assignment%204%20answers%202011 - CHM 1321A Assignment #4...

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CHM 1321A Assignment #4 Answers 1) Diethyl ether and 1-butanol have similar solubilities in water, but their boiling points are very different. Explain why these compounds have similar solubility properties but different boiling points. Each molecule has about the same amount of Van der Waals interactions, and the Van der Waals surfaces are relatively large. Each compound has a dipole, lone pairs on oxygen and is able to hydrogen bond with water. Therefore each compound has similar solubility in water. The hydrogen bonds in butanol are stronger that the dipole interactions in diethyl ether. Butanol has a higher boiling point because of the stronger hydrogen bonds. The intermolecular forces holding the butanol molecules together are stronger than those holding the diethyl ether molecules together. 2) Explain the difference in boiling point for the following pairs of compounds: Each molecule has about the same Van der Waals ability. N-methyl-pyrrolidine (on the left) is capable of dipole-dipole interactions. Piperidine (on the right) has a dipole and can also hydrogen bond with itself
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This note was uploaded on 08/24/2011 for the course ENGINEERIN 1122 taught by Professor Stadnik during the Spring '11 term at University of Ottawa.

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assignment%204%20answers%202011 - CHM 1321A Assignment #4...

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