Which of the following molecules has a net dipole moment? A) CCl₄ B) CO₂ C) BCl₃ D) NHF₂ E) SF₆

Question

Quizplus · Accepted Answer

In order for a molecule to have a net dipole moment, the molecule must have polar bonds and the bond dipoles cannot cancel each other out. 
A) CCl4 is a tetrahedral molecule with four polar C-Cl bonds that cancel each other out, resulting in a nonpolar molecule. 
B) CO is a linear molecule with polar C-O bonds that do not cancel each other out, but the molecule has a symmetrical geometry resulting in a nonpolar molecule. 
C) BCl3 is a trigonal planar molecule with three polar B-Cl bonds that cancel each other out, resulting in a nonpolar molecule. 
D) NHF is a trigonal pyramidal molecule with polar N-F bonds that do not cancel each other out, and the molecule has an asymmetrical geometry resulting in a net dipole moment. 
E) SF6 is an octahedral molecule with six polar S-F bonds that cancel each other out, resulting in a nonpolar molecule.

Which of the Following Molecules Has a Net Dipole Moment