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46 Cards in this Set
- Front
- Back
radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum
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electromagnetic radiation
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the distance between two consecutive peaks or troughs in a wave
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wavelength
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the number of waves (cycles) per second that pass a given point in space
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Frequency
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the constant relating the change in energy for a system to the frequency of the electromagnetic radiation absorbed or emitted; equal to 6.626 x 10-34 J x s
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Planck’s constant
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the concept that energy can occur only in discrete units called quanta
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quantization
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a quantum of electromagnetic radiation
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photon
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Einstein’s equation proposing that energy has a mass; E is energy, m is mass, and c is the speed of light
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E=mc2
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the statement that light exhibits both wave and particle properties
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dual nature of light
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the scattering of light from a regular array of points or lines, producing constructive and destructive interference
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diffraction
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a spectrum that exhibits all the wavelengths of visible light
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continuous spectrum
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a spectrum showing only certain discrete wavelengths
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line spectrum
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the lowest possible energy state of an atom or molecule
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ground state
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a stationary wave as on a string of a musical instrument; in the wave mechanical model, the electron in the hydrogen atom is considered to be a standing wave
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standing wave
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a function of the coordinates of an electron’s position in three dimensional space that describes the properties of the electron
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wave function
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a specific wave function for an electron in an atom. The square of this function gives the probability distribution for the electron
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orbital
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a model for the hydrogen atom in which the electron is assumed to behave as a standing wave
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quantum (wave) mechanical model
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a principle stating that there is a fundamental limitation to how precisely both the position and momentum of a particle can be known at a given time
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Heisenberg uncertainty principle
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the square of the wave function indicating the probability of finding an electron at a particular point in space
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probability distribution
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the quantum number relating to the size and energy of an orbital; it can have any positive integer value
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principal quantum number (n)
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the quantum number relating to the shape of an atomic orbital, which can assume any integral value from 0 to n-1 for each value of n
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angular quantum number- (l)
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the quantum number relating to the orientation of an orbital in space relative to the other orbital with the same l quantum number. It can have integral values between l and -l, including zero
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magnetic quantum number (ml)
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a set of orbital with a given azimuthal quantum number
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subshell
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an area of an orbital having zero electron probability
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node
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a group of orbital with the same energy
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degenerate orbitals
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a quantum number representing one of the two possible values for the electron spin; either +½ or -½
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electron spin quantum number
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in a given atom no two electrons can have the same set of four quantum numbers
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Pauli exclusion principle
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atom with more than one electron
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polyelectronic atoms
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the principle stating that as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to hydrogen-like orbitals
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aufbau principle
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the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli exclusion principle in a particular set of degenerate orbital, with all unpaired electrons having parallel spins
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Hund’s rule
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the electrons in the outermost principal quantum level of an atom
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valence electrons
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inner electrons in an atom; one not in the outermost (valence) principal quantum level
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core electrons
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several series of elements in which inner orbital (d or f) are being filled
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transition metals
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a group of 14 elements following lanthanum in the periodic table, in which the 4f orbital are being filled
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lanthanide series
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a group of 14 elements following actinium in the periodic table, in which the 5f orbital are being filled
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actinide series
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elements in the groups labeled 1A, 2A, 3A, 4A, 5A, 6A, 7A, and 8A in the periodic table. The group number gives the sum of the valence s and p electrons
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main-group elements (representative elements)
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the energy change associated with the addition of an electron to a gaseous atom
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electron affinity
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half the distance between the nuclei in a molecule consisting of identical atoms
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atomic radii
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elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties.
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metalloids (semimetals)
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inner electrons in an atom; one not in the outermost (valence) principal quantum level
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core electrons
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several series of elements in which inner orbital (d or f) are being filled
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transition metals
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a group of 14 elements following lanthanum in the periodic table, in which the 4f orbital are being filled
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lanthanide series
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a group of 14 elements following actinium in the periodic table, in which the 5f orbital are being filled
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actinide series
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elements in the groups labeled 1A, 2A, 3A, 4A, 5A, 6A, 7A, and 8A in the periodic table. The group number gives the sum of the valence s and p electrons
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main-group elements (representative elements)
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the energy change associated with the addition of an electron to a gaseous atom
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electron affinity
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half the distance between the nuclei in a molecule consisting of identical atoms
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atomic radii
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elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties.
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metalloids (semimetals)
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