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Ben 1B
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Postby Ben 1B » Fri Dec 06, 2019 4:29 pm

How do you solve 1D.23 which asks how many orbitals can have the following quantum numbers in an atom? Is there a shortcut to finding out how many orbitals can have certain quantum numbers? Thanks!

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Re: Orbitals

Postby SnehinRajkumar1L » Sat Dec 07, 2019 12:10 am

Well, in the case of the question, we can look at part a.
You know that n = 2 and l = 1, meaning that it is in the p orbital. So, the orientation of the p orbitals doesn't matter and thus, there are 3 possible orbitals.
For part b, there is only one that can have those three quantum numbers because it specifies the orientation as well.

Nikki Razal 1L
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Re: Orbitals

Postby Nikki Razal 1L » Sat Dec 07, 2019 12:50 am

Once you find out what "l" is, you can figure out how many orbitals there are because to find the number of orbitals you can plug "l" into the equation 2*l+1, and that will give you the number of orbitals. Or you can think that ml=-l,...0...,+l, and the number of values you get also = the number of orbitals.. For example, if l=1, ml= -1,0,1, and because there are 3 values for ml, you have 3 orbitals

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