Intermolecular Forces: Practice Questions

• a.Permanent dipole-permanent dipole interactions
• b.Electrostatic attraction between oppositely charged ions
• c.Hydrogen bonding between polar molecules
• d.Instantaneous dipole-induced dipole interactions

• a.Ethane has a larger surface area, leading to weaker London forces.
• b.The C-H bonds in ethane are more polar than the O-H bond in methanol.
• c.Methanol has a higher molar mass than ethane.
• d.Methanol molecules are held together by hydrogen bonds, which are stronger than London forces.

• a.

  The boiling temperatures decrease from \(CF_{4}\) to \(CI_{4}\) because the molar mass of the molecules increases, making them more difficult to vaporise.

• b.

  The boiling temperatures increase from \(CF_{4}\) to \(CI_{4}\) because the increasing number of electrons leads to a more polarisable electron cloud and stronger London forces.

• c.

  The boiling temperatures decrease from \(CF_{4}\) to \(CI_{4}\) because the bond polarity decreases as the electronegativity of the halogen decreases.

• d.

  The boiling temperatures increase from \(CF_{4}\) to \(CI_{4}\) because the permanent dipole-dipole interactions become stronger.

• a.\(CH_{3}CH_{2}OH\)
• b.\(CH_{3}OCH_{3}\)
• c.\(CH_{3}CHO\)
• d.\(CH_{3}COCH_{3}\)

• a.

  The nuclear charge increases, attracting neighboring nuclei more strongly.

• b.

  The atomic radius decreases, allowing closer packing.

• c.

  The electronegativity increases, creating permanent dipoles.

• d.

  The number of electrons increases, leading to stronger London forces.

Write your answer out first, then check it against the worked solution.

Write your answer out first, then check it against the worked solution.

Write your answer out first, then check it against the worked solution.