1D. 23)

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905416023
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Joined: Thu Jul 25, 2019 12:17 am

1D. 23)

Postby 905416023 » Mon Oct 21, 2019 10:43 pm

On problem 1D.23 I am having trouble. How do I begin to know how many orbitals can have the following quantum numbers in an atom? The concept, in general, confuses me, not just this specific question.

Natalie Nartz 4F
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Joined: Thu Jul 11, 2019 12:17 am

Re: 1D. 23)

Postby Natalie Nartz 4F » Tue Oct 22, 2019 12:54 am

For part A, n= 2 and l=1 which makes it 2p, the p-subshell has three orbitals: 2px, 2py, 2pz. For part B n=4 l=2 and ml= -2 which represents only one orbital

I hope this help

Justin Seok 2A
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Joined: Sat Aug 24, 2019 12:15 am

Re: 1D. 23)

Postby Justin Seok 2A » Tue Oct 22, 2019 10:21 am

Also for orbitals in general, n is the energy level, l is the subshell and ml is the orbitals within the subshell. So if you are only given n=2 for example, you would know that l can either be 0 or 1, or s or p, since l is 0, ... , n-1. For l, 0/s has 1 orbital, 1/p has 3 orbitals, 2/d has 5, and 3/f has 7. Since with n=2 we know l can be 0 or 1, the number of possible orbitals is 1+3, or 4.

805097738
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Joined: Wed Sep 18, 2019 12:20 am

Re: 1D. 23)

Postby 805097738 » Wed Oct 23, 2019 8:54 am

so if ml is given and it is one value, that represents one orbital?

Michelle Le 1J
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Joined: Fri Aug 09, 2019 12:16 am

Re: 1D. 23)

Postby Michelle Le 1J » Wed Oct 23, 2019 11:23 am

When ml is given, that means they already specified what orbital they are talking about, so I believe there is only one orbital.

KBELTRAMI_1E
Posts: 108
Joined: Sat Jul 20, 2019 12:17 am

Re: 1D. 23)

Postby KBELTRAMI_1E » Wed Oct 23, 2019 11:26 am

905416023 wrote:On problem 1D.23 I am having trouble. How do I begin to know how many orbitals can have the following quantum numbers in an atom? The concept, in general, confuses me, not just this specific question.


I believe we went over it in class. I would check google images for a diagram to be sure of the number of orbitals for each qn.


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