2.29 (6th Edition)

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Claudia Luong 4K
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2.29 (6th Edition)

Postby Claudia Luong 4K » Thu Oct 18, 2018 2:20 am

I am confused on parts b and d on this problem. How does specifying the magnetic quantum number change the number of orbitals and/or the number of electrons that the orbitals can hold?

2.29 How many electrons can have the following quantum numbers in an atom: (b) n =4, l= 2,
ml= 2; (d) n =3, l=2, ml =1

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Re: 2.29 (6th Edition)

Postby Chem_Mod » Thu Oct 18, 2018 9:35 am

Recall that the magnetic quantum number specifies which orbital we're looking at in a given subshell.
For example, in a p subshell (l=1), we have ml values (-1,0,1), and each of these correspond with a different p orbital orientation (px, py, pz). In each orbital, we can have 2 electrons maximum.

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