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) → (l) has to be at least 1 less than n, range of values from 0 up to (n-1)
• magnetic quantum number (mℓ) → range of values from -ℓ to +ℓ.
Let’s check each set of quantum numbers given:
a. n = 2; ℓ = 1; mℓ = -1
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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