Lyman series - wikipedia Lyman series In physics and chemistry, the Lyman series is a hydrogen spectral series of transitions and resulting ultraviolet emission lines 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, 3 to 1 is Lyman - beta, 4 to 1 is Lyman - gamma, and so on. 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. Contents 1 History 2 The Lyman series 3 Explanation and derivation 4 See also 5 References History This section needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. ( August 2015 ) 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 non-continuous or discrete. Here is an illustration of the first series of hydrogen emission lines : The Lyman series Historically, explaining the nature of the hydrogen spectrum was a considerable problem in physics. Nobody could predict the wavelengths 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 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. The Lyman series The version of the Rydberg formula that generated the Lyman series was : 1 λ = R H ( 1 − 1 n 2 ) ( R H ≈ 1.0968 × 10 7 m − 1 ≈ 13.6 eV h c ) ( displaystyle ( 1 over lambda ) = R_ ( \text ( H ) ) left ( 1 - ( \frac ( 1 ) ( n ^ ( 2 ) ) ) \right ) qquad left ( R_ ( \text ( H ) ) approx 1.0968 ( \times ) 10 ^ ( 7 ) , ( \text ( m ) ) ^ ( - 1 ) approx ( \frac ( 13.6 , ( \text ( eV ) ) ) ( hc ) ) \right ) ) 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 n = ∞ on the left. There are infinitely many spectral lines, but they become very dense as they approach n = ∞ ( the Lyman limit ), so only some of the first lines and the last one appear. The wavelengths in the Lyman series are all ultraviolet : n 5 6 7 8 9 10 11 ∞, the Lyman limit Wavelength ( nm ) 121.6 102.6 97.3 95.0 93.8 93.1 92.6 92.3 92.1 91.9 91.18 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, E n = − m e 4 2 ( 4 π ε 0 ħ ) 2 1 n 2 = − 13.6 eV n 2. ( displaystyle E_ ( n ) = - ( \frac ( me ^ ( 4 ) ) ( 2 ( 4 pi \varepsilon _ ( 0 ) hbar ) ^ ( 2 ) ) ) , ( \frac ( 1 ) ( n ^ ( 2 ) ) ) = - ( \frac ( 13.6 , ( \text ( eV ) ) ) ( n ^ ( 2 ) ) ). ) According to Bohr 's third assumption, whenever an electron falls from an initial energy level E to a final energy level E, the atom must emit radiation with a wavelength of λ = h c E i − E f. ( displaystyle lambda = ( \frac ( hc ) ( E_ ( \text ( i ) ) - E_ ( \text ( f ) ) ) ). ) There is also a more comfortable notation when dealing with energy in units of electronvolts and wavelengths in units of angstroms, λ = 12398.4 Å eV E i − E f. ( displaystyle lambda = ( \frac ( 12398.4 , ( \rm ( mathrm ( AA ) ) ) , ( \text ( eV ) ) ) ( E_ ( \text ( i ) ) - E_ ( \text ( f ) ) ) ). ) 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, 1 λ = E i − E f 12398.4 A ∘ eV = ( 12398.4 13.6 A ∘ ) − 1 ( 1 m 2 − 1 n 2 ) = R H ( 1 m 2 − 1 n 2 ) ( displaystyle ( \frac ( 1 ) ( lambda ) ) = ( \frac ( E_ ( \text ( i ) ) - E_ ( \text ( f ) ) ) ( 12398.4 , ( overset ( circ ) ( \rm ( A ) ) ) , ( \text ( eV ) ) ) ) = left ( ( \frac ( 12398.4 ) ( 13.6 ) ) , ( overset ( circ ) ( \rm ( A ) ) ) \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 ) ) Where R 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 with 1 to obtain 1 λ = R H ( 1 − 1 n 2 ) ( displaystyle ( \frac ( 1 ) ( lambda ) ) = R_ ( \text ( H ) ) left ( 1 - ( \frac ( 1 ) ( n ^ ( 2 ) ) ) \right ) ) 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 K - alpha Lyman continuum photon Moseley 's law Rydberg formula Balmer series References Jump up ^ `` Voyager Probes Detect `` invisible '' Milky Way Glow ``. National Geographic. December 1, 2011. Retrieved 2013 - 03 - 04. Jump up ^ Brehm, John ; Mullin, William ( 1989 ). Introduction to the Structure of Matter. John Wiley & Sons. p. 156. ISBN 0 - 471 - 60531 - X. Hydrogen spectral series Lyman series Balmer series Other series Retrieved from `` https://en.wikipedia.org/w/index.php?title=Lyman_series&oldid=771839626 '' Categories : Emission spectroscopy Hydrogen physics Hidden categories : Articles needing additional references from August 2015 All articles needing additional references Talk Contents About Wikipedia Čeština Deutsch Español فارسی Français 한국어 Hrvatski Italiano Lëtzebuergesch Lietuvių Nederlands 日本 語 Norsk nynorsk Polski Português Русский Slovenčina Slovenščina Srpskohrvatski / српскохрватски Türkçe Українська 中文 Edit links This page was last edited on 23 March 2017, at 20 : 30. Text is available under the Creative Commons Attribution - ShareAlike License ; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy. Wikipedia ® is a registered trademark of the Wikimedia Foundation, Inc., a non-profit organization. About Wikipedia

Question: what is the shortest wavelength of the lyman series
Answer: 121.6