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Which of the following set of molecules are having zero dipole moment?

  • A.HI, \(\mathrm{CO_{2}}\) and \(\mathrm{CCl_{4}}\)
  • B.\(\mathrm{H_{2}}\), \(\mathrm{CO_{2}}\) and \(\mathrm{BF_{3}}\)
  • C.\(\mathrm{NH_{3}}\), \(\mathrm{CO_{2}}\) and \(\mathrm{CCl_{4}}\)
  • D.HI, \(\mathrm{CH_{4}}\) and \(\mathrm{CCl_{4}}\)
  • E.HI, HCl and \(\mathrm{CCl_{4}}\)

Answer: B

The set with zero dipole moment is H2, CO2 and BF3.

H2 has a non-polar bond. CO2 is linear, so its two C=O dipoles cancel. BF3 is trigonal planar, so its three B-F dipoles cancel.

Every other set contains a polar molecule: HI and HCl are polar diatomics, and NH3 is pyramidal with a net dipole. CCl4 and CH4 are non-polar, but they appear only alongside a polar molecule. A molecule can have polar bonds and still a zero dipole moment if its shape is symmetric, as CO2, BF3 and CCl4 show.

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