Multiple Choice
Which of the following statements correctly describes the molecular polarity of PF3 and PCl3?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following molecules has no net dipole moment?
A
H2O
B
SO2
C
CO2
D
NH3
Verified step by step guidance1
Recall that a molecule's net dipole moment depends on both the polarity of its individual bonds and the geometry (shape) of the molecule.
Analyze the molecular geometry of each molecule: H2O is bent, SO2 is bent, CO2 is linear, and NH3 is trigonal pyramidal.
Consider the bond polarities: all these molecules have polar bonds due to differences in electronegativity between atoms.
For CO2, the molecule is linear and symmetrical, so the bond dipoles are equal in magnitude but opposite in direction, canceling each other out, resulting in no net dipole moment.
For the other molecules (H2O, SO2, NH3), their bent or pyramidal shapes cause the bond dipoles to not cancel, so they have a net dipole moment.
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