Correct statement regarding molecules `SF_(4),CF_(4) and XeF_(4)` are :

Options

A. `2,0` and `1` lone pairs of central atom respectively
B. `1,0` and `1` lone pairs of central atom respectively
C. `0,0` and `2` lone pairs of central atom respectively
D. `1,0` and `2` lone pairs of central atom respectively

Answer

To determine the correct statement regarding the number of lone pairs on the central atom for the molecules SF4, CF4, and XeF4, we will analyze each molecule step by step.

### Step 1: Analyze SF4 (Sulfur Tetrafluoride)
1. **Identify the central atom**: Sulfur (S).
2. **Determine the valence electrons**: Sulfur has 6 valence electrons (atomic number 16).
3. **Bonding with Fluorine**: Each Fluorine (F) has 7 valence electrons. In SF4, sulfur forms 4 bonds with 4 fluorine atoms.
4. **Calculate remaining electrons**:
- Total valence electrons from sulfur = 6
- Total valence electrons from 4 fluorine = 4 × 7 = 28
- Total valence electrons = 6 + 28 = 34
5. **Bonds formed**: 4 bonds use 4 of sulfur's electrons.
6. **Determine lone pairs**: Sulfur has 6 - 4 = 2 electrons left, which form 1 lone pair (2 electrons).

### Step 2: Analyze CF4 (Carbon Tetrafluoride)
1. **Identify the central atom**: Carbon (C).
2. **Determine the valence electrons**: Carbon has 4 valence electrons (atomic number 6).
3. **Bonding with Fluorine**: Carbon forms 4 bonds with 4 fluorine atoms.
4. **Calculate remaining electrons**:
- Total valence electrons from carbon = 4
- Total valence electrons from 4 fluorine = 4 × 7 = 28
- Total valence electrons = 4 + 28 = 32
5. **Bonds formed**: 4 bonds use all of carbon's electrons.
6. **Determine lone pairs**: Carbon has 0 electrons left, which means it has 0 lone pairs.

### Step 3: Analyze XeF4 (Xenon Tetrafluoride)
1. **Identify the central atom**: Xenon (Xe).
2. **Determine the valence electrons**: Xenon has 8 valence electrons (atomic number 54).
3. **Bonding with Fluorine**: Xenon forms 4 bonds with 4 fluorine atoms.
4. **Calculate remaining electrons**:
- Total valence electrons from xenon = 8
- Total valence electrons from 4 fluorine = 4 × 7 = 28
- Total valence electrons = 8 + 28 = 36
5. **Bonds formed**: 4 bonds use 4 of xenon's electrons.
6. **Determine lone pairs**: Xenon has 8 - 4 = 4 electrons left, which form 2 lone pairs (4 electrons).

### Summary of Lone Pairs
- **SF4**: 1 lone pair
- **CF4**: 0 lone pairs
- **XeF4**: 2 lone pairs

### Conclusion
The correct sequence of lone pairs for SF4, CF4, and XeF4 is 1, 0, and 2, respectively. Therefore, the correct option is D.