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Postby CalebBurns3L » Thu Nov 02, 2017 4:27 pm

I'm confused about how the l quantum number works. I understand that it determines shape in that l = 0 means s-orbital, l = 1 means p-orbital and so on. But if n>4 then can't l be greater than 3? What shape would an l number >3 have? Does it cycle through the shapes?

Thank you!

Julia Meno 1D
Posts: 28
Joined: Fri Sep 29, 2017 7:04 am

Re: Subshells

Postby Julia Meno 1D » Thu Nov 02, 2017 6:32 pm

Hey! I think for this class, we will only need to know what subshell corresponds to l when l is less than or equal to 3 (so l = 0, 1, 2, 3 or s-, p-, d-, f-orbital). But, you're correct in the sense that if n > 4, then l will continue to have its greatest value at n - 1. However I don't think we need to identify what subshells/shape it would have at that level :)

Pooja Nair 1C
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Joined: Thu Jul 13, 2017 3:00 am

Re: Subshells

Postby Pooja Nair 1C » Fri Nov 03, 2017 11:49 am

Theoretically, it's possible for l to be higher than 3 (you could potentially have a g orbital in which case the first occurance would be in 5g) but we don't directly address it in this class, so you only need to know up to f orbitals, and that for an f orbital, l = 3

Rithik Kumar 3E
Posts: 25
Joined: Fri Sep 29, 2017 7:06 am

Re: Subshells

Postby Rithik Kumar 3E » Wed Nov 15, 2017 12:55 am

I agree with the above posts. However, I believe that this course restricts us to consider orbital shapes up to the d and f orbitals or (l=2 and 3). As a general rule of thumb, however, as your "l" value increases, the orbital shape's complexity increases.

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