`CF_(4), SF_(4) and XeF_(4)` contain the following electronic structure on their central atoms. Which one is correct option ?

Options

A. 1, 2 and 3 lone pairs of electrons respectively
B. 0,1 and 2 lone pairs of electrons respectively
C. 1,1 and 1 lone pairs of electrons respectively
D. No lone pairs of electrons on anly molecule

Explanation

To determine the number of lone pairs in the molecules CF₄, SF₄, and XeF₄, we need to analyze the electronic structure of the central atoms in each molecule. Let's go through each molecule step by step.

### Step 1: Analyze CF₄ (Carbon Tetrafluoride)
1. **Identify the central atom**: The central atom in CF₄ is Carbon (C).
2. **Determine the number of valence electrons**: Carbon has 4 valence electrons (group 14).
3. **Count the bonds formed**: In CF₄, Carbon forms 4 bonds with 4 Fluorine (F) atoms.
4. **Calculate lone pairs**: Since all 4 valence electrons are used to form bonds, there are no electrons left for lone pairs.
- **Lone pairs in CF₄**: 0

### Step 2: Analyze SF₄ (Sulfur Tetrafluoride)
1. **Identify the central atom**: The central atom in SF₄ is Sulfur (S).
2. **Determine the number of valence electrons**: Sulfur has 6 valence electrons (group 16).
3. **Count the bonds formed**: In SF₄, Sulfur forms 4 bonds with 4 Fluorine atoms.
4. **Calculate lone pairs**: Sulfur uses 4 of its 6 valence electrons to form bonds, leaving 2 electrons.
- These 2 remaining electrons form 1 lone pair.
- **Lone pairs in SF₄**: 1

### Step 3: Analyze XeF₄ (Xenon Tetrafluoride)
1. **Identify the central atom**: The central atom in XeF₄ is Xenon (Xe).
2. **Determine the number of valence electrons**: Xenon has 8 valence electrons (group 18).
3. **Count the bonds formed**: In XeF₄, Xenon forms 4 bonds with 4 Fluorine atoms.
4. **Calculate lone pairs**: Xenon uses 4 of its 8 valence electrons to form bonds, leaving 4 electrons.
- These 4 remaining electrons can form 2 lone pairs.
- **Lone pairs in XeF₄**: 2

### Final Summary
- CF₄ has **0 lone pairs**.
- SF₄ has **1 lone pair**.
- XeF₄ has **2 lone pairs**.

Thus, the correct option is **B: 0, 1, and 2 lone pairs of electrons respectively**.

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