Shielding in Multi-Electron Atoms (1E.5)

[Julia Lindner 1I]

Are electrons with lower values of l (i.e. l=1) always better at shielding than electrons with higher values of l (i.e. l=2)? In other words, would an electron in the p-orbital be more effective at shielding than would an electron in the d-orbital? If so, why? Does this have to do with penetration to the nucleus or just the relative positions of the electrons?

[Kim Tran 1J]

Yes. Electrons with lower values of l are better at shielding. The lower the number of l, the closer it is to the nucleus. The electrons closer to the nucleus block (or shield) the outer electrons from getting close to the nucleus. The electron density of s- or p- orbital is much higher than the f- or d- orbital where electrons are spread further from each other, hence the electrons in s- or p- orbitals are better at shielding.