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| emission of electrons from a metal when light shines on it |
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| a particle of electromagnetic radiation having zero mass and carrying a quantum of energy leaving an atom |
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| state of low/regular energy |
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| proposed that electrons might have a wave-particle duality and proposed the correct explanation of why electrons may have only certain energies |
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| developed equation which treated electrons as moving around the nucleus in wave-like fashion which allowed for predicting electron locations |
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| Heisenberg Uncertainty Principle: it's impossible to measure both velocity & position of an electron at the same time |
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| indicates the main energy level occupied by the electron |
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| indicates the shape of the orbital |
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| indicates orientation of an orbital around the nucleus |
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| indicates direction of electron spin |
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| Pauli Exclusion Principle |
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| no 2 electrons in the same atom can have the same set of 4 quantum #s |
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| an electron occupies the lowest energy orbital that can receive it |
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- orbitals of equal energy are each occupied by 1 electron before any one orbital is occupied by a second electron
- all electrons in singly-occupied orbitals must have the same spin
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| Electron-Configuration Notation |
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| 4 different orbitals and their shapes |
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| speed of light (constant) |
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