Multiple Choice
Which of the following best describes the molecular polarity of BF_3?
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following is necessary for a molecule to be considered polar?
A
The molecule must be composed of identical atoms.
B
The molecule must have polar bonds and an asymmetric shape that prevents bond dipoles from canceling.
C
The molecule must have a symmetrical geometry so that all bond dipoles cancel.
D
The molecule must contain only nonpolar covalent bonds.
Verified step by step guidance1
Understand that molecular polarity depends on both the presence of polar bonds and the overall shape of the molecule.
Recall that a polar bond occurs when there is a difference in electronegativity between two bonded atoms, creating a bond dipole moment.
Recognize that even if a molecule has polar bonds, the molecule can be nonpolar if its shape is symmetrical, causing the bond dipoles to cancel out.
Identify that for a molecule to be polar, it must have polar bonds and an asymmetric (non-symmetrical) shape so that the bond dipoles do not cancel each other.
Conclude that the necessary condition for molecular polarity is having polar bonds combined with an asymmetric molecular geometry that prevents dipole cancellation.
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