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2014-12-24T20:55:52Z

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en>Jochen Burghardt: /* See also */ felt need to establish relation, which is not as obvious as the wording suggests at first glance

2014-02-03T20:32:24Z

See also: felt need to establish relation, which is not as obvious as the wording suggests at first glance

← Older revision		Revision as of 22:32, 3 February 2014
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	~~They call me Gabrielle~~. ~~I am a particular cashier and I~~'~~m charging pretty good financially~~. ~~As your girl what I definitely like~~ is ~~going~~ in the ~~market~~ to ~~karaoke but I do~~ not ~~have made a dime~~ with it. ~~My husband and [~~http://~~search~~.un.~~org~~/~~search?ie~~=~~utf8&site~~=~~un_org&output~~=~~xml_no_dtd&client~~=~~UN_Website_en&num~~=~~10&lr~~=~~lang_en&proxystylesheet~~=~~UN_Website_en~~&oe=~~utf8&q~~=~~I+decided&Submit~~=~~Go I decided] upon~~ to ~~reside~~ in ~~Guam~~ but ~~I will attain~~ to ~~move~~ in a ~~new year or two~~. ~~See all that~~ is ~~new on my website here~~: ~~http~~://~~prometeu~~.~~net~~<br><br>~~Visit my page; clash~~ of ~~clans hack android~~ [[http://~~prometeu~~.~~net visit the following internet page~~]]		In [[physics]] and [[chemistry]], the '''Lyman series''' is the series of transitions and resulting [[ultraviolet]] [[emission line]]s of the [[hydrogen]] [[atom]] as an [[electron]] goes from ''n'' ≥ 2 to ''n'' = 1 (where ''n'' is the [[principal quantum number]]) the lowest energy level of the electron. The transitions are named sequentially by Greek letters: from ''n'' = 2 to ''n'' = 1 is called [[Lyman-alpha line\|Lyman-alpha]], 3 to 1 is Lyman-beta, 4 to 1 is Lyman-gamma, etc. The series is named after its discoverer, [[Theodore Lyman]]. The greater the difference in the principal quantum numbers, the higher the energy of the electromagnetic emission.

			==History==
			The first line in the spectrum of the Lyman series was discovered in 1906 by Harvard physicist [[Theodore Lyman]], who was studying the ultraviolet spectrum of electrically excited hydrogen gas. The rest of the lines of the spectrum (all in the ultraviolet) were discovered by Lyman from 1906-1914.
			The spectrum of radiation emitted by hydrogen is [[quantisation (physics)\|non-continuous]] or discrete. Here is an illustration of the first series of hydrogen emission lines:

			[[File:LymanSeries.svg\|The Lyman Series]]

			Historically, explaining the nature of the hydrogen spectrum was a considerable problem in [[physics]]. Nobody could predict the [[wavelength]]s of the hydrogen lines until 1885 when the [[Balmer formula]] gave an empirical formula for the visible hydrogen spectrum. Within five years [[Johannes Rydberg]] came up with an [[empirical relationship\|empirical formula]] that solved the problem, presented first in 1888 and in final form in 1890. Rydberg managed to find a formula to match the known [[Balmer series]] emission lines, and also predicted those not yet discovered. Different versions of the Rydberg formula with different simple numbers were found to generate different series of lines.

			On December 1, 2011, it was announced that [[Voyager 1]] detected the first Lyman-alpha radiation originating from the [[Milky Way]] galaxy. Lyman-alpha radiation had previously been detected from other galaxies, but due to interference from the Sun, the radiation from the Milky Way was not detectable.<ref>{{cite web\|url=http://news.nationalgeographic.com/news/2011/12/111201-voyager-probes-milky-way-light-hydrogen-sun-nasa-space\|title=Voyager Probes Detect "invisible" Milky Way Glow\|publisher=National Geographic\|date=December 1, 2011\|accessdate=2013-03-04}}</ref>

			==The Lyman series==

			The version of the [[Rydberg formula]] that generated the Lyman series was:<ref name="Brehm-Mullin p156">John Brehm and William Mullin, Introduction to the Structure of Matter, John Wiley & Sons, Inc., 1989, p. 156 ISBN 0-471-60531-X</ref>

			:<math> {1 \over \lambda} = R_\text{H} \left( 1 - \frac{1}{n^2} \right) \qquad \left( R_\text{H} = 1.0968{\times}10^7\,\text{m}^{-1} = \frac{13.6\,\text{eV}}{hc} \right)</math>

			Where ''n'' is a natural number greater than or equal to 2 (i.e. ''n'' = 2,3,4,...).

