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the spontaneous emission of radiation accompanying a nuclear reaction
Radioactive
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a radioactive isotope
Radioisotopes
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a type of radioactive emission consisting of electrons. Stream of particles repelled by negative charged electrode and attracted to positive charge
Beta radiation
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type of radioactive emission consisting of a stream of high energy photons. Unaffected by either positive or negatively charged electrodes
Gamma radiation
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a nuclear reaction that converts a proton into a neutron plus an ejected positron
positron emission
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a type of radioactive emission; a helium nucleus. Consists of a stream of electrons repelled by positively charged electrodes and attracted to negatively charges. Have mass to charge ratio identifying them as helium nuclei 42He2+.
Alpha radiation
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a general term for both protons and neutrons
Nucleons
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a nuclear reaction in which a proton in the nucleus captures an inner-shell electron and is thereby converted into a neutron
Electron capture
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showed that there were three common types of radiation with markedly different properties, alpha, beta, and gamma
Ernest Rutheford (1871-1937) in 1897
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electromagnetic radiation
Radiant energy
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the range of different kinds of electromagnetic radiation
Electromagnetic spectrum
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the number of wave maxima that pass by a fixed point per unit of time
Frequency
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the length of a wave from one maximum to the next
Wavelength
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a waves height measured from the midpoint between peak and trough
Amplitude
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an equation that accounts for all lines in the hydrogen spectrum
Balmer-Rydberg equation
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the ejection of electrons from a metal on exposure to radiant energy.Photons – The smallest possible amount of radiant energy; a quantum
Photoelectric effect
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(h) 6.626 x 10-34J x s; a fundamental physical constant that relates energy to frequency, E=hv.
Planck’s postulate
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the amount of energy necessary to eject an electron from a metal
Work function
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the smallest possible amount of radiant energy
Quantum
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an equation that relates mass, wavelength, and velocity, m=h/lv
De Broglie hypothesis
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a model of atomic structure that concentrates on an electrons wave-like properties.
Quantum mechanical model
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the position and the velocity of an electron can never both be known beyond a certain level of certainty.
Heisenbergs uncertainty principle
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a grouping of orbitals according to principle quantum number
Shells
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a grouping of orbitals by angular-momentum quantum number
Subshells
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a region where a wave has zero amplitude
Node
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(ms) a variable that describes the spin of an electron, either +1/2 or – ½.
Spin quantum number
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No two electrons in an atom can have the same four quantum numbers.
Pauli exclusion principle
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a set of rules that guides the electron filling order of orbitals in atoms.
Aufbau principle
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the lowest-energy electron configuration of an atom.
Ground-state electron configuration
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having the same energy level.
Degenerate
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If two or more orbitals with the same energy are available, one electron goes into each until all are half full. The electrons in each of the singly occupied orbitals must have the same value for their spin quantum number.
Hund’s rule
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an element in groups 1A or 2A, in which s orbitals are filled.
s-block elements
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an element in groups 3A-8A, in which p orbitals are filled.
p-block elements
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a transition metal orbital in which d orbitals are filled.
d-block elements
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a lanthanide or actinide element in which f orbitals are filled.
f-block elements
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What fills up after 1s2?
2s2
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What fills up after2s2?
2p6
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What fills up after2p6?
3s2
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What fills up after 3s2?
3p6
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What fills up after 3p6?
4s2
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What fills up after 4s2?
3d10
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Electrons are pulled from 4s orbital before what?
3d
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