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

Options

A. ` 0`
B. ` 1`
C. ` 2`
D. ` 3`

Explanation

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

### Step 1: Determine the Valence Electrons of Xenon
Xenon (Xe) is a noble gas and has 8 valence electrons.

### Step 2: Count the Valence Electrons from Fluorine and Oxygen
- Each fluorine (F) contributes 1 valence electron, and since there are 4 fluorine atoms, they contribute a total of \( 4 \times 1 = 4 \) electrons.
- Oxygen (O) contributes 6 valence electrons.

### Step 3: Calculate the Total Valence Electrons
Now, we add the valence electrons from xenon, fluorine, and oxygen:
\[ \text{Total valence electrons} = \text{Valence electrons from Xe} + \text{Valence electrons from F} + \text{Valence electrons from O} = 8 + 4 + 6 = 18 \]

### Step 4: Draw the Lewis Structure
In the Lewis structure of \( \text{XeOF}_4 \):
- Xenon is the central atom.
- It forms single bonds with the 4 fluorine atoms and one double bond with the oxygen atom.
- Each bond uses 2 electrons.

### Step 5: Calculate Electrons Used in Bonding
- 4 single bonds to fluorine: \( 4 \times 2 = 8 \) electrons.
- 1 double bond to oxygen: \( 2 \) electrons (1 bond uses 2 electrons).
- Total electrons used in bonding = \( 8 + 2 = 10 \) electrons.

### Step 6: Calculate Remaining Electrons
Now, we subtract the bonding electrons from the total valence electrons:
\[ \text{Remaining electrons} = 18 - 10 = 8 \text{ electrons} \]

### Step 7: Determine Lone Pairs
The remaining 8 electrons will be placed as lone pairs:
- Each lone pair consists of 2 electrons.
- Therefore, the number of lone pairs = \( \frac{8}{2} = 4 \) lone pairs.

### Step 8: Lone Pairs on Xenon
However, since we are specifically interested in the lone pairs on the xenon atom itself:
- After forming bonds with 4 fluorine atoms and 1 oxygen atom, xenon has 2 electrons left, which form 1 lone pair.

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

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