Physics Book - User contributions [en]

Energy graphs and the Bohr model

2015-12-06T04:40:17Z

Caitlintaylor: /* See also */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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==

Ernest Rutherford created the Rutherford Model in 1911 which consisted of a planetary-model atom. His model had flaws including the fact that he thought the electron would lose energy gradually causing it to spiral inwards.
However, in 1913 Niehls Bohr proposed the Bohr Model which suggested new ideas regarding the motion of electrons. These new ideas fixed the flaws in the Rutherford Model but are oversimplifications of reality.
In 1925, a more accurate model of electron motion was proposed by Werner Heisenberg called quantum mechanics.
Today, the Bohr model is taught as a simplified way to understand the mechanics of electrons and can be used fairly accurately in simply elements such as hydrogen, consisting of one single electron.
A more complete history can be found on the main Bohr Model page.

== See also ==

Bohr Model Main Page

===External links===
[1][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp
[[Category:Energy]]

Energy graphs and the Bohr model

2015-12-06T04:39:55Z

Caitlintaylor: /* History */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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==

Ernest Rutherford created the Rutherford Model in 1911 which consisted of a planetary-model atom. His model had flaws including the fact that he thought the electron would lose energy gradually causing it to spiral inwards.
However, in 1913 Niehls Bohr proposed the Bohr Model which suggested new ideas regarding the motion of electrons. These new ideas fixed the flaws in the Rutherford Model but are oversimplifications of reality.
In 1925, a more accurate model of electron motion was proposed by Werner Heisenberg called quantum mechanics.
Today, the Bohr model is taught as a simplified way to understand the mechanics of electrons and can be used fairly accurately in simply elements such as hydrogen, consisting of one single electron.
A more complete history can be found on the main Bohr Model page.

== 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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp
[[Category:Energy]]

Energy graphs and the Bohr model

2015-12-06T04:39:00Z

Caitlintaylor:

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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==

Ernest Rutherford created the Rutherford Model in 1911 which consisted of a planetary-model atom. His model had flaws including the fact that he thought the electron would lose energy gradually causing it to spiral inwards.
However, in 1913 Niehls Bohr proposed the Bohr Model which suggested new ideas regarding the motion of electrons. These new ideas fixed the flaws in the Rutherford Model but are oversimplifications of reality.
In 1925, a more accurate model of electron motion was proposed by Werner Heisenberg called quantum mechanics.
Today, the Bohr model is taught as a simplified way to understand the mechanics of electrons and can be used fairly accurately in simply elements such as hydrogen, consisting of one single electron.

== 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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp
[[Category:Energy]]

Energy graphs and the Bohr model

2015-12-06T04:38:50Z

Caitlintaylor: /* History */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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==

Ernest Rutherford created the Rutherford Model in 1911 which consisted of a planetary-model atom. His model had flaws including the fact that he thought the electron would lose energy gradually causing it to spiral inwards.
However, in 1913 Niehls Bohr proposed the Bohr Model which suggested new ideas regarding the motion of electrons. These new ideas fixed the flaws in the Rutherford Model but are oversimplifications of reality.
In 1925, a more accurate model of electron motion was proposed by Werner Heisenberg called quantum mechanics.
Today, the Bohr model is taught as a simplified way to understand the mechanics of electrons and can be used fairly accurately in simply elements such as hydrogen, consisting of one single electron.

== 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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp
[[Category:Energy]]

Energy graphs and the Bohr model

2015-12-06T04:38:16Z

Caitlintaylor:

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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==

Ernest Rutherford created the Rutherford Model in 1911 which consisted of a planetary-model atom. His model had flaws including the fact that he thought the electron would lose energy gradually causing it to spiral inwards.
However, in 1913 Niehls Bohr proposed the Bohr Model which suggested new ideas regarding the motion of electrons. These new ideas fixed the flaws in the Rutherford Model but are oversimplifications of reality.
In 1925, a more accurate model of electron motion was proposed by Werner Heisenberg called quantum mechanics.
Today, the Bohr model is taught as a simplified way to understand the mechanics of electrons and can be used fairly accurately in simply elements such as hydrogen, consisting of one single electron.

