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Niels Bohr and Atomic Energy Levels
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  1. Niels Bohr and Atomic Energy Levels By Steven Scott and Bryan Denin

  2. Early Life Born October 7, 1885 Died November 18, 1962 Received Nobel Prize in 1922 Developed Bohr Model of the atom Attended University of Copenhagen

  3. Education Attended Gammelholm Latin School Attended Copenhagen University Won over 8 notable awards Founded the Institute of Theoretical Physics at Copenhagen University

  4. What is the Bohr Model? Introduced in 1913 Atom shown as small, positively charged nucleus  Surrounded by electrons that orbit around the nucleus

  5. Bohr’s Model of the Atom Suggested heavier atoms have more protons in the nucleus Each orbit could only hold a certain number of electrons After that orbit is full, next level would have to be used. This gives the atom a shell structure Bohr used the solar system as a reference on how electrons orbit the nucleus

  6. Meeting with Heisbenberg Uranium-235 could construct the atomic bomb Did not believe you could extract enough of the U-235 Did not show an opinion on the possible effects the nuclear energy could have

  7. Electron Energy Levels The Bohr model gives for a system where two charged points orbit each other The Bohr formula properly uses the reduced mass of electron and proton

  8. What was Accepted • Electrons orbit the nucleus in orbits that have a set size and energy • The energy of the orbit is related to its size • Radiation is absorbed or emitted when an electron moves from one orbit to another

  9. Bohr’s Supporting Evidence • Each element gives off a specific colour of light (emission spectra). It is unique to each element • This allowed Bohr to produce his model of the atom. To explain this emission spectra, he suggested that electrons occupy shells or orbitals. • Bohr based his model on the energy (light) emitted by different atoms

  10. What was Wrong with the Model Gives an incorrect value for the ground state orbital angular momentum Poor predictions about the spectra of larger atoms Does not explain fine structure and hyperfine structure in spectral lines  Fails to provide any understanding of why certain spectral lines are brighter than others

  11. Resources