Vocabulary
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each of the black spaces below before clicking
on it to display the answer.
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| Electromagnetic radiation-a form of energy that exhibits wavelike behavior as it travels trough 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-Electromagnetic radiation in this range of wavelengths |
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| Velocity of a wave- |
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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-a physical constant reflecting the sizes of quanta in quantum mechanics 6.626068 × 10-34 m2 kg / s |
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| Photon-a paricles of electromagnetic radiation that has zero rest mass and carries a quantum of energy |
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| Energy of a Photon-depends on the frequency or the radiation |
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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 it's 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- |
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| Interference-The wave properties of light lead to interference, but certain conditions of coherence must be met for these interference effects to be readily visible |
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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 (same definition for both of these so list them together)-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 locationof an electron |
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| Quantum numbers-a number that specifies 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-an electron that is not in 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 electrons |
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| s sublevel or sub-orbital-n=1,in an nth main energy level there are n Sublevels |
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| p sublevel or sub-orbital-n=2,,in an nth main energy level there are n Sublevels |
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| f sublevel or sub-orbital-n=4,in an nth main energy level there are n Sublevels |
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Created by:
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