== 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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp
[[Category:Energy]]

Energy graphs and the Bohr model

2015-12-06T04:37:41Z

Caitlintaylor: /* History */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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==

Ernest Rutherford created the Rutherford Model in 1911 which consisted of a planetary-model atom. His model had flaws including the fact that he thought the electron would lose energy gradually causing it to spiral inwards.
However, in 1913 Niehls Bohr proposed the Bohr Model which suggested new ideas regarding the motion of electrons. These new ideas fixed the flaws in the Rutherford Model but are oversimplifications of reality.
In 1925, a more accurate model of electron motion was proposed by Werner Heisenberg called quantum mechanics.
Today, the Bohr model is taught as a simplified way to understand the mechanics of electrons and can be used fairly accurately in simply elements such as hydrogen, consisting of one single electron.

== 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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp
[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T04:31:08Z

Caitlintaylor: /* References */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

4. http://skyserver.sdss.org/dr1/en/proj/advanced/spectraltypes/lines.asp
[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T04:30:56Z

Caitlintaylor: /* Connectedness */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T04:22:04Z

Caitlintaylor: /* Difficult */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]

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.

[[File:colorbohr3.jpg]]

Hydrogen specifically gives of lightwaves with the wavelengths that correspond to red, glue green, and violet.

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T04:21:42Z

Caitlintaylor:

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]
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.

[[File:colorbohr3.jpg]]
Hydrogen specifically gives of lightwaves with the wavelengths that correspond to red, glue green, and violet.

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T04:21:27Z

Caitlintaylor:

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.

images and content 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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]
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.

[[File:colorbohr3.jpg]]
Hydrogen specifically gives of lightwaves with the wavelengths that correspond to red, glue green, and violet.

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T04:21:11Z

Caitlintaylor: /* Examples */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]

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===
[[File:bohrmedium.jpg]]

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===

[[File:excitation.jpg]]
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.

[[File:colorbohr3.jpg]]
Hydrogen specifically gives of lightwaves with the wavelengths that correspond to red, glue green, and violet.

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T04:11:56Z

Caitlintaylor: /* Examples */

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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> 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 [http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels Bohr Model Glowscript]
[3]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

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]

[[File:ionizationenergy.jpg]]
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===
[[File:bohrmedium.jpg]]
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===

[[File:excitation.jpg]]
[[File:colorbohr3.jpg]]

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

3. http://www.glowscript.org/#/user/matterandinteractions/folder/matterandinteractions/program/08-Bohr-levels

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T03:50:14Z

Caitlintaylor: /* References */

Energy graphs and the Bohr model

2015-12-06T03:50:00Z

Caitlintaylor: /* The Main Idea */

Energy graphs and the Bohr model

2015-12-06T03:41:41Z

Caitlintaylor: /* A Computational Model */

Energy graphs and the Bohr model

2015-12-06T03:37:52Z

Caitlintaylor: /* Difficult */

File:Colorbohr3.jpg

2015-12-06T03:37:34Z

Caitlintaylor:

Energy graphs and the Bohr model

2015-12-06T03:31:57Z

Caitlintaylor: /* Difficult */

File:Colorbohr2.jpg

2015-12-06T03:31:31Z

Caitlintaylor:

Energy graphs and the Bohr model

2015-12-06T03:30:19Z

Caitlintaylor: /* Middling */

Energy graphs and the Bohr model

2015-12-06T03:30:05Z

Caitlintaylor: /* Difficult */

File:Excitation.jpg

2015-12-06T03:29:47Z

Caitlintaylor:

Energy graphs and the Bohr model

2015-12-06T03:15:46Z

Caitlintaylor: /* Difficult */

File:Colorbohr.jpg

2015-12-06T03:15:37Z

Caitlintaylor:

Energy graphs and the Bohr model

2015-12-06T03:03:10Z

Caitlintaylor: /* Middling */

File:Bohrmedium.jpg

2015-12-06T03:02:52Z

Caitlintaylor:

Energy graphs and the Bohr model

2015-12-06T02:47:31Z

Caitlintaylor: /* Simple */

Energy graphs and the Bohr model

2015-12-06T02:46:44Z

Caitlintaylor: /* A Mathematical Model */

Energy graphs and the Bohr model

2015-12-06T02:44:48Z

Caitlintaylor:

