The shape of `XeO_2F_2` molecule is

Options

A. Square planar
B. See - Saw
C. Tetrahedral
D. Trigonal bipyramidal

Answer

To determine the shape of the `XeO_2F_2` molecule, we can follow these steps:

### Step 1: Determine the Valence Electrons
First, we need to calculate the total number of valence electrons in the molecule. Xenon (Xe) has 8 valence electrons, each oxygen (O) has 6, and each fluorine (F) has 7. Therefore, the total is:

- Valence electrons from Xe: 8
- Valence electrons from 2 O: 2 × 6 = 12
- Valence electrons from 2 F: 2 × 7 = 14

Total = 8 + 12 + 14 = 34 valence electrons.

### Step 2: Draw the Lewis Structure
Next, we draw the Lewis structure for `XeO_2F_2`. Xenon will be the central atom, bonded to two oxygen atoms with double bonds and two fluorine atoms with single bonds.

- Place Xe in the center.
- Connect Xe to two O atoms with double bonds.
- Connect Xe to two F atoms with single bonds.

### Step 3: Count Lone Pairs
After placing the bonds, we need to account for the remaining valence electrons. Each double bond uses 4 electrons (2 pairs), and each single bond uses 2 electrons (1 pair).

- Total electrons used in bonds:
- 2 double bonds (4 electrons each) = 8 electrons
- 2 single bonds (2 electrons each) = 4 electrons
- Total used = 8 + 4 = 12 electrons.

Remaining electrons = 34 - 12 = 22 electrons.

Since each oxygen already has 4 electrons (from the double bonds), we can place 4 lone pairs (8 electrons) on each oxygen. The remaining electrons will be placed on the xenon.

### Step 4: Determine the Geometry
Now, we can determine the molecular geometry. The central atom (Xe) has:
- 4 bonding pairs (2 double bonds and 2 single bonds)
- 1 lone pair

This gives us a total of 5 electron pairs around the xenon atom. According to VSEPR theory, 5 electron pairs result in a trigonal bipyramidal arrangement. However, the presence of a lone pair will distort this geometry.

### Step 5: Identify the Final Shape
With one lone pair, the geometry will be distorted from trigonal bipyramidal to a seesaw shape.

### Conclusion
Thus, the shape of the `XeO_2F_2` molecule is **seesaw**.