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Which type of intermolecular force accounts for each of these differences? (a) ch3oh boils at 65 °c; ch3sh boils at 6 °c. (b) xe is a liquid at atmospheric pressure and 120 k, whereas ar is a gas under the same conditions. (c) kr, atomic weight 84 amu, boils at 120.9 k, whereas cl2, molecular weight about 71 amu, boils at 238 k. (d) acetone boils at 56 °c, whereas 2-methylpropane boils at -12 °c
Which type of intermolecular force accounts for each of these differences? (a) ch3oh boils at 65 °c; ch3sh boils at 6 °c. (b) xe is a liquid at atmospheric pressure and 120 k, whereas ar is a gas under the same conditions. (c) kr, atomic weight 84 amu, boils at 120.9 k, whereas cl2, molecular weight about 71 amu, boils at 238 k. (d) acetone boils at 56 °c, whereas 2-methylpropane boils at -12 °c
Final answer:The differences in boiling points are due to the varying strengths of intermolecular forces: methanol exhibits hydrogen bonding while methanethiol only has London dispersion forces; xenon's greater polarizability leads to stronger London forces compared to argon; chlorine's dipole-dipole attractions exceed krypton's dispersion forces; acetone's dipole-dipole interactions are stronger than 2-methylpropane's dispersion forces.Explanation:The differences in boiling points between the given substances can be attributed to different types of intermolecular forces (IMFs). Each substance has a dominant type of IMF which influences its phase changes, such as boiling.a. For CH3OH (methanol) and CH3SH (methanethiol), the significant difference in boiling points is due to CH3OH's ability to form hydrogen bonds due to the presence of an -OH group, which is a stronger IMF than the London dispersion forces present in CH3SH.b. Xe is a liquid at atmospheric pressure and 120 K while Ar is a gas because Xe, being heavier, has stronger London dispersion forces due to its greater polarizability.c. Kr boils at a lower temperature than Cl2 despite having a higher atomic weight because Cl2 molecules can exhibit stronger dipole-dipole attractions while Kr can only exhibit London dispersion forces.d. Acetone boils at a higher temperature than 2-methylpropane due to its ability to engage in dipole-dipole interactions because of its polar carbonyl group; conversely, 2-methylpropane can only exhibit London dispersion forces....