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41 Cards in this Set
- Front
- Back
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light
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electromagnetic waves
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radiation
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any energy from a source
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crest
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from origin to top of wave
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wave length
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crest to crest
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trough
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from origin to bottom of wave
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frequency
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# of wavelenths to pass a point in a given amount of time
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wavelength up
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frequency down
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energy up
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wavelength down
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frequency up
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energy up
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longest wavelength in visible spectrum
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red
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Violet
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smallest wavelength
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atomic emmission spectrum
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spectral lines that are characteristic of an element
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energy needed to move electron to different levels
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quantized
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plunck
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energy in e- changes only in discrete movements, not continuous flow
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quantam
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discrete unit necessary to move e- up on energy levels
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einstein
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photons-->packets of light, units of energy
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bohr
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electrons rotate
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quantum mechanical model
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no electron path for electron, can estimate
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electron cloud
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electrons
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heisenberg
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don't know where an electron is
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principle energy level
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n= (1,2,3....7..)
mac= 2n^2 |
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sub levels (orbitals)
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area around nucleus where it is likely to find electron
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s shape
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spherical
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p shape
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dumbell, figure 8
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d shape
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clover
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f shape
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complex
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electron configuration
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short hand method for describing how electrons are arranged in a nucleus
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aufbau principle
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states electrons will enter and fill orbitals of lowest energy first
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pauli exclusion principle
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no more than 2 electrons can occupy an orbital (opposite spin)
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Hund's Rule
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when electron occupy orbitals of equal energy then double up
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quantam numbers
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(address)**
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(n) the energy level
n=1,2,3... |
principle
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(l) the orbitals [s,p,d,f]
0-- (n-1) |
azimutal
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(m)exatly which orbital
(-l...0...l) |
magnetic
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(s) electrons sharing an orbita must have opposite spin
+1/2 or -1/2 |
spin
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copper
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green
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potassium
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purple
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sodium
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orange
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lithium
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red
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strontium
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orange red
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baryum
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yellow
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