Choose the allowed sets of quantum numbers from the following:
Correct answer: B. n = 3, l = 1, m = 0, s = +1/2
- A. n = 2, l = 2, m = 0, s = +1/2
- B. n = 3, l = 1, m = 0, s = +1/2
- C. n = 4, l = 3, m = 4, s = -1/2
- D. n = 4, l = 2, m = 4, s = -1/2
Explanation
The correct answer is Option B: n = 3, l = 1, m = 0, s = +1/2. This set of quantum numbers is valid because:n (principal quantum number) can be any positive integer.l (azimuthal quantum number) can be any integer from 0 to n-1.m (magnetic quantum number) can range from -l to +l.s (spin quantum number) can be either +1/2 or -1/2.In Option A, l = 2 is not allowed for n = 2, as l must be less than n. In Option C, m = 4 is outside the valid range for l = 3. Similarly, in Option D, m = 4 is outside the valid range for l = 2.
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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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