Physics Book - User contributions [en]

Electronic Energy Levels and Photons

2015-12-05T01:37:37Z

Aashnaps:

The concept that electrons traveled around a central nucleus was one of the most revolutionary discoveries in chemistry. In a classical Bohr model, electrons have discrete energy levels, and can reach higher energy levels by absorbing energy (usually in the form of a photon). Once the electron is exited, it returns to its rest state, emitting photons in the process.

==The Main Ideas==
===The Quantized Nature of Electronic Energy Levels===

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will be negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

A photon falls neither in the category of a particle nor in the category of a wave. A photon behaves like a particle with a velocity, however it has no mass, and ceases to exist once its energy is absorbed. It can be created or destroyed at anytime, and thus cannot truly be considered as being a particle. It can be imagined as a elementary package of energy. It is a product of the wave-particle duality of light, which states that light behaves both as a particle was well as a wave. The relationship between the frequency of the wave of light and the energy contained in the photon can be described using Planck's Constant.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization energy of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this atom, the difference between the the first (-13.6 eV) and second (-3.4 eV) energy level is 10.2 eV. This means that a photon needs to have a minimum energy of 10.2 eV to be absorbed by the electron and excite it.
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

==Examples==

===Photon Absorption===

If a hypothetical ion had the first 4 energy levels of -4, -2.3, -1.9, and -.8 eV, and an electron at rest was struck by a photon with 2.2 eV of energy, what is the highest excited state the electron could be at? How much energy would the photon leave with, if at all?

First, check the amount of energy need to go from the rest energy level to the first excited energy level: -2.3-(-4)= 1.7. 2.2>1.7, so the electron will be excited to at least this state. If 1.7 eV is absorbed, then 2.2-1.7= .5 eV is remaining. Then check if this sufficient to raise it one more energy level. -1.9-(-2.3)= .4. .5 is greater than .4, so the photon also has sufficient energy to raise it to the second energy level. after raising it to the second excited level, the photon has .5-.4= .1 eV of energy remaining. This .1 eV is not sufficient to raise it to the third excited energy level. So, the photon will be at the second excited energy level, and the photon will have .1 eV of energy remaining.

===Photon Emission===

If electrons of energy 12.8 eV are incident on a gas of hydrogen atoms in their ground state, what are the energies of the photons that are emitted by the excited gas?

First, determine that the difference between the rest energy level (-13.6 eV) and the 3rd excited state (-.85 eV) IS 12.75 eV, and the remaining .05 eV is not sufficient to raise it another energy level. Then consider the different paths the electron could take back to its rest position, and calculate the energies of the corresponding photon emissions. Firstly, the electron could return one energy level at a time, releasing a a photon each drop. The differences between each energy level are: 10.2, 1.89, and .66 eV. Alternatively, the electron could drop from the the fourth energy level directly back to the first. This photon would have an energy equal to the difference between the 2 energy levels: 12.75 eV. Also, it could drop from 4th to 2nd to 1st, and the photon that would be emitted between the 4th and 2nd is 2.55. We have already accounted for the drop between the 2nd and 1st. Lastly, the electron could go from 4th to 3rd to 1st. The drop from 4th to 3rd has already been accounted for, and the difference between the 3rd and l is 12.09. In conclusion, all the possible energies for the emitted photons, from highest to lowest are: 12.75, 12.09, 10.2,2.55,1.89, and .66 eV.

==Historical Context==

In the development of atomic theory, Rutherford discovered that atoms have a nucleus through his famous gold foil experiment. Then, Niels Bohr conjectured that electrons only travel in distinct energy levels around the nucleus. In 1913, Niels Bohr proposed a theory for the hydrogen atom based on quantum theory that energy is transferred only in certain well defined quantities. Electrons should move around the nucleus but only in prescribed orbits. When jumping from one orbit to another with lower energy, a light quantum is emitted. Bohr's theory could explain why atoms emitted light in fixed wavelengths.

