In which of the following the central atom has
two lone pairs of electrons ?

Options

A. `SF_(4)`
B. `BrF_(5)`
C. `SO_(2)`
D. `XeF_(4)`

Explanation

To determine which of the given compounds has a central atom with two lone pairs of electrons, we will analyze each option step by step.

### Step 1: Analyze SF4 (Sulfur Tetrafluoride)
- Sulfur (S) has 6 valence electrons.
- In SF4, sulfur forms 4 bonds with fluorine atoms, using 4 of its valence electrons.
- This leaves 2 electrons, which form 1 lone pair.
- **Conclusion**: SF4 has 1 lone pair of electrons on the central atom (sulfur).

### Step 2: Analyze BRF5 (Bromine Pentafluoride)
- Bromine (Br) has 7 valence electrons.
- In BRF5, bromine forms 5 bonds with fluorine atoms, using all 5 of its valence electrons.
- This leaves 2 electrons, which form 1 lone pair.
- **Conclusion**: BRF5 has 1 lone pair of electrons on the central atom (bromine).

### Step 3: Analyze SO2 (Sulfur Dioxide)
- Sulfur (S) has 6 valence electrons.
- In SO2, sulfur forms 2 double bonds with oxygen atoms, using 4 electrons.
- This leaves 2 electrons, which form 1 lone pair.
- **Conclusion**: SO2 has 1 lone pair of electrons on the central atom (sulfur).

### Step 4: Analyze XCF4 (Xenon Tetrafluoride)
- Xenon (Xe) has 8 valence electrons.
- In XCF4, xenon forms 4 bonds with fluorine atoms, using 4 of its valence electrons.
- This leaves 4 electrons, which can be arranged as 2 lone pairs.
- **Conclusion**: XCF4 has 2 lone pairs of electrons on the central atom (xenon).

### Final Answer:
The compound in which the central atom has two lone pairs of electrons is **XCF4**.

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