Use molecular orbital theory to determine whether f22+ is paramagnetic or diamagnetic.

Answers

Answer 1

Answer:

We have to know whether F₂²⁺ is paramagnetic or diamagnetic.

F₂²⁺ is paramagnetic.

If number of unpaired electron in any species is equal to zero, the species is diamagnetic and the species contains unpaired electrons, then the species is paramagnetic.

The magnetic property can be explained using molecular orbital theory.

Total number of electron present in F₂²⁺ is equal to 16 (i.e, 9+9-2). From the molecular orbital electronic configuration, number of electrons present in pi orbitals present is equal to 2.

So, F₂²⁺ is paramagnetic.

Answer 2

Answer:

Answer : $F_2^(2+)$ is paramagnetic.

Explanation :

According to the molecular orbital theory, the general molecular orbital configuration will be,

$(\sigma_(1s)),(\sigma_(1s)^*),(\sigma_(2s)),(\sigma_(2s)^*),[(\pi_(2p_x))=(\pi_(2p_y))],(\sigma_(2p_z)),[(\pi_(2p_x)^*)=(\pi_(2p_y)^*)],(\sigma_(2p_z)^*)$

As there are 9 electrons present in fluorine.

The number of electrons present in $F_2^(2+)$ molecule = 2(9) - 2 = 16

The molecular orbital configuration of $F_2^(2+)$ molecule will be,

$(\sigma_(1s))^2,(\sigma_(1s)^*)^2,(\sigma_(2s))^2,(\sigma_(2s)^*)^2,(\sigma_(2p_z))^2,[(\pi_(2p_x))^2=(\pi_(2p_y))^2],[(\pi_(2p_x)^*)^1=(\pi_(2p_y)^*)^1],(\sigma_(2p_z)^*)^0$

Paramagnetic compounds : They have unpaired electrons.

Diamagnetic compounds : They have no unpaired electrons that means all are paired.

The number of unpaired electron in molecule is, 2. So, this is paramagnetic. That means, more the number of unpaired electrons, more paramagnetic.

Thus, is paramagnetic.

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Answers

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Answers

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Answers

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Answers

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Answers

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Answers

Answer:

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