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Van Der Waals Attractions: Introduction
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<font face="Verdana, Arial, Helvetica, sans-serif" size="5" color="#FFFFFF"><strong>Van Der Waals Attractions:</strong> Introduction</font>
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<td><img src="chargeMainIdea.png" width="98" height="58"></td>
<td><font face="Verdana, Arial, Helvetica, sans-serif" size="4">All molecules
attract to each other using forces called "van der Waals attractions".<a href="script:page:0:message vdwDisclaimer.html">*</a> These attractions are responsible for:</font>
<ul>
<li>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">The
temperatures at which many substances boil.</font></li>
<li>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">The
ability for your immune system to recognize and disable pathogens
instead of attacking your own cells and organs.</font> </li>
<li>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">The
amazing climbing ability of Geckos.</font> </li>
</ul>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">In this
activity you will explore how molecular level attractions are the
foundation of these phenomena and many other everyday experiences. </font>
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<img src="chargeBullet.png" height="23" width="33">
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<strong><font color="#a65d2c" face="Verdana, Arial, Helvetica, sans-serif" size="5">Types
of Bonds and Polarity</font></strong>
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<img src="rule.png" height="6" width="18">
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<font size="4" face="Verdana, Arial, Helvetica, sans-serif">Two
atoms can bond to form a molecule in two ways:</font>
<ul>
<li>
<font size="4" face="Verdana, Arial, Helvetica, sans-serif">with
a non-polar covalent bond (when electrons are shared evenly) </font>
</li>
<li>
<font size="4" face="Verdana, Arial, Helvetica, sans-serif">with
a polar covalent bond (when there is an uneven sharing of the
electrons, causing the formation of a <a href="script:page:0:message partialCharge.html">partial
positive and partial negative</a> charge on the surface of the
molecule.) </font>
</li>
</ul>
<font face="Verdana, Arial, Helvetica, sans-serif">The polar or
non-polar nature of molecules is what gives many substances their
physical properties.<br><br></font>
<div align="center">
<img src="surfaceChargePanelComp.png" height="71" width="133">
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<img src="moleculeRep.jpg" height="270" width="300">
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<strong><font size="4" face="Arial, Helvetica, sans-serif">What is the
difference between polar and non-polar molecules (and don't just talk
about the colors used to represent them)?</font></strong>
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<img src="chargeBullet.png" height="23" width="33">
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<strong><font color="#a65d2c" face="Verdana, Arial, Helvetica, sans-serif" size="5">Seeing
van der Waals Attractions</font></strong>
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<td colspan="2">
<img src="rule.png" height="6" width="18">
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<font face="Verdana, Arial, Helvetica, sans-serif" size="4">All
molecules attract to each other, but there are different patterns
and strengths of attraction that occur. To the left is a bunch of
polar and non-polar molecules.</font>
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<img src="vdwPointerComp.png" width="102" height="100">
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<td colspan="2">
<font size="4" face="Verdana, Arial, Helvetica, sans-serif">Explore
how different or similar molecules form van der Waals attractions
when they are close together. Then answer the questions below.</font>
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<font face="Verdana, Arial, Helvetica, sans-serif" size="4">Use the <strong>take
a snapshot</strong> button above to capture a picture of some van der
Waals attractions. A window will open with your snapshot and some
annotation tools. Use these tools to indicate where you see van der Waals
attractions in your image.</font>
<blockquote>
<p>
<font size="4" face="Verdana, Arial, Helvetica, sans-serif"><img src="textAnnotation.gif" height="15" width="16">
  = add a text annotation<br></font><img src="drawRect.gif" height="12" width="16"><font size="4" face="Verdana, Arial, Helvetica, sans-serif"> =
draw a rectangle<br><img src="drawLine.gif" height="14" width="15"> =
draw a line </font>
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<strong><font size="4" face="Arial, Helvetica, sans-serif">Which of the
following formed van der Waals attractions (check all that apply):</font></strong>
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+ ends of polar molecules to + ends of other polar molecules
+ ends of polar molecules to - ends of other polar molecules
- ends of polar molecules to - ends of other polar molecules
non-polar molecules to other non-polar molecules
non-polar molecules to + parts of polar molecules
non-polar molecules to - parts of polar molecules
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</a></font>
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