Stack #155221
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| a form of energy that exhibits wavelike behavior as it travels through space | Electromagnetic Radiation
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| all the forms of electromagnetic radiation | Electromagnetic Spectrum
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| the distance between corresponding points on adjacent waves | Wavelength
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| the number of waves that pass a given point in a specific time, usually one second | Frequency
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| the emission of electrons from a metal when light shines on the metal | Photoelectric effect
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| the minimum quantity of energy that can be lost or gained by an atom | Quantum
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| a particle of electromagnetic radiation having zero mass and carrying a quantum of energy | Photon
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| the lowest energy state of an atom | Ground state
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| a state in which an atom has a higher potential energy than it has in its ground state | Excited state
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| when a narrow beam of the emitted light was shined through a prism, it was separated into a series of specific frequencies (and therefore specific wavelengths) of visible light – the bands of light are part of the line-emission spectrum | Line-emission spectrum
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| the emission of a continuous range of frequencies of electromagnetic radiation | Continuous spectrum
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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 | Heisenberg uncertainty principle
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| describes mathematically the waves properties of electrons and other very small particles | Quantum theory
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| a three-dimensional region around the nucleus that indicates the probable location of an electron | Orbital
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| specify the properties of atomic orbitals and the properties of electrons in orbitals | Quantum numbers
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| symbolized by n, indicates the main energy level occupied by the electron | Principal quantum number
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| symbolized by l, indicates the shape of the orbital | Angular momentum quantum number
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| symbolized by m, indicates the orientation of an orbital around the nucleus | Magnetic 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 orbital | Spin quantum number
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| the arrangement of electrons in an atom | Electron configuration
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| an electron occupies the lowest energy orbital that can receive it | Aufbau principle
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| no 2 electrons in the same atom can have the same set of four quantum numbers | Pauli exclusion principle
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| orbitals of equal energy are each occupied by one electron before any orbital is occupied b a second electron, and all electrons in singly occupied orbitals must have the same spin | Hund’s rule
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| electrons that are not in the highest occupied energy level | Inner-shell electrons
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| the Group 18 elements (helium, neon, argon, krypton, xenon, and radon) | Noble gasses
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| outer main energy level fully occupied [most cases-by 8 electrons] | Noble-gas configuration
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Created by:
ElizabethI
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