== See also ==

[[Photons]],
[[Bohr Model]],
[[Electronic Energy Levels]]

===External links===

http://physics.about.com/od/quantumphysics/f/quantumoptics.htm
http://dev.physicslab.org/document.aspx?doctype=3&filename=atomicnuclear_bohrmodelderivation.xml

==References==

https://www.youtube.com/watch?v=Y0048AI5uEQ

Matter and Interactions. 4th Edition.

http://www.nobelprize.org/nobel_prizes/physics/laureates/1922/bohr-facts.html

[[Category:Energy]]

Electronic Energy Levels and Photons

2015-12-02T23:57:25Z

Aashnaps:

Short Description of Topic

==The Main Ideas==
===The Quantized Nature of Electronic Energy Levels===

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will be negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

A photon falls neither in the category of a particle nor in the category of a wave. A photon behaves like a particle with a velocity, however it has no mass, and ceases to exist once its energy is absorbed. It can be created or destroyed at anytime, and thus cannot truly be considered as being a particle. It can be imagined as a elementary package of energy. It is a product of the wave-particle duality of light, which states that light behaves both as a particle was well as a wave. The relationship between the frequency of the wave of light and the energy contained in the photon can be described using Planck's Constant.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization energy of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this atom, the difference between the the first (-13.6 eV) and second (-3.4 eV) energy level is 10.2 eV. This means that a photon needs to have a minimum energy of 10.2 eV to be absorbed by the electron and excite it.
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

==Examples==

===Photon Absorption===

If a hypothetical ion had the first 4 energy levels of -4, -2.3, -1.9, and -.8 eV, and an electron at rest was struck by a photon with 2.2 eV of energy, what is the highest excited state the electron could be at? How much energy would the photon leave with, if at all?

First, check the amount of energy need to go from the rest energy level to the first excited energy level: -2.3-(-4)= 1.7. 2.2>1.7, so the electron will be excited to at least this state. If 1.7 eV is absorbed, then 2.2-1.7= .5 eV is remaining. Then check if this sufficient to raise it one more energy level. -1.9-(-2.3)= .4. .5 is greater than .4, so the photon also has sufficient energy to raise it to the second energy level. after raising it to the second excited level, the photon has .5-.4= .1 eV of energy remaining. This .1 eV is not sufficient to raise it to the third excited energy level. So, the photon will be at the second excited energy level, and the photon will have .1 eV of energy remaining.

===Photon Emission===

If electrons of energy 12.8 eV are incident on a gas of hydrogen atoms in their ground state, what are the energies of the photons that are emitted by the excited gas?

First, determine that the difference between the rest energy level (-13.6 eV) and the 3rd excited state (-.85 eV) IS 12.75 eV, and the remaining .05 eV is not sufficient to raise it another energy level. Then consider the different paths the electron could take back to its rest position, and calculate the energies of the corresponding photon emissions. Firstly, the electron could return one energy level at a time, releasing a a photon each drop. The differences between each energy level are: 10.2, 1.89, and .66 eV. Alternatively, the electron could drop from the the fourth energy level directly back to the first. This photon would have an energy equal to the difference between the 2 energy levels: 12.75 eV. Also, it could drop from 4th to 2nd to 1st, and the photon that would be emitted between the 4th and 2nd is 2.55. We have already accounted for the drop between the 2nd and 1st. Lastly, the electron could go from 4th to 3rd to 1st. The drop from 4th to 3rd has already been accounted for, and the difference between the 3rd and l is 12.09. In conclusion, all the possible energies for the emitted photons, from highest to lowest are: 12.75, 12.09, 10.2,2.55,1.89, and .66 eV.

==Historical Context==

In the development of atomic theory, Rutherford discovered that atoms have a nucleus through his famous gold foil experiment. Then, Niels Bohr conjectured that electrons only travel in distinct energy levels around the nucleus. In 1913, Niels Bohr proposed a theory for the hydrogen atom based on quantum theory that energy is transferred only in certain well defined quantities. Electrons should move around the nucleus but only in prescribed orbits. When jumping from one orbit to another with lower energy, a light quantum is emitted. Bohr's theory could explain why atoms emitted light in fixed wavelengths.

== See also ==

[[Photons]],
[[Bohr Model]],
[[Electronic Energy Levels]]

===External links===

http://physics.about.com/od/quantumphysics/f/quantumoptics.htm
http://dev.physicslab.org/document.aspx?doctype=3&filename=atomicnuclear_bohrmodelderivation.xml

==References==

https://www.youtube.com/watch?v=Y0048AI5uEQ

Matter and Interactions. 4th Edition.

http://www.nobelprize.org/nobel_prizes/physics/laureates/1922/bohr-facts.html

[[Category:Energy]]

Electronic Energy Levels and Photons

2015-12-02T23:56:24Z

Aashnaps:

Short Description of Topic

==The Main Ideas==
===The Quantized Nature of Electronic Energy Levels===

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will be negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

