d-block contraction

The d-block contraction (sometimes called scandide contraction) is a term used in chemistry to describe the effect of having full d orbitals on the period 4 elements. The elements in question are gallium, germanium, arsenic, selenium, bromine, and krypton. Their electronic configurations include completely filled d orbitals (d¹⁰). The d-block contraction is best illustrated by comparing some properties of the group 13 elements to highlight the effect on gallium.

Atomic radius of elements of the groups 2, 13 and 14, showing the "d-block contraction", especially for Ga and Ge

Element	Atomic electron config.	Sum 1st – 3rd I.Ps kJ/mol	M3+ electron config.	M3+ radius (pm)[1]
Boron, B	[He] 2s2 2p1	6887.4	[He]
Aluminium, Al	[Ne] 3s2 3p1	5139	[Ne]	53.5
Gallium, Ga	[Ar] 3d10 4s2 4p1	5521.1	[Ar] 3d10	62
Indium, In	[Kr] 4d10 5s2 5p1	5083	[Kr] 4d10	80
Thallium, Tl	[Xe] 4f14 5d10 6s2 6p1	5438.4	[Xe] 4f14 5d10	88.5

Gallium can be seen to be anomalous. The most obvious effect is that the sum of the first three ionization potentials of gallium is higher than that of aluminium, whereas the trend in the group would be for it to be lower. The second table below shows the trend in the sum of the first three ionization potentials for the elements B, Al, Sc, Y, and La. Sc, Y, and La have three valence electrons above a noble gas electron core. In contrast to the group 13 elements, this sequence shows a smooth reduction.

Element	Atomic electron config.	Sum 1st – 3rd I.Ps kJ/mol	M3+ electron config.	M3+ radius (pm)[2]
Boron, B	[He] 2s2 2p1	6887.4	[He]
Aluminium, Al	[Ne] 3s2 3p1	5139	[Ne]	53.5
Scandium, Sc	[Ar] 3d1 4s2	4256.7	[Ar]	74.5
Yttrium, Y	[Kr] 4d1 5s2	3760	[Kr]	90
Lanthanum, La	[Xe] 5d1 6s2	3455.4	[Xe]	103.2

Other effects of the d-block contraction are that the Ga³⁺ ion is smaller than expected, being closer in size to Al³⁺. Care must be taken in interpreting the ionization potentials for indium and thallium, since other effects, e.g. the inert-pair effect, become increasingly important for the heavier members of the group.
The cause of the d-block contraction is the poor shielding of the nuclear charge by the electrons in the d orbitals. The outer valence electrons are more strongly attracted by the nucleus causing the observed increase in ionization potentials. The d-block contraction can be compared to the lanthanide contraction, which is caused by inadequate shielding of the nuclear charge by electrons occupying f orbitals.

See also

• Periodic table
• Electronegativity
• Electron affinity
• Effective nuclear charge
• Electron configuration
• Exchange interaction
• Lanthanide contraction

References

• Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.