Multiple Choice
How does the polarity of two liquids affect their miscibility?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following molecules has a net dipole moment of zero?
A
SO2
B
NH3
C
CO2
D
H2O
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.
Identify the molecular geometry of each molecule: CO2 is linear, SO2 is bent, NH3 is trigonal pyramidal, and H2O is bent.
Consider the bond dipoles: CO2 has two polar C=O bonds that are equal in magnitude but oriented 180° apart, so their dipoles cancel out.
For SO2, NH3, and H2O, the molecular shapes are asymmetrical, causing their bond dipoles not to cancel, resulting in a net dipole moment.
Therefore, the molecule with a net dipole moment of zero is the one with a symmetrical linear shape and equal bond dipoles in opposite directions, which is CO2.
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