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| Question | Answer |
| The intermolecular force in CaBr2 is _____? | ion - ion |
| Which one of the following exhibits dipole - dipole attraction between molecules? XeF4, Br2, CO2, or BCl3 | XeF4 |
| What types of intermolecular forces exist between NH3 and CBr4? | London dispersion and hydrogen bonds |
| Of the following, H2, Cl2, N2, or Br2, which has the highest boiling point? | Br2 |
| What types of intermolecular forces exist between Br2 and CCl4? | London dispersion |
| What is the intermolecular force in CBr4? | London dispersion |
| Of the following substances, Kr, CH4, CO2, or H2O, which has the highest boiling point? | H2O |
| List the four major intermolecular forces in order from strongest to weakest? | ion - ion, hydrogen bonding, dipole - dipole and London dispersion |
| Which of the following, H2S, PH3, NH3, or SiH4, should have the lowest boiling point? | SiH4 |
| C12H26 molecules are held together by what intermolecular force? | London dispersion |
| Elemental iodine (I2) is a solid at room temperature, what is the major attractive force that exists among iodine molecules? | London dispersion |
| How do intermolecular forces effect the state of matter of a substance? | the stronger the intermolecular force the more likely the substance is to be a solid, weak intermolecular forces produce gases |
| Relate the strength of London dispersion forces to the size of the particles involved? | the larger a molecule is the larger the London dispersion force |
| Explain why water has a higher boiling point than methane, CH4? | Because water has hydrogen bonding and methane only has London dispersion |
| Determine the intermolecular force for each compound and then determine which compound has the highest boiling point: O2, H2, NH3, and SO2? | O2 = London dispersion, H2 = London dispersion, NH3 = hydrogen bonding and SO2 = dipole - dipole and NH3 has the highest boiling point |