Planck's Relation: Difference between revisions
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What is the energy of a single photon of orange light? | What is the energy of a single photon of orange light? | ||
Orange light has a radiation frequency of 435 THz. | Orange light has a radiation frequency of 435 THz. | ||
*For a difficult problem, see external links* | |||
E=hv | E=hv | ||
E=( 435*10^12)(6.626*10^-34) | E=( 435*10^12)(6.626*10^-34) | ||
E=2.88*10^-18 Joules | E=2.88*10^-18 Joules | ||
==Connectedness== | ==Connectedness== | ||
| Line 51: | Line 51: | ||
==History== | ==History== | ||
Max Planck, a German Scientist discovered Planck's Relation. He published his paper in 1900. He was doing research and realized that matter could only emit or absorb radiation at certain discrete energy levels. He found a constant that described the distance between the energy levels | Max Planck, a German Scientist discovered Planck's Relation. He published his paper in 1900. He was doing research and realized that matter could only emit or absorb radiation at certain discrete energy levels. He found a constant that described the distance between the energy levels. | ||
== See also == | == See also == | ||
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===External links=== | ===External links=== | ||
A | A difficult example of a problem calculating the energy in a mole of photons using Planck's Relation: [https://www.youtube.com/watch?v=M7UAPGD8ETU] | ||
==References== | ==References== | ||
Latest revision as of 23:35, 6 December 2015
Planck Relation
The Planck Relation helps us to be able to figure out the energy of a photon based on its frequency of radiation.
The Main Idea
The energy of a photon is related to the frequency of its radiation by Planck's constant, h. This has a value of 6.626*10^-34 Joules*seconds. Planck's relation allows us to find the energy of a photon, or its frequency (and wavelength) of its radiation.
A Mathematical Model
E=hv -h=6.626*10^-34 Joules*seconds
-E is the energy of a photon in Joules
-v is the frequency of the radiation of the proton in Hz
A Computational Model
Hyper physics has a program that allows users to input wavelength, frequency, or energy and find out the other two values. http://hyperphysics.phy-astr.gsu.edu/hbase/mod2.html#c3
Examples
Be sure to show all steps in your solution and include diagrams whenever possible
Simple
If a proton starts at frequency v, and its frequency increases, does its energy increase or decrease?
Its energy increases because E and v have a positive linear correlation. E=hv ?=h2v 2E=h2v
Middling
What is the energy of a single photon of orange light?
Orange light has a radiation frequency of 435 THz.
*For a difficult problem, see external links*
E=hv
E=( 435*10^12)(6.626*10^-34)
E=2.88*10^-18 Joules
Connectedness
This relation allows us to understand the photoelectric effect (why some metals emit electrons when light is shined on them) and Planck's Law of Black Body Radiation.
Every day in the biomedical device industry, new forms of treatment for cancer are being used. Proton emission therapy is a current method. If photons were ever used to combat disease, Planck's Relation could help engineers to calculate their energy or radiation frequency and wavelength in order to adjust these values to get the ones desired.
History
Max Planck, a German Scientist discovered Planck's Relation. He published his paper in 1900. He was doing research and realized that matter could only emit or absorb radiation at certain discrete energy levels. He found a constant that described the distance between the energy levels.
See also
Are there related topics or categories in this wiki resource for the curious reader to explore? How does this topic fit into that context?
Further reading
HyperPhysics page on Photoelectric Effect: http://hyperphysics.phy-astr.gsu.edu/hbase/mod2.html#c3
External links
A difficult example of a problem calculating the energy in a mole of photons using Planck's Relation: [1]
References
http://hyperphysics.phy-astr.gsu.edu/hbase/mod2.html#c3 https://www.youtube.com/watch?v=dSUvyERhtO8 This section contains the the references you used while writing this page