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25 Cards in this Set
- Front
- Back
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Electromagnetic Radiation
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A form of energy that exhibits wavelike behavior as it travels through space
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Electromagnetic Spectrum
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together, all the forms of electromagnetic radiation forms this
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Wavelength
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The distance between corresponding points on adjacent waves.
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Frequency (v)
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The number of waves that pass a given point in a specific time, usually one second.
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Photoelectric Effect
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The emission of electrons from a metal when light shines on the metal.
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Quantum
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The minimum quantity of energy that can be lost or gained by an atom.
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Photon
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A particle of electromagnetic radiation having zero mass and carrying a quantum of energy.
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Ground State
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Lowest energy state of an atom.
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Excited State
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a state in which an atom has a higher potential energy than it has in its ground state.
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Line-Emission Spectrum
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When a narrow beam of the emitted light was shined through a prism, it was separated into four specific colors of the visible spectrum. The four bonds of light were known as this.
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Continuous Spectrum
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The emission of a continuous range of frequencies of electromagnetic radiation.
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Heisenberg Uncertainty Principle
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States that it is impossible to determine simultaneously both the position and the velocity of an electron or any other particle.
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Quantum Theory
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Describes mathematically the wave properties of electrons and other very small particles.
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Orbital
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A three dimensional region around the nucleus that indicates the probable location of an electron
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Quantum Numbers
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Specify the properties of atomic orbitals and the properties of electrons in orbitals.
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Principal Quantum number
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Symbolized by n, indicates the main energy level occupied by the electron.
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Angular Momentum Quantum Number
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Specialized by l, indicates the shape of the orbital.
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Magnetic Quantum Number
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Symbolized by m, indicates the orientation of an orbital around the nucleus.
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Spin quantum number
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Has only two possible values: (+1/2, -1/2): which indicate the two fundamental spin states of an electron in an orbital
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Electron Configuration
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the arrangement of electrons in an atom
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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, and all electrons in singly occupied orbitals must have the same spin state.
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Noble Gases
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the Group 18 elements (Helium, Argon, Krypton, Xenon, and Radon)
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Noble-Gas configuration
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refers to an outer main energy level occupied, in most cases, by eight electrons
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