Emission and Absorption of Electromagnetic Energy

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Presentation transcript:

Emission and Absorption of Electromagnetic Energy

copper sodium lithium strontium

BOHR MODEL OF HYDROGEN ATOM Electron circles the nucleus in fixed energy ranges called orbits (energy levels) An electron can move from one energy level to another by gaining discrete amounts of energy. Electron can not be found between energy levels (energy levels are like rungs on a ladder…..) The lowest energy level is the closest to the nucleus.

How were these colors produced? By using the Bohr model, scientists can explain this phenomenon http://www.dlt.ncssm.edu/tiger/Flash/phase/ElectronOrbits.html * e- absorbs energy (in whole photons or quanta) to jump to a higher energy level (EXCITED STATE) * e- emits energy (in whole photons or quanta) to fall back to original energy level (GROUND STATE)

energy of light produced energy absorbed = energy released energy of light produced *some of this light is part of the visible spectrum, and can be seen as unique colors for different elements

Bohr model helped us to understand the movement of electrons around the nucleus. However, the model does not account for behavior of larger atoms with more than one electron.

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Wavelength vs Frequency Inversely proportional (i.e. when one goes up, the other goes down) http://amazing-space.stsci.edu/resources/explorations/light/makewaves-frames.html

Wave-Particle Duality of Electrons Electrons act as waves as well as particles Energy can act as particles as well as waves