Which of the following sets of quantum numbers (n, l, mₗ, mₛ) is NOT allowed for an electron in an atom?
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A.
(2, 1, −1, −1/2)
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B.
(4, 3, −4, +1/2)
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C.
(5, 2, 0, −1/2)
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D.
(3, 2, 1, +1/2)
Correct Answer:
B. (4, 3, −4, +1/2)
Explanation:
The set of quantum numbers (4, 3, -4, +1/2) is not allowed because the magnetic quantum number (ml) is restricted by the angular momentum quantum number (l). Specifically, ml must be an integer ranging from -l to +l. In this instance, since l equals 3, the possible values for ml are limited to the range of -3 to +3. A value of -4 falls outside these permitted boundaries, making the combination physically impossible according to the rules of quantum mechanics. All other options provided follow the standard requirements where n is a positive integer, l is between 0 and n-1, and ms is either +1/2 or -1/2.
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