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The spectral series of hydrogen, on a logarithmic scale. The emission spectrum of atomic hydrogen has been divided into a number of spectral series, with wavelengths given by the Rydberg formula. These observed spectral lines are due to the electron making transitions between two energy levels in an atom.
A Grotrian diagram of the hydrogen atom. Only transitions between adjacent columns are allowed, as per the selection rule =. A Grotrian diagram, or term diagram, shows the allowed electronic transitions between the energy levels of atoms. They can be used for one-electron and multi-electron atoms.
The "visible" hydrogen emission spectrum lines in the Balmer series. H-alpha is the red line at the right. Four lines (counting from the right) are formally in the visible range. Lines five and six can be seen with the naked eye, but are considered to be ultraviolet as they have wavelengths less than 400 nm.
Chemical Sciences: A Manual for CSIR-UGC National Eligibility Test for Lectureship and JRF/Emission spectrum; Chemical Sciences: A Manual for CSIR-UGC National Eligibility Test for Lectureship and JRF/Hydrogen spectral series; High School Chemistry/Light and the Atomic Spectra; Usage on en.wikiquote.org Wikiquote:Quote of the day/March 2011
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Source: File:Emission spectrum-H.png Created using the Balmer formula: = = Where is the wavelength. B is a constant with the value of 3.6456×10-7 m or 364.56 nm. n is equal to 2
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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 (groundstate).