How do you determine the maximum amount of electrons given quantum numbers?

Question

For example, given n=2, l=1, ml= -1, and ms = -1/2 what would be the maximum amount of electrons? my book isn't clear on it. thanks for the help!

Answer 1

All four numbers are characteristic of only one electron
Given the three first of them, you can have two electrons (ms of different signs)
Given the two first of them, you define the number of different (ml)s as the number of all the integers whose absolute value is greater or equal to the l value.
[an ml can lead to two (ms)s=electrons at most]
You can figure out the rest.

Answer 2

An odd question indeed. Your shell (n=2) has a maximum of 8, but your subshell (l=1) has a maximum of 6, your orbital (ml=-1) has a maximum of 2 and the spin state (ms=-1/2) restricts you to 1 electron. You can think of a set of quantum #s as a unique address for each electron. If you have 4 #'s, then it represents only 1 electron.

Answer 3

suppose n=x,then l=0 to x-1,for any value of l(ie from 0 to (x-1))ml will be from -l to l,for any value of ml there can be two electron havingopposite spin ie(1/2,-1/2)
in this problem n=2(till this there can be 8 electrons)
l=1(till this 6 electrons b'coz there r 3 (ie -1,0,1)value of ml and for every ml there r2 electrons)
ml=-1(for this there r 2 electrons)
finally for ms=-1/2 there is one electron )

Answer 4

Here's the formula: 2n^2
Be careful with the formula due to the fact that if only applies to maximum e' population questions.