AX is a covalent diatomic molecule where A an | vedclass

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(B) According to Molecular Orbital Theory,the bond order is calculated as $	ext{Bond Order} = \frac{N_b - N_a}{2}$.For a diatomic molecule with $15$

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$15$

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(B) According to Molecular Orbital Theory,the bond order is calculated as $	ext{Bond Order} = \frac{N_b - N_a}{2}$.For a diatomic molecule with $15$ electrons (like $NO$),the molecular orbital configuration is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1$.Number of bonding electrons $(N_b)$ = $2+2+2+2+2 = 10$.Number of antibonding electrons $(N_a)$ = $2+2+1 = 5$.$	ext{Bond Order} = \frac{10 - 5}{2} = \frac{5}{2} = 2.5$.Thus,the total number of electrons in $AX$ is $15$.

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

$AX$ is a covalent diatomic molecule where $A$ and $X$ are second row elements of the periodic table. Based on Molecular Orbital Theory,the bond order of $AX$ is $2.5$. The total number of electrons in $AX$ is ........... (Round off to the nearest integer).

Similar Questions

Which amongst the following is an incorrect statement?

According to $MO$ theory,the bond orders for $O_2^{2-}$,$CO$,and $NO^{+}$ respectively,are:

The lowest $O-O$ bond length in the following molecules is:

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

Which of the following statements are correct for the peroxide ion $(O_{2}^{2-})$?

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