State whether the statement is true or false.`XeF_(2) and ICl_(2)^(–)` are iso structural.

Answer

To determine whether the statement "XeF₂ and ICl₂⁻ are isostructural" is true or false, we need to analyze the molecular structures of both compounds.

### Step 1: Determine the molecular structure of XeF₂

1. **Valence Electrons Calculation**:
- Xenon (Xe) has an atomic number of 54 and has 8 valence electrons (5s² 5p⁶).
- Each fluorine (F) atom has 7 valence electrons (2s² 2p⁵). For two fluorine atoms, the total is 14 electrons.
- Total valence electrons for XeF₂ = 8 (from Xe) + 14 (from 2 F) = 22 electrons.

2. **Lewis Structure**:
- Xenon will form two bonds with the two fluorine atoms using 2 of its valence electrons.
- This leaves 6 electrons (3 lone pairs) on xenon.
- The Lewis structure shows Xe in the center with two F atoms bonded to it and three lone pairs of electrons on Xe.

3. **Hybridization**:
- The hybridization of Xe in XeF₂ is sp³d, as there are 2 bond pairs and 3 lone pairs.

4. **Molecular Geometry**:
- The molecular shape is linear due to the arrangement of the three lone pairs that repel the bond pairs.

### Step 2: Determine the molecular structure of ICl₂⁻

1. **Valence Electrons Calculation**:
- Iodine (I) has an atomic number of 53 and has 7 valence electrons (5s² 5p⁵).
- Each chlorine (Cl) atom has 7 valence electrons. For two chlorine atoms, the total is 14 electrons.
- The negative charge on ICl₂⁻ adds 1 additional electron.
- Total valence electrons for ICl₂⁻ = 7 (from I) + 14 (from 2 Cl) + 1 (from charge) = 22 electrons.

2. **Lewis Structure**:
- Iodine will form two bonds with the two chlorine atoms using 2 of its valence electrons.
- This leaves 6 electrons (3 lone pairs) on iodine.
- The Lewis structure shows I in the center with two Cl atoms bonded to it and three lone pairs of electrons on I.

3. **Hybridization**:
- The hybridization of I in ICl₂⁻ is also sp³d, as there are 2 bond pairs and 3 lone pairs.

4. **Molecular Geometry**:
- The molecular shape is linear due to the arrangement of the three lone pairs that repel the bond pairs.

### Conclusion

Both XeF₂ and ICl₂⁻ have the same molecular geometry (linear) and hybridization (sp³d) with the same arrangement of bond pairs and lone pairs. Therefore, they are isostructural.

**Final Answer**: The statement is **True**.

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