# Shielding effect of d electrons

In transition elements shielding effect is observed . Due to this zinc shows abnormality in atomic size. But at the same time we also say that gallium has same similar size as aluminium due to poor shielding effect of d electrons . Why is it that d electrons have good shielding effect in case of zinc but poor shielding effect in case of gallium?

• Slater's rule may be used for quantitative reasoning – Zenix Mar 26 '20 at 7:02

Two effects works first is $$Z_{eff}$$. Another effect is electronic repulsion.At the starting the no of electron in $$d-$$ orbital are less so $$Z_{eff}$$ is dominant over electronic repulsion but as we are moving alosng d-orbital electronic effect become dominant factor over $$Z_{eff}$$, So in the middle redius become almost constant and at the end it increases.
When we are talking about gallium and Aluminium radius comparision thats mean we are talking about group trends ,So in group trend abnormal size is due to poor shielding effect and relativistic effect. Normal trend on going down the size increases from aluminium to gallium size decreases because here a poor shielding of 3-d orbital present so $$Z_{eff}$$ penetarate and valence shell contract so size decreases.