`dpi -ppi` bond is present in

Options

A. `CO_(3)^(2-)`
B. `PO_4^(3-)`
C. `NO_3^(-)`
D. `NO_2^(-)`

Explanation

To determine where a Dπ-Pπ bond is present, we need to analyze the electronic configurations of the relevant elements.

### Step-by-Step Solution:

1. **Identify the Elements**: The question involves identifying the presence of a Dπ-Pπ bond in certain molecules, specifically looking at carbon, phosphorus, and nitrogen.

2. **Electronic Configuration of Carbon**:
- Carbon has an atomic number of 6.
- Its electronic configuration is:
\[ 1s^2 \, 2s^2 \, 2p^2 \]
- Since carbon does not have any d-orbitals in its valence shell (the highest energy level is n=2), it cannot form a Dπ-Pπ bond.

3. **Electronic Configuration of Phosphorus**:
- Phosphorus has an atomic number of 15.
- Its electronic configuration is:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^3 \]
- Phosphorus has d-orbitals available in the 3rd shell (3d), allowing for the possibility of forming a Dπ-Pπ bond.

4. **Electronic Configuration of Nitrogen**:
- Nitrogen has an atomic number of 7.
- Its electronic configuration is:
\[ 1s^2 \, 2s^2 \, 2p^3 \]
- Similar to carbon, nitrogen does not have d-orbitals in its valence shell, thus it cannot form a Dπ-Pπ bond.

5. **Conclusion**:
- Since only phosphorus has the necessary d-orbitals to form a Dπ-Pπ bond, the correct answer is that the Dπ-Pπ bond is present in phosphorus.

### Final Answer:
The Dπ-Pπ bond is present in phosphorus.