A photon falls neither in the category of a particle nor in the category of a wave. A photon behaves like a particle with a velocity, however it has no mass, and ceases to exist once its energy is absorbed. It can be created or destroyed at anytime, and thus cannot truly be considered as being a particle. It can be imagined as a elementary package of energy. It is a product of the wave-particle duality of light, which states that light behaves both as a particle was well as a wave. The relationship between the frequency of the wave of light and the energy contained in the photon can be described using Planck's Constant.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization energy of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this atom, the difference between the the first (-13.6 eV) and second (-3.4 eV) energy level is 10.2 eV. This means that a photon needs to have a minimum energy of 10.2 eV to be absorbed by the electron and excite it.
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

==Examples==

===Photon Absorption===

If a hypothetical ion had the first 4 energy levels of -4, -2.3, -1.9, and -.8 eV, and an electron at rest was struck by a photon with 2.2 eV of energy, what is the highest excited state the electron could be at? How much energy would the photon leave with, if at all?

First, check the amount of energy need to go from the rest energy level to the first excited energy level: -2.3-(-4)= 1.7. 2.2>1.7, so the electron will be excited to at least this state. If 1.7 eV is absorbed, then 2.2-1.7= .5 eV is remaining. Then check if this sufficient to raise it one more energy level. -1.9-(-2.3)= .4. .5 is greater than .4, so the photon also has sufficient energy to raise it to the second energy level. after raising it to the second excited level, the photon has .5-.4= .1 eV of energy remaining. This .1 eV is not sufficient to raise it to the third excited energy level. So, the photon will be at the second excited energy level, and the photon will have .1 eV of energy remaining.

===Photon Emission===

If electrons of energy 12.8 eV are incident on a gas of hydrogen atoms in their ground state, what are the energies of the photons that are emitted by the excited gas?

First, determine that the difference between the rest energy level (-13.6 eV) and the 3rd excited state (-.85 eV) IS 12.75 eV, and the remaining .05 eV is not sufficient to raise it another energy level. Then consider the different paths the electron could take back to its rest position, and calculate the energies of the corresponding photon emissions. Firstly, the electron could return one energy level at a time, releasing a a photon each drop. The differences between each energy level are: 10.2, 1.89, and .66 eV. Alternatively, the electron could drop from the the fourth energy level directly back to the first. This photon would have an energy equal to the difference between the 2 energy levels: 12.75 eV. Also, it could drop from 4th to 2nd to 1st, and the photon that would be emitted between the 4th and 2nd is 2.55. We have already accounted for the drop between the 2nd and 1st. Lastly, the electron could go from 4th to 3rd to 1st. The drop from 4th to 3rd has already been accounted for, and the difference between the 3rd and l is 12.09. In conclusion, all the possible energies for the emitted photons, from highest to lowest are: 12.75, 12.09, 10.2,2.55,1.89, and .66 eV.

==Historical Context==

In the development of atomic theory, Rutherford discovered that atoms have a nucleus through his famous gold foil experiment. Then, Niels Bohr conjectured that electrons only travel in distinct energy levels around the nucleus. In 1913, Niels Bohr proposed a theory for the hydrogen atom based on quantum theory that energy is transferred only in certain well defined quantities. Electrons should move around the nucleus but only in prescribed orbits. When jumping from one orbit to another with lower energy, a light quantum is emitted. Bohr's theory could explain why atoms emitted light in fixed wavelengths.

== See also ==

[[Photons]],
[[Bohr Model]],
[[Electronic Energy Levels]]

===External links===

http://physics.about.com/od/quantumphysics/f/quantumoptics.htm
http://dev.physicslab.org/document.aspx?doctype=3&filename=atomicnuclear_bohrmodelderivation.xml

==References==

https://www.youtube.com/watch?v=Y0048AI5uEQ

Matter and Interactions. 4th Edition.

In 1913, Niels Bohr proposed a theory for the hydrogen atom based on quantum theory that energy is transferred only in certain well defined quantities. Electrons should move around the nucleus but only in prescribed orbits. When jumping from one orbit to another with lower energy, a light quantum is emitted. Bohr's theory could explain why atoms emitted light in fixed wavelengths.
[[Category:Energy]]

Electronic Energy Levels and Photons

2015-12-02T23:40:38Z

Aashnaps:

Short Description of Topic

==The Main Ideas==
===The Quantized Nature of Electronic Energy Levels===

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will be negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

