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28 Cards in this Set
- Front
- Back
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mathmatical expression describing probability of finding an electron at various locations
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atomic orbital
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rule that electrons occupy orbitals of lowest energy first
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aufbau principle
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arrangement of electrons of an atom in its ground state into various orbitals
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electron configuration
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specific energies an electron in an atom can have
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energy level
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corresponds to an orbital of a different shape. SPDF
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sublevel
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lowest possible energy of an electron
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ground state
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high energy levels of an electron
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excited state
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impossible to know exactly both velocity and position of particle at same time
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Heinsberg's uncertainty principle
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one electron is on an orbital till each orbital has one. then pairing begins.
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Hund's Rule
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an atomic orbitalcan hold 2 electrons, with opposite spin
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Pauli Exclusion Principle
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any atom with a positive charge
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cation
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any atom with a negative charge
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anion
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atom or group of atoms with a negative or positive charge
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ion
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any metal in Group 1A of periodic table
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alkali metal
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any metal in group 2A of periodic table
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alkaline earth metals
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an element that has properties of both metals and nonmetals
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metalloid
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1/2 the distance between nuclei of 2 atoms when joined
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atomic radius
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ability of an atom to attract electrons when an atom is in a compound
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electronegativity
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vertical column of elements in periodic table
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group
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nonmetal in group 7A
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halogen
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element in lanthanide or actinide series
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inner transition metal
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energy required to remove an electron from atom in its gaseous state
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ionization energy
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group 8A. s and p sublevels are filled
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noble gas
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horizontal row of elements
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period
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periodic repetition of physical and chemical properties
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periodic law
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element in "A" group display wide range of properties
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representative elements
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group B. d sublevel is filling
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transition metal
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indication of relative size of atoms and ions
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ionic radius
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