Energy graphs and the Bohr model

2015-12-06T02:38:48Z

Caitlintaylor: /* References */

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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

The Bohr Model, as explained in the Bohr Model wiki page depicts the atom as a small, positively charged nucleus surrounded by electrons. In the Bohr Model, electrons 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, while orbits in between simply don't exist.[1] These levels are knows an quantized energy levels and are labeled with integer N known as quantum number where the lowest energy state is the ground state. As the electrons become further away from the nucleus, they become larger and have higher energy. 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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
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]

----
[[File:ionizationenergy.jpg]]

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html
----

2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T02:38:33Z

Caitlintaylor: /* References */

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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

The Bohr Model, as explained in the Bohr Model wiki page depicts the atom as a small, positively charged nucleus surrounded by electrons. In the Bohr Model, electrons 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, while orbits in between simply don't exist.[1] These levels are knows an quantized energy levels and are labeled with integer N known as quantum number where the lowest energy state is the ground state. As the electrons become further away from the nucleus, they become larger and have higher energy. 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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
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]

----
[[File:ionizationenergy.jpg]]

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

This section contains the the references you used while writing this page
1. http://csep10.phys.utk.edu/astr162/lect/light/bohr.html
2. http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T02:38:03Z

Caitlintaylor: /* Simple */

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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

The Bohr Model, as explained in the Bohr Model wiki page depicts the atom as a small, positively charged nucleus surrounded by electrons. In the Bohr Model, electrons 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, while orbits in between simply don't exist.[1] These levels are knows an quantized energy levels and are labeled with integer N known as quantum number where the lowest energy state is the ground state. As the electrons become further away from the nucleus, they become larger and have higher energy. 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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
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]

----
[[File:ionizationenergy.jpg]]

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T02:33:36Z

Caitlintaylor: /* External links */

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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

The Bohr Model, as explained in the Bohr Model wiki page depicts the atom as a small, positively charged nucleus surrounded by electrons. In the Bohr Model, electrons 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, while orbits in between simply don't exist.[1] These levels are knows an quantized energy levels and are labeled with integer N known as quantum number where the lowest energy state is the ground state. As the electrons become further away from the nucleus, they become larger and have higher energy. 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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
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.

----
[[File:ionizationenergy.jpg]]

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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][http://csep10.phys.utk.edu/astr162/lect/light/bohr.html]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T02:32:57Z

Caitlintaylor:

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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

The Bohr Model, as explained in the Bohr Model wiki page depicts the atom as a small, positively charged nucleus surrounded by electrons. In the Bohr Model, electrons 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, while orbits in between simply don't exist.[1] These levels are knows an quantized energy levels and are labeled with integer N known as quantum number where the lowest energy state is the ground state. As the electrons become further away from the nucleus, they become larger and have higher energy. 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> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
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.

----
[[File:ionizationenergy.jpg]]

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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===
[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T02:27:09Z

Caitlintaylor: /* Simple */

by Caitlin Taylor

[[File:[Example.jpg]]]==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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

Electronic Energy levels of a Hydrogen Atom

E = K + Uelectric

1)
<math> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
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.

----
[[File:ionizationenergy.jpg]]

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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===
[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

File:Ionizationenergy.jpg

2015-12-06T02:26:52Z

Caitlintaylor:

Energy graphs and the Bohr model

2015-12-06T02:25:30Z

Caitlintaylor: /* Simple */

by Caitlin Taylor

[[File:[Example.jpg]]]==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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

Electronic Energy levels of a Hydrogen Atom

E = K + Uelectric

1)
<math> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
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.

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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===
[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T02:14:28Z

Caitlintaylor: /* Examples */

by Caitlin Taylor

[[File:[Example.jpg]]]==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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

Electronic Energy levels of a Hydrogen Atom

E = K + Uelectric

1)
<math> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==
===Simple===
[[File:hydrogenenergylevels.jpg]]

----
This Bohr model picture helps you visualize the orbit radii of the different excited states of the hydrogen aton described in the bohr model.

