`CO_(2)` is isostructural with

Options

A. `SO_(2)`
B. `NO_(2)`
C. `C_(2)H_(2)`
D. `SnCl_(2)`

Answer

To determine which of the given compounds is isostructural with CO₂, we need to analyze the molecular geometry of each compound.

### Step-by-Step Solution:

1. **Identify the structure of CO₂:**
- CO₂ (carbon dioxide) has the structure O=C=O.
- The carbon atom is double bonded to two oxygen atoms.
- The molecular geometry of CO₂ is linear due to the absence of lone pairs on the central carbon atom.

2. **Analyze SO₂ (sulfur dioxide):**
- The structure of SO₂ is O=S=O with one lone pair on the sulfur atom.
- The presence of the lone pair causes the molecule to adopt a bent shape.
- Therefore, SO₂ is not isostructural with CO₂.

3. **Analyze NO₂ (nitrogen dioxide):**
- The structure of NO₂ is O=N-O with one unpaired electron (lone radical).
- The presence of the unpaired electron and the bent shape of the molecule means NO₂ is also not isostructural with CO₂.

4. **Analyze C₂H₂ (acetylene):**
- The structure of C₂H₂ is H-C≡C-H.
- The molecule has a triple bond between the two carbon atoms and is linear in shape.
- Thus, C₂H₂ is isostructural with CO₂.

5. **Analyze SnCl₂ (tin(II) chloride):**
- The structure of SnCl₂ is Cl-Sn-Cl with one lone pair on the tin atom.
- This results in a bent shape for SnCl₂.
- Therefore, SnCl₂ is not isostructural with CO₂.

### Conclusion:
From the analysis, the only compound that is isostructural with CO₂ is **C₂H₂**.