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Question

(C) The molecular orbital configuration of the $O_2$ molecule ($16$ electrons) is:$[\sigma (1s)^2, \sigma^*(1s)^2, \sigma (2s)^2, \sigma^*(2s)^2, \sig

Vedclass · Accepted Answer

$14$

Vedclass · Answer

(C) The molecular orbital configuration of the $O_2$ molecule ($16$ electrons) is:$[\sigma (1s)^2, \sigma^*(1s)^2, \sigma (2s)^2, \sigma^*(2s)^2, \sigma (2p_z)^2, \pi (2p_x)^2, \pi (2p_y)^2, \pi^*(2p_x)^1, \pi^*(2p_y)^1]$Counting the electrons in the filled orbitals:- $\sigma (1s)^2$: $2$ electrons ($1$ pair)- $\sigma^*(1s)^2$: $2$ electrons ($1$ pair)- $\sigma (2s)^2$: $2$ electrons ($1$ pair)- $\sigma^*(2s)^2$: $2$ electrons ($1$ pair)- $\sigma (2p_z)^2$: $2$ electrons ($1$ pair)- $\pi (2p_x)^2$: $2$ electrons ($1$ pair)- $\pi (2p_y)^2$: $2$ electrons ($1$ pair)Total number of pairs = $7$.Total number of paired electrons = $7 	imes 2 = 14$.

The number of electrons that are paired in an oxygen molecule $(O_2)$ is:

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