A photon falls neither in the category of a particle nor in the category of a wave. A photon behaves like a particle with a velocity, however it has no mass, and ceases to exist once its energy is absorbed. It can be created or destroyed at anytime, and thus cannot truly be considered as being a particle. It can be imagined as a elementary package of energy. It is a product of the wave-particle duality of light, which states that light behaves both as a particle was well as a wave. The relationship between the frequency of the wave of light and the energy contained in the photon can be described using Planck's Constant.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization energy of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this atom, the difference between the the first (-13.6 eV) and second (-3.4 eV) energy level is 10.2 eV. This means that a photon needs to have a minimum energy of 10.2 eV to be absorbed by the electron and excite it.
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

===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==

===Photon Absorption===

If a hypothetical ion had the first 4 energy levels of -4, -2.3, -1.9, and -.8 eV, and an electron at rest was struck by a photon with 2.2 eV of energy, what is the highest excited state the electron could be at? How much energy would the photon leave with, if at all?

First, check the amount of energy need to go from the rest energy level to the first excited energy level: -2.3-(-4)= 1.7. 2.2>1.7, so the electron will be excited to at least this state. If 1.7 eV is absorbed, then 2.2-1.7= .5 eV is remaining. Then check if this sufficient to raise it one more energy level. -1.9-(-2.3)= .4. .5 is greater than .4, so the photon also has sufficient energy to raise it to the second energy level. after raising it to the second excited level, the photon has .5-.4= .1 eV of energy remaining. This .1 eV is not sufficient to raise it to the third excited energy level. So, the photon will be at the second excited energy level, and the photon will have .1 eV of energy remaining.

===Photon Emission===

If electrons of energy 12.8 eV are incident on a gas of hydrogen atoms in their ground state, what are the energies of the photons that are emitted by the excited gas?

First, determine that the difference between the rest energy level (-13.6 eV) and the 3rd excited state (-.85 eV) IS 12.75 eV, and the remaining .05 eV is not sufficient to raise it another energy level. Then consider the different paths the electron could take back to its rest position, and calculate the energies of the corresponding photon emissions. Firstly, the electron could return one energy level at a time, releasing a a photon each drop. The differences between each energy level are: 10.2, 1.89, and .66 eV. Alternatively, the electron could drop from the the fourth energy level directly back to the first. This photon would have an energy equal to the difference between the 2 energy levels: 12.75 eV. Also, it could drop from 4th to 2nd to 1st, and the photon that would be emitted between the 4th and 2nd is 2.55. We have already accounted for the drop between the 2nd and 1st. Lastly, the electron could go from 4th to 3rd to 1st. The drop from 4th to 3rd has already been accounted for, and the difference between the 3rd and l is 12.09. In conclusion, all the possible energies for the emitted photons, from highest to lowest are: 12.75, 12.09, 10.2,2.55,1.89, and .66 eV.

===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 ==

[[Photons]],
[[Bohr Model]],
[[Electronic Energy Levels]]

===Further reading===

Books, Articles or other print media on this topic

===External links===

http://physics.about.com/od/quantumphysics/f/quantumoptics.htm
http://dev.physicslab.org/document.aspx?doctype=3&filename=atomicnuclear_bohrmodelderivation.xml

==References==

https://www.youtube.com/watch?v=Y0048AI5uEQ

Matter and Interactions. 4th Edition.

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

Electronic Energy Levels and Photons

2015-12-02T23:23:52Z

Aashnaps:

Short Description of Topic

==The Main Ideas==
===The Quantized Nature of Electronic Energy Levels===

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will be negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

A photon falls neither in the category of a particle nor in the category of a wave. A photon behaves like a particle with a velocity, however it has no mass, and ceases to exist once its energy is absorbed. It can be created or destroyed at anytime, and thus cannot truly be considered as being a particle. It can be imagined as a elementary package of energy. It is a product of the wave-particle duality of light, which states that light behaves both as a particle was well as a wave. The relationship between the frequency of the wave of light and the energy contained in the photon can be described using Planck's Constant.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization energy of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this atom, the difference between the the first (-13.6 eV) and second (-3.4 eV) energy level is 10.2 eV. This means that a photon needs to have a minimum energy of 10.2 eV to be absorbed by the electron and excite it.
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

===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==

===Photon Absorption===

If a hypothetical ion had the first 4 energy levels of -4, -2.3, -1.9, and -.8 eV, and an electron at rest was struck by a photon with 2.2 eV of energy, what is the highest excited state the electron could be at? How much energy would the photon leave with, if at all?

