Line spectrum, of hydrogen

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... 

The agreement between this relation and the observed line spectrum of hydrogen was far too good to be a mere coincidence. While the details of the election orbits employed by Bohr in his calculation may not be a part of the cnrrent paradigm, the concept of electronic energy levels is here to stay. 

In 1913 Niels Bohr proposed his atomic theory with the help of the line spectrum of hydrogen atoms and Planck s quantum theory. His postulates can be summarized as follows ... 

It was the analysis of the line spectrum of hydrogen observed by J. J. Balmer and others that led Neils Bohr to a treatment of the hydrogen atom that is now referred to as the Bohr model. In that model, there are supposedly allowed orbits in which the electron can move around the nucleus without radiating electromagnetic energy. The orbits are those for which the angular momentum, mvr, can have only certain values (they are referred to as quantized). This condition can be represented by the relationship... 

Introduction.—In spite of the almost innumerable studies which have been made of the secondary or many lined spectrum of hydrogen its detailed explanation remains far from complete. The problem is the more fascinating because it involves the structime of the hydrogen molecule and its solution must have an important bearing on the whole question of molecular structure. The recent work of Dieke, Witmer and others indicates increasingly rapid progress on the theoretical side of the problem and suggests to the writers that a preliminary report on certain experimental work may not be out of place. 

What is the significance of the line spectrum of hydrogen It indicates that only certain energies are allowed for the electron in the hydrogen atom. In other words, the energy of the electron in the hydrogen atom is quantized. 

The discrete line spectrum of hydrogen shows that only certain energies are possible that is, the electron energy levels are quantized. In contrast, if any energy level were allowed, the emission spectrum would be continuous. 

How was Bohr s atomic model able to explain the line spectrum of hydrogen ... 

Explain how the bright-line spectrum of hydrogen is consistent with Bohr s model of quantized energy states for the electrons in the hydrogen atom. 

Bohr s theory explained the line spectrum of hydrogen exactly. It did not explain measurements made for atoms other than hydrogen. 

Consider the bright line spectrum of hydrogen shown in Figure 11.11. Which line in the spectrum represents photons with the highest energy With the lowest energy ... 

The line spectrum of hydrogen in the visible region. [Reproduced from http //en.wikipedia.org/wiki /Hydrogen spectral series (accessed November 30, 2013).]... 

The complete line spectrum of hydrogen from the ultraviolet to the infrared. Transitions from the n, = oo energy level to the lowest energy level in each series correspond with the series limit, where the individual energy levels all start to blur together. [Blatt Communications.]... 

Example 3-4. Calculate the wavelengths (nm) of the five lines shown in Figure 3.16 for the line spectrum of hydrogen if = 2 for the Balmer series. 

The Paschen series of lines in the line spectrum of hydrogen occur in the near-IR. (a) Calculate the wavelength (in nm) of the series limit for the Paschen series of lines in the line spectrum of hydrogen, (b) The frequency of one line in the Paschen series of hydrogen is 2.34 x 10 Hz. Using the Bohr model of the atom with its circular orbits, sketch this specific electronic transition. 

Use the Rydberg equation to calculate the wavelengths of the first three lines in the Brackett series of the line spectrum of hydrogen. 

Line spectrum of hydrogen. Each line corresponds to the wavelength of the energy emitted when the electron of a hydrogen atom, which has absorbed energy, falls back to a lower principal energy level. 

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