Total number of lone pair of electrons is `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 can follow these steps:

### Step 1: Identify the central atom
The central atom in \( \text{XeOF}_4 \) is xenon (Xe).

**Hint:** Remember that in compounds, the central atom is usually the least electronegative element.

### Step 2: Determine the valence electrons of xenon
Xenon is a noble gas and has 8 valence electrons.

**Hint:** Check the periodic table to find the group number and corresponding valence electrons for noble gases.

### Step 3: Count the valence electrons contributed by other atoms
In \( \text{XeOF}_4 \):
- Oxygen (O) contributes 6 valence electrons.
- Each fluorine (F) contributes 7 valence electrons, and there are 4 fluorine atoms, so \( 4 \times 7 = 28 \) valence electrons from fluorine.

**Hint:** Remember to multiply the number of atoms by their respective valence electrons.

### Step 4: Calculate the total number of valence electrons
Total valence electrons = Valence electrons from Xe + Valence electrons from O + Valence electrons from F
\[ = 8 + 6 + 28 = 42 \text{ valence electrons} \]

**Hint:** Make sure to add all contributions correctly.

### Step 5: Determine the number of bonding pairs and lone pairs
In \( \text{XeOF}_4 \):
- Xenon forms 4 single bonds with the 4 fluorine atoms.
- Xenon forms a double bond with the oxygen atom.

This accounts for:
- 4 bonds to fluorine (4 pairs of electrons).
- 1 double bond to oxygen (2 pairs of electrons).

Total bonding pairs = 4 (from F) + 2 (from O) = 6 pairs of electrons.

**Hint:** Remember that each bond consists of 2 electrons.

### Step 6: Calculate the number of lone pairs
The total number of electron pairs (bonding + lone pairs) is calculated as follows:
\[ \text{Total pairs} = \frac{\text{Total valence electrons}}{2} = \frac{42}{2} = 21 \text{ pairs} \]
Since we have 6 bonding pairs, the number of lone pairs is:
\[ \text{Lone pairs} = \text{Total pairs} - \text{Bonding pairs} = 21 - 6 = 15 \text{ lone pairs} \]

**Hint:** Always subtract the number of bonding pairs from the total pairs to find lone pairs.

### Final Answer
The total number of lone pairs of electrons in \( \text{XeOF}_4 \) is **15**.