The structure of `XeOF_2` is:

Options

A. distorted octahedral
B. T-shaped
C. pyramidal
D. tetrahedral

Explanation

To determine the structure of `XeOF2`, we can follow these steps:

### Step 1: Determine the Valence Electrons
- **Xenon (Xe)** has 8 valence electrons.
- **Oxygen (O)** has 6 valence electrons.
- **Fluorine (F)** has 7 valence electrons, and since there are 2 fluorine atoms, we have \(2 \times 7 = 14\) valence electrons from fluorine.

Total valence electrons = \(8 (Xe) + 6 (O) + 14 (F) = 28\) valence electrons.

### Step 2: Determine the Steric Number
- The steric number is calculated by adding the number of bonded atoms and lone pairs on the central atom (Xe).
- In `XeOF2`, there are 2 fluorine atoms and 1 oxygen atom bonded to xenon, which gives us 3 bonded atoms.
- We will also consider the lone pairs on xenon.

To find the number of lone pairs:
- Each bond (2 F and 1 O) uses 2 electrons, so \(3 \text{ bonds} \times 2 = 6\) electrons are used.
- Remaining electrons = \(28 - 6 = 22\) electrons.
- Each lone pair uses 2 electrons, so \(22 \div 2 = 11\) lone pairs.

However, we need to check how many lone pairs are actually on xenon. The correct calculation is:
- For 3 bonds, we have \(3 \text{ bond pairs}\).
- The total number of electron pairs (bonding + lone pairs) = \(28 / 2 = 14\).
- Therefore, \(14 - 3 = 11\) lone pairs is incorrect. We need to adjust our understanding based on the geometry.

### Step 3: Hybridization
- The steric number is 5 (3 bond pairs + 2 lone pairs).
- The hybridization corresponding to a steric number of 5 is \(sp^3d\).

### Step 4: Determine the Geometry and Shape
- The geometry of `XeOF2` with a steric number of 5 and 2 lone pairs is trigonal bipyramidal.
- The presence of lone pairs will affect the shape. The lone pairs will occupy the equatorial positions to minimize repulsion.
- This leads to a T-shaped molecular geometry.

### Conclusion
The structure of `XeOF2` is T-shaped.