Week 4 Questions - Not really need PDF

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Intermolecular Forces 1. • Which of the following compound(s) exhibit only London Dispersion Forces? • Which compound(s) exhibit hydrogen-bonding forces? • Considering only compounds without hydrogen bonding interactions, which compounds have a dipole-dipole intermolecular force?

a) SF4 b) CO2 c) CH3CH2OH d) HF e) ICl5 f) XeF4

2. • Identify the most important/strongest type of force (ionic, hydrogen bonding, dipole-dipole or London Dispersion Forces) among atoms or molecules present in the solids of each of the following compounds. CF3(CF2CF2)nCF3 CO2 NaI NH4Cl MgCl2

3. • Rank the following compounds from lowest to highest boiling point. CH3CH2CH2Cl CH3CH2Cl CH3CH2CH2CH2Cl CH3Cl

4. • Rank the following compounds from lowest to highest melting point. CH4 MgO H2O H2S

5. Which of the following substances has the highest boiling point? a. CH3OCH3 b. CH3OH c. CH4 d. CH3CH3 e. CH3CH2OH

6. For which of the following substances will strong hydrogen bonds form between the molecules? (You may select more than one) a. HCOOH (formic acid) b. CH3CN c. CCl4 d. SiH4 e. CH3OH

7. Which of the following statements about intermolecular forces is incorrect? a. Intermolecular forces describe the attractions between two or more separate molecules b. The only intermolecular forces between nonpolar molecules are London dispersion forces c. Intermolecular forces only depend on the polarity of the molecules d. Hydrogen bonds are a special kind of dipole-dipole interaction e. The presence of hydrogen bonding accounts for many of the unique properties of water

8. For which of the following compounds is hydrogen bonding the strongest?

a. Butane

b. Propanol

c. Methoxyethane

d. Ethanoic Acid

9. What type(s) of intermolecular forces must be overcome when liquid hexane (CH3CH2CH2CH2CH2CH3) vaporizes? a. London dispersion forces b. Dipole-dipole forces c. Hydrogen bonds d. Covalent bonds...