Which one of the following pairs of species h | vedclass

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(A) The bond order of a diatomic species depends on the total number of electrons in the molecule or ion.Species with the same number of electrons are

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$CN^{-}$ and $NO^{+}$

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(A) The bond order of a diatomic species depends on the total number of electrons in the molecule or ion.Species with the same number of electrons are isoelectronic and generally possess the same bond order.Calculating the total number of electrons for each species:$CN^{-}$: $6 + 7 + 1 = 14$ electrons.$NO^{+}$: $7 + 8 - 1 = 14$ electrons.$CN^{+}$: $6 + 7 - 1 = 12$ electrons.$O_2^{-}$: $8 + 8 + 1 = 17$ electrons.Since $CN^{-}$ and $NO^{+}$ both have $14$ electrons,they have the same bond order (which is $3$).

Which one of the following pairs of species have the same bond order?

Similar Questions

The number of species from the following which are paramagnetic and with bond order equal to $1$ is:
$H_2, He_2^{+}, O_2^{+}, N_2^{2-}, O_2^{2-}, F_2, Ne_2^{+}, B_2$

Bond order normally gives an idea of the stability of a molecular species. All the molecules,namely $H_2$,$Li_2$,and $B_2$,have the same bond order,yet they are not equally stable. Their stability order is:

Consider the given figure showing the formation of $H^{+}_2$ ion depending on internuclear distance versus potential energy of the system.
Which is the correct statement?

Consider the following species: $CN^{+}$,$CN^{-}$,$NO$,and $CN$. Which one of these will have the highest bond order?

What is the bond order of $O_2^{2-}$?

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