Multiple Choice
Is the molecule BF_3 polar or nonpolar?
2
views
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which one of the following molecules has a zero dipole moment?
A
SO2
B
NH3
C
H2O
D
CO2
Verified step by step guidance1
Recall that the dipole moment of a molecule depends on both the polarity of individual bonds and the geometry of the molecule, which determines how these bond dipoles add vectorially.
Analyze the molecular geometry of each molecule: SO2 is bent, NH3 is trigonal pyramidal, H2O is bent, and CO2 is linear.
Consider the bond polarity: all these molecules have polar bonds due to differences in electronegativity between the atoms involved.
For molecules with bent or pyramidal shapes (SO2, NH3, H2O), the bond dipoles do not cancel out because they are not arranged in a straight line, resulting in a net dipole moment.
For CO2, the molecule is linear and symmetrical, so the two polar C=O bonds are equal in magnitude but opposite in direction, causing their dipole moments to cancel out and resulting in a zero net dipole moment.
Related Videos
Related Practice
Molecular Polarity practice set
Problem sets built by lead tutorsExpert video explanations