Why do N_2,NO^+,CN^-,and CO have the same bon | vedclass

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Question

(D) To determine the bond order,we calculate the total number of valence electrons for each species:SpeciesTotal Valence Electrons$NO^+$$5 + 6 - 1 = 1

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All of the above.

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(D) To determine the bond order,we calculate the total number of valence electrons for each species:SpeciesTotal Valence Electrons$NO^+$$5 + 6 - 1 = 10$$CN^-$$4 + 5 + 1 = 10$$CO$$4 + 6 = 10$$N_2$$5 + 5 = 10$Since all these species are isoelectronic (having $10$ valence electrons),they follow the same molecular orbital configuration,resulting in a bond order of $3.0$.

Why do $N_2$,$NO^+$,$CN^-$,and $CO$ have the same bond order?

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