Question

Which of the following set of quantum numbers (ordered n, ℓ, mℓ) are possible for an electron in an atom?

Check all that apply.

a,	4, 2, -1
b,	-4, 3, 1
c,	3, 1, -2
d,	3, 3, 1
e,	3, 2, 0
f,	2, 1, 3
g,	4, 2, -2

Answer 1

We know that principal quantum number is n, azimuthal quantum number is l amd magnetic quantum number is ml

n = 1, 2, 3, ..., n
l = 0 to n − 1 >> This includes all possible values up to n-1.
ml = all values from -l to +l >> example if l = 2 them ml = -2, -1, 0, +1, +2

a. here this is possible for all the quantum numbers

b. this not a possible configuration because n value cannot be negative

c. This is not possible because ml value lies between -1 to +1

d. This is not possible. l cannot equal to n

e. this is a possible configuration

f. it is not possible because ml value must lies between -1 to +1

g. This is a possible configuration