hf⁴⁺ is 0.78 Ångström. The radii are very closely similar even though the number of electrons increases from 40 to 72 and the atomic mass increases from 91.22 to 178.49 g/mol. The increase in mass and the unchanged radii lead to a steep increase in density from 6.51 to 13.35 g/cm3.

Zirconium and hafnium therefore have very similar chemical behaviour, having closely similar radii and electron configuration. Because of this hafnium (1923) was discovered 134 years later than zirconium (1789).