`XeF_2` molecule is :

Options

A. Trigonal planar
B. Square planar
C. Linear
D. Pyramidal

Answer

To determine the shape of the `XeF2` molecule, we can follow these steps:

### Step 1: Determine the Valence Electrons
- Xenon (Xe) is in group 18 and has 8 valence electrons.
- Each fluorine (F) atom is in group 17 and has 7 valence electrons. Since there are 2 fluorine atoms, they contribute a total of \(2 \times 7 = 14\) valence electrons.
- Therefore, the total number of valence electrons in `XeF2` is:
\[ 8 \, (\text{from Xe}) + 14 \, (\text{from 2 F}) = 22 \, \text{valence electrons} \]

### Step 2: Draw the Lewis Structure
- Place Xenon (Xe) in the center and bond it to the two fluorine (F) atoms.
- Each bond between Xe and F uses 2 electrons, so 4 electrons are used for the two bonds.
- This leaves us with:
\[ 22 - 4 = 18 \, \text{electrons remaining} \]
- Distribute the remaining electrons to satisfy the octet rule for the fluorine atoms. Each F atom will have 6 electrons (3 lone pairs) to complete its octet.
- After placing 12 electrons around the two fluorine atoms, we have:
\[ 18 - 12 = 6 \, \text{electrons remaining} \]
- Place the remaining 6 electrons as 3 lone pairs on the Xenon atom.

### Step 3: Calculate the Steric Number
- The steric number is calculated by adding the number of bonded atoms and lone pairs around the central atom (Xe).
- In `XeF2`, there are 2 bonded fluorine atoms and 3 lone pairs:
\[ \text{Steric Number} = 2 \, (\text{bonds}) + 3 \, (\text{lone pairs}) = 5 \]

### Step 4: Determine the Hybridization
- A steric number of 5 corresponds to `sp^3d` hybridization.

### Step 5: Determine the Molecular Geometry
- The basic geometry for `sp^3d` hybridization is trigonal bipyramidal.
- However, since there are 3 lone pairs, they will occupy the equatorial positions to minimize repulsion, leaving the two bonded fluorine atoms in the axial positions.
- This arrangement results in a linear shape for the `XeF2` molecule.

### Conclusion
The shape of the `XeF2` molecule is linear.

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