First, check the amount of energy need to go from the rest energy level to the first excited energy level: -2.3-(-4)= 1.7. 2.2>1.7, so the electron will be excited to at least this state. If 1.7 eV is absorbed, then 2.2-1.7= .5 eV is remaining. Then check if this sufficient to raise it one more energy level. -1.9-(-2.3)= .4. .5 is greater than .4, so the photon also has sufficient energy to raise it to the second energy level. after raising it to the second excited level, the photon has .5-.4= .1 eV of energy remaining. This .1 eV is not sufficient to raise it to the third excited energy level. So, the photon will be at the second excited energy level, and the photon will have .1 eV of energy remaining.

===Photon Emission===

If electrons of energy 12.8 eV are incident on a gas of hydrogen atoms in their ground state, what are the energies of the photons that are emitted by the excited gas?

First, determine that the difference between the rest energy level (-13.6 eV) and the 3rd excited state (-.85 eV) IS 12.75 eV, and the remaining .05 eV is not sufficient to raise it another energy level. Then consider the different paths the electron could take back to its rest position, and calculate the energies of the corresponding photon emissions. Firstly, the

===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 ==

[[Photons]],
[[Bohr Model]],
[[Electronic Energy Levels]]

===Further reading===

Books, Articles or other print media on this topic

===External links===

http://physics.about.com/od/quantumphysics/f/quantumoptics.htm
http://dev.physicslab.org/document.aspx?doctype=3&filename=atomicnuclear_bohrmodelderivation.xml

==References==

https://www.youtube.com/watch?v=Y0048AI5uEQ

Matter and Interactions. 4th Edition.

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

Electronic Energy Levels and Photons

2015-12-02T23:08:16Z

Aashnaps:

Short Description of Topic

==The Main Ideas==
===The Quantized Nature of Electronic Energy Levels===

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will be negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

A photon falls neither in the category of a particle nor in the category of a wave. A photon behaves like a particle with a velocity, however it has no mass, and ceases to exist once its energy is absorbed. It can be created or destroyed at anytime, and thus cannot truly be considered as being a particle. It can be imagined as a elementary package of energy. It is a product of the wave-particle duality of light, which states that light behaves both as a particle was well as a wave. The relationship between the frequency of the wave of light and the energy contained in the photon can be described using Planck's Constant.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization energy of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this atom, the difference between the the first (-13.6 eV) and second (-3.4 eV) energy level is 10.2 eV. This means that a photon needs to have a minimum energy of 10.2 eV to be absorbed by the electron and excite it.
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

===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==

===Photon Absorption===

If a hypothetical ion had the first 4 energy levels of -4, -2.3, -1.9, and -.8 eV, and an electron at rest was struck by a photon with 2.2 eV of energy, what is the highest excited state the electron could be at? How much energy would the photon leave with, if at all?

First, check the amount of energy need to go from the rest energy level to the first excited energy level: -2.3-(-4)= 1.7. 2.2>1.7, so the electron will be excited to at least this state. If 1.7 eV is absorbed, then 2.2-1.7= .5 eV is remaining. Then check if this sufficient to raise it one more energy level. -1.9-(-2.3)= .4. .5 is greater than .4, so the photon also has sufficient energy to raise it to the second energy level. after raising it to the second excited level, the photon has .5-.4= .1 eV of energy remaining. This .1 eV is not sufficient to raise it to the third excited energy level. So, the photon will be at the second excited energy level, and the photon will have .1 eV of energy remaining.

===Photon Emission===

===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 ==

[[Photons]]
[[Bohr Model]]
[[Electronic Energy Levels]]

===Further reading===

Books, Articles or other print media on this topic

===External links===

http://physics.about.com/od/quantumphysics/f/quantumoptics.htm
http://dev.physicslab.org/document.aspx?doctype=3&filename=atomicnuclear_bohrmodelderivation.xml

==References==

https://www.youtube.com/watch?v=Y0048AI5uEQ

Matter and Interactions. 4th Edition.

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

Electronic Energy Levels and Photons

2015-12-02T21:22:45Z

Aashnaps:

Short Description of Topic

==The Main Ideas==
===The Quantized Nature of Electronic Energy Levels===

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will be negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

A photon falls neither in the category of a particle nor in the category of a wave. A photon behaves like a particle with a velocity, however it has no mass, and ceases to exist once its energy is absorbed. It can be created or destroyed at anytime, and thus cannot truly be considered as being a particle. It can be imagined as a elementary package of energy. It is a product of the wave-particle duality of light, which states that light behaves both as a particle was well as a wave. The relationship between the frequency of the wave of light and the energy contained in the photon can be described using Planck's Constant.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization energy of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this atom, the difference between the the first (-13.6 eV) and second (-3.4 eV) energy level is 10.2 eV. This means that a photon needs to have a minimum energy of 10.2 eV to be absorbed by the electron and excite it.
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

===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==

===Photon Absorption===

If a hypothetical ion had the first 4 energy levels of -4, -2.3, -1.9, and -.8 eV, and an electron at rest was struck by a photon with 2.2 eV of energy, what is the highest excited state the electron could be at? How much energy would the photon leave with, if at all?

