All molecules can exhibit London dispersion forces, but dipole-dipole and hydrogen bonding are stronger attractions for molecules with similar masses/numbers of electrons when they are present. Which of these can ONLY exhibit London dispersion forces?

Dipole-dipole attractions occur between polar molecules. Which of these molecules is polar?

A Lewis structure for acetone is shown above. (There is a carbon atom at the center that isn't shown) What type of intermolecular forces will be present between the molecules of acetone in a pure sample of acetone? Select all that apply.

The weaker the intermolecular forces of a substance, the _____________ the boiling point.

Which of the following explains the relatively high melting and boiling point of water?

London dispersion forces are stronger between atoms or molecules with more electrons, and weaker between atoms or molecules with fewer electrons. Which of the following has the strongest London dispersion forces?

Which of the following intermolecular forces can all types of particles exhibit?

A Lewis structure for carbon dioxide is shown below. What types of intermolecular attractions can be present between molecules of carbon dioxide in a pure CO₂ sample? Select all that apply

Which of these molecules can participate in dipole-dipole attractions? Select all that apply.

Propane is a gas at room temperature, while bromine is a liquid at room temperature. Which statement correctly explains these observations?

Which numbered arrow in the image above points to a hydrogen bond?

What is the strongest type of intermolecular force one H₂S molecule will exhibit?

What is the strongest intermolecular force present between HCl molecules?

Which of the following would best remove Sharpie marker from your wall if this marker is known to be non-water soluble?

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

Rank these in order of strength:

covalent bond

London dispersion forces

hydrogen bond

dipole-dipole attraction