Total number of lone pair of electrons in ` XeOF_4` is :

Options

A. a.1
B. b.4
C. c.2
D. d.3

Explanation

To determine the total number of lone pairs of electrons in the molecule \( \text{XeOF}_4 \), we can follow these steps:

### Step 1: Determine the Valence Electrons
First, we need to find the total number of valence electrons in the molecule.

- Xenon (Xe) has 8 valence electrons.
- Oxygen (O) has 6 valence electrons.
- Each Fluorine (F) has 7 valence electrons, and there are 4 fluorine atoms.

Calculating the total:
\[ \text{Total valence electrons} = 8 (\text{Xe}) + 6 (\text{O}) + 4 \times 7 (\text{F}) = 8 + 6 + 28 = 42 \text{ electrons} \]

### Step 2: Determine the Molecular Geometry
Next, we need to determine the molecular geometry of \( \text{XeOF}_4 \).

- The central atom is xenon (Xe), which is bonded to one oxygen atom and four fluorine atoms.
- The molecular geometry of \( \text{XeOF}_4 \) is square pyramidal.

### Step 3: Draw the Lewis Structure
Now, we can draw the Lewis structure of \( \text{XeOF}_4 \):

1. Place xenon in the center.
2. Draw a double bond between xenon and oxygen.
3. Draw single bonds between xenon and each of the four fluorine atoms.
4. Each fluorine atom will have 3 lone pairs of electrons to complete their octet.

### Step 4: Count the Lone Pairs on Xenon
After drawing the Lewis structure, we can count the lone pairs of electrons on xenon:

- Xenon uses 6 electrons for bonding (2 for the double bond with oxygen and 4 for the single bonds with fluorine).
- This leaves \( 8 - 6 = 2 \) electrons that are not involved in bonding.

These 2 electrons are present as 1 lone pair on xenon.

### Conclusion
Thus, the total number of lone pairs of electrons in \( \text{XeOF}_4 \) is **1**.