Which of the following compounds have the same no. of lone pairs with their central atom?
(I) `XeF_(5)^(-)` (II)`BrF_(3)` (III) `XeF_(2)` (IV)`H_(3)S^(+)` (V) Triple methylene

Options

A. (IV) and (V)
B. (I) and (III)
C. (I) and (II)
D. II, IV and V

Explanation

To determine which of the given compounds have the same number of lone pairs on their central atom, we will analyze each compound step by step.

### Step 1: Analyze `XeF5^(-)`
- **Valence Electrons of Xenon (Xe)**: Xenon has 8 valence electrons.
- **Fluorine (F)**: Each fluorine contributes 1 electron, and there are 5 fluorines.
- **Total Electrons**: 8 (from Xe) + 5 (from 5 F) + 1 (extra electron from the negative charge) = 14 electrons.
- **Bond Pairs**: 5 (from 5 F).
- **Lone Pairs**: Total pairs of electrons = 14 / 2 = 7 pairs. Since 5 are bond pairs, the remaining are lone pairs: 7 - 5 = 2 lone pairs.

### Step 2: Analyze `BrF3`
- **Valence Electrons of Bromine (Br)**: Bromine has 7 valence electrons.
- **Total Electrons**: 7 (from Br) + 3 (from 3 F) = 10 electrons.
- **Bond Pairs**: 3 (from 3 F).
- **Lone Pairs**: Total pairs of electrons = 10 / 2 = 5 pairs. Since 3 are bond pairs, the remaining are lone pairs: 5 - 3 = 2 lone pairs.

### Step 3: Analyze `XeF2`
- **Valence Electrons of Xenon (Xe)**: Xenon has 8 valence electrons.
- **Total Electrons**: 8 (from Xe) + 2 (from 2 F) = 10 electrons.
- **Bond Pairs**: 2 (from 2 F).
- **Lone Pairs**: Total pairs of electrons = 10 / 2 = 5 pairs. Since 2 are bond pairs, the remaining are lone pairs: 5 - 2 = 3 lone pairs.

### Step 4: Analyze `H3S^(+)`
- **Valence Electrons of Sulfur (S)**: Sulfur has 6 valence electrons.
- **Total Electrons**: 6 (from S) + 3 (from 3 H) - 1 (due to positive charge) = 8 electrons.
- **Bond Pairs**: 3 (from 3 H).
- **Lone Pairs**: Total pairs of electrons = 8 / 2 = 4 pairs. Since 3 are bond pairs, the remaining are lone pairs: 4 - 3 = 1 lone pair.

### Step 5: Analyze `Triple Methylene (C2H4)`
- **Valence Electrons of Carbon (C)**: Each carbon has 4 valence electrons, and there are 2 carbons.
- **Total Electrons**: 4 (from 2 C) + 4 (from 4 H) = 8 electrons.
- **Bond Pairs**: 4 (2 C-C and 4 C-H bonds).
- **Lone Pairs**: Total pairs of electrons = 8 / 2 = 4 pairs. Since 4 are bond pairs, the remaining are lone pairs: 4 - 4 = 0 lone pairs.

### Summary of Lone Pairs:
1. `XeF5^(-)`: 2 lone pairs
2. `BrF3`: 2 lone pairs
3. `XeF2`: 3 lone pairs
4. `H3S^(+)`: 1 lone pair
5. `Triple Methylene`: 0 lone pairs

### Conclusion:
The compounds that have the same number of lone pairs on their central atom are:
- `XeF5^(-)` and `BrF3` (both have 2 lone pairs).