electron shielding 2.37(c) [ENDORSED]

[Caitlin Mispagel 1D]

Why is it that electrons having l=1 are better at shielding than electrons having l=2?

[Gurpreet Khamba 1J]

This is because when an electron has a position closer to the nucleus, l=1 or even 1=0, it blocks off more attraction than one in a position after it, in this case l=2.

[Michelle Dong 1F]

The electrons in l=1 (p subshell) are closer to the positive nucleus and thus are able to shield the outermost valence electrons more effectively than the electrons in l=2 (d subshell).

[dstemp]

Doesn't electron shielding also affect the effective nuclear charge? If so, do you know what the trend is on the periodic table for effective nuclear charge?