===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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===
[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

File:Hydrogenenergylevels.jpg

2015-12-06T02:07:15Z

Caitlintaylor: hydrogen energy levels diagram

hydrogen energy levels diagram

Energy graphs and the Bohr model

2015-12-06T01:42:31Z

Caitlintaylor: /* A Mathematical Model */

by Caitlin Taylor

[[File:[Example.jpg]]]==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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

Electronic Energy levels of a Hydrogen Atom

E = K + Uelectric

1)
<math> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==

Be sure to show all steps in your solution and include diagrams whenever possible

===Simple===
===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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===
[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T01:42:04Z

Caitlintaylor: /* The Main Idea */

by Caitlin Taylor

[[File:[Example.jpg]]]==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 explains how to illustrate excited states and photon emissions or absorptions.

===A Mathematical Model===

Electronic Energy levels of a Hydrogen Atom

E = K + Uelectric

1)
<math> E = {\frac{mv^2}{2}} - {\frac{{\frac{1}{2}}*{\frac{1}{4π ε0}}*{\frac{me^2}{h*}}}{N^2}}</math>

2)
<math> E = {\frac{13.6 eV}{N^2}}</math> where N = 1,2,3
What are the mathematical equations that allow us to model this topic. For example <math>{\frac{d\vec{p}}{dt}}_{system} = \vec{F}_{net}</math> where '''p''' is the momentum of the system and '''F''' is the net force from the surroundings.

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==

Be sure to show all steps in your solution and include diagrams whenever possible

===Simple===
===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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===
[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-06T01:26:52Z

Caitlintaylor:

by Caitlin Taylor

==The Main Idea==

Energy graphs and the Bohr model.
State, in your own words, the main idea for this topic

===A Mathematical Model===

What are the mathematical equations that allow us to model this topic. For example <math>{\frac{d\vec{p}}{dt}}_{system} = \vec{F}_{net}</math> where '''p''' is the momentum of the system and '''F''' is the net force from the surroundings.

===A Computational Model===

How do we visualize or predict using this topic. Consider embedding some vpython code here [https://trinket.io/glowscript/31d0f9ad9e Teach hands-on with GlowScript]

==Examples==

Be sure to show all steps in your solution and include diagrams whenever possible

===Simple===
===Middling===
===Difficult===

==Connectedness==
#How is this topic connected to something that you are interested in?
#How is it connected to your major?
#Is there an interesting industrial application?

==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===
[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]

==References==

This section contains the the references you used while writing this page

[[Category:Which Category did you place this in?]]

Energy graphs and the Bohr model

2015-12-03T20:31:12Z

Caitlintaylor: Created page with "Caitlin Taylor Short Description of Topic Contents [hide] 1 The Main Idea 1.1 A Mathematical Model 1.2 A Computational Model 2 Examples 2.1 Simple 2.2 Middling 2.3 Difficul..."

Caitlin Taylor

Short Description of Topic

Contents [hide]
1 The Main Idea
1.1 A Mathematical Model
1.2 A Computational Model
2 Examples
2.1 Simple
2.2 Middling
2.3 Difficult
3 Connectedness
4 History
5 See also
5.1 Further reading
5.2 External links
6 References
The Main Idea[edit]
State, in your own words, the main idea for this topic Electric Field of Capacitor

A Mathematical Model[edit]
What are the mathematical equations that allow us to model this topic. For example dp⃗ dtsystem=F⃗ net where p is the momentum of the system and F is the net force from the surroundings.

A Computational Model[edit]
How do we visualize or predict using this topic. Consider embedding some vpython code here Teach hands-on with GlowScript

Examples[edit]
Be sure to show all steps in your solution and include diagrams whenever possible

Simple[edit]
Middling[edit]
Difficult[edit]
Connectedness[edit]
How is this topic connected to something that you are interested in?
How is it connected to your major?
Is there an interesting industrial application?
History[edit]
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.

