"Isoelectronic molecules and ions have identical bond orders." Explain by examples.
(N/A) Isoelectronic species are those that contain the same total number of electrons. According to the Molecular Orbital Theory,if two or more diatomic molecules or ions are isoelectronic,they possess the same bond order.
Example-$1$: $F_{2}$ and $O_{2}^{2-}$ both contain $18$ electrons. Their bond order is $1$.
Example-$2$: $N_{2}$,$CO$,and $NO^{+}$ are isoelectronic,each containing $14$ electrons. They all exhibit a triple bond.
Example-$1$: $F_{2}$ and $O_{2}^{2-}$ both contain $18$ electrons. Their bond order is $1$.
Example-$2$: $N_{2}$,$CO$,and $NO^{+}$ are isoelectronic,each containing $14$ electrons. They all exhibit a triple bond.
| Molecule/ion | $N_{2}, CO, NO^{+}$ |
| Bond structure | $N \equiv N, C \equiv O, N \equiv O^{+}$ |
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