Intermolecular Forces Dipole-Dipole Hydrogen Bonding Dispersion Ion Dipole Interaction

Hydrogen bonding occurs when a hydrogen atom bonded to N, O, or F is attracted to another molecule's N, O or F atom. Which of the following can participate in hydrogen bonding?

• CBr₄

• NO₂

• H₂S

• NH₃

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?

• I₂

• NH₃

• OCl₂

• CH₃Cl

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

• H₂

• HCl

• Cl₂

• Br₂

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.

• ion-dipole attractions

• dipole-dipole attractions

• hydrogen bonding

• London dispersion forces

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

• higher

• lower

Which of the following has the highest boiling point?

• H₂
• NH₃
• N₂
• O₂

Tags

NGSS.HS-PS1-3

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

• Strong dipole-dipole attractions between water molecules

• Strong hydrogen bonds between water molecules

• London dispersion forces between water molecules

• Dipole-induced dipole attractions between water molecules

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?

• F₂

• Br₂

• I₂

• Cl₂

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

• London dispersion forces

• dipole-dipole forces

• hydrogen bonding

• none of the above

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

• London dispersion forces

• dipole-dipole attractions

• hydrogen bonds

• ion-dipole attractions