http://www.physicsbook.gatech.edu/api.php?action=feedcontributions&feedformat=atom&user=Ccooper71Physics Book - User contributions [en]2026-04-29T05:44:57ZUser contributionsMediaWiki 1.42.7http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16930Quantum Theory2015-12-05T23:50:28Z<p>Ccooper71: </p>
<hr />
<div>Topic Initiated by Erich Hoffstetter (no content added by this user)<br />
<br />
Current Content Created and Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Energy levels.jpg|thumb|Graph illustrating the ground and excited states achieved by electrons with applied radiation. As well, an illustration of how only exact quantities of energy applied have effective results.]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
[[File:Black line spectra.png|thumb|Multiple elements and their corresponding black line regions of the spectrum at wavelengths which their electrons absorb photons.]]<br />
<br />
<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
<br />
<br />
<br />
==Connectedness==<br />
Quantum physics is considered one of the fundamental concepts of modern physics studies, promoting the establishment of fields of study such as elementary particles, condensed matter, superconductivity, nuclear physics, chemistry, and other applications of radiation to matter. Understanding atomic structure and behavior with radiation is an important concept for studying most of the real world. Especially in fields of physical chemistry and even analytical chemistry are further developed by innovations in theory and thinking. From this understanding, instrumental observations of other parts of the solar system may be analyzed more effectively to determine chemical make-up and behavior on other bodies. Applications of absorbance and transmittance are useful in determining chemical composition, concentration, or effective uses of synthesized compounds.<br />
<gallery><br />
File:Energy analysis.png<br />
File:Product determination.png<br />
File:Further study.gif<br />
File:Reactor.gif<br />
</gallery><br />
<br />
<br />
<br />
<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
*[http://hyperphysics.phy-astr.gsu.edu/hbase/mod5.html Quantum Processes] Involving Photon Absorption and Emission<br />
*[http://blogs.jccc.edu/astronomy/textbook/unit-two-conceptual-and-observational-tools-of-astronomy/chapter-5-electromagnetic-radiation-and-matter/ Electromagnetic Radiation and Matter]<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
*"Chapter 5: Electromagnetic Radiation and Matter." Johnson County Community College. Web. 2015.<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16902Quantum Theory2015-12-05T23:48:10Z<p>Ccooper71: </p>
<hr />
<div>Topic Initiated by Erich Hoffstetter (no content)<br />
<br />
Current Content Created and Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Energy levels.jpg|thumb|Graph illustrating the ground and excited states achieved by electrons with applied radiation. As well, an illustration of how only exact quantities of energy applied have effective results.]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
[[File:Black line spectra.png|thumb|Multiple elements and their corresponding black line regions of the spectrum at wavelengths which their electrons absorb photons.]]<br />
<br />
<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
<br />
<br />
<br />
==Connectedness==<br />
Quantum physics is considered one of the fundamental concepts of modern physics studies, promoting the establishment of fields of study such as elementary particles, condensed matter, superconductivity, nuclear physics, chemistry, and other applications of radiation to matter. Understanding atomic structure and behavior with radiation is an important concept for studying most of the real world. Especially in fields of physical chemistry and even analytical chemistry are further developed by innovations in theory and thinking. From this understanding, instrumental observations of other parts of the solar system may be analyzed more effectively to determine chemical make-up and behavior on other bodies. Applications of absorbance and transmittance are useful in determining chemical composition, concentration, or effective uses of synthesized compounds.<br />
<gallery><br />
File:Energy analysis.png<br />
File:Product determination.png<br />
File:Further study.gif<br />
File:Reactor.gif<br />
</gallery><br />
<br />
<br />
<br />
<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
*[http://hyperphysics.phy-astr.gsu.edu/hbase/mod5.html Quantum Processes] Involving Photon Absorption and Emission<br />
*[http://blogs.jccc.edu/astronomy/textbook/unit-two-conceptual-and-observational-tools-of-astronomy/chapter-5-electromagnetic-radiation-and-matter/ Electromagnetic Radiation and Matter]<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
*"Chapter 5: Electromagnetic Radiation and Matter." Johnson County Community College. Web. 2015.<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16897Quantum Theory2015-12-05T23:47:49Z<p>Ccooper71: </p>
<hr />
<div>Topic Initiated by Erich Hoffstetter (no content)<br />
