Spectrum, of hydrogen

Bafmer series Frequencies of certain lines in the spectrum of hydrogen are simply related to each other, and can be expressed by a general formula. One group of lines is termed the Balmer series. Other series were later discovered in the spectrum of hydrogen by Lyman, Paschen, Brackett and Pfund. 

Improved spectroscopic methods showed that the spectrum of hydrogen contained many more lines than was originally supposed and that some of these lines were split further into yet more lines when... 

The hydrogen atom, containing a single electron, has played a major role in the development of models of electronic structure. In 1913 Niels Bohr (1885-1962), a Danish physicist, offered a theoretical explanation of the atomic spectrum of hydrogen. His model was based largely on classical mechanics. In 1922 this model earned him the Nobel Prize in physics. By that time, Bohr had become director of the Institute of Theoretical Physics at Copenhagen. There he helped develop the new discipline of quantum mechanics, used by other scientists to construct a more sophisticated model for the hydrogen atom. 

The Brackett series lines in the atomic spectrum of hydrogen result from transitions from n > 4 to n = 4. 

In 1885, Johann Balmet a mathematician, derived the following relation for the wavelength of lines in the visible spectrum of hydrogen... 

Wavelength (A) A characteristic property of a wave related to its color and equal to the length of a full wave, 133 atomic spectrum of hydrogen, 136 color and, 17t... 

Before we can analyze the spectrum of hydrogen atoms, we must become more familiar with light. In Chapter 14 light was characterized by frequency or wavelength. (Reread Section 14-3.1.) Now we shall consider another property of light... 

The ultraviolet absorption spectrum of hydrogen was analyzed by Dieke and Hopfield (8). They identified the three lowest... 

The Bohr atom went a long way toward explaining the nature of atoms, but there were problems. Although scientists could calculate the emission spectrum of hydrogen using the Bohr model, the model could not account for the spectra of heavier atoms. The biggest problem with the Bohr atom, however, lay in its lack of a... 

The discovery of two other series of emission lines of hydrogen came later. They are named for their discoverers the Lyman series in the ultraviolet range and Paschen series in the infrared region. Although formulas were devised to calculate the spectral lines, the physics behind the math was not understood until Niels Bohr proposed his quantized atom. Suddenly, the emission spectrum of hydrogen made sense. Each line represented the energy released when an excited electron went from a higher quantum state to a lower one. 

Over time, scientists sorted out the electron transitions that produce every line in the spectrum of hydrogen (Figure 4.4). The... 

The spectrum of hydrogen (Z = 1) is divided into a number of series of spectral lines, each series having a particular value for n. As many as six different series have been observed ... 

Fig. 17-3 The origin of the visible spectrum of hydrogen (not drawn to scale)...

Draw a picture of the electron jump corresponding to the first line in the visible emission spectrum of hydrogen according to the Bohr theory. 

Fig. 3. Spectrum of hydrogen on zinc oxide (P = 100 mm dashed line is background.)...

Eventually, other series of lines were found in other regions of the electromagnetic spectrum. The Lyman series was observed in the ultraviolet region, whereas the Paschen, Brackett, and Pfund series were observed in the infrared region of the spectrum. All of these lines were observed as they were emitted from excited atoms, so together they constitute the emission spectrum or line spectrum of hydrogen atoms. 

This accounts for the fact that the line spectrum of hydrogen shows only lines having certain wavelengths. In order for the electron to move in a stable orbit, the electrostatic attraction between it and the proton must be balanced by the centrifugal force that results from its circular motion. As shown in Figure 1.7, the forces are actually in opposite directions, so we equate only the magnitudes of the... 

Fig. 2. IR absorption spectrum of hydrogen passivated, B-doped Si measured at room temperature. [Reprinted with permission from the American Institute of Physics, Pankove, J.I., et al., (1985). Appl. Phys. Lett. 46, 421.]...

The analysis of the IR spectrum of hydrogen peroxide and cumyl hydroperoxide gave the following values of frequencies (cm-1) of valence and bond angle vibrations [60]. 

The first application of quantum theory to a problem in chemistry was to account for the emission spectrum of hydrogen and at the same time explain the stability of the nuclear atom, which seemed to require accelerated electrons in orbital motion. This planetary model is rendered unstable by continuous radiation of energy. The Bohr postulate that electronic angular momentum should be quantized in order to stabilize unique orbits solved both problems in principle. The Bohr condition requires that... 

Figure 12.6 The emission spectrum of hydrogen in the UY, visible and near infrared, showing the families of lines labeled Lyman (n = 1), Balmer (n — 2), and Paschen (n = 3).

Calculation of Vibrational Spectrum of Hydrogen Peroxide (HOOH). 

Figure 1.4. A part of the atomic spectrum of hydrogen (/. = wavelength)...

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