Question

Asked Apr 4, 2019

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Which of the following combinations of quantum numbers are allowed for an electron in a one-electron atom?

A) *n* = 7 , *l* = 5 , *m* = -2 , *m*_{s} = +1

B) *n* = 3 , *l* = 1 , *m* = 0 , *m*_{s} = -½

c) *n* = 4 , *l* = -4 , *m* = -5 , *m*_{s} = 0

Step 1

Principal quantum number is represented by n and values of n must be integers (1,2,3…)

When principal quantum number is n, then azimuthal quantum number (*l*) is from 0 to (n-1)

The values of magnetic quantum number (*m _{l}*) are

Spin quantum number (*m _{s}*) is always +1/2 or +1/2.

Step 2

(A) When n=7, the values of l are 0, 1, 2, 3, 4, 5, 6 and the values of *m _{l}* are (-6, -5, -4…4, 5, 6).

Step 3

(B) When n=3, the values of l are 0, 1, 2 and the values of *ml* are (-2,-1, 0, 1, 2). The given value of *ms*...

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