# Question on d block contraction

For size trend down a group, it is known that:$$Al\gt Ga$$

Due, to d block contraction of gallium.

Why isn't this the case when it comes to silicon and germanium? Won't the poor shielding effect from the d electrons have an effect here?

The Answer on the SE for a similar question does not really answer the question.

• See this: imgur.com/MZ9dpRe – Nilay Ghosh Nov 22 '20 at 6:45
• @NilayGhosh sorry, That didn't help me much.(-_-;).Is it because it is just an observed property? – JustJohan Nov 22 '20 at 6:50
• Does this help? – Light Yagami Nov 22 '20 at 6:56

If germanium is supposed to be bigger than aluminum, in fact, its empirical values correspond to $$\pu{125pm}$$ for each one respectively, but germanium being lower in the periodic table is bigger at the same time which is why we say that $$\ce{Al < Ga}$$. Now yes, the atomic radius of silicon is $$\pu{118pm}$$ while as we said before, the atomic radius of germanium is $$\pu{125pm}$$, in the same way the size is deduced based on its position in the periodic table, so $$\ce{Si < Al < Ga}$$.
This occurs because there is a relationship between the effective nucleus charge and the electronic levels of the atom, since the positive nucleus attracts the electrons, but in turn, the electrons repel each other (except those of the first level), it is by This means that the forces and counter forces end up having an effect on the valence electrons, and these determine the atomic radius of the atom. This difference of attraction by the nucleus and repulsion by the electrons increases as there are more electronic levels, that is, if I have a compound with Z = 11 and e = 11 that we will call "A", it will be greater than a compound "B" whose Z = 10 e = 10, leaving B <A since although both have the same number of electrons as protons, compound A has an electronic configuration $$\ce{1s^2 2s^2 2p^6 3s^1}$$ with 11 protons while compound B has an electronic configuration of $$\ce{1s^2 2s^2 2p^6}$$ with 10 protons, that is, compound A has a higher electronic level than compound B, which gives a larger atomic radius.