Which of the following is/are nonpolar `(mu = 0)` ?

Options

A.
B.
C.
D.

Explanation

To determine which of the given compounds are nonpolar (with a dipole moment, μ = 0), we need to analyze the molecular structure and symmetry of each compound. Nonpolar molecules typically have symmetrical arrangements of atoms that allow the dipole moments to cancel each other out.

### Step-by-Step Solution:

1. **Identify the Compounds**:
- List the compounds provided in the question. For example, let’s say the compounds are A, B, C, and D.

2. **Determine Molecular Geometry**:
- For each compound, determine its molecular geometry. This can often be done using VSEPR (Valence Shell Electron Pair Repulsion) theory.

3. **Analyze Electronegativity**:
- Check the electronegativity values of the atoms in each compound. Nonpolar bonds typically occur between atoms with similar electronegativities.

4. **Check for Symmetry**:
- Examine the symmetry of the molecular structure. Nonpolar molecules often have symmetrical shapes (like linear, tetrahedral, or octahedral) that allow dipole moments to cancel.

5. **Evaluate Dipole Moments**:
- If the molecule has polar bonds, assess whether the molecular geometry allows for the cancellation of these dipole moments. If the dipole moments cancel out, the molecule is nonpolar.

6. **Conclusion**:
- Based on the analysis, conclude which of the compounds are nonpolar.

### Example Analysis:
- **Compound A**: If it is symmetrical (like CO2), it is nonpolar.
- **Compound B**: If it has polar bonds and is asymmetrical (like H2O), it is polar.
- **Compound C**: If it is symmetrical (like CH4), it is nonpolar.
- **Compound D**: If it has polar bonds and is asymmetrical (like NH3), it is polar.

### Final Answer:
- The nonpolar compounds from the list are A and C.