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60 Cards in this Set
- Front
- Back
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Photoelectric effect |
Electrons are ejected from charged metal surfaces |
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Quantum theory |
Structure of matter at atomic level |
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Wavelength |
Distance from crest to crest or trough to trough |
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Frequency |
Number of times a wave passes a point per unit of time |
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Amplitude |
The heigh of the crest of depth of the trough |
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Wavelength and frequency related by |
λν = c |
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Atomic absorption spectra |
Characteristic dark lines produced when external source of light passes through free gaseous atoms |
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Atomic emission spectra |
Characteristic patterned of bright lines produced when atoms are vaporized in high temperature flames |
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Black body radiation |
Absorbs light when cold and emit when it's hot |
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Radiant energy is |
Quantized |
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Quantum |
Smallest discrete quantity of energy |
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Photon |
A quantum of electromagnetic radiation |
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Energy of photon |
E=hv or E=hc/ H= 6.626x10^-34 j•s |
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Quantized states |
Discrete energy levels |
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Work function ϕ |
Amount of energy needed to dialogue an electron from the surface of a metal |
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Work function equation |
Back (Definition) |
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Johann balmer |
Formulated empirical equation from experimental results no theoretical explanation. It fits with hydrogen emission spectrum |
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Electromagnetic radiation |
Any forms 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 ultraviolet rays visible light infrared radiation and radio waves |
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Photoelectric effect |
The release of electrons from a material as a result of electromagnetic radiation stoking it |
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Threshold frequency (Vo) |
The minimum frequency of light required to produce the photoelectric effect |
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Ground state |
Most stable, lowest energy state of a particle |
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Ground state |
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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Ground state |
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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Ground state |
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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Heisenberg uncertainty principle |
The principle that one cannot simultaneously know the exact position and the exact momentum of an electron |
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Ground state |
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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Heisenberg uncertainty principle |
The principle that one cannot simultaneously know the exact position and the exact momentum of an electron |
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Quantum number |
One of the 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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Angular momentum quantum number (l) |
An integer having any values from 0 to n (n-1) that defines the shape of an orbital |
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Angular momentum quantum number (l) |
An integer having any values from 0 to n (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 |
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Quantum number chart |
Back (Definition) |
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Spin quantum number |
+ 1/2 or -1/2 |
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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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P orbital shape |
Back (Definition) |
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P orbital shape |
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D orbital shape |
Back (Definition) |
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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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Core electrons |
Inner shell in an atom or ion that are not involved in chemical rxn |
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Core electrons |
Inner shell in an atom or ion that are not involved in chemical rxn |
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Valence electrons |
Electrons in the outermost occupied shell of an atom have the most influence on the atoms chemical behavior |
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Core electrons |
Inner shell in an atom or ion that are not involved in chemical rxn |
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Valence electrons |
Electrons in the outermost occupied shell of an atom have the most influence on the atoms chemical behavior |
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Valence shell |
Outer most occupied shell of an atom |
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Core electrons |
Inner shell in an atom or ion that are not involved in chemical rxn |
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Valence electrons |
Electrons in the outermost occupied shell of an atom have the most influence on the atoms chemical behavior |
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Valence shell |
Outer most occupied shell of an atom |
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Hunds rule |
Lowest energy electron configuration of an atom has the maximum number of unpaired electrons |
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Isoelectronic |
Describes atoms or ions that have identical electron configuration |
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Ionization energy |
The amount of energy required to remove 1 mole of electrons from 1 mole of ground state atoms or ions in the gas phase |
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Ionization energy |
The amount of energy required 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 |
Energy change that occurs when 1 mole of electrons combines with 1 mole of atoms or ions in the gas phase |
