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Molecular Geometry: Page 5
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<font face="Verdana, Arial, Helvetica, sans-serif" size="5" color="#FFFFFF"><strong>Molecular Geometry:</strong> Predicting Molecular Shapes, part 1</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">If you can predict how regions of electron density will behave, you can design and build some really amazing structures, one atom at a time. </font></td>
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<strong><font face="Verdana, Arial, Helvetica, sans-serif" color="#a65d2c" size="5">Designer
Molecules</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">One of the
newest, coolest areas of chemical science is nanotechnology, the science
of constructing tiny molecular machines. A kind of "building block" for
making the machines is shown at right — <b>a DNA tetrahedron,
designed and constructed in a laboratory, using the principles of
molecular geometry.</b></font>
<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">The
scientists who designed the DNA tetrahedron understand molecular
geometry well enough to <b>predict</b> the ways the atoms and electrons
would form a new molecule. </font>
</p>
<p>
<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">To
predict the shape that a molecule will have, you need to know how many
regions of electron density are around each atom in the molecule. This
information is shown in Lewis electron dot structures. </font></b>
</p>
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<br>
<font face="Verdana, Arial, Helvetica, sans-serif" size="2">A DNA
tetrahedron.<br>(Image by Nanorex, Inc. www.nanorex.com). </font>
</center>
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<img height="23" width="33" src="atomsBullet.png">
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<strong><font face="Verdana, Arial, Helvetica, sans-serif" color="#a65d2c" size="5">Predicting
molecular shape</font></strong>
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<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">By itself, a
chemical formula tells you exactly <b>how many and what kind of atoms
are in a molecule</b>. For example, carbon dioxide's formula, (CO</font><sub><b><font face="Verdana, Arial, Helvetica, sans-serif" size="2">2</font></b></sub><font face="Verdana, Arial, Helvetica, sans-serif" size="4">,
shown below) tells you that it contains one carbon and two oxygen atoms.
But, you get no information as to how the atoms are arranged. </font>
</p>
<p>
<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">That's
where Lewis structures come in. Using your knowledge of molecular
geometry, and working from the Lewis electron dot structure, you can
predict the shapes of molecules. </font></b>
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<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">To predict
the shape of a molecule from a Lewis structure, here's what to do:</font></b>
<ul>
<li>
<b><font face="Verdana, Arial, Helvetica, sans-serif" color="#852219" size="4">Step
1: </font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Note
the central atom in the structure.</font>
</li>
<li>
<b><font face="Verdana, Arial, Helvetica, sans-serif" color="#852219" size="4">Step
2: </font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Count
the regions of electron density surrounding it.</font>
</li>
<li>
<b><font face="Verdana, Arial, Helvetica, sans-serif" color="#852219" size="4">Step
3: </font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Think
about how the electrons will move away from each other to minimize
their repulsions. </font>
</li>
<li>
<b><font face="Verdana, Arial, Helvetica, sans-serif" color="#852219" size="4">Step
4: </font></b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Draw
a conclusion as to the positions the electrons will occupy-- that is,
decide on the electron geometry: linear, trigonal planar, or
tetrahedral. </font>
</li>
</ul>
<blockquote>
<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Follow
these steps, and use the Lewis electron dot structures on this page, to
answer the questions below.</font></b>
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<strong><font face="Arial, Helvetica, sans-serif" color="#852219" size="4">Step
1: </font><font face="Arial, Helvetica, sans-serif" color="#000000" size="4">Look
at the Lewis dot structure for CO<sub>2</sub> (above). What is the central
atom in CO<sub>2</sub>?</font></strong>
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carbon
oxygen
dioxide
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<strong><font face="Arial, Helvetica, sans-serif" color="#852219" size="4">Step
2:</font><font face="Arial, Helvetica, sans-serif" color="#000000" size="4">
How many regions of electron density are there around the central atom in
CO<sub>2</sub>?</font></strong>
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one
two
four
eight
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<strong><font face="Arial, Helvetica, sans-serif" color="#852219" size="4">Step
3: </font><font face="Arial, Helvetica, sans-serif" color="#000000" size="4">Think
about electron repulsions and how regions of electron density arrange
themselves around a central atom. Then...<br></font><font face="Arial, Helvetica, sans-serif" color="#852219" size="4">Step
4: </font><font face="Arial, Helvetica, sans-serif" color="#000000" size="4">Predict
the shape of carbon dioxide: </font></strong>
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linear
trigonal planar
tetrahedral
two-ended
tri-atomic
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<b><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Use the
sequence of steps outlined above to answer the next question.</font></b>
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<strong><font face="Arial, Helvetica, sans-serif" size="4">Predict the
shape of boron trifluoride: </font></strong>
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linear
trigonal planar
tetrahedral
triplanar
flat triatomic
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