Question detail
How does the presence of lone pairs affect the molecular shape and dipole cancellation?
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. They create asymmetry in the molecule
- B. They increase the bond angles
- C. They have no effect on the shape
- D. They decrease the number of bonds
Answer
They create asymmetry in the molecule
Explanation
The correct option is They create asymmetry in the molecule. They create asymmetry in the molecule is the best answer because it directly supports the AQA A-Level Chemistry objective to use molecular shape to decide whether bond dipoles cancel. This reasoning is anchored to Electronegativity and bond polarity in Bonding, and it separates dipole from similar A-Level ideas rather than relying on a vague recall statement. Other options are weaker if they use the wrong evidence, calculation, mechanism, observation, unit, or conclusion for this subtopic.
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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