Which of the following molecules has no dipole moment ?

Options

A. `CH_3 Cl`
B. `CH Cl_3`
C. `CH_2 Cl_2`
D. `C Cl_4`

Explanation

To determine which of the given molecules has no dipole moment, we will analyze each molecule based on its molecular geometry and the electronegativity of its constituent atoms.

### Step-by-Step Solution:

1. **Identify the Molecules**:
- A) CH3Cl (Chloromethane)
- B) CHCl3 (Chloroform)
- C) CH2Cl2 (Dichloromethane)
- D) CCl4 (Carbon Tetrachloride)

2. **Analyze CH3Cl**:
- Structure: Tetrahedral
- Bond Dipoles: The C-Cl bond is polar due to the difference in electronegativity between C and Cl.
- Resulting Dipole Moment: The dipole moments do not cancel out, resulting in a net dipole moment.
- Conclusion: **CH3Cl has a dipole moment.**

3. **Analyze CHCl3**:
- Structure: Tetrahedral
- Bond Dipoles: Similar to CH3Cl, the C-Cl bonds are polar.
- Resulting Dipole Moment: The dipole moments from the three C-Cl bonds do not cancel out, leading to a net dipole moment.
- Conclusion: **CHCl3 has a dipole moment.**

4. **Analyze CH2Cl2**:
- Structure: Tetrahedral
- Bond Dipoles: The C-Cl bonds are polar, and there are two of them.
- Resulting Dipole Moment: The dipole moments do not cancel out due to the asymmetry of the molecule, resulting in a net dipole moment.
- Conclusion: **CH2Cl2 has a dipole moment.**

5. **Analyze CCl4**:
- Structure: Tetrahedral
- Bond Dipoles: All four C-Cl bonds are polar.
- Resulting Dipole Moment: However, due to the symmetrical arrangement of the four identical C-Cl bonds, the dipole moments cancel each other out.
- Conclusion: **CCl4 has no dipole moment.**

### Final Answer:
The molecule that has no dipole moment is **D) CCl4**.