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Unique light patterns emitted by excited atoms
All wavelengths present; smooth rainbow red to violet
Hot solids or liquids (e.g. tungsten filaments)
Specific wavelengths as distinct lines on dark background
Hot gases or electric discharge through gas
Electrons exist only in specific energy levels, not in between
n=1n = 1n=1, lowest energy level where electrons normally exist
n=2,3,4n = 2, 3, 4n=2,3,4, etc.; higher energy levels above ground state
A fixed energy value that an electron in an atom can have
Electron falls to lower level, energy released as photon
E=hfE = hfE=hf where hhh is Planck's constant, fff is frequency
h=6.63×10−34h = 6.63 \times 10^{-34}h=6.63×10−34 J·s
c=fλc = f\lambdac=fλ where c=3.00×108c = 3.00 \times 10^8c=3.00×108 m/s
Inversely related: higher energy = shorter wavelength (bluer)
Visible spectral lines from transitions ending at n=2n = 2n=2
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