See also[edit]
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[edit]
Books, Articles or other print media on this topic

External links[edit]
[1]

References[edit]
This section contains the the references you used while writing this page

Main Page

2015-12-03T20:30:12Z

Caitlintaylor: /* Energy */

__NOTOC__
Welcome to the Georgia Tech Wiki for Intro Physics. This resources was created so that students can contribute and curate content to help those with limited or no access to a textbook. When reading this website, please correct any errors you may come across. If you read something that isn't clear, please consider revising it!

Looking to make a contribution?
#Pick a specific topic from intro physics
#Add that topic, as a link to a new page, under the appropriate category listed below by editing this page.
#Copy and paste the default [[Template]] into your new page and start editing.

Please remember that this is not a textbook and you are not limited to expressing your ideas with only text and equations. Whenever possible embed: pictures, videos, diagrams, simulations, computational models (e.g. Glowscript), and whatever content you think makes learning physics easier for other students.

== Source Material ==
All of the content added to this resource must be in the public domain or similar free resource. If you are unsure about a source, contact the original author for permission. That said, there is a surprisingly large amount of introductory physics content scattered across the web. Here is an incomplete list of intro physics resources (please update as needed).
* A physics resource written by experts for an expert audience [https://en.wikipedia.org/wiki/Portal:Physics Physics Portal]
* A wiki book on modern physics [https://en.wikibooks.org/wiki/Modern_Physics Modern Physics Wiki]
* The MIT open courseware for intro physics [http://ocw.mit.edu/resources/res-8-002-a-wikitextbook-for-introductory-mechanics-fall-2009/index.htm MITOCW Wiki]
* An online concept map of intro physics [http://hyperphysics.phy-astr.gsu.edu/hbase/hph.html HyperPhysics]
* Interactive physics simulations [https://phet.colorado.edu/en/simulations/category/physics PhET]
* OpenStax algebra based intro physics textbook [https://openstaxcollege.org/textbooks/college-physics College Physics]
* The Open Source Physics project is a collection of online physics resources [http://www.opensourcephysics.org/ OSP]
* A resource guide compiled by the [http://www.aapt.org/ AAPT] for educators [http://www.compadre.org/ ComPADRE]

== Organizing Categories ==
These are the broad, overarching categories, that we cover in two semester of introductory physics. You can add subcategories or make a new category as needed. A single topic should direct readers to a page in one of these catagories.

