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(a) Write down the quantum numbers for the states described in spectroscopic notation as^{2}S_{3/2},^{3}D_{2}and^{5}P_{3}.

(b) Determine if any of these states are impossible, and if so, explain why. (Please note that these could describe states with more than one electron.)

My Attempt

A)

I came up with the quantum numbers for everything that I'm pretty sure is correct. Was hoping I could get a double check on this.

^{2}S_{3/2}l = 0, s = 1/2, j = 3/2

^{3}D_{2}l = 2, s = 1, j = 2

^{5}P_{3}l = 1, s = 2, j = 3

B)

I'm almost 100% confident that^{2}S_{3/2}is impossible because when l = 0, j must = 1/2.

I'm not sure about the other two because I don't know all the rules for what s can be compared to l and j.

Any help would be greatly appreciated. Thank you!

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# Homework Help: Spectroscopic Notation Problem

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