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| electromagnetic radiation |
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Definition
| Form of energy that exhibits wavelike behavior as it travels through empty space. Example: visible light. |
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| Shortest distance between equivalent points on a continuous wave( usually expressed in m, cm, or nm... 1nm= 1x10^-9 m ) |
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| The # of waves that pass a given point per second. The S.I. unit is Hertz(Hz). One Hz= 1 wave per second. |
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| The wave's height from the origin to a crest, or from the origin to a trough, not affected by wavelength or frequency. |
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| Electromagnetic Spectrum(EM spectrum) |
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Definition
| Includes all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths. |
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| The minimum amount of energy that can be gained or lost by an atom. |
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| Has value of 6.626x10^-34 J.S. J stands for joule( S.I. unit of energy) |
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| Photoelectrons are emitted from a metal's surface when light of a certain frequency, or higher than a certain frequency shines on the surface. |
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| Massless particle that carries a quantum of energy. E photon= hv. the E is energy, h is plancks constant, and v is velocity |
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| The set of frequencies of the electromagnetic waves emmited by atoms of the element. this can identify an element. |
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| Lowest allowable energy state of an atom. Example: when an atom gains energy, it's in an excited state. |
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| The number assigned to each orbit of an electron. |
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| Predicts that all moving particles have wave characteristics. wavelength= h/mv |
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| Heisenberg uncertainty principle |
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Definition
| it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time. |
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| Quantum Mechanical Model of The Atom(Wave mechanical Model of The Atom) |
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Definition
| Atomic model in which electrons are treated as waves. |
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| 3-dimensional region around the nucleus of an atom that describes an electron's probable location. |
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| Assigned by the quantum mechanical model to indicate the relative sizes and energies of atomic orbitals. |
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| The major energy level of an atom. |
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| The energy level contained within a principal energy level. |
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| Arrangement of electrons in an atom, which is prescribed by three rules- the aufbau principle, the Pauli Exclusion principle, and Hund's rule. |
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Definition
| Each electron occupies the lowest energy orbital available. |
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| Pauli Exclusion principle |
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Definition
| A maximum of 2 electrons can occupy an atomic orbital but only if the electrons have opposite spins. |
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Definition
| Single electrons with the same spin must occupy each equal- energy orbital before additional electrons with opposite spins can occupy the same orbitals. |
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| Electron in an atom's outermost orbital; determines the chemical properties of an element. |
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| Has the element's symbol, representing the atomic nucleus and inner-level electrons, that is surrounded by dots, representing the atom's valence electrons. |
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