Which of the following is a possible set of quantum numbers for an electron n, l, m subscript l, m subscript s ?
A. (1, 1, 0, 1/2)
B. (2, 1, 1, 1/2)
C. (3, 2, 3, -1/2)
D. (3, -2, 1, -1/2)
Stacey Warren - Expert brainly.com
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N = principle quantum number, tells you your energy level.
L = shape that's the way I think of L
m = can be less than or equal to L, shows how many orientations the orbitals can have. Can't be greater than L
S = spin can either be +1/2 or -1/2 don't remember exactly.
Say if we have 2P
P orbitals have 3 possible orientations,
L = 1
M = +1 -1 0 corresponding to the Px,Py,Pz
You can have spin up or down
If we have l = 2
That means we can have
-2, -1, 0, 1, 2 which is five orientations
Two electrons for each orbital so that's 10 total. That would give us a D orbital.
a D orbital would have l = 2 and would start at principle quantum number of 3
You know that the spin can either be +1/2 or -1/2 so that won't tell you which one is right. So based off of what I said can you predict what the answer would be?