1. Niels Bohr (1913) Bright-Line Spectrum Energy Levels Planetary Model
tried to explain presence of specific colors in hydrogen’s spectrum
Energy Levels
electrons can only exist in specific energy states
Planetary Model

2. Orbits or Energy levels
Area where e- are trapped within an atom
Atoms have multiple orbits

3. Electrons Produce Light!!
Electrons (e-) move within atoms
(e-) movement is caused by energy
(e-) move in different orbits

4. Photons A particle form of light or electromagnetic radiation
A photon walks into a hotel and checks in. "Do you want a hand with your luggage?" asks the receptionist. "No thanks", replies the photon, "
I’m travelling light".

5. Excited state Electrons jump to a higher orbit
Caused by atoms absorbing energy

6. Ground state Electron falls back to lower level (ground state)
Energy is released as electromagnetic radiation (E.R) (photon)

7. Transition of n
3→2
4→2
5→2
6→2
7-2
Wavelength (nm)
650
500
450
425
400
color
red
blue
green
violet UV

8. Quantum or jump
  when an e_ jumps orbits it transports to the next orbit!!!

9. A photon can be released as any electromagnetic energy
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10. Spectral lines summed up
e- are in fixed orbits
2. e- can get excited, and jump to a higher orbit, if they absorb the appropriate energy
3. e- will fall back to lower level (ground state) and release a photon of similar energy (visible light)

11. 5 points of the Bohrs Model
1. elements produce spectral lines also known as energy levels

12. 2. Energy levels are represented by letters

13. 3. Energy levels get larger the farther away they are from the nucleus

14. 4. larger the energy level more electrons they can hold
5 Each energy level can only hold so many electrons

16. Problems?
Why do electrons they stay in their orbits?