![]() ![]() Niels Bohr, a Danish scientist, explained this line spectrum while developing a model for the atom: Bohr said that the electron had to release energy to change its energy so the differences between the energies of light seen in the atomic spectrum should correspond to the differences in energies of the energy levels. He used these energies to find the energies that the single electron in the hydrogen atom could have. Bohr found the energy of the colors of light that the hydrogen atom released. This led Bohr to theorize that electrons only have certain energies in an atom and they had to be in energy levels. Each color corresponds to a specific amount of energy however when the light given off by the hydrogen atom was passed through a prism, only certain colors of light could be seen. When white light is diffracted with a prism, all the colors of the visible spectrum can be seen. The Bohr model was based on his observations of the atomic emissions spectrum of the hydrogen atom. The Rutherford model had several flaws that the Bohr model overcame. This model was proposed in 1913 by Niels Bohr and was really an expansion on the Rutherford model of 1911. The energy difference between the initial and final orbit is emitted by the atom in bundles of electromagnetic radiation called photons. When an electron changes orbits, it does so in a sudden quantum leap. A simple definition of Bohr’s atomic model is: electrons orbit the nucleus at set distances.
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