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

The dipole moment of a molecule depends on molecular geometry and the vector sum of bond dipole moments.

Analysis:

• \( \mathrm{CCl_4} \): Tetrahedral, symmetric, net dipole moment = 0.
• \( \mathrm{CO_2} \): Linear, symmetric, net dipole moment = 0.
• \( \mathrm{BF_3} \): Trigonal planar, symmetric, net dipole moment = 0.

Therefore, all given molecules have zero dipole moments.

The correct answer is (D) None of these.