Which of the following is iso-structural with `CO_2` ?

Options

A. `NO_2`
B. `N_2O_4`
C. NO
D. `N_2O`

Explanation

To determine which of the following compounds is iso-structural with \( CO_2 \), we need to analyze the structure and hybridization of \( CO_2 \) and compare it with other compounds.

### Step-by-Step Solution:

1. **Identify the Structure of \( CO_2 \)**:
- Carbon dioxide (\( CO_2 \)) has a linear structure.
- The molecular geometry is linear because it has two double bonds (C=O) and no lone pairs on the central carbon atom.

2. **Determine the Hybridization of \( CO_2 \)**:
- The central carbon atom in \( CO_2 \) is sp hybridized.
- This is due to the presence of two regions of electron density (the two double bonds).

3. **Look for Compounds with Similar Structures**:
- To find an iso-structural compound, we need to look for other molecules that are also linear and have sp hybridization.
- Common candidates to consider include \( N_2O \), \( N_2O_4 \), \( H_2O \), etc.

4. **Analyze the Candidates**:
- **\( N_2O \)**: This molecule is linear and has a similar structure to \( CO_2 \).
- **\( N_2O_4 \)**: This molecule is not linear; it has a different structure (it is a dimer of \( NO_2 \)).
- **\( H_2O \)**: This molecule has a bent structure, not linear.

5. **Conclusion**:
- The compound that is iso-structural with \( CO_2 \) is \( N_2O \) because it has the same linear structure and sp hybridization.

### Final Answer:
The compound iso-structural with \( CO_2 \) is \( N_2O \).