Hydrogen bright-line spectrum

The electronic transitions that produce the bright-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. 

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 ... 

What do the bright lines of light represent in the visible spectrum of the hydrogen atom ... 

The Bohr Model The Bohr model was a first attempt to explain the bright-line spectra of atoms. While it did predict the spectrum of the hydrogen atom, it failed to predict the spectra of other atoms and was consequently replaced by the quantum-mechanical model. 

Schematic representation of an apparatus that measures the emission spectrum of a gaseous element. Emission lines appear bright against a dark background. The spectmm shown is the emission spectrum for hydrogen atoms.

Figure 2. The strong absorption feature centred near 3375 A in the near-ultraviolet (UV) spectrum of the bright QSO Q1331+170 is a good example of a damped Lya line, in this case produced by a column density of neutral hydrogen atoms 1V(H I) = 1.5 x 1021 cm-2. This spectrum was recorded in the early 1990s with the Image Photon Counting System on the ISIS spectrograph of the 4.2 m William Herschel telescope on La Palma (Pettini et al. 1994).

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