			Therefore, the lines seen in the image above are the wavelengths corresponding to ''n''=2 on the right, to <math>n= \infty </math> on the left (there are infinitely many spectral lines, but they become very dense as they approach to <math>n= \infty </math> ([[Lyman limit]]), so only some of the first lines and the last one appear).

			The wavelengths (nm) in the Lyman series are all ultraviolet:
			{\| class="wikitable"
			! <math>n</math>
			\|align="center"\|2
			\|align="center"\|3
			\|align="center"\|4
			\|align="center"\|5
			\|align="center"\|6
			\|align="center"\|7
			\|align="center"\|8
			\|align="center"\|9
			\|align="center"\|10
			\|align="center"\|11
			\|align="center"\|<math>\infty</math>
			\|-
			! Wavelength (nm)
			\|121.6
			\|102.6
			\|97.3
			\|95.0
			\|93.8
			\|93.1
			\|92.6
			\|92.3
			\|92.1
			\|91.9
			\|91.18 ([[Lyman limit]])
			\|}

			==Explanation and derivation==

			In 1913, when [[Niels Bohr]] produced his [[Bohr model]] theory, the reason why hydrogen spectral lines fit Rydberg's formula was explained. Bohr found that the electron bound to the hydrogen atom must have quantized energy levels described by the following formula,

			:<math> E_n = - \frac{me^4}{2(4\pi\varepsilon_0\hbar)^2}\,\frac{1}{n^2} = - \frac{13.6\,\text{eV}}{n^2}. </math>

			According to Bohr's third assumption, whenever an electron falls from an initial energy level <math>E_\text{i}</math> to a final energy level <math>E_\text{f}</math>, the atom must emit radiation with a wavelength of

			:<math> \lambda = \frac{hc}{E_\text{i} - E_\text{f}}. </math>

			There is also a more comfortable notation when dealing with energy in units of [[electronvolt]]s and wavelengths in units of [[angstrom]]s,

			:<math> \lambda = \frac{12398.4\,{\rm \AA}\,\text{eV}}{E_\text{i} - E_\text{f}}. </math>

			Replacing the energy in the above formula with the expression for the energy in the hydrogen atom where the initial energy corresponds to energy level ''n'' and the final energy corresponds to energy level ''m'',

			:<math> \frac{1}{\lambda} =
			\frac{E_\text{i} - E_\text{f}}{12398.4\,{\rm \AA}\,\text{eV}} =
			\left(\frac{12398.4}{13.6}\,{\rm \AA}\right)^{-1} \left(\frac{1}{m^2} - \frac{1}{n^2} \right) =
			R_\text{H} \left(\frac{1}{m^2} - \frac{1}{n^2} \right) </math>

			Where <math>R_\text{H}</math> is the same [[Rydberg constant]] for hydrogen from Rydberg's long known formula.

			For the connection between Bohr, Rydberg, and Lyman, one must replace ''m'' by 1 to obtain

			:<math> \frac{1}{\lambda} = R_\text{H} \left( 1 - \frac{1}{n^2} \right) </math>

			which is Rydberg's formula for the Lyman series. Therefore, each wavelength of the emission lines corresponds to an electron dropping from a certain energy level (greater than 1) to the first energy level.

			== See also ==

			* [[Bohr model]]
			* [[H-alpha]]
			* [[Hydrogen spectral series]]
			* [[Lyc photon]]
			* [[Rydberg formula]]
			* [[K-alpha]]
			* [[Moseley's law]]

			==References==
			{{Reflist\|colwidth=30em}}

			==External links==
			*[http://homepage.mac.com/dtrapp/ePhysics.f/labII__10.html Lyman discovers series]

			{{Hydrogen spectral series-footer}}

			[[Category:Emission spectroscopy]]
			[[Category:Hydrogen physics]]

99.238.32.134: /* Further reading */

2012-08-19T19:15:28Z

Rewriting - Revision history

en>AnomieBOT: Dating maintenance tags: {{Cn}}

en>Bmcm: /* String rewriting systems */ Tidied up/inserted markup for consistent typography of math notation in running text

en>Jochen Burghardt: /* See also */ felt need to establish relation, which is not as obvious as the wording suggests at first glance

99.238.32.134: /* Further reading */

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