1.D.23  [ENDORSED]

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Postby RRahimtoola1I » Wed Oct 16, 2019 2:21 pm

"How many orbitals can have the following quantum numbers in an atom:(a)n=2, l=1; (b)n=4, l=2, ml=22; (c)n=2; (d)n=3, l=2, ml=1?"

For a, is the number of orbitals only dependent on the subshell (p) and the amount of orientations possible for it?

For b and d, is it only 1 because the orientation is specific? Does the electron spin not matter?

For c, is it 4 because if n=2, then there is 2s, 2p, 2d, 2f? If n=1 would it be 1s only be 1 because p, d, and f don't have a subshell where n=1?

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Re: 1.D.23  [ENDORSED]

Postby RoshniVarmaDis1K » Wed Oct 16, 2019 2:34 pm

a) n=2, l=1 represents the 2p subshell, which would have three orbitals.
b) n=4, l=2, ml=2 represents a specific orbital in the 4d subshell, so only one orbital could have these numbers.
c) n=2 represents 2s and 2p, which would have a total of four orbitals.
d) n=3, l=2, ml=1 represents a specific orbital in the 3d subshell, so only one orbital could have these numbers.

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Re: 1.D.23

Postby MAC 4G » Thu Oct 17, 2019 3:57 pm

For A, n=2 means we're looking at the second shell. And l = 1 means we're looking at a p orbital. Because the magnetic quantum number is not specified, we don't know the orientation. This means that it could be any of the three p orbitals. Therefore, 3 orbitals can have these quantum numbers.

For C, given only n=2 means all we know is that we are looking at the second shell. In the second shell, we have one s orbital and 3 p orbitals. Therefore, 4 orbitals can have this quantum number.

For B and D is 1 because they both have 3 quantum numbers that identify 1 orbital

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