Figure 7.3.5 The Emission Spectra of Elements Compared with Hydrogen. Atomic hydrogen displays emission spectrum. The orbital changes of hydrogen electrons that give rise to some spectral lines are shown in Figure 1. The strongest lines in the hydrogen spectrum are in the far UV Lyman series starting at 124 nm and below. 6 Interlude: Spectra in Astronomy Bohr’s Explanation for Hydrogen Spectrum Prepared By: Sidra Javed When current is passed through Hydrogen gas in the discharge tube at low pressure, the molecules of Hydrogen break in to atoms. 0. Prepared By: Sidra Javed 8. Gases; 2. Extending hydrogen's emission spectrum into the UV and IR. The three prominent hydrogen lines are shown at the right of the image through a 600 lines/mm diffraction grating. Similar pictures can be drawn for atoms other than hydrogen. That red light has a wave length of 656 nanometers. An approximate classification of spectral colors: Violet (380-435nm) Blue(435-500 nm) Cyan (500-520 nm) Green (520-565 nm) Yellow (565- 590 nm) Orange (590-625 nm) It is possible to detect patterns of lines in both the ultra-violet and infra-red regions of the spectrum as well. At left is a hydrogen spectral tube excited by a 5000 volt transformer. Learning Strategies There is a lot more to the hydrogen spectrum than the three lines you can see with the naked eye. Atomic; 3. You'd see these four lines of color. IMFs; 4. Thermo; FAQs; Links. It is called a spectral line. This spectrum enfolds several spectral series. So this is the line spectrum for hydrogen. Once the electrons in the gas are excited, they make transitions between the energy levels. Lyman series of hydrogen atom lies in the ultraviolet region, Balmer series lies in visible region, Paschen series lies in near infrared region whereas Bracket, Pfund as well as Humphrey series lie in far infrared region of electromagnetic spectrum. So, since you see lines, we call this a line spectrum. Whenever an electron in a hydrogen atom jumps from higher energy level to the lower energy level, the difference in energies of the two levels is emitted as a radiation of particular wavelength. Units . However, because these other atoms ordinarily have more than one electron each, the orbits of their electrons are much more complicated, and the spectra are more complex as well. This concept describes the hydrogen atom emission spectrum and explains the origins of the spectral lines. By comparing these lines with the spectra of elements measured on Earth, we now know that the sun contains large amounts of hydrogen, iron, and carbon, along with smaller amounts of other elements. 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