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22 Cards in this Set
- Front
- Back
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Excited state (of an electron) |
Highest energy level |
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Ground state (pertaining to an electron) |
Lowest energy level |
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When an e- is excited, it absorbs energy (photons). As is it falls back from the excited state to ground state, it releases the energy in the form of light. |
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E=hv |
V=frequency H=planck's constant (6.626×10^ -34) E=energy |
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Frequency |
The higher the frequency, the higher the energy. |
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deBroglie |
E- have dual waves and particle natjre E=hv -to determine energy from the wavelength E- are considered waves around nucleus |
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R O Y G B I V |
- visible light spectrum - red= longest wavelength, lowest frequency - violet= shortest wavelength, highest frequency |
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Hund's Rule |
Fill all orbitals with ONE e- before you double them up |
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Pauli Expulsion Principle |
No two e- can have the same four quantum numbers |
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Auffbau Principle |
An e- will occupy the lowest orbital that can receive it |
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Eisenburg |
You CANNOT detect the location or velocity of an e- |
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Chromim Copper Tungsten |
Don't follow the rules because they are more stable in a lower configuration |
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2n^2= |
Number of electrons *n=energy level |
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Speed of light |
3×10^8 |
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Quantum Numbers |
Principle Quantum Number: n, energy level, 1- 7 Angular Momentum Number: l, shape, s=○, p=dumbell Magnetic Number: orientation of orbital around 0 Spin: opposite spins, +1/2 - 1/2 |
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Bohr Model |
E- travel in orbitals around the nucleus- WRONG!!! |
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Always a Noble Gas if... |
8 e- in highest energy level (1,2,3,4,5...) All sublevels are full--> NONREACTIVE |
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Photoectric effect |
When you shine light on metal, it releases e- |
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Quantum |
Minimum quantity of energy that can be lost or gained by an atom |
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Photon |
Particle of electromagnetic radiation that has 0 mass and carries quantum energy |
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Electromagnetic radiation |
Form of energy that exhibits wave-like behavior |
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Electron configuration |
Arrangement of e- Ground state e- co figuration Lowest energy arrangement |
