shielding and penetrating

[Monica Soliman 3F]

Can someone explain shielding and penetrating in relation to L? How does it change if l increases or decreases?

[Stuti Pradhan 2J]

Since the s orbital is around the nucleus, s electrons are able to shield outer electrons well. On the other hand, p orbitals have a node where the nucleus is, so they are not able to shield outer electrons well. I also believe that d orbital electrons are not able to shield electrons very well either.

In regards to l, the electrons are less successful in shielding as the value of l increases. This would also support the overall trend in effective nuclear charge increasing from left to right across the periodic table.

Hope this helps!

[Chenning Yang Dis3l]

Thank you for the information! It really helps!

[SamayaJoshi1A]

Also something to remember is that the effective nuclear charge is never proportional to the number of levels. For example if there is an electron in the second level, it does not have half the strength of the one in the first level. It all depends on other factors.

[Joshua Eidam 2A]

Also I think it is important to notice that other electrons contribute to the shielding effect with the negative repulsion. I found this on a website and I thought it was helpful: "In hydrogen-like atoms, which have just one electron, the net force on the electron is as large as the electric attraction from the nucleus. However, when more electrons are involved, each electron (in the n-shell) feels not only the electromagnetic attraction from the positive nucleus but also repulsion forces from other electrons in shells from 1 to n-1."

https://courses.lumenlearning.com/intro ... ar-charge/

Hope this helps.

[CesarLec1]

The electrons in the inner levels take the brunt of the nuclear charge and the e- in the outer shells feel less of the effect thus they can escape more easily.