2.37

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Emily 1E
Posts: 27
Joined: Fri Apr 06, 2018 11:03 am

2.37

Postby Emily 1E » Sun May 06, 2018 4:52 pm

Part b) of this question where you have to determine whether the statements are true or false is: Electrons in an s-orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge because an electron in an s-orbital can penetrate to the nucleus of the atom.

What exactly does it mean by "electron in an s-orbital can penetrate to the nucleus of the atom." and how is this different from other orbitals?

AnthonyDis1A
Posts: 30
Joined: Fri Apr 06, 2018 11:05 am

Re: 2.37

Postby AnthonyDis1A » Sun May 06, 2018 10:48 pm

I think it just means that the s-orbitals are closer to the nucleus. There is a greater density of s-orbital electrons near the nucleus than that of other subshells.

RubyLake1F
Posts: 41
Joined: Fri Apr 06, 2018 11:03 am

Re: 2.37

Postby RubyLake1F » Sun May 06, 2018 10:49 pm

I think that 'penetration' to the nucleus means how close an electron can get to the nucleus. Electrons in the S sub shell have the lowest energy because they are closest to the nucleus (remembering that the closer an electron is to the nucleus the lower/more negative it's energy is) so they are better able to penetrate to the nucleus, which also means that they shield the outer electrons (eg. those in the p orbitals or in outer shells) from the effective nuclear charge. The answer to b) should be "true".

105012653 1F
Posts: 30
Joined: Fri Apr 06, 2018 11:02 am

Re: 2.37

Postby 105012653 1F » Thu Jun 14, 2018 1:03 pm

also was confused about this question..


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