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