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36 Cards in this Set
- Front
- Back
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Excited State
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State in which an electron has a higher energy than it normally should
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Orbital
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Three-Dimensional space around the nucleus that indicates the probable location of an electron of certain energy
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Photon
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Quantum of energy
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Frequency
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Number of waves that pass a given point in a specific time
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N
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Tells the energy level of the electron
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M
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Tells which orbital in a set of orbitals
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S
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Tells the spin of the electron
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Quantum
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Minimum quantity of energy that can be lost or gained by an atom
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Noble- Gas Configuration
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An outer main energy level fully occupied
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Inner Shell Electrons
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Elecrons that are not in the highest occupied energy level
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Quantum Theory
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Describes mathematically the wave properties of electrons
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Electromagnetic Radiation
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Form of energy that exhibits wavelike behavior
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Ground State
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Lowest energy state of an electron
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Photoelectric Effect
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Emission of electrons from a metal when light shines on the metal
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Wavelength
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Distance between corresponding points on adjacent waves
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L
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Tells which type of orbital
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Aufbau Principle
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An electron occupies the lowest energy orbital that can receive it
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Pauli Exclusion Principle
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No two electrons in the same atom can have the same set of four quantum numbers
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Hund's Rule
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Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron
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Heisenberg's Uncertainty Principle
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It is impossible to determine simultaneously both the postion and velocity of an electron at the same time
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Number of Orbitals
S |
1
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Number of Orbitals
P |
3
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Number of Orbitals
D |
5
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Number of Orbitals
F |
7
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Electrons per Orbital
S |
2
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Electrons per Orbital
P |
6
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Electrons per Orbital
D |
10
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Electrons per Orbital
F |
14
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Electrons per Level
1 st Level |
2
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Electrons per Level
2 nd Level |
8
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Electrons per Level
3 rd Level |
18
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Electrons per Level
4 th Level |
32
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Shape of S
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Sphere
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Shape of P
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Pear
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Shape of D
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Double Pear
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Shape of F
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Fancy
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