<div class="toccolours mw-collapsible mw-collapsed">
===Interactions===
<div class="mw-collapsible-content">
*[[Kinds of Matter]]
**[[Ball and Spring Model of Matter]]
*[[Detecting Interactions]]
*[[Fundamental Interactions]]
*[[Determinism]]
*[[System & Surroundings]]
*[[Newton's First Law of Motion]]
*[[Newton's Second Law of Motion]]
*[[Newton's Third Law of Motion]]
*[[Gravitational Force]]
*[[Electric Force]]
*[[Conservation of Energy]]
*[[Conservation of Charge]]
*[[Terminal Speed]]
*[[Simple Harmonic Motion]]
*[[Speed and Velocity]]
*[[Electric Polarization]]
*[[Perpetual Freefall (Orbit)]]
*[[2-Dimensional Motion]]
*[[Center of Mass]]
*[[Reaction Time]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Theory===
<div class="mw-collapsible-content">
*[[Einstein's Theory of Special Relativity]]
*[[Quantum Theory]]
*[[Big Bang Theory]]
*[[Maxwell's Electromagnetic Theory]]
*[[Atomic Theory]]
*[[String Theory]]
*[[Elementary Particles and Particle Physics Theory]]
*[[Law of Gravitation]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Notable Scientists===
<div class="mw-collapsible-content">
*[[Christian Doppler]]
*[[Albert Einstein]]
*[[Ernest Rutherford]]
*[[Joseph Henry]]
*[[Michael Faraday]]
*[[J.J. Thomson]]
*[[James Maxwell]]
*[[Robert Hooke]]
*[[Carl Friedrich Gauss]]
*[[Nikola Tesla]]
*[[Andre Marie Ampere]]
*[[Sir Isaac Newton]]
*[[J. Robert Oppenheimer]]
*[[Oliver Heaviside]]
*[[Rosalind Franklin]]
*[[Erwin Schrödinger]]
*[[Enrico Fermi]]
*[[Robert J. Van de Graaff]]
*[[Charles de Coulomb]]
*[[Hans Christian Ørsted]]
*[[Philo Farnsworth]]
*[[Niels Bohr]]
*[[Georg Ohm]]
*[[Galileo Galilei]]
*[[Gustav Kirchhoff]]
*[[Max Planck]]
*[[Heinrich Hertz]]
*[[Edwin Hall]]
*[[James Watt]]
*[[Count Alessandro Volta]]
*[[Josiah Willard Gibbs]]
*[[Richard Phillips Feynman]]
*[[Sir David Brewster]]
*[[Daniel Bernoulli]]
*[[William Thomson]]
*[[Leonhard Euler]]
*[[Robert Fox Bacher]]
*[[Stephen Hawking]]
*[[Amedeo Avogadro]]
*[[Wilhelm Conrad Roentgen]]
*[[Pierre Laplace]]
*[[Thomas Edison]]
*[[Hendrik Lorentz]]
*[[Jean-Baptiste Biot]]
*[[Lise Meitner]]
*[[Lisa Randall]]
*[[Felix Savart]]
*[[Heinrich Lenz]]
*[[Max Born]]
*[[Archimedes]]
*[[Jean Baptiste Biot]]
*[[Carl Sagan]]
*[[Eugene Wigner]]
*[[Marie Curie]]
*[[Pierre Curie]]
*[[Werner Heisenberg]]
*[[Johannes Diderik van der Waals]]
*[[Louis de Broglie]]
*[[Aristotle]]
*[[Émilie du Châtelet]]
*[[Blaise Pascal]]
*[[Benjamin Franklin]]
*[[James Chadwick]]
*[[Henry Cavendish]]
*[[Thomas Young]]
*[[James Prescott Joule]]
*[[John Bardeen]]
*[[Leo Baekeland]]
*[[Alhazen]]
*[[Willebrod Snell]]
*[[Johannes Kepler]]
*[[Johann Wilhelm Ritter]]
*[[Philipp Lenard]]
*[[Xuesen Qian]]

</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Properties of Matter===
<div class="mw-collapsible-content">
*[[Mass]]
*[[Velocity]]
*[[Relative Velocity]]
*[[Density]]
*[[Charge]]
*[[Spin]]
*[[SI Units]]
*[[Heat Capacity]]
*[[Specific Heat]]
*[[Wavelength]]
*[[Conductivity]]
*[[Malleability]]
*[[Weight]]
*[[Boiling Point]]
*[[Melting Point]]
*[[Inertia]]
*[[Non-Newtonian Fluids]]
*[[Color]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Contact Interactions===
<div class="mw-collapsible-content">
* [[Young's Modulus]]
* [[Friction]]
* [[Tension]]
* [[Hooke's Law]]
*[[Centripetal Force and Curving Motion]]
*[[Compression or Normal Force]]
* [[Length and Stiffness of an Interatomic Bond]]
* [[Speed of Sound in a Solid]]
* [[Iterative Prediction of Spring-Mass System]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Momentum===
<div class="mw-collapsible-content">
* [[Vectors]]
* [[Kinematics]]
* [[Conservation of Momentum]]
* [[Predicting Change in multiple dimensions]]
* [[Derivation of the Momentum Principle]]
* [[Momentum Principle]]
* [[Impulse Momentum]]
* [[Curving Motion]]
* [[Multi-particle Analysis of Momentum]]
* [[Iterative Prediction]]
* [[Analytical Prediction]]
* [[Newton's Laws and Linear Momentum]]
* [[Net Force]]
* [[Center of Mass]]
* [[Momentum at High Speeds]]
* [[Change in Momentum in Time for Curving Motion]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Angular Momentum===
<div class="mw-collapsible-content">
* [[The Moments of Inertia]]
* [[Moment of Inertia for a ring]]
* [[Rotation]]
* [[Torque]]
* [[Systems with Zero Torque]]
* [[Systems with Nonzero Torque]]
* [[Right Hand Rule]]
* [[Angular Velocity]]
* [[Predicting the Position of a Rotating System]]
* [[Translational Angular Momentum]]
* [[The Angular Momentum Principle]]
* [[Angular Momentum of Multiparticle Systems]]
* [[Rotational Angular Momentum]]
* [[Total Angular Momentum]]
* [[Gyroscopes]]
* [[Angular Momentum Compared to Linear Momentum]]

