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<div class="moz-cite-prefix">On 02/09/2016 12:35 PM, wrote:<br>
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cite="mid:4ef34afac31b4b18894fa4429fc11c32@spiderman.MercerU.local"
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<p>Hi Dr. Pounds, </p>
<p>I was looking over chapter 11 and I am still confused on the
intermolecular forces.
</p>
<p>Could you please explain the difference between an induced
dipole and a regular dipole-dipole for interaction.
</p>
<p><br>
</p>
<p>Thanks! <br>
</p>
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<br>
So in a regular dipole-dipole interaction you have two molecules
that are already dipoles. <br>
<br>
Think about two CO molecules coming together -- that would be an
example of a dipole-dipole interaction.<br>
<br>
<br>
In an induced dipole you have either an ion, or a molecule that has
a dipole, coming in close proximity to a molecule that is neither an
ion or a dipole. <br>
<br>
Think about CO coming in close proximity to Xenon. The "more
positive part" of the CO (near the carbon) attracts some of the
electrons to one side of the Xenon atom and thus. Since there is a
small imbalance in the number of electrons in Xe (you may have some
now closer to the C on the CO) you have "INDUCED" a small dipole on
Xe.<br>
<br>
<pre class="moz-signature" cols="72">--
Andrew J. Pounds, Ph.D. (<a class="moz-txt-link-abbreviated" href="mailto:pounds_aj@mercer.edu">pounds_aj@mercer.edu</a>)
Professor of Chemistry and Computer Science
Mercer University, Macon, GA 31207 (478) 301-5627
<a class="moz-txt-link-freetext" href="http://faculty.mercer.edu/pounds_aj">http://faculty.mercer.edu/pounds_aj</a>
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