To determine which molecule among the given options has the highest dipole moment, we will analyze the molecular structures and electronegativities of the atoms involved.
### Step-by-Step Solution:
1. **Identify the Molecules**: The molecules given are CH3Cl (methyl chloride), CH2Cl2 (methylene dichloride), CHCl3 (chloroform), and CCl4 (carbon tetrachloride).
2. **Understand Electronegativity**:
- The electronegativity values are as follows:
- Hydrogen (H) < Carbon (C) < Chlorine (Cl)
- This means that chlorine, being the most electronegative, will attract electrons more strongly than carbon and hydrogen.
3. **Analyze CH3Cl**:
- In CH3Cl, the dipole moments from the C-H bonds are small, while the dipole moment from the C-Cl bond is significant because Cl is much more electronegative than C.
- The net dipole moment will be directed towards Cl, but it will be less than that of CHCl3 due to the presence of three H atoms.
4. **Analyze CH2Cl2**:
- In CH2Cl2, there are two C-Cl bonds and two C-H bonds. The dipoles from the C-Cl bonds will partially cancel out due to their opposite directions.
- Thus, the resultant dipole moment will be less than that of CH3Cl.
5. **Analyze CHCl3**:
- In CHCl3, there are three C-Cl bonds and one C-H bond. The three C-Cl dipoles will add up significantly, resulting in a larger net dipole moment directed towards Cl.
- This indicates that CHCl3 has a higher dipole moment than both CH3Cl and CH2Cl2.
6. **Analyze CCl4**:
- In CCl4, the molecule is symmetrical, and although there are four C-Cl bonds, their dipoles cancel each other out completely.
- Therefore, the dipole moment of CCl4 is zero.
7. **Conclusion**:
- Based on the analysis, the order of dipole moments from highest to lowest is:
- CHCl3 > CH3Cl > CH2Cl2 > CCl4
- Thus, the molecule with the highest dipole moment is **CHCl3** (chloroform).
### Final Answer:
The molecule with the highest dipole moment is **CHCl3**.
