![]() These series are named after their innovators as revealed listed below. These spectral lines can be classified into five groups called spectral series. Example Spectra: Hydrogen-Like Atoms Hydrogen-like atoms are those atoms with only one electron remaining, regardless of the number of protons in the nucleus. This difficulty may be overcome by taking. The wavelengths of these lines depend on the visible, ultraviolet and infrared areas. For example, the intensity of the spectrum of a metal or alloy may vary with the metallurgical history of the sample. This light when viewed through a spectrometer shows numerous separated sharp lines. Hydrogen is filled in a discharge tube at a very low pressure a bluish light is given off from the discharge tube. This led to the birth to modern astrophysics. Using this unique identifer, we have found out how hot the stars are, as well as what type of elements were they made of. Hydrogen-spectrum is an important example of the atomic spectrum. The Atomic Emission Spectra usefulness can be compared to the usefulness of a fingerprint- the atomic emission spectra finger print makes a unique identifier. Figure 10.7.1 shows a portion of the energy level diagram for sodium, which consists of a series of discrete lines at wavelengths that correspond to the difference in energy between two atomic orbitals. Spectroscopy can be very useful in helping scientists understand how an object like a black hole, neutron star, or active galaxy produces light, how fast it is. In emission spectrum, these lines appear bright due to the fact that the matching wavelengths are being given off by the element, whereas they appear dark in absorption spectrum because the wavelengths are being absorbed by the element. Atomic emission occurs when a valence electron in a higher energy atomic orbital returns to a lower energy atomic orbital. It is interesting to keep in mind that the positions or the wavelengths of lines appearing in both emission and absorption spectra are precisely the same. The wavelengths of the radiation that have actually been absorbed by the element look like dark lines and the background are bright. The spectrum of this radiation is called an atomic absorption spectrum. When a beam of white light is passed through a gaseous sample of an element, the element takes in certain wavelengths while the rest of wavelengths travel through it. This is called an atomic emission spectrum. Atomic spectra consist of narrow peaks (a few nanometers bandwidth) providing two types of analytical information: qualitative analysis (characteristic frequency or wavelength of the absorbed or emitted photon) and quantitative analysis (signal intensity at a given wavelength). The spectrum of this radiation contained bright lines against a dark background. When solids are volatilized or elements in their gaseous states are heated to high temperature or subjected to an electrical discharge, radiation of specific wavelengths are emitted. There are two ways in which an atomic spectrum can be seen. ![]()
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