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| explained atomic emission spectra; E=hv |
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- e- travel circular paths (orbits) around nucleus
- e- have fixed amount of energy; e- located at certain energy levels
student of Rutherford; Danish physicist
one e- system: Atomic Emission Spectrum of H atom |
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| Spectral lines: set of wavelengths e- goes to n=1, UV light given off |
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| e- goes to n=2, visible light given off |
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| e- goes to n=3, infrared light given off |
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all matter has wave and particle characteristics
λ = h/mv
*v:velocity |
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| -- Uncertainty Principle: impossible to know momentum and position of particle at same time; disproves Bohr's e- orbit idea |
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| mathematical model of the atom (quantum mechanical model) |
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| e- enters orbitals of lowest energy first |
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| Pauli Exclusion Principle |
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| an atomic orbital contains a max or 2e- with opposite spins |
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| when e- occupy orbitals of = energy, one e- enters each orbital until all orbitals... up up up |
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| Octet Rule: atoms gain or lose e- in order to obtain e- configuration of noble gas |
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described tiny packets of Radiant Energy as photons: behave as paricles not waves (Planck's theory)
E=mc2 |
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