</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Energy===
<div class="mw-collapsible-content">
*[[The Photoelectric Effect]]
*[[Photons]]
*[[The Energy Principle]]
*[[Predicting Change]]
*[[Rest Mass Energy]]
*[[Kinetic Energy]]
*[[Potential Energy]]
**[[Potential Energy for a Magnetic Dipole]]
**[[Potential Energy of a Multiparticle System]]
*[[Work]]
*[[Thermal Energy]]
*[[Conservation of Energy]]
*[[Electric Potential]]
*[[Energy Transfer due to a Temperature Difference]]
*[[Gravitational Potential Energy]]
*[[Point Particle Systems]]
*[[Real Systems]]
*[[Spring Potential Energy]]
**[[Ball and Spring Model]]
*[[Internal Energy]]
**[[Potential Energy of a Pair of Neutral Atoms]]
*[[Translational, Rotational and Vibrational Energy]]
*[[Franck-Hertz Experiment]]
*[[Power (Mechanical)]]
*[[Transformation of Energy]]

*[[Energy Graphs]]
**[[Energy graphs and the Bohr model]]
*[[Air Resistance]]
*[[Electronic Energy Levels]]
*[[Second Law of Thermodynamics and Entropy]]
*[[Specific Heat Capacity]]
*[[Electronic Energy Levels and Photons]]
*[[Energy Density]]
*[[Bohr Model]]
*[[Quantized energy levels]]
*[[Path Independence of Electric Potential]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Collisions===
<div class="mw-collapsible-content">
*[[Collisions]]
*[[Maximally Inelastic Collision]]
*[[Elastic Collisions]]
*[[Inelastic Collisions]]
*[[Head-on Collision of Equal Masses]]
*[[Head-on Collision of Unequal Masses]]
*[[Frame of Reference]]
*[[Rutherford Experiment and Atomic Collisions]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Fields===
<div class="mw-collapsible-content">
* [[Electric Field]] of a
** [[Point Charge]]
** [[Electric Dipole]]
** [[Capacitor]]
** [[Charged Rod]]
** [[Charged Ring]]
** [[Charged Disk]]
** [[Charged Spherical Shell]]
** [[Charged Cylinder]]
** [[Charge Density]]
**[[A Solid Sphere Charged Throughout Its Volume]]
*[[Electric Potential]]
**[[Potential Difference Path Independence]]
**[[Potential Difference in a Uniform Field]]
**[[Potential Difference of point charge in a non-Uniform Field]]
**[[Sign of Potential Difference]]
**[[Potential Difference in an Insulator]]
**[[Energy Density and Electric Field]]
** [[Systems of Charged Objects]]
*[[Electric Force]]
*[[Polarization]]
**[[Polarization of an Atom]]
*[[Charge Motion in Metals]]
*[[Charge Transfer]]
*[[Magnetic Field]]
**[[Right-Hand Rule]]
**[[Direction of Magnetic Field]]
**[[Magnetic Field of a Long Straight Wire]]
**[[Magnetic Field of a Loop]]
**[[Magnetic Field of a Solenoid]]
**[[Bar Magnet]]
**[[Magnetic Dipole Moment]]
***[[Stern-Gerlach Experiment]]
**[[Magnetic Force]]
**[[Earth's Magnetic Field]]
*[[Combining Electric and Magnetic Forces]]
**[[Magnetic Torque]]
**[[Hall Effect]]
**[[Lorentz Force]]
**[[Biot-Savart Law]]
**[[Biot-Savart Law for Currents]]
**[[Integration Techniques for Magnetic Field]]
**[[Sparks in Air]]
**[[Motional Emf]]
**[[Detecting a Magnetic Field]]
**[[Moving Point Charge]]
**[[Non-Coulomb Electric Field]]
**[[Motors and Generators]]
**[[Solenoid Applications]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Simple Circuits===
<div class="mw-collapsible-content">
*[[Components]]
*[[Steady State]]
*[[Non Steady State]]
*[[Charging and Discharging a Capacitor]]
*[[Thin and Thick Wires]]
*[[Node Rule]]
*[[Loop Rule]]
*[[Resistivity]]
*[[Power in a circuit]]
*[[Ammeters,Voltmeters,Ohmmeters]]
*[[Current]]
**[[AC]]
*[[Ohm's Law]]
*[[Series Circuits]]
*[[Parallel Circuits]]
*[[RC]]
*[[AC vs DC]]
*[[Charge in a RC Circuit]]
*[[Current in a RC circuit]]
*[[Circular Loop of Wire]]
*[[Current in a RL Circuit]]
*[[RL Circuit]]
*[[LC Circuit]]
*[[Surface Charge Distributions]]
*[[Feedback]]
*[[Transformers (Circuits)]]
*[[Resistors and Conductivity]]
*[[Semiconductor Devices]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Maxwell's Equations===
<div class="mw-collapsible-content">
*[[Gauss's Flux Theorem]]
**[[Electric Fields]]
**[[Magnetic Fields]]
*[[Ampere's Law]]
**[[Magnetic Field of Coaxial Cable Using Ampere's Law]]
**[[Magnetic Field of a Long Thick Wire Using Ampere's Law]]
**[[Magnetic Field of a Toroid Using Ampere's Law]]
*[[Faraday's Law]]
**[[Curly Electric Fields]]
**[[Inductance]]
***[[Transformers from a physics standpoint]]
***[[Energy Density]]
**[[Lenz's Law]]
***[[Lenz Effect and the Jumping Ring]]
**[[Motional Emf using Faraday's Law]]
*[[Ampere-Maxwell Law]]
*[[Superconductors]]
**[[Meissner effect]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Radiation===
<div class="mw-collapsible-content">
*[[Producing a Radiative Electric Field]]
*[[Sinusoidal Electromagnetic Radiaton]]
*[[Lenses]]
*[[Energy and Momentum Analysis in Radiation]]
**[[Poynting Vector]]
*[[Electromagnetic Propagation]]
**[[Wavelength and Frequency]]
*[[Snell's Law]]
*[[Effects of Radiation on Matter]]
*[[Light Propagation Through a Medium]]
*[[Light Scaterring: Why is the Sky Blue]]
*[[Light Refraction: Bending of light]]
*[[Cherenkov Radiation]]
</div>
</div>
<div class="toccolours mw-collapsible mw-collapsed">

