7th Period Vocabulary for Discussion of How Atoms are Arranged (Chapter 4) Tanya
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| Electromagnetic radiation | a form of energy that exhibits wavelike behavior as it travels through space
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| Electromagnetic spectrum | all the forms of electromagnetic radiation
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| Wavelength | the distance between corresponding points on adjacent waves
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| Frequency | the number of waves that pass a given point in a specific time, usually one second
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| Visible Light | part of the electromagnetic spectrum that is roughly in the middle of the whole spectrum and is used by most organisms to be able to see
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| Velocity of a wave | product of wavelength and frequency
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| photoelectric effect | the emission of electrons from a metal when light shines on the metal
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| quantum | the minimum quantity of energy that can be gained or lost by an atom
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| Planck’s Constant | fundamental physical constant; h
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| Photon | a particle of electromagnetic radiation that has zero rest mass and carries a quantum of energy
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| Energy of a Photon | Ephoton
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| Ground State | the lowest energy state of an atom
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| Excited State | 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 | a series of specific wavelengths of emitted light created when the visible portion of light from excited atoms is shined through a prism
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| continuous spectrum | the emission of a continuous range of frequencies of electromagnetic radiation
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| Bohr radius | the radius of the s orbital in hydrogen
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| Interference | waves overlapping that results in a reduction of energy in some areas and an increase of energy in others
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| Heisenberg Uncertainty Principle | it is impossible to determine simultaneously both the position and velocity of an electron or any other particle
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| Quantum Theory or Quantum Mechanics | a mathematical description of the wave properties of electrons and other very small particles
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| Orbital | a three-dimensional region around the nucleus that indicates the probable location of an electron
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| Quantum numbers | numbers that specify the properties of atomic orbitals and the properties of electrons in orbitals
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| Principle Quantum number (n) | the quantum number that indicates the main energy level occupied by the electron
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| Angular momentum quantum number (l ) | the quantum number that indicates the shape of the orbital
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| Magnetic quantum number (m) | the quantum number that indicates the orientation of an orbital around the nucleus
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| Spin quantum number (s) | the quantum number that has only two possible values, +1/2 and -1/2, which indicate the two fundamental spin states of an electron in an orbital
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| Aufban Principle | an electron occupies the lowest- energy orbital that can receive it
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| Electron Configuration | the arrangement of electrons in an atom
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| Pauli Exclusion Principle | no two electrons in the same atom can have the same set of four quantum numbers
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| Hund’s Rule | 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
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| Valence Electron | an electron that is available to be lost, gained, or shared in the formation of chemical compounds
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| Inner-shell electrons | electrons that are not in the highest occupied energy level
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| Highest occupied level | the electron-containing main energy level with the highest principal quantum number
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| Noble Gas Configuration | an outer main energy level fully occupied, in most cases, by eight electrons
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| s sublevel or sub-orbital | spherical shaped; only one sublevel is possible per n value
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| p sublevel or sub-orbital | dumbbell shaped; three sub levels possible per p n value (x, y, z axis)
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| f sublevel or sub-orbital | more complex shaped; seven sub levels possible per n value
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