Recall that there are several types of intermolecular forces (IMF):
1. Ion-dipole interaction – occurs between an ion and a polar covalent compound; strongest IMF
2. Hydrogen bonding – occurs in compounds where hydrogen is directly connected to an electronegative element such as N, O, or F; 2nd strongest IMF
3. Dipole-dipole interaction – occurs between two polar covalent compounds; 3rd strongest IMF
4. Dispersion forces – occurs in all compounds and is the primary IMF exhibited by nonpolar compounds; weakest IMF
Compounds with strong intermolecular forces have high boiling points. This is because they require more energy to be able to break the bonds during the phase transition.
What type of intermolecular force accounts for the following differences in each case?
CH3OH boils at 65 °C, CH3SH boils at 6 °C
a. London dispersion forces.
b. Dipole-dipole bonding.
c. Hydrogen bonding.
d. Ion-dipole bonding.
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