Part I: Intermolecular Forces 1. The Lewis structures for diethyl ether CHJCH.oC

Question

Part I: Intermolecular Forces 1. The Lewis structures for diethyl ether CHJCH.oCHzCH) and ethanol (CH,CHzoh) are shown below. Complete parts a-f C C (a) List the intermolecular forces that are present in a sample of diethyl ether. (b) List the intermolecular forces that are present in a sample ofethanol. (c) Diethyl ether boils at 34.6 °C while ethanol boils at 78.3°C, Explain the difference in boiling points in terms of intermolecular forces. (d) Calculate the amount of heat required to vaporize 0.25 mol of diethyl ether at its boiling point (note: Google and the textbook are your friend!). (e) Calculate the amount of heat required to vaporize 0.25 mol of ethanol at its boiling point. (f Which substance requires more heat to vaporize? Does this make sense? Provide a brief explanation based on boiling points and intermolecular forces.

Explanation / Answer

a. Being a polar species dietyl ether molecules will exibit disperson and dipole-dipole forces.

b. Etanol molecules exibit strong intermolecular forces called hydrogen bonding (electrostatic force of attraction b/w H- atom and a highly electronegative atom like O, F, N etc.).

c. Bioiling point of Etanol is higher than ether due to strong intermolecular H-bonds

f. Heat of vaporization is the heat absirbed by a liquid to vaporise it,s certain quantity at a constant temperature.

As presence of H-bond holds ethanol molecules tightly, more heat is needed to vaporise it than ether having weak dispersion forces.

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