In which of the following pairs do the molecu | vedclass

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(A) For a molecule to be isoelectronic,it must have the same number of electrons.For $CN^{-}$: Total electrons = $6 (C) + 7 (N) + 1 = 14$.For $CO$: To

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$CN^{-}$,$CO$

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(A) For a molecule to be isoelectronic,it must have the same number of electrons.For $CN^{-}$: Total electrons = $6 (C) + 7 (N) + 1 = 14$.For $CO$: Total electrons = $6 (C) + 8 (O) = 14$.Both $CN^{-}$ and $CO$ are isoelectronic with $14$ electrons.Using Molecular Orbital Theory,the bond order is calculated as: $B.O. = \frac{1}{2} [N_b - N_a] = \frac{1}{2} [10 - 4] = 3$.Thus,both molecules have a bond order of $3$ and are isoelectronic.

List-$I$ (Molecule / ion)	List-$II$ (Bond order)
$1$. $NO$	$i$. $1.5$
$2$. $CO$	$ii$. $2.0$
$3$. $O_2^{-}$	$iii$. $2.5$
$4$. $O_2$	$iv$. $3.0$

In which of the following pairs do the molecules have a bond order of $3$ and are isoelectronic?

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Match List-$I$ with List-$II$ and select the correct option:
List-$I$ (Molecule / ion) List-$II$ (Bond order)
$1$. $NO$ $i$. $1.5$
$2$. $CO$ $ii$. $2.0$
$3$. $O_2^{-}$ $iii$. $2.5$
$4$. $O_2$ $iv$. $3.0$

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