Question

Among the following molecules, the one with the highest dipole moment is:

• A. \(CH_3Cl\)
• B. \(CH_3CH_2Cl\)
• C. \(CHCl_3\)
• D. \(CCl_4\)

Hint:

Dipole moments depend on electronegativity differences and the spatial orientation of the bonds. Symmetrical molecules cancel out the effects of all dipole moments of individua bonds, and as such, the molecule has no net dipole moment.

Answer 1

The Correct Option is A

Dipole moment measures the separation of positive and negative charges in a molecule. It depends on bond polarity and molecular geometry:
\(\text{CH}_3\text{Cl}\): Significant dipole moment due to one polar C-Cl bond and asymmetric geometry.
\(\text{CH}_2\text{Cl}_2\): Lower dipole moment as the two C-Cl bonds partially cancel each other.
\(\text{CHCl}_3\): Further reduced dipole moment due to three C-Cl bonds.
\(\text{CCl}_4\): No dipole moment due to perfect symmetry.
Thus, \(\text{CH}_3\text{Cl}\) has the highest dipole moment due to its single polar bond and lack of significant cancellation.