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(D) The electronic configuration of an oxygen molecule $(O_2)$ according to Molecular Orbital Theory is:$O_2: KK(\sigma 2s)^2 (\sigma^* 2s)^2 (\sigma

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$8$

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(D) The electronic configuration of an oxygen molecule $(O_2)$ according to Molecular Orbital Theory is:$O_2: KK(\sigma 2s)^2 (\sigma^* 2s)^2 (\sigma 2p_z)^2 (\pi 2p_x)^2 (\pi 2p_y)^2 (\pi^* 2p_x)^1 (\pi^* 2p_y)^1$Counting the total number of electrons: $2 + 2 + 2 + 2 + 2 + 1 + 1 = 16$ electrons.Since each pair consists of $2$ electrons,the total number of electron pairs is $16 / 2 = 8$.However,in the context of bonding and lone pairs in the Lewis structure: Each $O$ atom has $6$ valence electrons. Total valence electrons = $12$. In the $O=O$ structure,there are $2$ bonding pairs and $4$ lone pairs,totaling $6$ pairs. Given the standard molecular orbital interpretation for total electron pairs (including core electrons): Total electrons = $16$,so total pairs = $8$.

$1$. Burning candle	$i$. Line spectrum
$2$. Sodium vapour	$ii$. Continuous spectrum
$3$. Bunsen flame	$iii$. Band spectrum
$4$. Dark lines in solar spectrum	$iv$. Absorption spectrum

What is the total number of electron pairs in an oxygen molecule $(O_2)$?

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