Content Created and Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Energy levels.jpg|thumb|Graph illustrating the ground and excited states achieved by electrons with applied radiation. As well, an illustration of how only exact quantities of energy applied have effective results.]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
[[File:Black line spectra.png|thumb|Multiple elements and their corresponding black line regions of the spectrum at wavelengths which their electrons absorb photons.]]<br />
<br />
<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
<br />
<br />
<br />
==Connectedness==<br />
Quantum physics is considered one of the fundamental concepts of modern physics studies, promoting the establishment of fields of study such as elementary particles, condensed matter, superconductivity, nuclear physics, chemistry, and other applications of radiation to matter. Understanding atomic structure and behavior with radiation is an important concept for studying most of the real world. Especially in fields of physical chemistry and even analytical chemistry are further developed by innovations in theory and thinking. From this understanding, instrumental observations of other parts of the solar system may be analyzed more effectively to determine chemical make-up and behavior on other bodies. Applications of absorbance and transmittance are useful in determining chemical composition, concentration, or effective uses of synthesized compounds.<br />
<gallery><br />
File:Energy analysis.png<br />
File:Product determination.png<br />
File:Further study.gif<br />
File:Reactor.gif<br />
</gallery><br />
<br />
<br />
<br />
<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
*[http://hyperphysics.phy-astr.gsu.edu/hbase/mod5.html Quantum Processes] Involving Photon Absorption and Emission<br />
*[http://blogs.jccc.edu/astronomy/textbook/unit-two-conceptual-and-observational-tools-of-astronomy/chapter-5-electromagnetic-radiation-and-matter/ Electromagnetic Radiation and Matter]<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
*"Chapter 5: Electromagnetic Radiation and Matter." Johnson County Community College. Web. 2015.<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16824Quantum Theory2015-12-05T23:39:53Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Energy levels.jpg|thumb|Graph illustrating the ground and excited states achieved by electrons with applied radiation. As well, an illustration of how only exact quantities of energy applied have effective results.]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
[[File:Black line spectra.png|thumb|Multiple elements and their corresponding black line regions of the spectrum at wavelengths which their electrons absorb photons.]]<br />
<br />
<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
<br />
<br />
<br />
==Connectedness==<br />
Quantum physics is considered one of the fundamental concepts of modern physics studies, promoting the establishment of fields of study such as elementary particles, condensed matter, superconductivity, nuclear physics, chemistry, and other applications of radiation to matter. Understanding atomic structure and behavior with radiation is an important concept for studying most of the real world. Especially in fields of physical chemistry and even analytical chemistry are further developed by innovations in theory and thinking. From this understanding, instrumental observations of other parts of the solar system may be analyzed more effectively to determine chemical make-up and behavior on other bodies. Applications of absorbance and transmittance are useful in determining chemical composition, concentration, or effective uses of synthesized compounds.<br />
<gallery><br />
File:Energy analysis.png<br />
File:Product determination.png<br />
File:Further study.gif<br />
File:Reactor.gif<br />
</gallery><br />
<br />
<br />
<br />
<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
*[http://hyperphysics.phy-astr.gsu.edu/hbase/mod5.html Quantum Processes] Involving Photon Absorption and Emission<br />
*[http://blogs.jccc.edu/astronomy/textbook/unit-two-conceptual-and-observational-tools-of-astronomy/chapter-5-electromagnetic-radiation-and-matter/ Electromagnetic Radiation and Matter]<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
*"Chapter 5: Electromagnetic Radiation and Matter." Johnson County Community College. Web. 2015.<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Reactor.gif&diff=16786File:Reactor.gif2015-12-05T23:36:24Z<p>Ccooper71: </p>
<hr />
<div></div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Further_study.gif&diff=16783File:Further study.gif2015-12-05T23:36:10Z<p>Ccooper71: </p>
<hr />
<div></div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Product_determination.png&diff=16713File:Product determination.png2015-12-05T23:27:50Z<p>Ccooper71: </p>
<hr />
<div></div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Energy_analysis.png&diff=16710File:Energy analysis.png2015-12-05T23:27:34Z<p>Ccooper71: </p>
<hr />
