Multiple Choice
How many of the following molecules are polar: BrF_3, CS_2, SF_4, SO_3?
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following molecules has a net dipole moment?
A
PCl_5
B
SF_6
C
NH_4^+
D
H_2S
Verified step by step guidance1
Understand that a molecule's net dipole moment depends on both the polarity of its individual bonds and the molecular geometry, which determines if these bond dipoles cancel out or add up.
Analyze PCl_5: It has a trigonal bipyramidal shape with symmetrical bond arrangement, so the bond dipoles cancel out, resulting in no net dipole moment.
Analyze SF_6: It has an octahedral geometry, which is highly symmetrical, causing all bond dipoles to cancel and resulting in no net dipole moment.
Analyze NH_4^+: It has a tetrahedral shape with identical N-H bonds symmetrically arranged, so the dipoles cancel out, giving no net dipole moment.
Consider H_2S: It has a bent molecular geometry due to lone pairs on sulfur, causing the bond dipoles not to cancel, which results in a net dipole moment.
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