The correct geometry and hybridisation for `XeF_(4)` are

Options

A. octahedral, `sp^(3)d^(2)`
B. trigonal bipyramidal, `sp^(3)d`
C. planar triangle, `sp^(3)d^(3)`
D. square planar, `sp^(3)d^(2)`

Explanation

To determine the correct geometry and hybridization for \( \text{XeF}_4 \), we can follow these steps:

### Step 1: Determine the Valence Electrons
Xenon (Xe) is a noble gas and has 8 valence electrons. Each fluorine (F) atom has 7 valence electrons, and since there are 4 fluorine atoms, they contribute a total of \( 4 \times 7 = 28 \) electrons. Therefore, the total number of valence electrons in \( \text{XeF}_4 \) is:
\[ 8 + 28 = 36 \text{ electrons} \]

### Step 2: Draw the Lewis Structure
In the Lewis structure of \( \text{XeF}_4 \):
- Xenon forms 4 single bonds with 4 fluorine atoms, using 4 of its 8 valence electrons.
- This leaves 4 electrons remaining, which will be placed as 2 lone pairs on the xenon atom.

The Lewis structure can be represented as:
```
F
|
F - Xe - F
|
F
```
With two lone pairs on the xenon atom.

### Step 3: Determine the Number of Electron Pairs
Now we count the number of bonding pairs and lone pairs:
- **Bonding pairs**: 4 (from the 4 Xe-F bonds)
- **Lone pairs**: 2 (on the xenon atom)

### Step 4: Calculate the Steric Number
The steric number is the sum of the number of bonding pairs and lone pairs:
\[ \text{Steric Number} = \text{Number of Bonding Pairs} + \text{Number of Lone Pairs} = 4 + 2 = 6 \]

### Step 5: Determine Hybridization
The hybridization can be determined from the steric number:
- A steric number of 6 corresponds to \( \text{sp}^3\text{d}^2 \) hybridization.

### Step 6: Determine the Geometry
With a steric number of 6 and 2 lone pairs, the molecular geometry is derived from the arrangement of the bonding pairs:
- The electron pair geometry is octahedral.
- The molecular geometry, considering the positions of the lone pairs, is square planar.

### Conclusion
Thus, the correct geometry and hybridization for \( \text{XeF}_4 \) are:
- **Geometry**: Square planar
- **Hybridization**: \( \text{sp}^3\text{d}^2 \)

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