Energy graphs and the Bohr model
This page gives a more in-depth explanation of how to use energy graphs to comprehend the Bohr model. It explains how to illustrate excited states and photon emissions or absorptions.
by Caitlin Taylor
The Main Idea
Energy graphs and the Bohr model.
This page gives a more in-depth explanation of how to use energy graphs to comprehend the Bohr model. It specifically explains how to illustrate the various aspects such as excited states and photon emissions or absorptions on the energy graphs as well as what each component corresponds to.
A Mathematical Model
The Bohr Model, as explained in more detail on the Bohr Model wiki, page depicts the atom as a small, positively charged nucleus surrounded by electrons which can only be at certain different distances from the proton to which it is bound. Energy is quantized which means that only orbits with certain radii are allowed.[1] These levels are labeled with integer N, known as quantum number, where the lowest energy state is the ground state. Beyond an energy called the ionization potential the single electron of the hydrogen atom is no longer bound to the atom. The Bohr model works well for very simple atoms such as hydrogen.
Electronic Energy levels of a Hydrogen Atom
E = K + Uelectric
1) [math]\displaystyle{ E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}} }[/math]
2) [math]\displaystyle{ E = {\frac{13.6 eV}{N^2}} }[/math] where N = 1,2,3
A Computational Model
Visualize this topic given this glow script written by matter and interactions Bohr Model Glowscript [3]
Examples
Simple
This Bohr model picture helps you visualize the orbit radii of the different excited states of the hydrogen atom described in the Bohr model. It displays how the distances in orbit radii get increasingly larger. This also means that due to the fact that the distance from the center is much larger, the ionization energy is much less. [2]
This visualization of the orbitals in a more graphical way shows that as the distance from the center becomes larger, the ionization energy is much less. [2]
Middling
This graph explains in more detail how each level corresponds to less energy. If the energy reached zero, the electron would be free from the hydrogen nucleus because no energy is holding it on. The levels get exponentially closer as they approach the ionization energy
Difficult
When energy is added, the electron moves up to the next orbital. This is called atomic excitation. This energy is released as a photon (light energy) and the electron moves back down.
Hydrogen specifically gives of lightwaves with the wavelengths that correspond to red, glue green, and violet.
Connectedness
Though it is not related to my major, one of my favorite classes I took at Georgia Tech was Earth and Atmospheric Sciences. I found it immensely fascinating when I realized that the same ideology is used as described here as is used to determine the composition of things in space. These emission spectra can be utilized to determine the type of elements that are in stars. Without this method, we would not know what stars are composed of. The ability to study the emission spectra gives us the capabilities to understand where stars come from as well as ideas of the origins of our universe. [4]
History
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.
See also
Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?
Further reading
Books, Articles or other print media on this topic
External links
[1][1]
References
1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html
2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html
4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp