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To enter the gas phase, a liquid must overcome the intermolecular forces holding its particles together. These attractive forces are called London dispersion forces, and they increase with the size and mass of the molecules. For example, nonpolar F2 molecules experience stronger dispersion forces than polar HCl molecules. Therefore, the normal boiling point of HCl is higher than that of F2.
Assuming that their shapes are similar and that their molar masses are equal, order the following compounds from lowest to highest boiling point: dimethylether (CH3OCH3), ethanol (CH3CH2OH), and propane (CH3CH2CH3). Explain why each compound has its boiling point. Note: Boiling points are a measure of the strength of IMFs, including hydrogen bonding.