Which of the following species have the same shape?

Options

A. `CO_(2)`
B. `C Cl_(4)`
C. `O_(3)`
D. `NO_(2)^(-)`

Explanation

To determine which of the given species have the same shape, we will calculate the steric number for each species and then identify their shapes based on the steric number and the presence of lone pairs.

### Step-by-Step Solution:

1. **Identify the Species**: The species we will analyze are CO2, CCl4, O3, and NO2^-.

2. **Calculate the Steric Number for CO2**:
- Central atom: Carbon (C)
- Valence electrons of C: 4
- Bonds formed: 2 double bonds with oxygen (O).
- Bond pairs: 2 (each double bond counts as one bond pair).
- Lone pairs: 0.
- Steric number = Bond pairs + Lone pairs = 2 + 0 = 2.
- Hybridization: sp.
- Shape: Linear.

3. **Calculate the Steric Number for CCl4**:
- Central atom: Carbon (C)
- Valence electrons of C: 4
- Bonds formed: 4 single bonds with chlorine (Cl).
- Bond pairs: 4.
- Lone pairs: 0.
- Steric number = 4 + 0 = 4.
- Hybridization: sp³.
- Shape: Tetrahedral.

4. **Calculate the Steric Number for O3 (Ozone)**:
- Central atom: Oxygen (O)
- Valence electrons of O: 6
- Bonds formed: 2 single bonds and 1 lone pair.
- Bond pairs: 2.
- Lone pairs: 1.
- Steric number = 2 + 1 = 3.
- Hybridization: sp².
- Shape: Angular.

5. **Calculate the Steric Number for NO2^- (Nitrite ion)**:
- Central atom: Nitrogen (N)
- Valence electrons of N: 5
- Bonds formed: 2 single bonds with oxygen and 1 lone pair.
- Bond pairs: 2.
- Lone pairs: 1.
- Steric number = 2 + 1 = 3.
- Hybridization: sp².
- Shape: Angular.

6. **Compare the Shapes**:
- CO2: Linear
- CCl4: Tetrahedral
- O3: Angular
- NO2^-: Angular

### Conclusion:
The species that have the same shape are **O3 (ozone)** and **NO2^- (nitrite ion)**, both of which are **angular**.