atoms quantized energy 1.bohr model of the atom 2.standing waves 3.quantum energy of colors
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ATOMS Quantized Energy
1. Bohr model of the atom 2. Standing waves3. Quantum energy of colors
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Bohr Model (particle picture)Assumptions• Nuclear model• Discrete electron orbits n = 1,2,3,..• Light absorbed/emitted as quantum of energy when electron jumps orbit• Energy change = h f
= Planck constant x light frequency*
* Speed = frequency x wavelength c = f λ
Bohr’s Hydrogen Formula
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Explains Hydrogen visible colors (Balmer spectrum, jumps to n=2)
Predicted Hydrogen UV spectrum(jumps to n=1)
Led to atomic understanding of Chemistry… and huge fame for Bohr
WHY discrete orbits?
Electrons as Matter waves
Standing Waves
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Analogy: Standing waves on a stringWavelength
λ = 2L
λ = L
λ = 2L/3
λ = L/2
.
.
λ = 2L/n
1st Harmonic(Fundamental)
2nd Harmonic
3rd Harmonic
.
.
.
Sound waves – Origin of character of musical notes
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AnswerElectron Standing Waves (3 dimensional)
Only discrete electron λ fits* in atom
De Broglie p = h / λ Discrete electron momentum & energy
Discrete photon frequency when electron jumps between energy
*Fit = constructive interference
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Schrodinger’s Equation for atoms
• Electron (probability) standing waves
• Discrete energy changes -> discrete photon wavelengths emitted/absorbed
• Characteristic colors of materials (analogy to sounds of musical notes)
• Lowest (fundamental, n=1 ) standing wave -> atomic stability