half full?

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Alondra Juarez section 1E
Posts: 47
Joined: Fri Sep 29, 2017 7:03 am

half full?

Postby Alondra Juarez section 1E » Sun May 06, 2018 5:14 pm

What is meant by the phrase it is half full in the context of orbitals? for example how do we know when an orbital is half full or completely full?

AshleyLamba1H
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am

Re: half full?

Postby AshleyLamba1H » Sun May 06, 2018 5:22 pm

An atom is half full when one electron is in each orbital. An atom is completely full when there are two electrons in each orbital. Remember that electrons fill all the empty orbitals first before pairing with electrons in them.

Amanda 1A
Posts: 31
Joined: Fri Apr 06, 2018 11:01 am

Re: half full?

Postby Amanda 1A » Sun May 06, 2018 6:49 pm

I don't know if I heard this right, but why are half-filled orbitals more stable?

Alexander Hari 1L
Posts: 30
Joined: Wed Feb 14, 2018 3:02 am

Re: half full?

Postby Alexander Hari 1L » Sun May 06, 2018 7:10 pm

Amanda, half-filled orbitals or full orbitals are more stable than a subshell with only a few electrons because the atom is trying to gain or lose electrons to meet either of those stages. For example a 2p orbital can contain up to 6 electrons. It's happier state is either 3 or 6, and if it is at 4 it is unhappy and will try to lose an electron to go back to 3.

Chem_Mod
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Joined: Thu Aug 04, 2011 1:53 pm
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Re: half full?

Postby Chem_Mod » Sun May 06, 2018 10:01 pm

Because it avoids spin-spin interactions.

Jennifer Tuell 1B
Posts: 34
Joined: Fri Apr 06, 2018 11:05 am

Re: half full?

Postby Jennifer Tuell 1B » Sun May 06, 2018 10:27 pm

This is similar to how for Chromium and Copper the electron configuration is more stable for example Cr [Ar] 3d5 4s1 is more stable than
Cr [Ar] 3d4 4s2.


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