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Summary of what you've learned so far
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<font face="Verdana, Arial, Helvetica, sans-serif" size="5" color="#FFFFFF"><strong>Energetic States and Photons:</strong> Summary of what you have learned so far</font>
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<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">1. Different
atoms have different energy levels.<br><br>2. When an atom jumps from
one energy level to a lower one, it emits a photon of a particular
frequency.<br><br>3. The energy of the photon is equal to the difference
between the atom's energy levels. The photon carries the energy that was
previously stored in the atom.<br><br>4. Atoms can also absorb photons
but only if they have exactly the right frequency to match the
difference between the energy levels.<br><br>5. For visible light, the
color of a photon is related to its energy. Blue photons have the most
energy, green photons have less energy, red photons have the least
energy of all. Infrared and ultraviolet photons are invisible. Infrared
photons don't have enough energy to stimulate your eye, ultraviolet
photons have too much.<br><br></font>
</p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">For a real
world example of all this think about heating an iron rod. As it gets
hotter and hotter it starts to glow. At first it glows red because it only
has enough energy to emit red photons. As it gets hotter it turns white
because it is now emitting photons of all colors. And before it was even
hot enough to glow, you could feel the heat radiating from it in the form
of invisible, infrared photons. (If you heated it enough the photons would
become invisible again: they would be ultraviolet. But the rod would melt
before it got that hot.)</font>
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<td><img src="lightMainIdea.png" width="98" height="58"></td>
<td><font face="Verdana, Arial, Helvetica, sans-serif" size="4">Now here's a chance to play around and see if you can learn more. In the model below, try changing the energy levels of the atoms and see what happens. Can you make green photons? Can you make ultraviolet ones? Do you think energy is conserved in these interactions?</font></td>
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<font face="Verdana, Arial, Helvetica, sans-serif" size="4">What happens
if you give an atom multiple energy levels? Try it and see! (You can add
an energy level just double clicking in the energy level diagram.) </font>
<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">In our model
an atom can go from any energy level to any other. If it goes from a
higher level to a lower one, it emits a photon; to go from a low energy
level to a higher one it has to absorb a photon. In either case, the
energy exactly balances -- the energy of the photon is always equal to
the difference between the energies of the two atomic levels. <strong>This
means that every atom has a unique and characteristic set of photons
that it can either emit or absorb, corresponding to all the possible
differences between its energy levels. </strong></font>
</p>
<p>
<font face="Verdana, Arial, Helvetica, sans-serif" size="4">So just by
looking at the photons that are emitted or absorbed by a bunch of atoms,
we can tell which atoms they are! That's a very powerful thing to be
able to do, and it will be the next thing we study in the unit on -- TA
DAH!...</font><br><strong><font face="Verdana, Arial, Helvetica, sans-serif" size="6" color="red">Spectroscopy!
</font></strong>
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