Question

Which of the following has a non-zero dipole moment?

• A. \( \mathrm{CCl_4} \)
• B. \( \mathrm{CO_2} \)
• C. \( \mathrm{BF_3} \)
• D. None of these

Hint:

For a molecule to have a non-zero dipole moment, it must have an asymmetric distribution of electron density or molecular geometry that prevents the cancellation of bond dipoles.

Answer 1

The Correct Option is D

A molecule's dipole moment is determined by its geometry and the resultant vector of individual bond dipole moments.

Analysis:

• \( \mathrm{CCl_4} \): Exhibits a tetrahedral structure, is symmetrical, and possesses a net dipole moment of 0.
• \( \mathrm{CO_2} \): Possesses a linear and symmetrical arrangement, resulting in a net dipole moment of 0.
• \( \mathrm{BF_3} \): Features a trigonal planar geometry, is symmetrical, and has a net dipole moment of 0.

Consequently, all molecules presented have zero dipole moments.

The appropriate selection is (D) None of these.