Which of the following set of quantum numbers (ordered n, ℓ, mℓ, ms) are possible for an electron in an atom? check all that apply. view available hint(s) hint 1. how to approach the problem hint 2. identify issues with an example set of quantum numbers opened hint check all that apply. 4, 2, 3, -1/2 2, 1, 0, 1 3, 1, 0, -1/2 4, 3, -2, 1/2 -3, 2, 2, -1/2 4, 2, -1, -1/2 2, 2, 2, 1/2 3, 2, -3, 1/2

a. no   b. no   c. yes (3d₀² electron)   d. yes (4f₋₂¹ electron)   e. no   f. yes (4d₋₁² electron)   g. no   h. no

Explanation:

n = principle quantum number = energy level or ring e⁻ is in

l = shape of e⁻ orbital => s = 0, p = 1, d = 2, f = 3

m = orientation of orbital

-3    -2  -1    0   1  2  3

                  s

           p₋₁  p₀  p₁

      d₋₂ d₋₁ d₀ d₁ d₂

 f₋₃  f₋₂  f₋₁  f₀  f₁  f₂  f₃

mₙ +1/2 (1st e⁻ added), -1/2(2nd e⁻ added)

The possible combination of quantum numbers are;

1) 4, 2, 3, -1/2

2) 3, 1, 0, -1/2

3) 4, 3, -2, 1/2

4) 4, 2, -1, -1/2

5) 3, 2, -3, 1/2

In chemistry, four sets of quantum numbers describe an electron. These are;

The principal quantum number shows the energy level in which the electron is found. The azimuthal quantum number shows the energy sub-level where the electron is found. The magnetic quantum number shows the orientation of the orbital in which the electron is found while the spin quantum number shows the direction in which the electron spins.

The principal quantum number must take positive integer values from 1 to infinity. The maximum value of the azimuthal quantum number for a given value of n is n-1. The values of the magnetic quantum number for a given  l ranges from -l to +l. The spin quantum  number can only take values of ± 1/2.

Considering all these, the arrangement of quantum numbers(ordered n, ℓ, mℓ, ms);

1) 4, 2, 3, -1/2

2) 3, 1, 0, -1/2

3) 4, 3, -2, 1/2

4) 4, 2, -1, -1/2

5) 3, 2, -3, 1/2

are possible.

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