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Chemical Bonds: Simplified surface view of a molecule.
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<font face="Verdana, Arial, Helvetica, sans-serif" size="5" color="#FFFFFF"><strong>Chemical Bonds:</strong> Simplified surface view of a molecule.</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">The three major categories of bond types are: non-polar covalent, polar covalent, and ionic. Electronegativity, the ability for an atom to attract another atom's electrons, is the key to which bond will form. Below is an introduction to one way of visualizing the way electrons are shared (or not) between atoms.</font></td>
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<font face="Verdana, Arial, Helvetica, sans-serif" size="4">This is
a view of the simplest two atom molecule. In the next few pages you
will explore the types of bonds that can form between two atoms. To
facilitate your understanding, a simplified view of the electrons
will be shown. </font>
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<img src="surfaceDiagramComp.png" width="343" height="123">
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<img src="surfaceChargeComp.png" width="209" height="332">
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<font face="Verdana, Arial, Helvetica, sans-serif" size="4">The
three main categories of bonds (non-polar covalent, polar covalent,
and ionic) are formed when electrons are shared in varying degrees
between atoms. The sharing can be as follows:</font>
<ul>
<li>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">completely
equal or only slightly unequal sharing </font>
</li>
<li>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">somewhat
unequal sharing </font>
</li>
<li>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">so
imbalanced that we don't really consider the electrons to be
shared, but instead they are thought of as transferred from one
atom to another</font>
</li>
</ul>
<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">When
electrons are shared evenly, the entire surface of the molecule
shows no imbalance of charge. However, when electrons tend to be
found closer to one atom versus another, the surface of the
molecule near the atom with the better hold on the electrons
becomes relatively more negative than the surface near the other
atom (which becomes relatively positive). </font>
</p>
<br>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4"><strong>Electronegativity
is the term used to describe how well an atom attracts electrons
from another atom.</strong> </font>
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<font face="Verdana, Arial, Helvetica, sans-serif" color="#000000" size="4">The
picture of a molecule that is colored slightly red and blue shows a bond
between two atoms. One atom has a higher electronegativity than the other.</font><font face="Verdana, Arial, Helvetica, sans-serif" color="#660000" size="4">
<strong>Right-click (or control click) on the red-white-and-blue molecule,
select "annotate" from the popup menu, and use the annotation tools ( <img src="textAnnotation.gif" height="15" width="16">
 <img src="drawLine.gif" height="14" width="15">  <img src="drawRect.gif" height="12" width="16">
) at the top of the new window to label which atom has the higher
electronegativity. Explain your choice in the text area below the picture.</strong></font>
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