shielding effect of s and p-orbitals

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Sue Xu 2K
Posts: 58
Joined: Fri Sep 29, 2017 7:06 am

shielding effect of s and p-orbitals

Postby Sue Xu 2K » Thu Nov 02, 2017 6:45 pm

In the homework question 2.37 it says "an electron in an s-orbital can penetrate to the nucleus of the atom". What does it mean by "penetrate"?

Amanda Hagen 1L
Posts: 26
Joined: Fri Sep 29, 2017 7:04 am

Re: shielding effect of s and p-orbitals

Postby Amanda Hagen 1L » Thu Nov 02, 2017 10:12 pm

S-electrons can "penetrate" the nucleus (be found at the nucleus) because it has a nonzero probability at the nucleus. Therefore the s-oribtal has a spherical shape encompassing the nucleus, while the higher orbitals (p,d,f) have nodal planes (zero probability of being found) at the nucleus.

Sophie Krylova 2J
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Joined: Fri Sep 29, 2017 7:06 am

Re: shielding effect of s and p-orbitals

Postby Sophie Krylova 2J » Fri Nov 03, 2017 6:20 am

How does the ability to "penetrate" the nucleus account for higher Zeff?

Hyein Cha 2I
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Re: shielding effect of s and p-orbitals

Postby Hyein Cha 2I » Fri Nov 03, 2017 7:00 am

sofiakrylova3j wrote:How does the ability to "penetrate" the nucleus account for higher Zeff?


Ability to penetrate means that the electron can be closer to the nucleus, thus the net positive charge experienced by the electron will be stronger than the net positive charge experienced by the electron that's farrr away from the nucleus, making Zeff higher.

Jessica Schirmer 1J
Posts: 20
Joined: Fri Sep 29, 2017 7:04 am

Re: shielding effect of s and p-orbitals

Postby Jessica Schirmer 1J » Fri Nov 03, 2017 8:54 am

An e- in a s-orbital can penetrate the nucleus because according to Schrodinger's wave equation, the 3D shape/probability of the s-orbital has no nodes (probability never reaches zero).


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