Question

Use molecular orbital theory to determine the ground state electron configuration of f2 and f2+

Answer 1

Atomic number of F = 9

Electron configuration of F:-

⁹F = 1s² 2s² 2p⁵

Incase of F2: Total electrons: 9 + 9 = 18

For F2 the ground state electron configuration would be:

F2 = (1σ)²(1σ*)²(2σ)²(2σ*)²(2pσ)²(2pπ)⁴(2pπ*)⁴

Incase of F2+: There is loss of one electron from neutral F2. Total electrons: 18-1 = 17

For F2+ the ground state electron configuration would be:

F2 = (1σ)²(1σ*)²(2σ)²(2σ*)²(2pσ)²(2pπ)⁴(2pπ*)³

Answer 2

The number of electrons in the molecule of $\rm F_2$ are 18. The number of electrons in the molecule of $\rm F_2^+$ are 17.

The Fluorine has atomic number 9. It states that it has 9 electrons in its orbitals.

In the molecule of $\rm F_2$ there are 2 F atoms, so there are total 18 electrons.

The electronic configuration for the distribution of 18 electrons according to the MOT will be:

(1σ)²(1σ*)²(2σ)²(2σ*)²(2pσ)²(2pπ)⁴(2pπ*)⁴

For the molecule of $\rm F_2^+$, there is 1 electron removed from the molecule. There will be the presence of 17 electrons in the molecule.

The ground state electronic configuration for the molecule will be:(1σ)²(1σ*)²(2σ)²(2σ*)²(2pσ)²(2pπ)⁴(2pπ*)³

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