Which pair among the following does not have | vedclass

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(A) The bond order is calculated using the formula: $	ext{Bond order} = \frac{	ext{Number of bonding electrons} - 	ext{Number of antibonding electr

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

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(A) The bond order is calculated using the formula: $	ext{Bond order} = \frac{	ext{Number of bonding electrons} - 	ext{Number of antibonding electrons}}{2}$.$A) CN^{-}$ ($14$ electrons,bond order $= 3$) and $NO^{-}$ ($16$ electrons,bond order $= 2$). These do not have the same bond order.$B) CN^{-}$ ($14$ electrons,bond order $= 3$) and $CO$ ($14$ electrons,bond order $= 3$). These have the same bond order.$C) O_2^{2-}$ ($18$ electrons,bond order $= 1$) and $B_2$ ($10$ electrons,bond order $= 1$). These have the same bond order.$D) O_2^{+}$ ($15$ electrons,bond order $= 2.5$) and $NO^{+}$ ($14$ electrons,bond order $= 3$). These do not have the same bond order.Note: In many standard competitive exams,this question is presented such that only one pair is incorrect. Given the options,both $A$ and $D$ have different bond orders. However,$O_2^{+}$ $(2.5)$ and $NO^{+}$ $(3)$ is a classic example of unequal bond orders.

Which pair among the following does not have the same bond order?

Similar Questions

$AX$ 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).

The bond energies in $NO$,$NO^{+}$,and $NO^{-}$ follow the order:

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

$CN^-$ and $N_2$ are isoelectronic,but $N_2$ is chemically inert compared to $CN^-$. The reason is:

The species,which has the bond order same as that of $F_2$ molecule is

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