Molecular Geometry Analysis for V-Shape Identification

To determine which molecules possess a V-shape, we analyze their molecular geometry using VSEPR theory. The V-shape, or bent geometry, occurs when a central atom has two bonding pairs and one or more lone pairs, or two bonding pairs and no lone pairs but with specific hybridization leading to bent shape. We examine each molecule:

1. $\text{O}_{3}$ (Ozone)

• Central Atom: O
• Valence electrons: 6 e⁻ × 3 = 18 e⁻
• Steric Number (SN) on central O = 3 (2 bonding regions + 1 lone pair)
• Electron Geometry: Trigonal Planar
• Molecular Geometry: Bent (V-shape)

2. $\text{N}_{3}^{-}$ (Azide ion)

• Central Atom: Middle N
• Valence electrons: (5 e⁻ × 3) + 1 e⁻ = 16 e⁻
• Steric Number (SN) on central N = 2 (2 bonding regions + 0 lone pairs)
• Electron Geometry: Linear
• Molecular Geometry: Linear

3. $\text{CO}_{3}^{2-}$ (Carbonate ion)

• Central Atom: C
• Valence electrons: 4 e⁻ + (6 e⁻ × 3) + 2 e⁻ = 24 e⁻
• Steric Number (SN) on central C = 3 (3 bonding regions + 0 lone pairs)
• Electron Geometry: Trigonal Planar
• Molecular Geometry: Trigonal Planar

4. $\text{NO}_{2}^{-}$ (Nitrite ion)

• Central Atom: N
• Valence electrons: 5 e⁻ + (6 e⁻ × 2) + 1 e⁻ = 18 e⁻
• Steric Number (SN) on central N = 3 (2 bonding regions + 1 lone pair)
• Electron Geometry: Trigonal Planar
• Molecular Geometry: Bent (V-shape)

5. $\text{NO}_{3}^{-}$ (Nitrate ion)

• Central Atom: N
• Valence electrons: 5 e⁻ + (6 e⁻ × 3) + 1 e⁻ = 24 e⁻
• Steric Number (SN) on central N = 3 (3 bonding regions + 0 lone pairs)
• Electron Geometry: Trigonal Planar
• Molecular Geometry: Trigonal Planar

Conclusion on Molecular Shapes

The molecules identified with a V-shape (Bent molecular geometry) are:

• $\text{O}_{3}$ (A)
• $\text{NO}_{2}^{-}$ (D)

Molecules $\text{N}_{3}^{-}$, $\text{CO}_{3}^{2-}$, and $\text{NO}_{3}^{-}$ do not have a V-shape.

Final Answer Derivation

The molecules possessing a V-shape are $\text{O}_{3}$ (A) and $\text{NO}_{2}^{-}$ (D). Therefore, the correct option is the one listing A and D only.