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

A molecule's dipole moment quantifies the separation of its positive and negative charges, influenced by bond polarity and molecular geometry:
\(\text{CH}_3\text{Cl}\): Possesses a substantial dipole moment due to its single polar C-Cl bond and asymmetrical structure.
\(\text{CH}_2\text{Cl}_2\): Exhibits a reduced dipole moment because its two C-Cl bonds partially counteract each other.
\(\text{CHCl}_3\): Shows a further diminished dipole moment with three C-Cl bonds.
\(\text{CCl}_4\): Has no dipole moment, attributable to its perfect molecular symmetry.
Consequently, \(\text{CH}_3\text{Cl}\) displays the highest dipole moment, a result of its singular polar bond and minimal vector cancellation.