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Spin Quantum Number

Which set of ...

Question

Which set of quantum numbers is not possible?

A

n = 1, l = 0,

m_{l}

= 0,

m_{s}

= 0

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B

n = 1, l = 0,

m_{l}

= 0,

m_{s}

= + 1/2

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C

n = 2, l = 1,

m_{l}

= 1,

m_{s}

= + 1/2

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D

n = 1, l = 0,

m_{l}

= 0,

m_{s}

= + 1/2

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Solution

The correct option is A n = 1, l = 0, $m_{l}$ = 0, $m_{s}$ = 0
Each electron in atom is described by a set of four numbers
1) Principal quantum number (n)
2) Angular momentum quantum number (l)
3) Magnetic quantum number ( $m_{l}$ )
4) Spin quantum number ( $m_{s}$ )
Spin quantum number refers to the two possible orientation of the spin of an electron.
The value of spin quantum number can never be a zero, because electrons always have spin either positive or negative. Hence, n = 1, l = 0, $m_{l}$ = 0, $m_{s}$ = 0, this set of quantum number 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}

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

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

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

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

n = 4, l = 2, m_{l} = - 2, m_{s} = - 1 / 2

n = 3, l = 2, m_{l} = 1, m_{s} = + 1 / 2

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

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

The correct order of their increasing energies will be:

Q. Explain giving reasons which of the following sets of quantum numbers are not possible.
(a )

n = 0

l = 0

m_{1} = 0

m_{s} = + 1 / 2

n = 1

l = 0

m_{1} = 0

m_{s} = - 1 / 2

n = 1

l = 1

m_{1} = 0

m_{s} = + 1 / 2

n = 2

l = 1

m_{1} = 0

m_{s} = - 1 / 2

n = 2

l = 3

m_{1} = - 3

m_{s} = + 1 / 2

n = 3

l = 1

m_{1} = 0

m_{s} = + 1 / 2

Explain, giving reasons, which of the following sets of quantum numbers are not possible.
a) n = 0 l = 0 ml = 0 $m, = + \frac{1}{2}$
b) n = 1 l = 0 ml = 0 $m, = - \frac{1}{2}$
c) n = 1 l = 1 ml = 0 $m, = + \frac{1}{2}$
d) n = 2 l = 1 ml = 0 $m, = - \frac{1}{2}$
e) n = 3 l = 3 ml = – 3 $m, = + \frac{1}{2}$
f) n = 3 l = 1 ml = 0 $m, = + \frac{1}{2}$

Question 18

Out of the following pairs of electrons, identify the pairs of electrons present in degenerate orbitals.

(a) (i) $n = 3, l = 2, m_{l} = - 2, m_{s} = - \frac{1}{2}$ (ii) $n = 3, l = 2, m_{l} = - 1, m_{s} = - \frac{1}{2}$

(b) (i) $n = 3, l = 1, m_{l} = 1, m_{s} = + \frac{1}{2}$ (ii) $n = 3, l = 2, m_{l} = - 1, m_{s} = + \frac{1}{2}$

(c) (i) $n = 4, l = 1, m_{l} = 1, m_{s} = + \frac{1}{2}$ (ii) $n = 3, l = 2, m_{l} = 1, m_{s} = + \frac{1}{2}$

(d) (i) $n = 3, l = 2, m_{l} = + 2, m_{s} = - \frac{1}{2}$ (ii) $n = 3, l = 2, m_{l} = + 2, m_{s} = + \frac{1}{2}$

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