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Select the correct set of quantum numbers (n, l, ml) for the third electron removed in the formation of a cation for iron, Fe3+.

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pstnonsonjoku

Answer:

The third electron to be removed has to be in;

n = 3

l = 2

ml = -2, -1, 0, 1, 2

Explanation:

There are four basic quantum numbers;

i) principal quantum number (n)

ii) Azimuthal, Obital or Subsidiary quantum number (l)

iii) Magnetic quantum number (ml)

iv) Spin quantum number (ms)

The electronic configuration of Fe3+ is:

1s2 2s2 2p6 3s2 3p6 3d5

The third electron to be removed has to be in;

n = 3

l = 2

ml = -2, -1, 0, 1, 2

dsdrajlin

The third electron removed in the formation of a Fe³⁺ has the quantum numbers:

  • n: 3
  • l: 2
  • ml: -2

Iron has an atomic number of 26, so it has the following electron configuration:

[tex]Fe: [Ar] 4s^{2} 3d^{6}[/tex]

To form cations, it first loses the electrons from the outermost shell (4s). The electron configuration of Fe²⁺ is:

[tex]Fe^{2+} : [Ar] 4s^{0} 3d^{6}[/tex]

Then, it will lose an electron from the highest energy level (3d) to form Fe³⁺.

[tex]Fe^{3+} : [Ar] 4s^{0} 3d^{5}[/tex]

The third electron lost from Fe to form Fe³⁺ was in 3d⁶.

  • The principal quantum number (n) coincides with the energy level: 3.
  • The azimuthal quantum number (l) corresponding to the sublevel d is 2.
  • The magnetic quantum number (ml) goes from -l to +l. Once each orbital has at least 1 electron (5 electrons), the second electron goes to the orbital with ml = -2.

The third electron removed in the formation of a Fe³⁺ has the quantum numbers:

  • n: 3
  • l: 2
  • ml: -2

Learn more: https://brainly.com/question/16746749

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