Lone pair and `pi`-bonds exist in

Options

A. `XeF_(2)`
B. `XeO_(3)`
C. `XeF_(6)`
D. `XeO_(4)`

Answer

To determine which of the given compounds (XeF2, XeO3, XeF6) contains both lone pairs and pi bonds, we will analyze each compound step by step.

### Step 1: Analyze XeF2
1. **Valence Electrons**: Xenon (Xe) has 8 valence electrons. Each fluorine (F) contributes 7 valence electrons. For XeF2:
- Total = 8 (Xe) + 2 × 7 (F) = 22 valence electrons.

2. **Lewis Structure**:
- Place Xe in the center and bond it to two F atoms.
- After forming two single bonds (2 electrons), we have 20 electrons left.
- Distribute the remaining electrons to complete the octets of the F atoms (2 electrons each).
- The remaining 16 electrons will be placed as lone pairs on Xe.
- Result: Xe has 3 lone pairs and 2 sigma bonds (no pi bonds).

3. **Conclusion**: XeF2 has lone pairs but no pi bonds.

### Step 2: Analyze XeO3
1. **Valence Electrons**: Xenon has 8 valence electrons and each oxygen has 6. For XeO3:
- Total = 8 (Xe) + 3 × 6 (O) = 26 valence electrons.

2. **Lewis Structure**:
- Place Xe in the center and bond it to three O atoms.
- Form double bonds with two of the O atoms (4 electrons each) and a single bond with one O atom.
- After forming bonds, distribute the remaining electrons to complete the octets of the O atoms.
- Result: Xe has 1 lone pair, 3 sigma bonds, and 2 pi bonds (from the double bonds).

3. **Conclusion**: XeO3 has both lone pairs and pi bonds.

### Step 3: Analyze XeF6
1. **Valence Electrons**: For XeF6:
- Total = 8 (Xe) + 6 × 7 (F) = 50 valence electrons.

2. **Lewis Structure**:
- Place Xe in the center and bond it to six F atoms.
- After forming six single bonds (6 electrons), we have 44 electrons left.
- Distribute the remaining electrons as lone pairs on Xe.
- Result: Xe has 1 lone pair and 6 sigma bonds (no pi bonds).

3. **Conclusion**: XeF6 has a lone pair but no pi bonds.

### Final Conclusion
- **XeF2**: Lone pairs, no pi bonds.
- **XeO3**: Lone pairs and pi bonds.
- **XeF6**: Lone pairs, no pi bonds.

Thus, the compound that contains both lone pairs and pi bonds is **XeO3**.