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44 Cards in this Set
- Front
- Back
Electromagnetic Radiation |
Any form of radiant energy in the electromagnetic spectrum |
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Electromagnetic Spectrum |
A continuous range of radiant energy that includes gamma rays, X-rays, ultraviolent radiation, visible light, infrared radiation, and radio waves |
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Wavelength (λ) |
The distance from crest to crest or trough to trough on a wave |
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Frequency (ν) |
The number of crests of a wave that pass a stationary point of reference per second |
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Hertz (Hz) |
The SI unit of frequency with units of reciprocal seconds: 1 Hz = 1 s^-1 = 1 cycle per second (cps) |
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Fraunhofer Lines |
A set of dark lines in the otherwise continuous solar spectrum |
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Atomic Emission Spectra |
Characteristic patterns of bright lines produced when atoms are vaporized in high-temperature flames or electrical discharges |
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Atomic Absorption Spectra |
Characteristic patterns of dark lines produced when an external source of radiation passes through free, gaseous atoms |
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Quantum |
The smallest discrete quantity of a particular form of energy |
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Planck Constant (h) |
The proportionality constant between the energy and frequency of electromagnetic radiation expressed in E = hv; h = 6.626 x 10^-34 J x s |
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Quantum Theory |
A model based on the idea that energy is absorbed and emitted in discrete quantities of energy called quanta |
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Quantized |
Having values restricted to whole-number multiples of a specific base value |
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Photon |
A quantum of electromagnetic radiation |
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Photoelectric Effect |
The release of electrons from a material as a result of electromagnetic radiation striking it |
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Threshold Frequency (v0) |
The minimum frequency of light required to produce the photoelectric effect |
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Work Function (Φ) |
The amount of energy needed to dislodge an electron from the surface of a material |
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Ground State |
The most stable, lowest energy state of a particle |
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Excited State |
Any energy state above the ground state |
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Electron Transition |
Movement of an electron between energy levels |
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Matter Wave |
The wave associated with any moving partible |
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Standing Wave |
A wave confined to a given space with a wavelength λ related to the length L of the space by L = n(λ/2), where n is a whole number |
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Node |
A location in a standing wave that experiences no displacement |
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Heisenberg Uncertainty Principle |
The principle that one cannot simultaneously know the exact position and the exact momentum of an elevation |
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Wave Mechanics or Quantum Mechanics |
A mathematical description of the wavelike behavior of electrons and other particles |
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Schrodinger Wave Equation |
A description of how the electron matter wave varies with location and time around the nucleus of a hydrogen atom |
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Wave Function (φ) |
A solution to the Schrodinger wave equation |
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Orbitals |
Defined by the square of the wave function (φ^2); regions in an atoms where the probability of finding and electron is high |
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Quantum Number |
One of four related numbers that specify the energy, shape, and orientation of orbitals in an atom and the spin orientation of electrons in the orbitals |
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Principal Quantum Number (n) |
A positive integer describing the relative size and energy of an atomic orbital or group of orbitals in an atom |
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Angular Momentum Quantum Number (cursive l) |
An integer having any value from 0 to (n-1) that defines the shape of an orbital |
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Magnetic Quantum Number (ml) |
Defines the orientation of an orbital in space; an integer that may have any value from -l to +l, where l is the angular momentum quantum number |
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Spin Quantum Number (ms) |
Either +1/2 or -1/2, indicating the spin orientation of an electron |
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Pauli Exclusion Principle |
No two electrons in an atom can have the same set of four quantum numbers |
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Aufbau Principle |
The method of building electron configurations of atoms by adding one electron at a time as atomic number increases across the rows of the periodic table |
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Electron Configuration |
The distribution of electrons among the orbitals or an atom or ions |
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Effective Nuclear Charge (Zeff) |
The attraction toward the nucleus experienced by an electron in an atom; the positive charge on the nucleus reduced by the extent to which other electrons in the atom shield the electron from the nucleus |
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Core Electrons |
Electrons in the filled, inner shells in an atom or ion that are not involved in chemical reactions |
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Valence Electrons |
Electrons in the outermost occupied shell of an atom having the most influence on the atom's chemical behavior |
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Valence Shell |
The outermost occupied shell of an atom |
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Hund's Rule |
The lowest energy electron configuration of an atom has the maximum number of unpaired electrons, all of which have the same spin, in degenerate orbitals |
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Orbital Diagram |
Depiction of the arrangement of electrons in an atom or ion using boxes to represent orbitals |
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Isoelectronic |
Describes atoms or ions that have identical electron configuration |
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Ionization Energy (IE) |
The amount of energy needed to remove 1 mole of electrons from 1 mole of ground-state atoms or ions in the gas phase |
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Electron Affinity (EA) |
The energy change that occurs when 1 mole of electrons combines with 1 mole of atoms or ions in the gas phase |