The number of bonding and non-bonding electro | vedclass

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(C) The nitrate ion $(NO_3^-)$ has a central nitrogen atom bonded to three oxygen atoms.In the Lewis structure of $NO_3^-$,the nitrogen atom forms one

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$4, 0$

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(C) The nitrate ion $(NO_3^-)$ has a central nitrogen atom bonded to three oxygen atoms.In the Lewis structure of $NO_3^-$,the nitrogen atom forms one double bond with one oxygen atom and two single bonds with the other two oxygen atoms.This results in a total of $4$ bonding electron pairs (one double bond counts as $2$ bonding pairs,and two single bonds count as $2$ bonding pairs).The nitrogen atom has $5$ valence electrons. In $NO_3^-$,it uses all $5$ electrons for bonding (one lone pair is donated to form a coordinate bond or shared in resonance structures,resulting in $0$ lone pairs on $N$).Thus,the number of bonding electron pairs is $4$ and non-bonding electron pairs is $0$.

List-$I$ (Molecule)	List-$II$ (Shape)
$A$. $XeF_4$	$I$. Square pyramidal
$B$. $ClF_3$	$II$. Pentagonal bipyramidal
$C$. $BrF_5$	$III$. Square planar
$D$. $IF_7$	$IV$. Bent $T$-shape

The number of bonding and non-bonding electron pairs on the $N$ atom in $NO_3^-$ are respectively ..........

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List-$I$ (Molecule) List-$II$ (Shape)

$A$. $XeF_4$ $I$. Square pyramidal

$B$. $ClF_3$ $II$. Pentagonal bipyramidal

$C$. $BrF_5$ $III$. Square planar

$D$. $IF_7$ $IV$. Bent $T$-shape

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