Question detail
In a molecule with polar bonds, what is the effect of a symmetrical shape on the overall dipole moment?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Bonding
Question
- A. It increases the overall dipole moment
- B. It decreases the overall dipole moment
- C. It has no effect on the dipole moment
- D. It makes the molecule non-polar
Answer
It makes the molecule non-polar
Explanation
A symmetrical shape can cause the bond dipoles to cancel each other out, resulting in a non-polar molecule despite having polar bonds. This is directly related to the learning objective regarding molecular shape and dipole cancellation.
Common mistake
Bond Dipole Cancellation
Students often incorrectly assume that if a molecule has polar bonds, it must be a polar molecule without considering its shape.
To determine if bond dipoles cancel, first identify the molecular shape. Use the VSEPR theory to predict the shape based on electron pair repulsion. If the shape is symmetrical, the dipoles may cancel out, resulting in a non-polar molecule. For example, in carbon dioxide (CO2), the linear shape leads to cancellation of dipoles, making it non-polar.
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