Which of the following species is non polar with presence of polar bond and lone pair of electron on central atom.

Options

A. `CO_(2)`
B. `SF_(4)`
C. `XeF_(4)`
D. `CF_(4)`

Answer

To determine which of the given species is non-polar while having a polar bond and a lone pair of electrons on the central atom, we can follow these steps:

### Step 1: Understand the Definitions
- **Polar Bond**: A bond between two atoms that have different electronegativities, resulting in a dipole moment.
- **Non-Polar Molecule**: A molecule that has an even distribution of charge, meaning that any dipole moments cancel each other out.
- **Lone Pair**: A pair of valence electrons that are not shared with another atom.

### Step 2: Analyze Each Option
1. **CO2 (Carbon Dioxide)**:
- Structure: Linear (O=C=O)
- Polar Bonds: Yes, due to the difference in electronegativity between carbon and oxygen.
- Lone Pairs: No lone pairs on the central atom (carbon).
- Conclusion: Non-polar, but does not meet the criteria (no lone pair). **(Incorrect option)**

2. **SF4 (Sulfur Tetrafluoride)**:
- Structure: Seesaw
- Polar Bonds: Yes, due to the difference in electronegativity between sulfur and fluorine.
- Lone Pairs: Yes, there is one lone pair on sulfur.
- Conclusion: Polar molecule because the dipoles do not cancel out. **(Incorrect option)**

3. **XeF4 (Xenon Tetrafluoride)**:
- Structure: Square planar
- Polar Bonds: Yes, due to the difference in electronegativity between xenon and fluorine.
- Lone Pairs: Yes, there are two lone pairs on xenon.
- Conclusion: Non-polar molecule because the dipoles cancel out. **(Correct option)**

4. **CF4 (Carbon Tetrafluoride)**:
- Structure: Tetrahedral
- Polar Bonds: Yes, due to the difference in electronegativity between carbon and fluorine.
- Lone Pairs: No lone pairs on carbon.
- Conclusion: Non-polar, but does not meet the criteria (no lone pair). **(Incorrect option)**

### Step 3: Final Conclusion
The only species that is non-polar while having polar bonds and lone pairs on the central atom is **XeF4**.

### Final Answer
**The correct option is XeF4.**