(B) The total number of electrons in $B_2$ is $5 + 5 = 10 \ e^-$. According to Molecular Orbital Theory, the electronic configuration is: $\sigma 1s^2

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two unpaired electrons in $\pi$ $MO$

(B) The total number of electrons in $B_2$ is $5 + 5 = 10 \ e^-$. According to Molecular Orbital Theory, the electronic configuration is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \pi 2p_x^1, \pi 2p_y^1$. Due to the presence of $2$ unpaired electrons in the $\pi 2p$ bonding molecular orbitals, $B_2$ exhibits paramagnetic behaviour.

Class 11 Chemistry Chemical Bonding and Molecular Structure Molecular orbital theory

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The paramagnetic behaviour of $B_2$ is due to the presence of

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A
two unpaired electrons in $\pi^*$ $MO$
B
two unpaired electrons in $\pi$ $MO$
C
two unpaired electrons in $\sigma$ $MO$
D
two unpaired electrons in $\sigma^*$ $MO$

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Chemical Bonding and Molecular Structure

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Molecular orbital theory

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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

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