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16 Cards in this Set

  • Front
  • Back
Hund's rule
orbitals of equal enery are each occupied by one electron before any orbital is occupied by a second electron and all electrons in singly occupied orbitals have the same spin
highest occupied level
the eletron-containing main energy level with the highest principal quantum number
inner-shell electrons
electrons that are not in the highest occupied energy level
noble gases
group 18 elements
heisenberg uncertainty principle
it is impossible to deteermine simultaneously both the position and velocity of an electron or any other particle
noble-gas configuration
an outer aim energy level fully occupied, in most cases, by 8 electrons
quantum theory
describes mathematically the wave properties of electrons and other very small particles
angular momentum quantum number
symbolized by l, indicates shape of the orbital
magnetic quantum number
symbolized by m, indicates the orientation of an orbital around the nucleus
spin quantum number
2 possible values, -1/2, +1/2

which indicate the two fundamental spin states of an electron in an orbital
electron configuration
arrangement of electrons in an atom
Aufbau principle
an electron occupies the lowest energy orbital that can recieve it
Pauli Exclusion Principle
no two electrons in the same atom can have the same set of four quantum numbers
principal quantum number
symbolized by n, indicates the main energy level occupied by the electron
quantum numbers
specify the properties of atomic orbitals and the properties of electrons in orbitals
three dimensional region around the nucleus that indicates the probably location of an electron