In the following which one will have zero dipole moment ?

Options

A. `BF_(3)`
B. `C Cl_(4)`
C. `BeCl_(2)`
D. All of these

Answer

To determine which of the given compounds has a zero dipole moment, we need to analyze the molecular geometry and hybridization of each compound. Let's break down the solution step by step.

### Step 1: Identify the Compounds
The question provides four compounds. We need to analyze each one to determine their dipole moments. The compounds mentioned are:
1. BF3 (Boron Trifluoride)
2. CCl4 (Carbon Tetrachloride)
3. BeCl2 (Beryllium Dichloride)

### Step 2: Determine the Hybridization and Geometry
- **BF3**:
- Hybridization: sp²
- Geometry: Trigonal planar
- **CCl4**:
- Hybridization: sp³
- Geometry: Tetrahedral
- **BeCl2**:
- Hybridization: sp
- Geometry: Linear

### Step 3: Draw the Structures
- **BF3**: The structure has Boron at the center with three Fluorine atoms at 120° angles.

- **CCl4**: The structure has Carbon at the center with four Chlorine atoms arranged tetrahedrally.

- **BeCl2**: The structure has Beryllium at the center with two Chlorine atoms on either side, forming a linear shape.

### Step 4: Analyze the Dipole Moments
- **BF3**:
- Each B-F bond has a dipole moment directed towards Fluorine due to its higher electronegativity. However, because of the trigonal planar geometry and equal bond angles (120°), the dipole moments cancel each other out. Therefore, the net dipole moment is zero.

- **CCl4**:
- Each C-Cl bond has a dipole moment directed towards Chlorine. The tetrahedral geometry means that the dipole moments from the four bonds also cancel each other out due to symmetry. Thus, the net dipole moment is zero.

- **BeCl2**:
- Each Be-Cl bond has a dipole moment directed towards Chlorine. In the linear geometry, the two dipole moments are equal in magnitude and opposite in direction (180° apart), which results in a net dipole moment of zero.

### Conclusion
All three compounds (BF3, CCl4, and BeCl2) have a net dipole moment of zero due to their symmetrical arrangements. Therefore, the correct answer is that all of these compounds have zero dipole moments.

### Final Answer
**All of the above compounds (BF3, CCl4, BeCl2) have zero dipole moment.**

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