The N-O bond in `NO_(2)^(-)` is shorter than N-O bond in `NO_(3)^(-)`. Account for this observation.

Explanation

To understand why the N-O bond in \( NO_2^- \) is shorter than the N-O bond in \( NO_3^- \), we need to analyze the bonding characteristics and resonance structures of both ions.

### Step 1: Draw the Lewis Structures
- For \( NO_2^- \):
- Nitrogen (N) has 5 valence electrons, and each oxygen (O) has 6 valence electrons. The negative charge adds one extra electron.
- The total number of valence electrons is \( 5 + 2 \times 6 + 1 = 18 \).
- The Lewis structure shows one N=O double bond and one N-O single bond, with the negative charge localized on one of the oxygen atoms.

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