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22 Cards in this Set
- Front
- Back
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Short hand |
[ ] X spdf^x |
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Long hand |
X spdf ^x |
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Orbital |
Arrows |
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Principal quantum number |
Energy level |
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Angular momentum quantum number |
Shape |
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Magnetic quantum number |
Orientation |
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Spin quantum number |
+ or - 1/2; clockwise/counter-clockwise |
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Aufbau |
Have to fill previous sublevel before moving on to the next |
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Hund |
Each orbital must have one electron before a second is added |
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Pauli exclusion |
No 2 electrons can have the same set of four quantum numbers |
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S orbital |
Spherical, 1 orientation, holds up to 2 electrons |
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P orbital |
Peanut, 2nd energy level, 3 orientations, holds up to 6 electrons |
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D orbital |
4 leaf clover, 3rd energy level, 5 orientations, holds up to 10 electrons |
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F orbital |
Mix of d and p shape, 4th energy level, 7 orientations, holds up to 14 electrons |
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Each orbital can hold up to __ electrons |
2 |
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Principal Energy Level equation |
2n^2 |
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Dot notation order |
1, 2, skip transition metals, 3, 4, 5, 6, 7, 8 (transition metals have 2) |
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De Broglie |
Electron behavior might be explained if we treat electrons, as a particle, as a wave |
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Heisenberg |
Can't know both the position and energy/speed of a particle at the same time |
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Schrödinger |
Derived from an equation that treated the hydrogen atom's electron as a wave Wave equation provided scientists a means to work around Heisenberg's dilemma |
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Energy level variable |
n |
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# of orbitals variable |
n^2 |
