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Van Der Waals Attractions: Strengthening London Dispersion Attraction
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<font face="Verdana, Arial, Helvetica, sans-serif" size="7" color="#FFFFFF"><strong>Evaporation</strong>
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<td><font face="Verdana, Arial, Helvetica, sans-serif" size="4">London Dispersion attractions between molecules, the weakest intermolecular forces, are not all the same. Some are stronger than others. Below you will explore the relationship between size, shape, and increased London Dispersion attraction.</font></td>
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<font size="4" face="Verdana, Arial, Helvetica, sans-serif">Select a
pair of molecules to test from the menu below the model, press the "run"
button, and then use the arrow keys to pull on one of the molecules.</font>
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select a pair of molecules here
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<font size="4" face="Arial, Helvetica, sans-serif"><strong>Which molecule
pairs had the strongest attraction (check all that apply):</strong></font>
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the two small molecules
the two large straight molecules
the large straight and bent molecules
the large straight and circular molecules
the large curved and circular molecules
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<font size="4" face="Arial, Helvetica, sans-serif"><strong>Propane boils
at -42°C, butane at 0°C, and pentane at 36°C. They are all straight
molecules. Which one is the biggest? </strong></font>
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propane
butane
pentane
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<font size="4" face="Arial, Helvetica, sans-serif"><strong>Small molecules
did not attract well. However, only some of the large ones had a strong
attraction. Describe how both size and shape play a role in the strength
of the London Dispersion attraction.</strong></font>
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