What are the four main types of intermolecular forces of attraction?

• London dispersion forces, ion-dipole forces, dipole-dipole forces, hydrogen bonding forces

• Covalent bonds, ionic bonds, metallic bonds, hydrogen bonds

• Hydrogen bonds, London dispersion forces, ionic bonds, covalent bonds

• Van der Waals forces, ionic bonds, covalent bonds, dipole-dipole forces

Which type of intermolecular force is the weakest?

• Hydrogen bonding

• Ion-dipole interactions

• Dipole-dipole forces

• London dispersion forces

What type of interaction occurs between two oppositely charged particles?

• Ion-ion interaction

• Hydrogen bonding

• Dipole-dipole interaction

• London dispersion forces

Which type of interaction is responsible for the dissolution of ionic solids in polar solvents?

• London dispersion forces

• Ion-dipole interactions

• Dipole-dipole interactions

• Ion-ion interactions

What is a characteristic of dipole-dipole interactions?

• They are the strongest type of intermolecular force.

• They occur between nonpolar molecules.

• They are present in polar molecules.

• They only occur in ionic compounds.

Which of the following molecules exhibits hydrogen bonding?

• N2

• H2O

• CH4

• O2

What is the primary factor that determines the strength of ion-ion interactions?

• The distance between the particles

• The size of the molecules

• The temperature of the solution

• The type of solvent used

Which of the following compounds is likely to have the highest boiling point due to hydrogen bonding?

• C2H6

• H2O

• N2

• CH4

What is polarizability?

• The ability of a molecule to form hydrogen bonds

• The temperature at which a substance boils

• The measure of how easy it is to distort the electron distribution of a molecule

• The strength of ionic bonds in a compound

Which of the following statements is true about London dispersion forces?

• They occur in all electrically neutral molecules.

• They are present only in polar molecules.

• They are the strongest type of intermolecular force.

• They are stronger than hydrogen bonds.