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Aufbau Principle
States that when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy
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Pauli Exclusion Principle
within an atom, no two electrons can have the same set of quantum numbers
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Hund's Rule
when an electron is added to a subshell, it will always occupy an empty orbital if one is available
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Diamagnetic elements
- have all of their electrons spin paired
- not affected by magnetic fields
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Paramagnetic Elements
- do not have all of their electrons spin paired
- affected by magnetic fields
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Quantized
electrons can only exist at specific energy levels, separated by specific intervals
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Milikan's Experiment
able to calculate the charge on an electron by examining the behavior of charged oil drops in an electric field
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Thomson's Experiment
watched the deflection of charges in a cathode ray tube and put forth the idea that atoms are composed of positive and negative charges
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Rutherford's Experiment
led him to conclude that all of the positive charge in an atom was concentrated in the center and that an atom is mostly empty space
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Neils Bohr
- took quantum theory and used it to predict that electrons orbit the nucleus at specific fixed radii, like planets orbiting the Sun
- does not work for complex atoms
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Heisenburg Uncertainty Principle
it is impossible to know both the position and momentum of an electron at a particular instant
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