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II. Bohr Model of the Atom (p. 125-128) CH. 5 - ELECTRONS IN ATOMS C. JOHANNESSON A. Line-Emission Spectrum excited state ENERGY IN PHOTON OUT ground state C. JOHANNESSON B. Bohr Model e- exist only in orbits with specific amounts of energy called energy levels Therefore… ◦ e- can only gain or lose certain amounts of energy ◦ only certain photons are produced C. JOHANNESSON C. JOHANNESSON B. Bohr Model 65 4 Energy of photon depends on the difference in energy levels 3 Bohr’s calculated energies matched the IR, visible, and UV lines for the H atom 2 1 C. JOHANNESSON C. Other Elements Each element has a unique bright-line emission spectrum. ◦ “Atomic Fingerprint” Helium Bohr’s calculations only worked for hydrogen! C. JOHANNESSON D. Bohr Practice Use the Bohr Model/EM Spectrum on p. 8 of your reference tables. 1. What type of light is produced when an electron moves from n=4 to n=1? 2. What wavelength is produced when an electron moves from n=3 to n=2? 3. What color of light is number 2? 4. Which has more energy: red light or violet light? 5. Which has less energy: Radio waves or ultraviolet radiation? 6. Which has a smaller wavelength green or infrared? C. JOHANNESSON