The `XeF_(4)` structure involves

Options

A. `sp^(3)` hybridization
B. `sp^(3)d` hybridization
C. `sp^(3)d^(2)` hybridization
D. `sp^(3)d^(3)` hybridization

Answer

To determine the structure of Xenon Tetrafluoride (XeF₄), we can follow these steps:

### Step 1: Determine the Valence Electrons
Xenon (Xe) is in group 18 of the periodic table and has 8 valence electrons. Each fluorine (F) atom contributes 1 valence electron, and since there are 4 fluorine atoms, they contribute a total of 4 electrons. Therefore, the total number of valence electrons in XeF₄ is:
\[ 8 \text{ (from Xe)} + 4 \times 1 \text{ (from 4 F)} = 12 \text{ valence electrons} \]

### Step 2: Draw the Lewis Structure
In the Lewis structure, we place the xenon atom in the center and surround it with the four fluorine atoms. Each fluorine atom forms a single bond with xenon, using 8 of the 12 valence electrons (4 bonds x 2 electrons per bond). This leaves us with 4 electrons.

### Step 3: Assign Lone Pairs
The remaining 4 electrons will be assigned as lone pairs on the xenon atom. Since xenon can accommodate more than 8 electrons due to its ability to utilize d orbitals, we can place 2 lone pairs on xenon.

### Step 4: Determine the Hybridization
To find the hybridization of xenon in XeF₄, we consider the number of bonding pairs and lone pairs:
- 4 bonding pairs (from the 4 Xe-F bonds)
- 2 lone pairs

This gives a total of 6 electron pairs around the xenon atom. The hybridization corresponding to 6 electron pairs is \( sp^3d^2 \).

### Step 5: Determine the Molecular Geometry
With 4 bonding pairs and 2 lone pairs, the molecular geometry is derived from an octahedral arrangement. The lone pairs will occupy positions that minimize repulsion, leading to a square planar shape for the molecule.

### Step 6: Final Structure
Thus, the structure of XeF₄ is square planar, with the xenon atom in the center, the four fluorine atoms at the corners of a square, and the two lone pairs positioned above and below the plane of the fluorine atoms.

### Summary
- **Valence Electrons**: 12
- **Lewis Structure**: Xe in the center with 4 F atoms
- **Lone Pairs**: 2 on Xe
- **Hybridization**: \( sp^3d^2 \)
- **Molecular Geometry**: Square planar