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22 Cards in this Set
- Front
- Back
Short hand |
[ ] X spdf^x |
|
Long hand |
X spdf ^x |
|
Orbital |
Arrows |
|
Principal quantum number |
Energy level |
|
Angular momentum quantum number |
Shape |
|
Magnetic quantum number |
Orientation |
|
Spin quantum number |
+ or - 1/2; clockwise/counter-clockwise |
|
Aufbau |
Have to fill previous sublevel before moving on to the next |
|
Hund |
Each orbital must have one electron before a second is added |
|
Pauli exclusion |
No 2 electrons can have the same set of four quantum numbers |
|
S orbital |
Spherical, 1 orientation, holds up to 2 electrons |
|
P orbital |
Peanut, 2nd energy level, 3 orientations, holds up to 6 electrons |
|
D orbital |
4 leaf clover, 3rd energy level, 5 orientations, holds up to 10 electrons |
|
F orbital |
Mix of d and p shape, 4th energy level, 7 orientations, holds up to 14 electrons |
|
Each orbital can hold up to __ electrons |
2 |
|
Principal Energy Level equation |
2n^2 |
|
Dot notation order |
1, 2, skip transition metals, 3, 4, 5, 6, 7, 8 (transition metals have 2) |
|
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 |
|
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 |
|
Energy level variable |
n |
|
# of orbitals variable |
n^2 |