Which of the following quantum numbers represent the impossible arrangement(s) of $n, l, m_{l}, m_{s}$ respectively?

3, 2, 2, + \frac{1}{2}

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3, 2, 3, + \frac{1}{2}

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4, 0, 0, + \frac{1}{2}

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5, 3, 0, + \frac{1}{2}

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Solution

The correct option is D $3, 2, 3, + \frac{1}{2}$
Option B, i.e., 3, 2, 3, +1/2 represents the impossible arrangement of the quantum numbers.
In this arrangement, the value of $m_{l}$ is 3 which is greater than the value of l, which is 2.
This is not possible.

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Similar questions

Q. Arrange the electrons represented by the following sets of quantum numbers in decreasing order of energy.
(i)

n = 4, l = 0, m_{l} = 0, m_{s} = + \frac{1}{2}

(ii)

n = 3, l = 1, m_{l} = 1, m_{s} = - \frac{1}{2}

(iii)

n = 3, l = 2, m_{l} = 0, m_{s} = + \frac{1}{2}

(iv)

n = 3, l = 0, m_{l} = 0, m_{s} = - \frac{1}{2}

The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. If any of these combination(s) has/have the same energy lists:
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2. n = 3, l = 2, ml= 1 , ms = +1/2
3. n = 4, l = 1, ml = 0 , ms = +1/2
4. n = 3, l = 2, ml = –2 , ms = –1/2
5. n = 3, l = 1, ml = –1 , ms= +1/2
6. n = 4, l = 1, ml = 0 , ms = +1/2

Q. The quantum number of four electrons are given below:
I.