Which of the following has `ppi-dpi` bonding?

Options

A. `NO_3^(-)`
B. `SO_3^(2-)`
C. `BO_3^(3-)`
D. `CO_3^(2-)`

Explanation

To determine which of the given species exhibits P-Pi-D-Pi bonding, we will analyze each option based on the presence of d orbitals and the types of bonds formed.

### Step-by-Step Solution:

1. **Identify the given species**: The species provided are:
- Nitrate ion (NO3^-)
- Sulphite ion (SO3^2-)
- Borate ion (BO3^3-)
- Carbonate ion (CO3^2-)

2. **Analyze the elements involved**:
- **Nitrate ion (NO3^-)**: Contains nitrogen (N) and oxygen (O). Both nitrogen and oxygen are in the second period of the periodic table, where d orbitals are not present. Therefore, P-Pi-D-Pi bonding is not possible here.
- **Sulphite ion (SO3^2-)**: Contains sulfur (S) and oxygen (O). Sulfur is in the third period and has vacant d orbitals. This allows for the possibility of P-Pi-D-Pi bonding with one of the oxygen atoms.
- **Borate ion (BO3^3-)**: Contains boron (B) and oxygen (O). Boron is also in the second period, and thus does not have d orbitals available for bonding. Therefore, P-Pi-D-Pi bonding is not possible here.
- **Carbonate ion (CO3^2-)**: Contains carbon (C) and oxygen (O). Carbon is in the second period, and like nitrogen and boron, it does not have d orbitals. Thus, P-Pi-D-Pi bonding is not possible here.

3. **Conclusion**: The only species that can exhibit P-Pi-D-Pi bonding is the **sulphite ion (SO3^2-)** because sulfur has vacant d orbitals that can participate in bonding with oxygen.

### Final Answer:
The species that exhibits P-Pi-D-Pi bonding is **SO3^2-** (sulphite ion).