3 Intermolecular Forces You Must Know to PASS Chemistry

The video tutorial explains intermolecular forces, focusing on hydrogen bonding, dipole-dipole forces, and London dispersion forces. It describes how these forces arise from attractions between charged regions of molecules, affecting their physical and chemical properties. Hydrogen bonding is the strongest, occurring in polar molecules with hydrogen bonded to nitrogen, oxygen, or fluorine. Dipole-dipole forces occur in polar molecules without hydrogen bonding. London dispersion forces, the weakest, are present in all molecules, especially non-polar ones, due to temporary dipoles.

What does the dotted line between molecules typically represent?

• A metallic bond

• A hydrogen bond

• An ionic bond

• A covalent bond

Which of the following is NOT a requirement for hydrogen bonding?

• Strong intermolecular attraction

• Sharing of electrons

• Presence of a polar molecule

• Hydrogen bonded to nitrogen, oxygen, or fluorine

What is the main difference between a hydrogen bond and a chemical bond?

• Chemical bonds are weaker

• Hydrogen bonds involve electron sharing

• Hydrogen bonds are not true bonds

• Chemical bonds do not involve charges

What causes dipole-dipole forces to form between molecules?

• Movement of electrons

• Attraction between opposite charges

• Presence of temporary dipoles

• Equal sharing of electrons

Which molecule is used as an example to explain dipole-dipole forces?

• CO

• H2O

• N2

• O2

What is unique about London dispersion forces compared to other intermolecular forces?

• They are present only in polar molecules

• They involve permanent dipoles

• They are present in all molecules

• They are the strongest

Why are London dispersion forces considered the weakest?

• They involve permanent dipoles

• They are temporary and fluctuate

• They require specific atoms

• They involve electron sharing