Emission spectra, atomic

How is the atomic emission spectrum of an element related to these flame tests ... 

Each line in an atomic emission spectrum corresponds to the energy given out when an excited electron moves to a state of lower energy. This can either be to a lower excited state or back to the ground state. Atomic emission spectra provide good evidence for discrete (quantised) energy levels in atoms. 

There are definite distinct lines in the atomic emission spectrum of hydrogen. These lines are seen in the visible part of the spectrum and there is also a series of lines in the infrared and another series in the ultraviolet part of the electromagnetic spectrum. So, although hydrogen is the simplest element with only one electron per atom, its atomic emission spectrum is fairly complicated. 

You can get more information on the atomic emission spectrum of hydrogen by watching the video clips at www. brightredbooks.net... 

In 1913 Bohr amalgamated classical and quantum mechanics in explaining the observation of not only the Balmer series but also the Lyman, Paschen, Brackett, Pfund, etc., series in the hydrogen atom emission spectrum, illustrated in Figure 1.1. Bohr assumed empirically that the electron can move only in specific circular orbits around the nucleus and that the angular momentum pe for an angle of rotation 9 is given by... 

The atomic emission spectrum of hydrogen is composed of many lines but these fall into separate sets or series. The first series to be discovered, not surprisingly, were those lines in the visible part of the spectrum. In 1885, a Swiss schoolmaster, Johann Balmer, noticed that the wavelengths, A, of the lines in this series could be predicted using a mathematical formula. He did not see why he just saw the relationship. This was the first vital step. 

As a result of his work, the lines in the visible spectrum are known as the Balmer series. The other series of lines in the atomic emission spectrum of hydrogen were discovered later (the next wasn t discovered until 1908). These series are named after the scientists who discovered them for example, the series in the ultraviolet region is known as the Lyman series after Theodore Lyman. 

Each element s atomic emission spectrum is unique and can be used to determine if that element is part of an unknown compound. For example, when a platinum wire is dipped into a strontium nitrate solution and then inserted into a burner flame, the strontium atoms emit a characteristic red color. You can perform a series of flame tests yourself by doing the miniLAB below. 

The atomic emission spectrum of hydrogen consists of four distinct coiored iines of different frequencies. This type of spectrum is aiso known as a iine spectrum. Which iine has the highest energy ... 

Recall that hydrogen s atomic emission spectrum is discontinuous that is, it is made up of only certain frequencies of light. Why are elements atomic emission spectra discontinuous rather than continuous Niels Bohr, a young Danish physicist working in Rutherford s laboratory in 1913, proposed a quantum model for the hydrogen atom that seemed to answer this question. Impressively, Bohr s model also correctly predicted the frequencies of the lines in hydrogen s atomic emission spectrum. 

In contrast to the continuous spectrum produced by white light, an element s atomic emission spectrum consists of a series of hne lines of individual colors. 

According to the Bohr model of the atom, hydrogen s atomic emission spectrum results from electrons dropping from higher-energy atomic orbits to lower-energy atomic orbits. 

Mercury s atomic emission spectrum is shown below. Estimate the wavelength of the orange line. What is its frequency What is the energy of an orange photon emitted by the mercury atom ... 

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