![]() Rutherford’s earlier model of the atom had also assumed that electrons moved in circular orbits around the nucleus and that the atom was held together by the electrostatic attraction between the positively charged nucleus and the negatively charged electron. ![]() By 1925, scientists proposed a new kind of mechanics called quantum physics, and more advanced research was conducted on atoms larger than hydrogen. He collected data of the atomic emission spectrum for the hydrogen atom and extended it to a model for other atoms. the wavelengths of these spectrum lines are characteristic of the element and make. Bohr’s model required only one assumption: The electron moves around the nucleus in circular orbits that can have only certain allowed radii. He proposed that electrons travel around the nucleus in well-defined orbits. Which is the absorption spectrum, What is released when an excited electron returns to a lower energy state and more. Actually, if you just burned hydrogen and looked at its spectra, you would get the Emission Spectra and not the Absorption Spectra, and this Emission Spectra would only show the bunch of blue lines, one purple line, and one red line. ![]() In 1913, a Danish physicist, Niels Bohr (1885–1962 Nobel Prize in Physics, 1922), proposed a theoretical model for the hydrogen atom that explained its emission spectrum. Study with Quizlet and memorize flashcards containing terms like Which transition by an electron will release the greatest amount of energy, The emission spectrum of iodine is shown below. All the other colors shown are just part of the natural light being shown down on the element. Where \(n_1\) and \(n_2\) are positive integers, \(n_2 > n_1\), and \( \Re \) the Rydberg constant, has a value of 1.09737 × 10 7 m −1. Where all wavelengths and frequencies are represented (rainbow) The emitted light corresponds to. ![]()
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