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Atomic Spectrum of Hydrogen :
When Hydrogen gas is heated or subjected to electric discharge, its electron moves to higher energy orbits by absorbing energy. Subsequently when electron comes back energy is emitted in the form of radiations of particular wavelength depending upon difference of energies of the orbits.
More is the difference of energy of the two orbits shorter will be the wavelength of the radiations emitted. When these radiations are made to pass through spectroscope, they bend through different angles such that radiations with shorter wavelength are bent through greater angle and thus fall on different position on the screen and produce spectrum. The spectrum of Hydrogen has several groups (series) of spectral lines which include following series.
Atomic Hydrogen Spectral Lines:
Lyman series (Ultra violet region ) where n1 = 1 and n2 = 2,3,4,5,6,7
Balmer series (Visible region ) where n1 = 2 and n2 = 3,4,5,6,7
Paschen series (near I.R region ) where n1 = 3 and n2 = 4,5,6,7
Brackett series (mid I.R region ) where n1 = 4 and n2 = 5,6,7
Pfund series ( Far I.R region) where n1 = 5 and n2 = 6,7
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