Question detail
What is the primary reason for the higher boiling point of water compared to methane?
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. Water has stronger hydrogen bonds than the London dispersion forces in methane.
- B. Water has a higher molecular weight than methane.
- C. Water is a polar molecule while methane is non-polar.
- D. Water has more electrons than methane.
Answer
Water has stronger hydrogen bonds than the London dispersion forces in methane.
Explanation
Water's higher boiling point is due to the presence of hydrogen bonds, which are significantly stronger than the London dispersion forces present in methane. This results in more energy being required to break the intermolecular forces in water.
Common mistake
Misunderstanding Intermolecular Forces
Students often confuse the strength of intermolecular forces with the boiling point of a substance, thinking that all substances with high boiling points have strong intermolecular forces without considering molecular size and shape.
To accurately explain boiling point trends, remember that stronger intermolecular forces lead to higher boiling points, but also consider how molecular size and surface area affect these forces. For example, larger molecules have more surface area for London dispersion forces, which can increase boiling points despite weaker individual interactions.
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