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16 Cards in this Set
- Front
- Back
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Bohr
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-electron doesn;t emit radition n atom. Longer orbits have more energy than smaller ones. Oribits at specific energy levels. Found emittion spectrum for just hydrogen. Photons create bright line spectrum. Electrons changing orbits. quantized energy levels.
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Crookes
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-tube with electrodes, a conductor, and created a beam of charged particles. Created Cathode Ray. knew there were negativly charged particles, because it was drawn to the anode.
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Dalton
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-atom was uniform throughout, a sphere. Combonation in ratios to make compounds-law of multiple ratios. in constant motion, induvidual atoms. Billard ball theory.
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Heisenberg
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-electron as a particle instead of a wavelength and still came to the conclusion of an electron cloud where the electron could be.
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Millikan
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-measured charge of an electron by spraying oil into a charged chamber and timing how long it took for the drop to rise and fall.
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Planck
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-energy of atoms had a relationship to the wavelength being emitted by the substance.
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Rutherford
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-Gold foil experiment-concluded that there was a center of positively charged ions called nucleus where electrons revolved.
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Schrodinger
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-electron cloud where electron could be. Describe as wave.
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Thomson
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-used cathode ray idea and deflected particles using magnets. Concluded there were subatomic particles in atoms. Found that there could be a pistive particles too. Plum pudding atom.
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Gold Foil experiment
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Rutherford- alpha particles were shot through a piece of gold foil with flourescent screen around it. If everything had been uniform, the partiles would have gone through, but some were deflected to other parts. Bounce back made him think there was a very dense nucleus.
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uncertainty pricnciple. Who? what?
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heisenberg. You can't determine the position and velocity of an electron at the same time. You would mess up the measurements when you took one very accuratly. So you had to get them inaccuratly. This creates the idea of an electron cloud.
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n=
n^2= |
the energy level the electron is on
-the # of orbitals. |
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l=
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the shape of the orbital.
l=0 then s orbital l=1 then p orbital l=2 then d orbital |
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m=
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orientation of the orbital in space
if l=0 then m=0 if l=1 then m=-1,0,1 they represent the planes in space |
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s=
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the spin of the elctron.
-1/2 or 1/2 |
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2 wavelength energy equations
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E=hv (energy equals planck's constant multiplied by frequency)
c=hv (velocity of light equals plank's constant multiplied by frequency) |
