The paramagnetic nature of the oxygen molecul | vedclass

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(C) According to the Molecular Orbital Theory $(MOT)$,the electronic configuration of the oxygen molecule $(O_2)$ is: $\sigma 1s^2, \sigma^* 1s^2, \si

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Molecular orbital theory

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(C) According to the Molecular Orbital Theory $(MOT)$,the electronic configuration of the oxygen molecule $(O_2)$ is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$. Due to the presence of two unpaired electrons in the antibonding $\pi^*$ molecular orbitals,the oxygen molecule exhibits paramagnetic behavior. This phenomenon cannot be explained by the Valence Bond Theory or other classical models.

Pair of species	Identical property
$A$. $B_2 \& O_2$	$P$. Bond order $= 2.5$
$B$. $Be_2 \& H_2^{2-}$	$Q$. Paramagnetic nature
$C$. $N_2^{+} \& N_2^{-}$	$R$. Diamagnetic nature
$D$. $O_2^{+} \& O_2^{-}$	$S$. Doesn't exist

The paramagnetic nature of the oxygen molecule $(O_2)$ is best explained on the basis of:

Similar Questions

Match the following:

Pair of species Identical property

$A$. $B_2 \& O_2$ $P$. Bond order $= 2.5$

$B$. $Be_2 \& H_2^{2-}$ $Q$. Paramagnetic nature

$C$. $N_2^{+} \& N_2^{-}$ $R$. Diamagnetic nature

$D$. $O_2^{+} \& O_2^{-}$ $S$. Doesn't exist

What is $LCAO$? Explain.

The pairs of species of oxygen and their magnetic behaviour are noted below. Which of the following presents the correct description?

How many among the given species have a bond order of $0.5$?
$H_2^{+}, He_2^{+}, He_2^{-}, B_2^{+}, F_2^{-}, Be_2^{2-}$

In oxygen $(O_2)$ and carbon $(C_2)$ molecules,the bonding is:

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