Explain why the quantum number set (3, 2, -3, +½) is not possible for an electron in a ground-state atom.
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mmm this beyond me to answer...@confluxepic
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tag them all in one post
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@dan815 he might know because i tried but i can't figure it out and its way out of what i learned so im sorry i can't help
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I don't know about chemistry :T sorry
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omg no one is coming to help me i literally tagged everyone
@aaronq is the Chemistry master.
he's not on thts the problem :( and i asked praetorian but he didn't come either
He'll be on soon hopefully. (:
lol yea but i don't have all night and this question counts for alot
but whatever can u stay
no one is on this category and only one person comes and they say idk and then leave
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But you see, Aaron is the genius in this subject. But put in some effort in to your question.
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Idk, maybe this helps? https://answers.yahoo.com/question/index?qid=20110309140604AAlWUwP
Maybe this: http://www.answerbit.com/explain-why-the-quantum-number-set-3-2--3-is-not-possib-20111121082209AAZ9rN3
Maybe even this: http://openstudy.com/study#/updates/5070680de4b0c2dc83408097
This? :P http://openstudy.com/study#/updates/50c2bee6e4b066f22e106117
Maybe this might also help you: http://openstudy.com/study#/updates/5288eeaae4b0b33765120410
Well, take a look at those links, if you still don't understand it, then post what you don't understand, and what you know about this topic, and then just hope that aaronq comes online as soon as possible. :)
ok thanks so much
No problem (:
The values of later quantum numbers depend on the values of earlier quantum numbers. It's for this reason, as you'll see, the combination given in the question is not possible for a ground-state electron. Explanation follows...bear with me :P The first quantum number, n, is the principal quantum number, which indicates what energy level we're dealing with. In this case, the first quantum number is 3, so we're dealing with the 3rd energy level. The second quantum number, l, is the azimuthal quantum number, which indicates what energy sublevel within the energy level we're dealing with (e.g. s, p, d...). The possible values of the second quantum number depend on the value of the first quantum number. In fact, l can only take on values between 0 and n-1. Since n was 3 in this case, l can be 0, 1, or 2 (corresponding to s, p, and d). The second quantum number given in the question is 2, which is an allowed value for l. The third quantum number, m(l), is the magnetic quantum number, which indicates what orbital within the energy sublevel we're dealing with. The possible values of the third quantum number depend on the value of the second quantum number. In fact, m(l) can only take on values from -l to l. Since l in this case was 2, m(l) can be -2, -1, 0, 1, or 2. According to the question, however, the third quantum number is -3, which is NOT an allowed value for m(l) in a ground-state electron. This is why the combination of quantum numbers given does not make sense. Finally, for completeness, the fourth quantum number, m(s), is the spin quantum number, describes the spin of the electron in the orbital of interest. Every orbital can hold 2 electrons, with one electron having m(s)=-½, and the other electron having m(s)=½. The value of m(s) is always either ½ or -½, so it does not depend on the previous three quantum numbers. Hope that made sense, but if you have any questions let me know!
Nice answer matt
Haha thanks...hope it's as clear to @tywower as it was to you :P
ok, so you have (n, l, m\(_l\), m\(_s\)) n = your principal quantum number, but n must be positive and greater than 0 l = your angular quantum number, which describes orbital shape, and can be any value from n-1 m\(_l\) can be any number between -l, 0, l so therefore, if you have n = 3 \(l\) can be any valye between 0- 2, because remember l = n-1 and n = 3 3 - 1 = 2 therefore, your m\(_l\) values can range from -2, -1, 0, 1, 2 according to pauli exclusion principle, no two electrons in the same atom can have identical values for all four of their quantum numbers. What this means is that no more than two electrons can occupy the same orbital, and that two electrons in the same orbital must have opposite spins.
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