<div></div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16706Quantum Theory2015-12-05T23:27:22Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Energy levels.jpg|thumb|Graph illustrating the ground and excited states achieved by electrons with applied radiation. As well, an illustration of how only exact quantities of energy applied have effective results.]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
[[File:Black line spectra.png|thumb|Multiple elements and their corresponding black line regions of the spectrum at wavelengths which their electrons absorb photons.]]<br />
<br />
<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
<br />
<br />
<br />
==Connectedness==<br />
Quantum physics is considered one of the fundamental concepts of modern physics studies, promoting the establishment of fields of study such as elementary particles, condensed matter, superconductivity, nuclear physics, chemistry, and other applications of radiation to matter. Understanding atomic structure and behavior with radiation is an important concept for studying most of the real world. Especially in fields of physical chemistry and even analytical chemistry are further developed by innovations in theory and thinking. From this understanding, instrumental observations of other parts of the solar system may be analyzed more effectively to determine chemical make-up and behavior on other bodies. Applications of absorbance and transmittance are useful in determining chemical composition, concentration, or effective uses of synthesized compounds.<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
*[http://hyperphysics.phy-astr.gsu.edu/hbase/mod5.html Quantum Processes] Involving Photon Absorption and Emission<br />
*[http://blogs.jccc.edu/astronomy/textbook/unit-two-conceptual-and-observational-tools-of-astronomy/chapter-5-electromagnetic-radiation-and-matter/ Electromagnetic Radiation and Matter]<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
*"Chapter 5: Electromagnetic Radiation and Matter." Johnson County Community College. Web. 2015.<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16571Quantum Theory2015-12-05T23:13:11Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Energy levels.jpg|thumb|Graph illustrating the ground and excited states achieved by electrons with applied radiation. As well, an illustration of how only exact quantities of energy applied have effective results.]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
[[File:Black line spectra.png|thumb|Multiple elements and their corresponding black line regions of the spectrum at wavelengths which their electrons absorb photons.]]<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
*[http://hyperphysics.phy-astr.gsu.edu/hbase/mod5.html Quantum Processes] Involving Photon Absorption and Emission<br />
*[http://blogs.jccc.edu/astronomy/textbook/unit-two-conceptual-and-observational-tools-of-astronomy/chapter-5-electromagnetic-radiation-and-matter/ Electromagnetic Radiation and Matter]<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
*"Chapter 5: Electromagnetic Radiation and Matter." Johnson County Community College. Web. 2015.<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16526Quantum Theory2015-12-05T23:06:25Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
*[http://hyperphysics.phy-astr.gsu.edu/hbase/mod5.html Quantum Processes] Involving Photon Absorption and Emission<br />
*[http://blogs.jccc.edu/astronomy/textbook/unit-two-conceptual-and-observational-tools-of-astronomy/chapter-5-electromagnetic-radiation-and-matter/ Electromagnetic Radiation and Matter]<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
*"Chapter 5: Electromagnetic Radiation and Matter." Johnson County Community College. Web. 2015.<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Energy_levels.jpg&diff=16489File:Energy levels.jpg2015-12-05T23:01:22Z<p>Ccooper71: </p>
<hr />
<div></div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Black_line_spectra.png&diff=16486File:Black line spectra.png2015-12-05T23:01:08Z<p>Ccooper71: </p>
<hr />
<div></div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16483Quantum Theory2015-12-05T23:00:42Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
<br />
Applying visible radiation to pure samples allowed scientists to determine which wavelengths of the visible spectrum are absorbed by certain materials and which wavelengths are a reflected. This procedure explained both why we perceive certain colors for specific elements and the black lines of the spectra emitted from samples; the black lines are the locations in the spectra of photons with wavelengths absorbed by the electrons of the atom since they have the exact amount of energy needed to transition to another energy level. All of the other wavelengths are sent away from the atom and eventually taken in by receptors in our eyes.<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16375Quantum Theory2015-12-05T22:48:59Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
==Mathematical Application==<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.<br />
