(a) Write the resonance structures of `NO_2^(Ө)` (nitrite) and `NO_3^(Ө)` (nitrate ion) in terms of :
(i) outer shell `overline e^, s` with formal charges
(ii) overlapping atomic orbitals.
( c) Compare the resonance (delocalisation) energy adn stabilities of `NO_2^(Ө)` and `NO_3^(Ө)`.
(b) (i) Write the resonance contributing and hybrid structures of (I) `N_2 O` (II) `H_2 C - N_2` (diazomethane).
(ii) Give the hybridised state of each atom in each structure.
(iii) Discuss their bond length in each resonance contributing structure and compare with those in hybrid structures.

Explanation

### Step-by-Step Solution

#### (a) Resonance Structures of `NO_2^(-)` (Nitrite Ion)

1. **Draw the Lewis Structure**:
- Nitrogen (N) is the central atom bonded to two oxygen (O) atoms.
- One oxygen is double bonded to nitrogen, and the other is single bonded.
- Assign lone pairs: The double-bonded oxygen has two lone pairs, while the single-bonded oxygen has three lone pairs and carries a negative charge.
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