1D.23

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Norah Gidanian 3J
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Joined: Wed Sep 30, 2020 9:49 pm
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1D.23

Postby Norah Gidanian 3J » Tue Oct 20, 2020 10:12 am

How many orbitals can have the following quantum numbers in an atom: (a) n = 2, l = 1; (b) n = 4, l = 2, ml = 22; (c) n = 2; (d) n = 3, l = 2, ml = 11?

How would you do part c without being given the value of l?

TrishaP_3E
Posts: 40
Joined: Wed Sep 30, 2020 9:58 pm

Re: 1D.23

Postby TrishaP_3E » Tue Oct 20, 2020 1:00 pm

I think because l isn't specified, you would have to count all of the orbitals that would be within the 2 subshells, so 2s and 2p.

Sophia Wendin 2B
Posts: 40
Joined: Wed Sep 30, 2020 9:48 pm

Re: 1D.23

Postby Sophia Wendin 2B » Tue Oct 20, 2020 1:31 pm

Since we are only given n, the answer is all of the orbitals in the n=2 energy level. So the answer would be 4 since there is 1 2s orbital and 3 for 2p!


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