Understanding Boiling Points Through Intermolecular Forces

What are intermolecular forces?

• Forces within a molecule

• Forces between molecules

• Forces that only occur in solids

• Forces that break chemical bonds

Which of the following is NOT a type of intermolecular force?

• Hydrogen bonding

• Ionic bonding

• Dipole-dipole interactions

• London dispersion forces

Why do liquids with stronger intermolecular forces have higher boiling points?

• Because they require less energy to boil

• Because they evaporate more quickly

• Because they require more energy to overcome the intermolecular forces

• Because they are less dense

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What role does hydrogen bonding play in the boiling point of water?

• It lowers the boiling point

• It has no effect on the boiling point

• It increases the boiling point

• It only affects the freezing point

Which type of intermolecular force is the weakest?

• Hydrogen bonding

• Dipole-dipole interactions

• London dispersion forces

• Covalent bonding

What happens to the boiling point of a liquid as the strength of its intermolecular forces increases?

• It decreases

• It remains the same

• It increases

• It first increases, then decreases

Which of the following molecules would likely have the highest boiling point based on its intermolecular forces?

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• Hydrogen bonding

• Dipole-dipole interactions

• London dispersion forces

• Ionic bonding

Why do molecules with larger molar masses generally have higher boiling points?

• They have stronger ionic bonds

• They have more electrons, leading to stronger London dispersion forces

• They are more likely to be gases at room temperature

• They have stronger hydrogen bonds

What effect does branching in hydrocarbons have on their boiling point?

• Increases the boiling point

• Decreases the boiling point

• Has no effect on the boiling point

• Initially decreases, then increases the boiling point