2 orbitals occupied

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Crystal Odipo 1F
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Joined: Wed Sep 30, 2020 9:53 pm

2 orbitals occupied

Postby Crystal Odipo 1F » Sun Oct 25, 2020 9:19 pm

I understand how 2 different orbitals can be occupied like if n=2, 2-1=1, l can be 0 or 1 making it a p and s orbital.

Samudrala_Vaishnavi 3A
Posts: 93
Joined: Wed Sep 30, 2020 9:34 pm

Re: 2 orbitals occupied

Postby Samudrala_Vaishnavi 3A » Mon Oct 26, 2020 8:58 am

I may not answer your question fully but this is what I am getting. You are on the right track in your thinking. These "orbitals" that you calculated from n=2 are correct. However, they refer to separate subshells which have their own number of orbitals of which the electrons (two per orbital) can fill. You would determine the number of orbitals and types of orbitals within a subshell using the magnetic quantum number which is (l, l-1, -l). So for l=1, the p-orbital or subshell has (1,0,-1) or a range of (-1, 0, 1) so it has 3 orbitals which can each be filled each with two electrons. So a filled p-orbital or subshell, really means filling three orbitals (6 electrons total).

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