Intermolecular Forces In Diethyl Ether

Vapor Pressure: H-bonding vs. dipole-dipole allure

The measurement of pressure exerted past a vapor is demonstrated using barometers. The vapor pressures of butanol and diethyl ether are compared.

Diethyl ether has a much college vapor pressure level than butanol. In addition to the London forces which are about the same for both molecules, diethyl ether has but intermolecular dipole-dipole forces, much weaker than the hydrogen-bond intermolecular forces of the butanol.

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Keywords

vapor pressure, atmospheric pressure, barometric force per unit area, barometer, intermolecular forces, hydrogen bond, gases and liquids, organic, phase changes, physical properties, polar molecules

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The molecular formulas for butanol and diethyl ether are the same. However, their structures are ~~very~~ different. Butanol molecules grade hydrogen bonds, while diethyl ether molecules can but form dipole-dipole interactions. Which forcefulness is stronger?

When butanol is injected into the open end of the barometer, the butanol rises to the top and vaporizes. The mercury cavalcade is depressed to 721 millimeters. When diethyl ether is injected, the diethyl ether rises to the top and vaporizes. The mercury column is depressed to 264 millimeters.

Diethyl ether has a much higher vapor force per unit area than butanol. In addition to the London forces which are about the aforementioned for both molecules, diethyl ether has only intermolecular dipole-dipole forces, much weaker than the hydrogen-bail intermolecular forces of the butanol.