Which set of quantum numbers is not possible?
Correct answer: C. n = 2, l = 2, m = 1
- 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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About Quantum Numbers
Quantum numbers describe an electron's energy level, subshell, orbital orientation and spin. You examine the principal, azimuthal, magnetic and spin quantum numbers, their allowed values, orbital capacity and how they determine electronic configurations and distinguish electrons within an atom.
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