The shape of `"XeOF"_(2)` on the basis of VSEPR theory is

Options

A. trigonal bipyramidal
B. square pyramidal
C. octahedral
D. pentagonal planar

Explanation

To determine the shape of \( \text{XeOF}_2 \) based on VSEPR theory, we will follow these steps:

### Step 1: Determine the Valence Electrons
Xenon (Xe) is in group 18 and has 8 valence electrons. Oxygen (O) is in group 16 and has 6 valence electrons. Each fluorine (F) atom is in group 17 and has 7 valence electrons.

Calculating the total valence electrons:
- Xe: 8
- O: 6
- F: 7 (for 2 F atoms, we have \( 7 \times 2 = 14 \))

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

### Step 2: Determine the Bonds and Lone Pairs
In \( \text{XeOF}_2 \):
- Xenon forms a double bond with oxygen (using 4 electrons).
- Xenon forms single bonds with two fluorine atoms (using 2 electrons for each bond, totaling 4 electrons).

Thus, the bonds consume:
- 4 electrons (double bond with O)
- 4 electrons (two single bonds with F)

Total electrons used for bonding = \( 4 + 4 = 8 \) electrons.

Remaining electrons = \( 28 - 8 = 20 \) electrons.

### Step 3: Calculate Lone Pairs on Xenon
The remaining 20 electrons will be used as lone pairs on xenon. Each lone pair consists of 2 electrons, so:
- Number of lone pairs = \( \frac{20}{2} = 10 \) lone pairs.

However, we need to consider the actual arrangement.

### Step 4: Count the Bonding Regions
- 1 double bond with oxygen = 1 bonding region
- 2 single bonds with fluorine = 2 bonding regions

Total bonding regions = \( 1 + 2 = 3 \).

### Step 5: Determine the Lone Pairs
Since we have 3 bonding regions, we can calculate the number of lone pairs:
- Total valence electrons = 8 (Xe) + 6 (O) + 14 (F) = 28
- Electrons used in bonds = 8
- Remaining electrons = 20
- Each lone pair consists of 2 electrons, so the number of lone pairs on Xe = \( \frac{20}{2} = 10 \).

### Step 6: Hybridization
The total number of regions (bonding + lone pairs) around xenon is:
- 3 bonding regions + 2 lone pairs = 5 regions.

The hybridization corresponding to 5 regions is \( sp^3d \).

### Step 7: Determine the Geometry
The geometry of \( sp^3d \) is trigonal bipyramidal. However, the presence of lone pairs affects the shape:
- The two lone pairs will occupy the equatorial positions to minimize repulsion.

### Step 8: Final Shape
With two lone pairs in the equatorial position and three bonding pairs (one double bond with oxygen and two single bonds with fluorine), the resulting molecular shape is T-shaped.

### Conclusion
The shape of \( \text{XeOF}_2 \) based on VSEPR theory is T-shaped.

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