intermolecular forces

Which type of intermolecular force is the strongest?

• Hydrogen bonding

• Dipole-Dipole

• London Dispersion

All molecules feel this kind of intermolecular forces

• Hydrogen bonding

• Dipole-Dipole

• London dispersion

Only polar molecules feel this kind of intermolecular forces

• Hydrogen bonding

• Dipole-Dipole

• London dispersion

Only polar molecules with H-F, H-N, or H-O bonds feel this kind of Intermolecular forces

• Hydrogen Bonding

• Dipole-Dipole

• London Dispersion

What is the strongest kind of intermolecular forces that occurs between molecules of NH3?

• Hydrogen bonding

• Dipole-Dipole

• London Dispersion

Ethanol is much more soluble in water than is ethyl ethanoate. Which one of the following statements correctly accounts for this?

• Ethanol is a polar molecule, but ethyl ethanoate is non-polar

• Ethanol is a non-polar molecule, but ethyl ethanoate is polar

• A hydrogen bond forms between the hydrogen of the -OH group in ethanol and the oxygen of a water molecule

• A hydrogen bond forms between the hydrogen of the -OH group in ethanol and the hydrogen of a water molecule.

Why is the boiling point of methane greater than that of neon?

• A molecule of methane has a greater mass than a molecule of neon

• A molecule of methane has more electrons than a molecule of neon

• Molecules of methane have stronger intermolecular forces than those of neon

• Molecules of methane from hydrogen bonds, but those of neon do not

• The molecule of methane is polar, but that of neon is not

Which of the following statements best explains why the boiling point of butanone (79.6 ^oC) is higher than that of pentane (36.1 ^oC)?

• The relative molecular mass of butanone is higher than that of pentane

• The butanone molecule has a larger surface area than the pentane molecule

• The covalent bond in the butanone molecule are stronger than those in the pentane molecule

• There are hydrogen bonds between butanone molecules, but not between pentane molecules

• There are dipole-dipole forces between butanone molecules, but not only van der Waals' forces between pentane molecules

Which of the following statements describes a phenomenon which can be explained by intermolecular hydrogen bonding?

• The melting points of the Group 1 hydroxides increase with increasing relative molecular mass (M_r)

• The boiling points of the alkanes increase with increasing relative molecular mass.

• CH₃OCH₃ (M_r = 46) has a higher boiling point than CH₃CH₂CH₃ (M_r = 44)

• Hydrogen chloride forms an acidic solution when dissolved in water.

• Ice has a lower density of water at 0 ^oC.

Graphite can be used as a lubricant; diamond cannot. This is because graphite has

• mobile ions

• delocalised electrons

• a hexagonal arrangement of atoms in the layers

• covalent bonds between atoms in the layers

• van der Waals' forces between the layers of atoms

Tags

NGSS.HS-PS1-3