Intermolecular Forces: แบบฝึกหัด

• 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.

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