Problem: Which set of quantum numbers cannot specify an orbital? a. n = 2, l = 1, ml = -1 b. n = 3, l = 2, ml = 0 c. n = 3, l = 3, ml = 2 d. n = 4, l = 3, ml = 0

FREE Expert Solution

To solve this problem, let’s first define the values of the first three quantum numbers:

 principal quantum number (n)  energy level in orbitals and its value could be any positive integer starting from 1 to infinity

 angular momentum quantum number ((l) has to be at least 1 less than n, range of values from 0 up to (n-1)

• magnetic quantum number (m) → range of values from - to +.


Let’s check each set of quantum numbers given: 

a. n = 2;  = 1; m = -1

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Problem Details

Which set of quantum numbers cannot specify an orbital? 

a. n = 2, l = 1, ml = -1 

b. n = 3, l = 2, ml = 0 

c. n = 3, l = 3, ml = 2 

d. n = 4, l = 3, ml = 0

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