Multiple Choice
Which of the following statements about nonpolar molecules is true?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following molecules will have a net dipole moment?
A
O_2
B
CO
C
CCl_4
D
BF_3
Verified step by step guidance1
Step 1: Understand that a molecule's net dipole moment depends on both the polarity of its individual bonds and the molecular geometry, which determines if bond dipoles cancel out or add up.
Step 2: Analyze O_2: It is a diatomic molecule consisting of two identical oxygen atoms, so the bond is nonpolar, resulting in no net dipole moment.
Step 3: Analyze CO: It is a diatomic molecule with different atoms (carbon and oxygen), creating a polar bond due to the difference in electronegativity, so it has a net dipole moment.
Step 4: Analyze CCl_4: It has four polar C–Cl bonds arranged symmetrically in a tetrahedral shape, causing the bond dipoles to cancel out, resulting in no net dipole moment.
Step 5: Analyze BF_3: It has three polar B–F bonds arranged symmetrically in a trigonal planar shape, causing the bond dipoles to cancel out, resulting in no net dipole moment.
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