Intermolecular Forces
Chemistry ⇒ Chemical Bonding and Structure
Intermolecular Forces starts at 10 and continues till grade 12.
QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Intermolecular Forces.
How you perform is determined by your score and the time you take.
When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 10
A student notices that pentane (C5H12) has a higher boiling point than methane (CH4). Explain why this is the case.
A student observes that acetone evaporates faster than water at room temperature. Explain this observation in terms of intermolecular forces.
Describe how the molecular size affects the strength of London dispersion forces.
Describe the difference between intermolecular and intramolecular forces.
Describe the role of intermolecular forces in the formation of a meniscus in a liquid.
Describe what is meant by a 'temporary dipole' in the context of London dispersion forces.
Explain why ethanol (C2H5OH) can form hydrogen bonds but ethane (C2H6) cannot.
Explain why ice floats on water in terms of intermolecular forces and structure.
Explain why noble gases can be liquefied at low temperatures.
Explain why water has a higher boiling point than methane.
Which type of intermolecular force exists between all molecules, regardless of polarity?
A liquid is observed to have a very high surface tension and a low rate of evaporation at room temperature. What can you infer about the strength of its intermolecular forces?
A student compares the boiling points of two isomers: n-pentane and neopentane. Both have the same molecular formula (C5H12), but n-pentane has a higher boiling point. Explain this observation in terms of intermolecular forces and molecular shape.
Arrange the following substances in order of increasing strength of intermolecular forces: CO2, H2O, CH4.
Explain why the boiling point of HF is significantly higher than that of HCl, even though both are hydrogen halides.
