The ground state magnetic property of B_{2} a | vedclass

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Question

(A) According to molecular orbital theory, the electronic configuration for $B_{2}$ ($10$ electrons) is: $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^

Vedclass · Accepted Answer

$B_{2}$ paramagnetic and $C_{2}$ diamagnetic

Vedclass · Answer

(A) According to molecular orbital theory, the electronic configuration for $B_{2}$ ($10$ electrons) is: $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{2}, \sigma^{*} 2s^{2}, \pi 2p_{x}^{1} = \pi 2p_{y}^{1}$.Since it contains two unpaired electrons, $B_{2}$ is paramagnetic.The electronic configuration for $C_{2}$ ($12$ electrons) is: $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{2}, \sigma^{*} 2s^{2}, \pi 2p_{x}^{2} = \pi 2p_{y}^{2}$.Since all electrons are paired, $C_{2}$ is diamagnetic.

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 ground state magnetic property of $B_{2}$ and $C_{2}$ molecules will be

Similar Questions

Which of the following molecules is paramagnetic?

Calculate the bond order for $H_2^+$,$He_2^+$,and $He_2^{2+}$.

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

Identify the set containing isoelectronic species.

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