`XeF_2` and `XeF_4` have

Options

A. Linear and Square planar structures respectively
B. Square planar and Linear structures respectively
C. Square planar structure
D. Linear structure

Answer

To determine the shapes of XeF₂ and XeF₄, we need to analyze the molecular geometry based on the number of bonding pairs and lone pairs of electrons around the central atom, xenon (Xe).

### Step 1: Determine the Valence Electrons
- **Xe (Xenon)** has 8 valence electrons.
- **F (Fluorine)** has 7 valence electrons, and there are 2 fluorine atoms in XeF₂ and 4 in XeF₄.

**For XeF₂:**
- Total valence electrons = 8 (from Xe) + 2 × 7 (from 2 F) = 22 electrons.

**For XeF₄:**
- Total valence electrons = 8 (from Xe) + 4 × 7 (from 4 F) = 36 electrons.

### Step 2: Draw the Lewis Structure
- **XeF₂:**
- Place Xe in the center and bond it to two F atoms.
- After forming 2 bonds (2 pairs of electrons), we have 18 electrons left.
- Distribute these 18 electrons as 3 lone pairs on Xe.

- **XeF₄:**
- Place Xe in the center and bond it to four F atoms.
- After forming 4 bonds (4 pairs of electrons), we have 8 electrons left.
- Distribute these 8 electrons as 2 lone pairs on Xe.

### Step 3: Determine the Steric Number
- The steric number is calculated as the number of bonded atoms plus the number of lone pairs.

**For XeF₂:**
- Steric number = 2 (bonds with F) + 3 (lone pairs) = 5.

**For XeF₄:**
- Steric number = 4 (bonds with F) + 2 (lone pairs) = 6.

### Step 4: Determine the Molecular Geometry
- **XeF₂:**
- With a steric number of 5, the molecular geometry is **linear** due to the presence of 3 lone pairs which occupy equatorial positions in a trigonal bipyramidal arrangement.

- **XeF₄:**
- With a steric number of 6, the molecular geometry is **square planar** due to the presence of 2 lone pairs which occupy axial positions in an octahedral arrangement.

### Summary of Shapes
- **XeF₂**: Linear
- **XeF₄**: Square Planar

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