<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16363Quantum Theory2015-12-05T22:47:29Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.<br />
<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16339Quantum Theory2015-12-05T22:44:45Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.<br />
<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
*History and Explanation of [http://dwb.unl.edu/Teacher/NSF/C04/C04Links/www.fwkc.com/encyclopedia/low/articles/q/q021000030f.html Quantum Theory]<br />
*Defining [http://whatis.techtarget.com/definition/quantum-theory "What is quantum theory?"]<br />
<br />
==References==<br />
<br />
*Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. 323-340,445-450. Print.<br />
*"The Fundamental Forces of Nature." Web. Nd. [http://csep10.phys.utk.edu/astr162/lect/cosmology/forces.html]<br />
<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16242Quantum Theory2015-12-05T22:29:58Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.<br />
<br />
[[File:Adsporption and emission of photon and energy levels.jpg|thumb|Adsorption and Emission of Energy by Electrons]]<br />
Important to note: If another particle such as an electron collides with the electron of our system, then the amount of energy imparted to our system's electron may any amount required to move up by one or more energy level up to a maximum equal to the total kinetic energy of the colliding electron. If our system's electron gains energy from radiation, such as a photon, then the electron will absorb it completely; therefore, this instance may only occur if the total energy of the photon is equal to the amount required to move up by one or more energy levels.<br />
<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16180Quantum Theory2015-12-05T22:23:08Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.<br />
<br />
[[Adsporption_and_emission_of_photon_and_energy_levels.jpg|thumb| Adsorption and Emission of Energy by Electrons]]<br />
<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Adsporption_and_emission_of_photon_and_energy_levels.jpg&diff=16175File:Adsporption and emission of photon and energy levels.jpg2015-12-05T22:22:21Z<p>Ccooper71: </p>
<hr />
<div></div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=16159Quantum Theory2015-12-05T22:20:55Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations and others which are very useful in introductory physics problems.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {hν}</math> in units of joules (J)<br />
<br />
where Planck's constant (h) = 64985 Joules/Coloumb and<br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}{λ}}</math><br />
<br />
*The radius of an electron's orbit may be determined from:<br />
<br />
<math>{r} = {\frac{Nλ}{2π}}</math> or <math>{r} = {\frac{Nh}{2π|\vec{p}|}}</math><br />
where N is the energy level in which the electron is orbiting and λ is the wavelength<br />
<br />
*From the derivation of the orbit's radius, we can find the angular momentum of the electron:<br />
<br />
<math>{\vec{L}} = {\vec{r}x\vec{p}} = {\frac{Nh}{2π}}</math><br />
<br />
*The centripetal force holding the electron in circular motion is the electromagnetic force produce from the positive charges of the protons in the nucleus and negative charges of the electrons:<br />
<br />
<math> {F_{perpendicular}} = {\frac{mv^2}{r}}</math> <math> {F_{electromagnetic}} = {\frac{1}{4πε_0}\frac{q_e^2}{r^2}}</math><br />
<br />
from this radius of the orbit may also be found with <math>{r} = {\frac{N^2h^2}{ke^24π^2m}}</math> where <math>{k} = {\frac{1}{4πε_0}}</math><br />
<br />
*The total energy of an electron, specifically in the case of the hydrogen atom:<br />
<br />
<math>{E} = {\frac{-13.6}{N^2}}</math> in units of electron volts (eV) where <math>{1eV} = {1.6x10^{-19} J}</math><br />
<br />
*Other energy calculations for an electron orbiting a hydrogen nucleus:<br />
<br />
Potential Energy <math>{U} = {{-}\frac{1}{4πε_0}\frac{q_e^2}{r}}</math> may also be found with <math>{U} = {\frac{-27.2}{N^2}}</math><br />
<br />
Kinetic Energy <math>{K} = {\frac{1}{2}\frac{kq_e^2}{r}}</math><br />
<br />
Total Energy <math>{E_T} = {{U}+{K}} = {{U} + {\frac{-U}{2}}} = {\frac{U}{2}}</math> <br />
<br />
<br />
==Examples==<br />
===Excitation of Hydrogen's Electron===<br />
If energy is imparted on the orbiting electron of a hydrogen atom, the resulting transfer of energy will raise the energy level of the electron. Since the electron's only applying force prior to the incident energy is the electromagnetic force holding it to the atom, its total energy is negative. Adding energy increases the value of its total energy by an amount equal to that energy adsorbed; furthermore, the only amounts of energy that the electron will take in are those exactly equal to the amount required to completely move it one or more energy levels (meaning it cannot orbit between energy levels, as that event is not stable and the particle will shift immediately to change it). Although electrons are known to move up in energy levels (excited states), it will always release the energy almost immediately after in order to transition back down to a lower energy state (the lowest level known as the ground state E1) where the atom will be more stable and balanced. Applying the full energy that binds the electron to the atom will be a resulting level greater than the extent of the nucleus' attractive force, and the electron will be released from orbit, effectively ionizing the atom.<br />