===Sound===
<div class="mw-collapsible-content">
*[[Doppler Effect]]
*[[Nature, Behavior, and Properties of Sound]]
*[[Resonance]]
*[[Sound Barrier]]
</div>
</div>
<div class="toccolours mw-collapsible mw-collapsed">

===Waves===
<div class="mw-collapsible-content">
*[[Multisource Interference: Diffraction]]
*[[Standing waves]]
*[[Gravitational waves]]
*[[Wave-Particle Duality]]
*[[Electromagnetic Waves]]
*[[Electromagnetic Spectrum]]
*[[Color Light Wave]]
*[[Mechanical Waves]]
*[[Pendulum Motion]]
</div>
</div>
<div class="toccolours mw-collapsible mw-collapsed">

===Real Life Applications of Electromagnetic Principles===
<div class="mw-collapsible-content">
*[[Electromagnetic Junkyard Cranes]]
*[[Maglev Trains]]
*[[Spark Plugs]]
*[[Metal Detectors]]
*[[Speakers]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Optics===
<div class="mw-collapsible-content">
*[[Mirrors]]
</div>
</div>

<div class="toccolours mw-collapsible mw-collapsed">

===Computing===
<div class="mw-collapsible-content">
*[[VPython]]
*[[VPython basics]]
</div>
</div>

== Resources ==
* Commonly used wiki commands [https://en.wikipedia.org/wiki/Help:Cheatsheet Wiki Cheatsheet]
* A guide to representing equations in math mode [https://en.wikipedia.org/wiki/Help:Displaying_a_formula Wiki Math Mode]
* A page to keep track of all the physics [[Constants]]