Which set of quantum numbers is not possible?
- A. n = 2, l = 1, m = 0
- B. n = 3, l = 2, m = -2
- C. n = 2, l = 2, m = 1
- D. n = 4, l = 0, m = 0
Explanation
The azimuthal quantum number l is restricted to values from 0 up to n minus 1, so with n equal to 2 the only allowed values of l are 0 and 1. A set with n equal to 2 and l equal to 2 would describe a 2d orbital, which does not exist. Every other set listed satisfies both that rule and the requirement that m lies between minus l and plus l.
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