3.1 Intermolecular Forces Pre Test

• It does not show how hydrogen bonds are constantly forming, breaking, and reforming, which results in a net force of attraction between the molecules.

• It does not show how the interactions between ions and the induced molecular dipoles result in a net force of attraction between the molecules.

• It does not show how the interacting permanent dipoles of the molecules result in a net force of attraction between the molecules.

• It does not show how the temporary fluctuating dipoles of the molecular electron clouds result in a net force of attraction between the molecules.

• 
  F2 is soluble in water, whereas HF is insoluble in water.

• The F2 molecule has a greater mass than the HF molecule has.

• Liquid F2 has weak dispersion force attractions between its molecules, whereas liquid HF has strong ionic interactions between H+ and F− ions.

• Liquid F2 has weak dispersion force attractions between its molecules, whereas liquid HF has both weak dispersion force attractions and hydrogen bonding interactions between its molecules.

What type of interactions occur between polar molecules that possess permanent dipoles?

• London dispersion forces

• Hydrogen bonding

• Ionic bonding

• Dipole-dipole interactions

Hydrogen bonding is responsible for the unique properties of water and the high boiling points of compounds such as ammonia and ___

What are the three main types of intermolecular forces?

• London dispersion forces

• Dipole-dipole interactions

• Hydrogen bonding

• Van der Waals forces

What type of interaction occurs when hydrogen is covalently bonded to highly electronegative atoms?

• Ionic bonding

• Van der Waals forces

• Hydrogen bonding

• Covalent bonding

What is the weakest type of intermolecular force?

What role do intermolecular forces play in determining the physical properties of substances?