First, check the amount of energy need to go from the rest energy level to the first excited energy level: -2.3-(-4)= 1.7. 2.2>1.7, so the electron will be excited to at least this state. If 1.7 eV is absorbed, then 2.2-1.7= .5 eV is remaining. Then check if this sufficient to raise it one more energy level. -1.9-(-2.3)= .4. .5 is greater than .4, so the photon also has sufficient energy to raise it to the second energy level. after raising it to the second excited level, the photon has .5-.4= .1 eV of energy remaining. This .1 eV is not sufficient to raise it to the third excited energy level. So, the photon will be at the second excited energy level, and the photon will have .1 eV of energy remaining.

===Photon Emission===

===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 ==

[[Photons]]

===Further reading===

Books, Articles or other print media on this topic

===External links===

http://physics.about.com/od/quantumphysics/f/quantumoptics.htm
http://dev.physicslab.org/document.aspx?doctype=3&filename=atomicnuclear_bohrmodelderivation.xml

==References==

https://www.youtube.com/watch?v=Y0048AI5uEQ

Matter and Interactions. 4th Edition.

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

Electronic Energy Levels and Photons

2015-12-02T20:40:33Z

Aashnaps:

Electronic Energy Levels and Photons

2015-12-02T20:15:31Z

Aashnaps:

Electronic Energy Levels and Photons

2015-12-02T20:08:21Z

Aashnaps:

Electronic Energy Levels and Photons

2015-12-02T19:47:31Z

Aashnaps:

Electronic Energy Levels and Photons

2015-12-02T19:19:07Z

Aashnaps:

Electronic Energy Levels and Photons

2015-12-02T19:00:30Z

Aashnaps:

Short Description of Topic

==The Main Idea==

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will me negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. Once the electron absorbs a photon, it is excited by the energy. After the electron is excited, it drops down and releases a photon with the energy difference between the two energy levels. It can drop to any energy level below it, and thus the resulting photons can be of several energies. If the photon gained is the the opposite of the K+U value for the energy level, then the electron is said to have been ionized. The ionization energy of an atom is the energy needed to ionize an electron that is at rest.

===The Nature of a Photon===

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV). If you substitute values of N into the equation you can build the atom shown. As the value of N increases, the space between each energy level decreases. The energy difference between the rest energy level and the first excited energy level is the largest. Because the energy of the rest energy level is -13.6 eV, the ionization of an electron at rest in a hydrogen atom is 13.6 eV. In other words, if the electron at rest absorbs a photon with 13.6 eV, the electron is "freed" from the atom. In this
[[File:hydrogen.png|200px|thumb|left|Hydrogen and its energy levels]]

===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===

Internet resources on this topic

==References==

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

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

Electronic Energy Levels and Photons

2015-12-02T18:42:58Z

Aashnaps:

Short Description of Topic

==The Main Idea==

Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Each electronic energy level is a number that represents the sum of the kinetic and potential energy (K+U). Because the electronic potential energy between the positive protons in the nucleus and the surrounding negative electrons will always be negative, the value of K+U will me negative. Because electrons are only stable at those energy levels, an electron can only absorb certain quantized energies from photons. After the electron is excited, it drops down and releases a photon. It can drop to any energy level below it, and thus the resulting photons can be of several energies.

===A Mathematical Model of the Bohr Hydrogen Atom===

For example, the electronic energy levels for a hydrogen atom can be modeled by the equation: <math>{\frac{-13.6}{N^2}} = {K+U}</math> where '''N''' is the energy level. N=1 is the rest energy level; N=2 is the the first excited energy level; and N=3 is the second level, etc. This formula gives energy levels in terms of electron volts (eV).
[[File:pic1.png|200px|thumb|left|Hydrogen and its energy levels]]

===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===

Internet resources on this topic

==References==

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

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

File:Hydrogen.png

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Aashnaps: Aashnaps uploaded a new version of "File:Hydrogen.png"

Electronic Energy Levels and Photons

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File:Hydrogen.png

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Electronic Energy Levels and Photons

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Electronic Energy Levels and Photons

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File:Hydrogen.gif

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Electronic Energy Levels and Photons

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Aashnaps:

Electronic Energy Levels and Photons

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Electronic Energy Levels and Photons

2015-12-01T06:30:10Z

Aashnaps: Created page with "Short Description of Topic ==The Main Idea== Electrons can be excited by absorbing energy from photons. Electrons can only be excited to certain electronic energy levels. Ea..."

