Effective nuclear charge

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ATingin_3I
Posts: 51
Joined: Fri Aug 30, 2019 12:17 am

Effective nuclear charge

Postby ATingin_3I » Mon Oct 28, 2019 3:40 pm

Is it true that the effective nuclear charge felt by an electron in the outermost shell of an atom is equal to the group # found on the periodic table? If so, why is this? And is this a reliable "trick" we can use?

DarrenKim_1H
Posts: 123
Joined: Fri Sep 20, 2019 12:17 am
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Re: Effective nuclear charge

Postby DarrenKim_1H » Mon Oct 28, 2019 9:52 pm

Hi Anna,

I believe what you are referring to is Slater's rule and it allow you to estimate the effective nuclear charge from the real number of protons in the nucleus and the effective shielding of electrons in each orbital "shell."

Brian Tangsombatvisit 1C
Posts: 119
Joined: Sat Aug 17, 2019 12:15 am

Re: Effective nuclear charge

Postby Brian Tangsombatvisit 1C » Mon Oct 28, 2019 10:01 pm

I'm not sure how to exactly calculate the effective nuclear charge felt by an electron when there's electron shielding. Professor Lavelle said in lecture that the outer electrons feel a reduced electrostatic attraction to the nucleus, resulting in an effective nuclear charge. It's not quite clear how to calculate this reduced charge, but I would say just know that there is a reduced charge as a result of the inner electrons shielding the outer electrons.

The formula to calculate the Zeff is probably not within the scope of this class, otherwise Professor Lavelle would have given the formula to us in lecture.

Paul Hage 2G
Posts: 105
Joined: Thu Jul 25, 2019 12:17 am

Re: Effective nuclear charge

Postby Paul Hage 2G » Mon Oct 28, 2019 10:33 pm

The effective nuclear charge felt by an electron in the outermost shell of an atom would be equal to the atomic number minus the number of shielding electrons (core electrons, not including valence electrons). Hope that helps.


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