1D.23

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Brandon Valafar
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Joined: Sat Aug 17, 2019 12:16 am
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1D.23

Postby Brandon Valafar » Sun Oct 20, 2019 5:37 pm

I am so confused on this problem? Can anyone help?
How many orbitals can have the following quantum numbers in an atom:(a)n=2,l=1; (b)n=4,l=2,ml=-2; (c)n=2;(d)n=3,l=2,ml=1 ?

Solutions manual says the answers are 3,1,4,1 but I have no idea how they got that.

Matt F
Posts: 100
Joined: Sat Aug 17, 2019 12:17 am

Re: 1D.23

Postby Matt F » Sun Oct 20, 2019 6:05 pm

Basically the question is asking how many possible values of ml there are for the given set of quantum numbers. Remember, the value of ml ranges from l to -l. For b) and d), the answer is 1 since they give you ml already. For a), the answer is 3 since ml can be 1, 0, or -1 given l=1. For c), the answer is 4 since l could be 1 or 0, meaning that ml can be 1,0, or -1, or 0 (if l=0).


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