The magnetic quantum number m for an electron in a 2p subshell can take the values
Correct answer: B. minus 1, 0 and plus 1
- A. 0 only
- B. minus 1, 0 and plus 1
- C. minus 2 to plus 2
- D. plus 1 only
Explanation
The magnetic quantum number runs from minus l to plus l, and for a p subshell l equals 1, giving three values that correspond to the three perpendicular orientations of the p orbital. A d subshell with l equal to 2 would give five values. The number of values is always 2l plus 1.
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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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