The species which has pyramidal shape is

Options

A. `PCI_(3)`
B. `SO_(3)`
C. `CO_(3)^(2-)`
D. `NO_(3)^(Θ)`

Explanation

To determine which species has a pyramidal shape, we will analyze the given options: PCl3, SO3, CO3^2-, and NO3^-. We will use the concept of hybridization and the presence of bond pairs and lone pairs of electrons.

### Step-by-Step Solution:

1. **Understanding Pyramidal Shape**:
- A pyramidal shape typically corresponds to a molecule that has sp³ hybridization, which consists of three bond pairs and one lone pair of electrons.

2. **Analyzing PCl3**:
- **Valence Electrons**: Phosphorus (P) has 5 valence electrons. Chlorine (Cl) has 7 valence electrons, and there are 3 Cl atoms.
- **Hybridization Calculation**:
\[ \text{Hybridization} = \frac{1}{2} \left( \text{Valence electrons of P} + \text{Number of monovalent atoms} - \text{Cationic charge} + \text{Anionic charge} \right) \]
\[ = \frac{1}{2} \left( 5 + 3 - 0 + 0 \right) = \frac{8}{2} = 4 \]
- **Hybridization Type**: Since the hybridization is 4, it corresponds to sp³.
- **Bond Pairs and Lone Pairs**: Phosphorus forms 3 bonds with Cl and has 1 lone pair. Therefore, PCl3 has a pyramidal shape.

3. **Analyzing SO3**:
- **Valence Electrons**: Sulfur (S) has 6 valence electrons, and there are 3 oxygen (O) atoms.
- **Hybridization Calculation**:
\[ = \frac{1}{2} \left( 6 + 0 - 0 + 0 \right) = \frac{6}{2} = 3 \]
- **Hybridization Type**: This corresponds to sp² hybridization.
- **Shape**: SO3 has a trigonal planar shape.

4. **Analyzing CO3^2-**:
- **Valence Electrons**: Carbon (C) has 4 valence electrons, and there are 3 oxygen atoms.
- **Hybridization Calculation**:
\[ = \frac{1}{2} \left( 4 + 0 - 0 - 2 \right) = \frac{2}{2} = 1 \]
- **Hybridization Type**: This corresponds to sp² hybridization.
- **Shape**: CO3^2- also has a trigonal planar shape.

5. **Analyzing NO3^-**:
- **Valence Electrons**: Nitrogen (N) has 5 valence electrons, and there are 3 oxygen atoms.
- **Hybridization Calculation**:
\[ = \frac{1}{2} \left( 5 + 0 - 0 + 1 \right) = \frac{6}{2} = 3 \]
- **Hybridization Type**: This corresponds to sp² hybridization.
- **Shape**: NO3^- also has a trigonal planar shape.

6. **Conclusion**:
- Among the given species, only PCl3 has a pyramidal shape due to its sp³ hybridization, which includes 3 bond pairs and 1 lone pair.

### Final Answer:
The species which has a pyramidal shape is **PCl3**.