Among the following molecules, `(i)XeO_(3)(ii)XeOF_(4)(iii)XeF_(6)` those having same number of lone pairs on `Xe` are:

Options

A. (i) and (ii) only
B. (i) and (iii) only
C. (ii) and (iii) only
D. (i),(ii) and (iii)

Answer

To determine which of the given molecules, \( \text{XeO}_3 \), \( \text{XeOF}_4 \), and \( \text{XeF}_6 \), have the same number of lone pairs on xenon (Xe), we will analyze each molecule step by step.

### Step 1: Analyze \( \text{XeO}_3 \)
1. **Valence Electrons**: Xenon (Xe) has 8 valence electrons. Each oxygen (O) contributes 6 valence electrons, and there are 3 oxygen atoms.
- Total valence electrons = \( 8 + (3 \times 6) = 26 \) electrons.

2. **Bonding**: In \( \text{XeO}_3 \), xenon forms 3 single bonds with oxygen atoms and one double bond with one of the oxygen atoms.
- This accounts for \( 6 + 2 = 8 \) electrons used in bonding.

3. **Remaining Electrons**:
- Total electrons = 26
- Electrons used in bonding = 8
- Remaining electrons = \( 26 - 8 = 18 \) electrons.

4. **Lone Pairs**:
- The remaining 18 electrons will be distributed as lone pairs. Since each lone pair consists of 2 electrons, we have \( 18 / 2 = 9 \) lone pairs.
- However, we only need to consider the lone pairs on xenon. After forming the bonds, xenon has 1 lone pair left.

### Step 2: Analyze \( \text{XeOF}_4 \)
1. **Valence Electrons**:
- Total valence electrons = \( 8 + 6 + (4 \times 7) = 8 + 6 + 28 = 42 \) electrons.

2. **Bonding**:
- In \( \text{XeOF}_4 \), xenon forms 4 single bonds with fluorine atoms and 1 double bond with oxygen.
- This accounts for \( 4 + 2 = 6 \) electrons used in bonding.

3. **Remaining Electrons**:
- Total electrons = 42
- Electrons used in bonding = 6
- Remaining electrons = \( 42 - 6 = 36 \) electrons.

4. **Lone Pairs**:
- The remaining 36 electrons will be distributed as lone pairs. After bonding, xenon has 1 lone pair left.

### Step 3: Analyze \( \text{XeF}_6 \)
1. **Valence Electrons**:
- Total valence electrons = \( 8 + (6 \times 7) = 8 + 42 = 50 \) electrons.

2. **Bonding**:
- In \( \text{XeF}_6 \), xenon forms 6 single bonds with fluorine atoms.
- This accounts for \( 6 \times 1 = 6 \) electrons used in bonding.

3. **Remaining Electrons**:
- Total electrons = 50
- Electrons used in bonding = 6
- Remaining electrons = \( 50 - 6 = 44 \) electrons.

4. **Lone Pairs**:
- The remaining 44 electrons will be distributed as lone pairs. After bonding, xenon has 1 lone pair left.

### Conclusion
- **Lone Pairs on Xe**:
- \( \text{XeO}_3 \): 1 lone pair
- \( \text{XeOF}_4 \): 1 lone pair
- \( \text{XeF}_6 \): 1 lone pair

Thus, all three molecules have the same number of lone pairs on xenon, which is 1.

### Final Answer
The molecules that have the same number of lone pairs on Xe are \( \text{XeO}_3 \), \( \text{XeOF}_4 \), and \( \text{XeF}_6 \).