![]() A line spectrum is a series of lines that represent the different energy levels of the an atom. The available energy of excitation is somewhat less in the second case. The Balmer Rydberg equation explains the line spectrum of hydrogen. A metal hydride may first be formed and this in a two body collision with a hydrogen atom may react to give H 2 and an excited metal atom. In this unit we will examine several different atomic spectra. A three body collision of two hydrogen atoms and a metal atom may result in recombination of the hydrogen and excitation of the metal atom. These characteristic sets of frequencies for different atoms are known as atomic spectra. For the Atomic Spectra review, we are calculating the Rydberg equation for various electron transitions for the Hydrogen atom. Theory of excitation of spectra by atomic hydrogen.-Two possibilities are suggested. Caesium, magnesium, thallium and zinc gave no line spectra. Mercury gave the complete hydride spectrum and faint emission of λ 2537. ![]() Potassium showed the first resonance doublet faintly. Attempts to develop a theoretical understanding of the states of the hydrogen atom have been important to the history of quantum mechanics, since all other atoms can be roughly. Sodium and cadmium gave strong emission of their first resonance lines and no other lines. Hydrogen-like atoms are those atoms with only one electron remaining, regardless of the number of protons in the nucleus. Atomic spectroscopy shows that there is a discrete infinite set of states in which a hydrogen (or any) atom can exist, contrary to the predictions of classical physics. Spectroscopic excitation of Na, K, Cs, Mg, Cd, Zn, Hg, Tl vapors by atomic hydrogen.-Hydrogen from a Wood discharge tube flowed into a tube containing metal vapor and the spectrum emitted by the mixture was observed. ![]()
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