`XeF_2` Xenon involves the hybridisation:

Options

A. sp
B. `sp^2`
C. `sp^3d`
D. `sp^3`

Answer

To determine the hybridization of xenon in the compound \( \text{XeF}_2 \), we can follow these steps:

### Step 1: Determine the Valence Electrons of Xenon
Xenon (Xe) is a noble gas and has 8 valence electrons.

### Step 2: Count the Number of Fluorine Atoms
In \( \text{XeF}_2 \), there are 2 fluorine atoms. Each fluorine atom forms a single bond with xenon, using 1 of xenon's valence electrons.

### Step 3: Calculate the Steric Number
The steric number is calculated using the formula:
\[ \text{Steric Number} = \text{Number of Bonding Pairs} + \text{Number of Lone Pairs} \]
- **Number of Bonding Pairs**: There are 2 bonds formed with the 2 fluorine atoms.
- **Number of Lone Pairs**: After forming 2 bonds, xenon will have \( 8 - 2 = 6 \) electrons left, which can be grouped into 3 lone pairs.

Thus, the steric number is:
\[ \text{Steric Number} = 2 + 3 = 5 \]

### Step 4: Determine the Hybridization
The hybridization corresponding to a steric number of 5 is \( \text{sp}^3\text{d} \).

### Step 5: Conclusion
Therefore, the hybridization of xenon in \( \text{XeF}_2 \) is \( \text{sp}^3\text{d} \).

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