In which of the following the central atom use `sp^(2)` hybrid orbitals in its bonding

Options

A. `CH_(4)`
B. `CO_(2)`
C. `BF_(3)`
D. `BeF_(2)`

Explanation

To determine which of the given molecules has a central atom that uses `sp²` hybrid orbitals in its bonding, we will analyze each molecule step by step.

### Step 1: Analyze CH₄ (Methane)
- **Structure**: The central atom is Carbon (C).
- **Bonds**: Carbon forms four single bonds with four Hydrogen atoms.
- **Hybridization**: Since Carbon has four bonds, it uses `sp³` hybridization.

### Step 2: Analyze CO₂ (Carbon Dioxide)
- **Structure**: The central atom is Carbon (C).
- **Bonds**: Carbon forms two double bonds with two Oxygen atoms.
- **Hybridization**: Since Carbon forms two sigma bonds (and two pi bonds), it uses `sp` hybridization.

### Step 3: Analyze BF₃ (Boron Trifluoride)
- **Structure**: The central atom is Boron (B).
- **Bonds**: Boron forms three single bonds with three Fluorine atoms.
- **Hybridization**: Since Boron forms three sigma bonds, it uses `sp²` hybridization. This molecule is planar.

### Step 4: Analyze BeF₂ (Beryllium Fluoride)
- **Structure**: The central atom is Beryllium (Be).
- **Bonds**: Beryllium forms two single bonds with two Fluorine atoms.
- **Hybridization**: Since Beryllium forms two sigma bonds, it uses `sp` hybridization. This molecule is linear.

### Conclusion
After analyzing all the molecules, we find that the only molecule where the central atom uses `sp²` hybrid orbitals is **BF₃ (Boron Trifluoride)**.

### Final Answer
The central atom uses `sp²` hybrid orbitals in **BF₃**.

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