In the n=3 principal level, what is the maximum number of electrons that could have l=2?

Solution:

Let's go over the quantum numbers.

n = Energy Level

n can be be any positive integer: 1,2,3,4,5,6....

l = Angular Momentum Quantum Number (Orbital shape)

l can go from 0 to n-1

Example: If n=2→ l: 0,1. If n=4→ l= 0,1,2,3.

ml = Magnetic Quantum Number ( Orbital Orientation)

ml can go from -l....0....+l

Example if l=3 → ml = -3,-2,-1,0,1,2,3

If l=2, then ml = -2,-1,0,1,2. Each ml value can hold a maximum of two electrons (with opposite spins), giving a total of 5×2=10electrons.

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