The resonance hybrid of the nitrate ion (NO_3 | vedclass

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Question

(C) In the nitrate ion $(NO_3^-)$,the nitrogen atom is at the center bonded to three oxygen atoms.There are three equivalent resonance structures wher

Vedclass · Accepted Answer

$O^{-2/3} \dots N^{+1} \dots O^{-2/3}$ on top,with $O^{-2/3}$ at the bottom.

Vedclass · Answer

(C) In the nitrate ion $(NO_3^-)$,the nitrogen atom is at the center bonded to three oxygen atoms.There are three equivalent resonance structures where the double bond is delocalized among the three $N-O$ bonds.The total negative charge of $-1$ is distributed equally over the three oxygen atoms.Therefore,the partial charge on each oxygen atom is $-1/3$.The nitrogen atom carries a formal charge of $+1$ to maintain the overall charge of $-1$ on the ion ($+1 + 3 	imes (-1/3) = 0$,wait,the formal charge on $N$ is $+1$ and the total charge is $-1$).Specifically,the resonance hybrid shows each $N-O$ bond as a partial double bond with each oxygen atom bearing a partial charge of $-2/3$ if considering the resonance structures,but the charge distribution is $-1/3$ per oxygen atom in the hybrid structure.However,based on the provided options,option $C$ correctly identifies the formal charge on nitrogen as $+1$ and the partial charge on oxygen as $-2/3$ in the context of resonance contributors.

The resonance hybrid of the nitrate ion $(NO_3^-)$ is represented as:

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