`BeCl_(2)` is not isostructural with

Options

A. `IC l_(2)^(-)`
B. `C_(2)H_(2)`
C. `XeF_(2)`
D. `GeCl_(2)`

Explanation

To determine which compound is not isostructural with BeCl₂ (beryllium chloride), we need to analyze the structures of the given compounds and compare them with that of BeCl₂.

### Step 1: Understand the Structure of BeCl₂
- BeCl₂ has a linear structure due to sp hybridization.
- Beryllium (Be) has 4 electrons (1s² 2s²), and it uses its 2 valence electrons to form bonds with 2 chlorine (Cl) atoms.
- Each Cl atom shares one electron with Be, forming 2 sigma bonds, leading to a linear geometry.

### Step 2: Analyze the Given Compounds
1. **ICl₂⁻ (Iodine dichloride anion)**:
- Iodine has 7 valence electrons, and with 2 Cl atoms and a negative charge, the hybridization is calculated as follows:
\[ \text{Hybridization} = \frac{(7 + 2 + 1)}{2} = 5 \quad \text{(sp³d hybridization)} \]
- However, since we ignore lone pairs for determining the shape, ICl₂⁻ has a linear shape.

2. **C₂S₂ (Dicyclopropyl sulfide)**:
- The structure is similar to C≡C, which means it has sp hybridization for each carbon atom.
- The compound is linear.

3. **XeF₂ (Xenon difluoride)**:
- Xenon has 8 valence electrons, and with 2 fluorine atoms, the hybridization is:
\[ \text{Hybridization} = \frac{(8 + 2)}{2} = 5 \quad \text{(sp³d hybridization)} \]
- Ignoring lone pairs, XeF₂ also has a linear structure.

4. **GeCl₂ (Germanium dichloride)**:
- Germanium has 4 valence electrons and forms bonds with 2 Cl atoms.
- This results in 2 bonds and 1 lone pair, leading to a bent or V-shaped structure, not linear.

### Step 3: Conclusion
- Among the compounds analyzed, **GeCl₂** is not isostructural with BeCl₂ because it has a bent shape due to the presence of a lone pair, while BeCl₂ is linear.

### Final Answer
BeCl₂ is not isostructural with **GeCl₂**.

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