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Molecular Geometry: Page 4
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<font face="Verdana, Arial, Helvetica, sans-serif" size="5" color="#FFFFFF"><strong>Molecular Geometry:</strong> Regions of Electron Density</font>
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<td><img src="atomMainIdea.png" width="98" height="58"></td>
<td><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Regions of electron density are where electrons "hang out". These regions include shared electrons in bonds, but also refer to unshared electrons.</font></td>
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<strong><font face="Verdana, Arial, Helvetica, sans-serif" color="#a65d2c" size="5">Covalent
Bonds are Regions of Electron Density</font></strong>
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<img height="6" width="18" src="rule.png">
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<font face="Verdana, Arial, Helvetica, sans-serif" size="4">In molecular
hydrogen (H<sub>2</sub>, shown at right) each hydrogen atom contributes
one electron to a single bond between two atoms. <b>This bond, like any
covalent bond, is one region of electron density.</b> The electrons are
found in an area betweeen and around the atoms that are bonded. Here are
some different ways of showing the electrons that form covalent bonds.</font>
<p>
<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Bond
diagrams </font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">use
lines for each shared pair. </font>
</p>
<p>
<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Lewis dot
structures</font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">
show unshared (non-bonding) electrons as well as shared electrons.</font>
</p>
<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">An<b>
"orbital view"</b> shows a hazy blue area where you are most
likely to find shared electrons. </font>
</p>
<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">In the <b>"ball
and stick plus" view</b> a 'stick' bond shows us how the atoms are
connected and a region of electron density is also shown.</font>
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<strong><font face="Verdana, Arial, Helvetica, sans-serif" color="#a65d2c" size="5">Any
Unshared Electron Pair is a Region of Electron Density </font></strong>
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<img height="6" width="18" src="rule.png">
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<b><font face="Verdana, Arial, Helvetica, sans-serif" size="5">Unshared
electrons</font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="5">
</font>
<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">Ammonia (NH</font><sub><font face="Verdana, Arial, Helvetica, sans-serif" size="3">3</font></sub><font face="Verdana, Arial, Helvetica, sans-serif" size="4">,
shown at right) has one unshared pair of electrons in addition to three
shared pairs. The unshared pair is important. It occupies an orbital, is
repulsed by the shared electrons, and repulses them as well. <b>So NH</b></font><b><sub><font face="Verdana, Arial, Helvetica, sans-serif" size="3">3</font></sub><font face="Verdana, Arial, Helvetica, sans-serif" size="4">
has a total of four regions of electron density. </font></b>
</p>
<br>
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<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">   Your
task:</font></b>
<ul>
<li>
<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Right-click
(or control-click on a Mac) on the image to the right and
select "Annotate". </font></b>
</li>
<li>
<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Choose
EITHER the Lewis OR the ball & stick "plus" structure shown in
the snapshot, and use the "draw a rectangle" button <img src="drawRect.gif">
to draw a box around each region of electron density.</font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">
</font>
</li>
</ul>
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