a. Which is generally stronger, intermolecular or intramolecular forces? Intramolecular forces include covalent bonds, ionic bonding, and metallic bonding.
b. Which of these kinds of interactions are broken when a liquid is converted to a gas?
Which type of intermolecular forces accounts for each of these differences:
a. CH3OH boils at 65 °C and CH3SH boils at 6 °C.
b. Xe is a liquid at atmospheric pressure and 120 K and Ar is a gas under the same conditions.
c. Acetone boils at 56 °C and 2-methylpropane boils at -12 °C. (Lewis structures below)
Select which molecule will have the stronger intermolecular dispersion forces?
a. Br2 or O2
b. CH3CH2CH2SH or CH3CH2CH2OH
c. SiH4 vs GeH4
Using your knowledge of intermolecular forces, rationalize the difference in boiling points for each pair:
a. HF (20 °C) vs HCl (-85 °C)
b. CHCl3 (61 °C) and CHBr3 (150 °C)
c. Br2 (59 °C) and ICl (97 °C)
Based on the type or types of intermolecular forces, predict the substances in each pair that has the higher boiling point:
a. Propane (C3H8) or n-butane (C4H10)
b. Diethyl ether (CH3CH2OCH2CH3) or 1-butanol (CH3CH2CH2CH2OH)
c. Sulfur dioxide (SO2) or sulfur trioxide (SO3)
Carbon tetrachloride CCl4 and chloroform CHCl3, are common organic liquid. Carbon tetrachloride’s normal boiling point is 77 °C; chloroforms normal boiling point is 61 °C. Which statement is the best explanation of this data?
a. Chloroform can hydrogen bond, but carbon tetrachloride cannot.
b. Carbon tetrachloride has a larger dipole moment than chloroform.
c. Carbon tetrachloride’s large size and mass results in a more polarizable molecule and results in stronger dispersion forces.
Based on their composition and structure list, CH2Cl2, CH3CH2CH3, and CH3CH2OH in order of:
a. Increasing intermolecular forces
b. Increasing viscosity
c. Increasing surface tension
The fluorocarbon compound C2Cl3F3 has a normal boiling point 47.6 °C. The specific heats of and C2Cl3F3
(l) C2Cl3F3 (g) are 0.91 J/g·K and 0.67 J/g·K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat required to convert 35.0 g of C2Cl3F3 from a liquid at 10.00 °C to a gas at 105.00 °C.