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Donna Nguyen 2L
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Joined: Sat Aug 24, 2019 12:17 am


Postby Donna Nguyen 2L » Wed Oct 23, 2019 1:30 am

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?

How would I approach this problem?

Ashley Osorio
Posts: 54
Joined: Thu Jul 11, 2019 12:17 am

Re: 1D.23

Postby Ashley Osorio » Wed Oct 23, 2019 1:56 am

We focus on the l values here. For a, since l=1, that means ml can be -1,0, or 1. That's a total of three values, so it has 3 orbitals (this applies to c as well).
However, I'm actually lost as how to solve b and d. Does the fact that we have an ml value change the number of orbitals, or does it still fall on the value of l?

Posts: 102
Joined: Thu Jul 11, 2019 12:17 am

Re: 1D.23

Postby ALegala_2I » Wed Oct 23, 2019 9:02 am

For b and d, you would go off of the ml number. In a 4p atom in which l=1, there are 3 possibly orbitals orientations as stated above. This means that an electron in the 4p orbital could have the following configurations: n=4, l=1, ml = 1; n=4, l=1, ml = 0, and n=4, l=1, ml = -1. When you are given the ml number, it is talking about a specific orientation of an orbital. So the possibility that an electron in an atom has a specific n, l, and ml number is only existent in one orbital.

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