Main Page

2015-12-01T05:05:48Z

Aashnaps:

__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]]
*[[System & Surroundings]]
*[[Newton's First Law of Motion]]
*[[Newton's Second Law of Motion]]
*[[Newton's Third Law of Motion]]
*[[Gravitational Force]]
*[[Electric Force]]
*[[Terminal Speed]]
*[[Simple Harmonic Motion]]
*[[Speed and Velocity]]
*[[Electric Polarization]]

</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]]

</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]]
</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]]
*[[Weight]]
*[[Boiling Point]]
*[[Melting Point]]
</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]]
</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]]
* [[Momentum Principle]]
* [[Impulse Momentum]]
* [[Curving Motion]]
* [[Multi-particle Analysis of Momentum]]
* [[Iterative Prediction]]
* [[Newton's Laws and Linear Momentum]]
* [[Net Force]]
* [[Center of Mass]]
</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 a Change in Rotation]]
* [[Translational Angular Momentum]]
* [[The Angular Momentum Principle]]
* [[Rotational Angular Momentum]]
* [[Total Angular 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]]
*[[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]]
*[[Energy Graphs]]
*[[Air Resistance]]
*[[Electronic Energy Levels]]
*[[Second Law of Thermodynamics and Entropy]]
*[[Specific Heat Capacity]]
*[[Electronic Energy Levels and Photons]]
*[[Energy Density]]
*[[Relativistic Kinetic Energy]]
</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]]
*[[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]]
**[[A Solid Sphere Charged Throughout Its Volume]]
*[[Electric Potential]]
**[[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]]
*[[Electric Force]]
*[[Polarization]]
*[[Charge Motion in Metals]]
*[[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 Force]]
**[[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]]
</div>
</div>

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

===Simple Circuits===
<div class="mw-collapsible-content">
*[[Components]]
*[[Steady State]]
*[[Non Steady State]]
*[[Node Rule]]
*[[Loop Rule]]
*[[Power in a circuit]]
*[[Ammeters,Voltmeters,Ohmmeters]]
*[[Current]]
*[[Ohm's Law]]
*[[Series Circuits]]
*[[RC]]
*[[Circular Loop of Wire]]
*[[RL Circuit]]
*[[LC Circuit]]
*[[Surface Charge Distributions]]
*[[Feedback]]
*[[Transformers]]
*[[Kirchoff's Circuit Laws]]
</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]]
*[[Faraday's Law]]
**[[Curly Electric Fields]]
**[[Inductance]]
**[[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]]
*[[Electromagnetic Propagation]]
**[[Wavelength and Frequency]]
*[[Snell's Law]]
*[[Light Propagation Through a Medium]]
*[[Light Scaterring: Why is the Sky Blue]]
</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>
*[[blahb]]
</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]]
* An overview of [[VPython]]

Main Page

2015-11-30T19:03:40Z

Aashnaps: /* 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.

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===Interactions===
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*[[Kinds of Matter]]
*[[Detecting Interactions]]
*[[Fundamental Interactions]]
*[[System & Surroundings]]
*[[Newton's First Law of Motion]]
*[[Newton's Second Law of Motion]]
*[[Newton's Third Law of Motion]]
*[[Gravitational Force]]
*[[Terminal Velocity and Friction Due to Air]]
*[[Simple Harmonic Motion]]
*[[Speed and Velocity]]
*[[Electric Polarization]]

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===Theory===
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*[[Einstein's Theory of Special Relativity]]
*[[Quantum Theory]]
*[[Big Bang Theory]]