<br />
[[adsporption and emission of photon and energy levels.jpeg|thumb| Adsorption and Emission of Energy by Electrons]]<br />
<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=15721Quantum Theory2015-12-05T21:27:19Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E = hν}</math><br />
<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=15710Quantum Theory2015-12-05T21:24:32Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {h}{v}</math><br />
where planck's constant (h) = 64985 J/C and <br />
ν(nu) is the frequency of the radiation, which is also <math>{ν} = {\frac{c}}{λ}</math><br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=15649Quantum Theory2015-12-05T21:16:33Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===Mathematical Application===<br />
From the development of the quantum theory, we obtain fundamental equations.<br />
<br />
* As Einstein determined, the incident energy that may be absorbed or emitted from electrons (or any particle for this case) depends on the frequency of the radiation:<br />
<br />
<math>{E} = {h}{nu}</math><br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=15527Quantum Theory2015-12-05T21:03:09Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
==History==<br />
<br />
The theory and all of its applications, much like any other scientific development of the 20th century, comes from contributions of multiple notable scientists over the course of many years. Initially, Newtonian Laws dominated physics, but the atom was represented by the plum pudding model, which developed after the discovery of the electron and the idea that atom must be made from more particles than previously suspected. None of the leading theories at the time, though, could explain electric discharges or the phenomenon of black lines appearing in the spectra from light passed through various materials. Some scientists were unsure of whether electrons existed as particles or if the electrons themselves were the energy and radiation observed from interactions with atoms. One of the earliest elements that lead to the current model was [[Max Planck]]'s idea that energy could be quantified or defined by smaller units, which he called "quanta". Later, [[Albert Einstein]] applied Planck's work to radiation via what is called the photoelectric effect, where he determined that the results of electron particle interaction with incident radiation, not just energy, depended specifically upon the frequency of the radiation. [[Niels Bohr]] determined his model of atomic structure in 1913; rejecting that idea that electrons orbiting the nucleus eventually lose energy and fall into the nucleus, he proposed that electrons were held in fixed orbits by electromagnetic forces and that they could shift to other orbits, or other energy levels, by absorption or emission of energy. [[Werner Heisenberg]] also suggested that electrons simply could not possibly be defined by an exact location or momentum by physicists, not without applying some radiation incident to the electron and measuring the disturbance of the system in effect- this idea known as the [[uncertainty principle]]. All of these ideas come together to form our current understanding of quantum physics, which greatly impacts the practice of modern physics.<br />
<br />
<br />
===A Mathematical Model===<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=15243Quantum Theory2015-12-05T20:26:36Z<p>Ccooper71: /* The Main Idea */</p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions. After many notable physicists had hypothesized and disproved various theories to describe the structure of the atom, scientists arrived at the Bohr Model, which currently has the most support from other work and theories from quantum mechanics. After the Rutherford's Gold Foil Experiment, the idea came about that the atom actually exists as many particles held together or near each other by electromagnetic force, which is the attraction or repulsion of charged particles, or the strong force, which holds protons and neutrons together at the nucleus of an atom, and that between these particles there is nothing but empty space. Why these particles stay together in certain configurations and their reactions to incidence with energy or other other particles is explained by quantum physics.<br />
<br />
<br />
<br />
<br />
===A Mathematical Model===<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
==History==<br />
<br />
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=15131Quantum Theory2015-12-05T20:13:41Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg|thumb|Current model of the atom.]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions.<br />
