Here's the question you clicked on:
IsTim
If every electron must have a unique set of 4 quantum numbers, how many different electrons (Sets of 4 quantum numbers) can there be for each principal quantum number from n=1 to n=3?
Well, for n =1, there can only be 2 electrons, so 2 sets of unique quantum #s. For n = 2, there can be 8 electrons, so 8 sets unique of quantum #s. For n = 3, there are 18 electrons and so 18 sets...
Here' my answer and the reasoning behind it: For each principal quantum number from n=1 to n=3, there must be 12 electrons. I got this answer by counting spin quantum # in Tbl. 4, a summary of quantum numbers.
How did yo uget your answer???
For n=1, there is only one s-orbital, which can accomodate only two electrons. For n=2, you'll get s and p(6 elecrtons) orbitals both. And for n=3, you get s and p and d orbitals(10). The no. of electrons cannot be same in all the shells. Rogue is right.
Hmm, my explanation wasn't posted either... 4th time today! Not fun retyping... Mani's answer is pretty good :)