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===Notable Scientists===
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*[[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]]
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===Properties of Matter===
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*[[Mass]]
*[[Velocity]]
*[[Relative Velocity]]
*[[Density]]
*[[Charge]]
*[[Spin]]
*[[SI Units]]
*[[Heat Capacity]]
*[[Specific Heat]]
*[[Wavelength]]
*[[Conductivity]]
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===Contact Interactions===
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* [[Young's Modulus]]
* [[Friction]]
* [[Tension]]
* [[Hooke's Law]]
*[[Centripetal Force and Curving Motion]]
*[[Compression or Normal Force]]
* [[Length and Stiffness of an Interatomic Bond]]
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===Momentum===
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* [[Vectors]]
* [[Kinematics]]
* [[Conservation of Momentum]]
* [[Predicting Change in multiple dimensions]]
* [[Momentum Principle]]
* [[Impulse Momentum]]
* [[Curving Motion]]
* [[Multi-particle Analysis of Momentum]]
* [[Iterative Prediction]]
* [[Newton's Laws and Linear Momentum]]
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===Angular Momentum===
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* [[The Moments of Inertia]]
* [[Rotation]]
* [[Torque]]
*[[Systems with Zero Torque]]
*[[Systems with Nonzero Torque]]
* [[Right Hand Rule]]
* [[Angular Velocity]]
* [[Predicting a Change in Rotation]]
* [[Conservation of Angular Momentum]]
*[[Rotational Angular Momentum]]
*[[Total Angular Momentum]]

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===Energy===
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*[[The Energy Principle]]
*[[Predicting Change]]
*[[Rest Mass Energy]]
*[[Kinetic Energy]]
*[[Potential Energy]]
*[[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]]
*[[Internal Energy]]
*[[Translational, Rotational and Vibrational Energy]]
*[[Franck-Hertz Experiment]]
*[[Power]]
*[[Energy Graphs]]
*[[Air Resistance]]
*[[Electronic Energy Levels]]
*[[Second Law of Thermodynamics and Entropy]]
*[[Specific Heat Capacity]]
*[[Quantized Energy Levels]]
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===Collisions===
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*[[Collisions]]
*[[Maximally Inelastic Collision]]
*[[Elastic Collisions]]
*[[Inelastic Collisions]]
*[[Head-on Collision of Equal Masses]]
*[[Head-on Collision of Unequal Masses]]
*[[Rutherford Experiment and Atomic Collisions]]
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===Fields===
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* [[Electric Field]] of a
** [[Point Charge]]
** [[Electric Dipole]]
** [[Capacitor]]
** [[Charged Rod]]
** [[Charged Ring]]
** [[Charged Disk]]
** [[Charged Spherical Shell]]
** [[Charged Cylinder]]
**[[A Solid Sphere Charged Throughout Its Volume]]
*[[Electric Potential]]
**[[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]]
*[[Electric Force]]
*[[Polarization]]
*[[Charge Motion in Metals]]
*[[Magnetic Field]]
**[[Right-Hand Rule]]
**[[Direction of Magnetic Field]]
**[[Magnetic Field of a Long Straight Wire]]
**[[Magnetic Field of a Loop]]
**[[Bar Magnet]]
**[[Magnetic Force]]
**[[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]]
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===Simple Circuits===
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*[[Components]]
*[[Steady State]]
*[[Non Steady State]]
*[[Node Rule]]
*[[Loop Rule]]
*[[Power in a circuit]]
*[[Ammeters,Voltmeters,Ohmmeters]]
*[[Current]]
*[[Ohm's Law]]
*[[Series Circuits]]
*[[RC]]
*[[Circular Loop of Wire]]
*[[RL Circuit]]
*[[LC Circuit]]
*[[Surface Charge Distributions]]
*[[Feedback]]
*[[Transformers]]
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===Maxwell's Equations===
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*[[Gauss's Flux Theorem]]
**[[Electric Fields]]
**[[Magnetic Fields]]
*[[Ampere's Law]]
**[[Magnetic Field of Coaxial Cable Using Ampere's Law]]
*[[Faraday's Law]]
**[[Curly Electric Fields]]
**[[Inductance]]
**[[Lenz's Law]]
***[[Lenz Effect and the Jumping Ring]]
*[[Ampere-Maxwell Law]]
**[[Superconducters]]
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===Radiation===
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*[[Producing a Radiative Electric Field]]
*[[Sinusoidal Electromagnetic Radiaton]]
*[[Lenses]]
*[[Energy and Momentum Analysis in Radiation]]
*[[Electromagnetic Propagation]]
*[[Snell's Law]]
*[[Light Propagation Through a Medium]]
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===Sound===
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*[[Doppler Effect]]
*[[Nature, Behavior, and Properties of Sound]]
*[[Resonance]]
*[[Sound Barrier]]
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*[[blahb]]
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== 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]]
* An overview of [[VPython]]