The dipole moment is zero for the compound

Explanation

To determine which compound has a dipole moment of zero, we need to analyze the molecular geometry and the arrangement of polar bonds in each compound. The dipole moment is a vector quantity that depends on both the magnitude and direction of the individual bond dipoles. If the bond dipoles cancel each other out, the overall dipole moment will be zero.

### Step-by-Step Solution:

1. **Identify the Compounds**: List the compounds given in the question. For example, let's consider three compounds:
- Compound A: CH3Cl
- Compound B: CO2
- Compound C: CH4

2. **Analyze Compound A (CH3Cl)**:
- CH3Cl has a polar bond between carbon and chlorine. The dipole moment points towards chlorine.
- The CH3 group has a symmetrical arrangement, but the presence of chlorine creates an overall dipole moment.
- **Conclusion**: The dipole moment is not zero.

3. **Analyze Compound B (CO2)**:
- CO2 has a linear structure with two polar C=O bonds.
- The dipole moments of the two C=O bonds are equal in magnitude but opposite in direction, leading to cancellation.
- **Conclusion**: The dipole moment is zero.

4. **Analyze Compound C (CH4)**:
- CH4 has a tetrahedral structure with four C-H bonds.
- The C-H bonds are relatively non-polar, and the symmetrical arrangement of the bonds results in cancellation of dipole moments.
- **Conclusion**: The dipole moment is zero.

5. **Final Decision**:
- Among the analyzed compounds, CO2 and CH4 have a dipole moment of zero due to their symmetrical geometry and cancellation of bond dipoles. However, if the question specifies only one compound, CO2 is often highlighted as a classic example of a compound with zero dipole moment.

### Final Answer:
The dipole moment is zero for the compound CO2.