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25 Cards in this Set
- Front
- Back
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A negatively charged subatomic particle having a tiny mass |
Electron (e^ -) |
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A positively charged subatomic particle having an approximate mass of 1 amu |
Proton (p +) |
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A neutral subatomic particle having an approximate mass of 1 amu |
Neutron (n^0) |
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A region in the center of an atom containing protons and neutrons |
Atomic nucleus |
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A value indicating the number of protons in the nucleus of an atom |
Atomic number (Z) |
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A value indicating the number of protons and neutrons in the nucleus of an atom |
Mass Number (A) |
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A symbolic method for expressing the composition of an atomic nucleus |
Atomic notation |
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Atoms of the same element that have a different number of neutrons |
Isotope |
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A unit of mass exactly equal to 1/2 the mass of a C-12 atom |
Atomic mass Unit (amu) |
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The average mass of all the naturally occurring isotopes of an element |
Atomic Mass |
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The distance a light wave travels to complete one cycle |
Wavelength |
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The number of times a light wave completes a cycle in one second |
Frequency |
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The general term that can refer to either visible or invisible radiant energy |
Light |
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A range of light energy extending from violet to red, that is, approximately 400-700 nm |
Visible spectrum |
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A range of light energy extending from gamma rays to microwaves |
Radiant energy spectrum |
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A band of light energy that is uninterrupted |
Continuous Spectrum |
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A particle of radiant energy |
Photon |
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A model of the atom that describes electrons circling the nucleus in orbits |
Bohr atom |
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An orbit of specific energy that electrons occupy as they circle the nucleus |
Energy level |
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A collection of narrow bands of light produced by atoms of a given element releasing energy |
Emission line spectrum |
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An Electron energy level that results from splitting a main energy level |
Energy Sublevel |
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A shorthand description of the arrangement of electrons by sublevels according to increasing energy |
Electron configuration |
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The statement that is impossible to precisely measure the location and energy of a particle at the same time |
Uncertainty Principle |
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A sophisticated model of the atom that describes the energy of an Electron in terms of its probability of being found in a particular location about the nucleus |
Quantum mechanical Atom |
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A region about the nucleus in which there is a high probability of finding an electron with a given energy |
Orbital |
