`C_(2)H_(2)` is isostructural with :

Options

A. `H_(2)O_(2)`
B. `NO_(2)`
C. `SnCl_(2)`
D. `CO_(2)`

Answer

To determine which molecule is isostructural with \( C_2H_2 \) (ethyne), we need to analyze the structure and hybridization of \( C_2H_2 \) first.

### Step 1: Identify the Structure of \( C_2H_2 \)

1. **Valence Electrons**: Each carbon atom has 4 valence electrons. Since there are 2 carbon atoms, they contribute a total of \( 4 \times 2 = 8 \) valence electrons. Each hydrogen atom has 1 valence electron, and with 2 hydrogen atoms, they contribute \( 1 \times 2 = 2 \) valence electrons. Thus, the total number of valence electrons in \( C_2H_2 \) is \( 8 + 2 = 10 \).

2. **Bond Formation**: The two carbon atoms form a triple bond with each other, using 6 electrons (3 pairs), and each carbon atom forms a single bond with one hydrogen atom, using 2 electrons (1 pair).

3. **Hybridization**: The carbon atoms in \( C_2H_2 \) undergo \( sp \) hybridization because they are involved in a triple bond (1 sigma and 2 pi bonds) and have no lone pairs. The geometry of the molecule is linear due to the \( sp \) hybridization.

### Step 2: Identify Possible Isostructural Molecules

Now that we know \( C_2H_2 \) is linear and has \( sp \) hybridization, we need to find other molecules that share these characteristics.

1. **Check the Given Options**: We need to analyze the structure and hybridization of the given options (not specified in the question, but let’s assume common candidates).

2. **Example Candidate - \( CO_2 \)**:
- **Valence Electrons**: Carbon has 4 and each oxygen has 6, so \( 4 + 6 \times 2 = 16 \) valence electrons.
- **Bond Formation**: Carbon forms double bonds with both oxygen atoms.
- **Hybridization**: The carbon atom is \( sp \) hybridized, and the molecule is linear.

3. **Conclusion**: Since \( CO_2 \) is linear and has \( sp \) hybridization, it is isostructural with \( C_2H_2 \).

### Final Answer:
\( C_2H_2 \) is isostructural with \( CO_2 \).

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