<br />
<br />
===A Mathematical Model===<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
==History==<br />
<br />
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.<br />
<br />
== See also ==<br />
*[[Atomic Theory]]<br />
*[[Bohr Model]]<br />
*[[Electronic Energy Levels and Photons]]<br />
*[[Rutherford Experiment and Atomic Collisions]]<br />
<br />
===Further reading===<br />
<br />
Chabay R., Sherwood B. Matter and Interactions. 4th ed. Hoboken, NJ: Wiley, 2015. Print.<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Theory]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=15039Quantum Theory2015-12-05T20:01:14Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
[[File:Atom intro.jpg]]<br />
<br />
==The Main Idea==<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions.<br />
State, in your own words, the main idea for this topic<br />
Electric Field of Capacitor<br />
<br />
===A Mathematical Model===<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
==History==<br />
<br />
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.<br />
<br />
== See also ==<br />
<br />
Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?<br />
<br />
===Further reading===<br />
<br />
Books, Articles or other print media on this topic<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Which Category did you place this in?]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=14942Quantum Theory2015-12-05T19:47:25Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions.<br />
[[File:Atom intro.jpg]]<br />
<br />
==The Main Idea==<br />
<br />
State, in your own words, the main idea for this topic<br />
Electric Field of Capacitor<br />
<br />
===A Mathematical Model===<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
==History==<br />
<br />
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.<br />
<br />
== See also ==<br />
<br />
Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?<br />
<br />
===Further reading===<br />
<br />
Books, Articles or other print media on this topic<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Which Category did you place this in?]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=File:Atom_intro.jpg&diff=14936File:Atom intro.jpg2015-12-05T19:46:27Z<p>Ccooper71: A basic representation of the atom with a nucleus comprised of neutron and protons as the center of a cloud of orbiting electrons.</p>
<hr />
<div>A basic representation of the atom with a nucleus comprised of neutron and protons as the center of a cloud of orbiting electrons.</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=14926Quantum Theory2015-12-05T19:43:48Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
Quantum theory is the accepted modern explanation of the observed behaviors of matter based upon atomic energy and particle interactions.<br />
<br />
==The Main Idea==<br />
<br />
State, in your own words, the main idea for this topic<br />
Electric Field of Capacitor<br />
<br />
===A Mathematical Model===<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
==History==<br />
<br />
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.<br />
<br />
== See also ==<br />
<br />
Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?<br />
<br />
===Further reading===<br />
<br />
Books, Articles or other print media on this topic<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Which Category did you place this in?]]</div>Ccooper71http://www.physicsbook.gatech.edu/index.php?title=Quantum_Theory&diff=14887Quantum Theory2015-12-05T19:35:49Z<p>Ccooper71: </p>
<hr />
<div>Claimed by Chris Cooper<br />
<br />
This topic covers the modern theory explaining the observed behaviors of matter based upon atomic energy and particle interactions.<br />
<br />
==The Main Idea==<br />
<br />
State, in your own words, the main idea for this topic<br />
Electric Field of Capacitor<br />
<br />
===A Mathematical Model===<br />
<br />
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.<br />
<br />
===A Computational Model===<br />
<br />
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]<br />
<br />
==Examples==<br />
<br />
Be sure to show all steps in your solution and include diagrams whenever possible<br />
<br />
===Simple===<br />
===Middling===<br />
===Difficult===<br />
<br />
==Connectedness==<br />
#How is this topic connected to something that you are interested in?<br />
#How is it connected to your major?<br />
#Is there an interesting industrial application?<br />
<br />
==History==<br />
<br />
Put this idea in historical context. Give the reader the Who, What, When, Where, and Why.<br />
<br />
== See also ==<br />
<br />
Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?<br />
<br />
===Further reading===<br />
<br />
Books, Articles or other print media on this topic<br />
<br />
===External links===<br />
<br />
Internet resources on this topic<br />
<br />
==References==<br />
<br />
This section contains the the references you used while writing this page<br />
<br />
[[Category:Which Category did you place this in?]]</div>Ccooper71