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51 Cards in this Set
- Front
- Back
anion
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a negative ion
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halogens
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the elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine)
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alkaline-earth metals
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the elements of Group 2 (beryllium, magnesium, calcium, strontium, barium, and radium)
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periodic table
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an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group
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Henry Moseley
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organized the periodic table by atomic number rather than atomic mass
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isotope
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an atom of the same element that has a different mass
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John Dalton
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in 1808, proposed the first comprehensive theory of the atom
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noble gases
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group 18 elements (helium, neon, argon, krypton, xenon, and radon)
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electron configuration
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the arrangement of electrons in an atom
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orbital
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a three-dimensional region around the nucleus that indicates the probable location of an electron
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Niels Bohr
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created a model of the atom in which the electrons were found at fixed orbits around the nucleus
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frequency
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the number of waves that pass a given point in a specific time, usually one second
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molar mass
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the mass of one mole of a pure substance
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law of conservation of mass
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mass is neither created nor destroyed
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atomic number
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the number of protons in the nucleus of each atom of that element
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Ernest Rutherford
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conducted the gold foil experiment that led to the discovery of the nucleus
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atom
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the smallest particle of an atom that retains the chemical properties of that element
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covalent bonding
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chemical bonding that results from the sharing of electron pairs between two atoms
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molecule
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a neutral group of atoms that are held together by covalent bonds
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octet rule
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chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level
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valence electrons
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electrons available to be lost, gained, or shared in an atom
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metallic bonding
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chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
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malleability
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ability to be hammered into thin sheets
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intermolecular forces
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forces of attraction between different molecules
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polyatomic ion
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a charged group of covalently bonded atoms
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chemical bond
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a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
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ionic bonding
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chemical bonding that results from the electrical attraction between larger numbers of cations and anions
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polar
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bonds that have an uneven distribution of charge
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bond energy
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energy required to break a chemical bond and form neutral isolated atoms
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formula unit
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simplest collection of atoms from which an ionic compound’s formula can be derived
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ductility
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ability to be extruded through a small opening and made into a wire
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resonance
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bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
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VSEPR theory
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repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible
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Joseph John Thomson
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conducted experiments cathode rays that led to the discovery of the electron
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mass number
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the total number of protons and neutrons in the nucleus of an isotope
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mole
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the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12
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electromagnetic radiation
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a form of energy that exhibits wavelike behavior as it travels through space
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photoelectric effect
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the emission of electrons from a metal when light shines on the metal
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photon
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a particle of electromagnetic radiation having zero rest mass and carrying a quantum of energy
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ground state
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the lowest energy state of an atom
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Heisenberg uncertainty principle
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it is impossible to determine simultaneously both the position and velocity of an electron or other particle
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Aufbau principle
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an electron occupies the lowest-energy orbital that can receive it
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Hund’s rule
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orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin
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Demitri Mendeleev
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credited with the creation of the modern periodic table
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periodic law
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the physical and chemical properties of the elements are periodic functions of their atomic numbers
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alkali metals
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the elements of Group 1 (lithium, sodium, potassium, rubidium, cesium, and francium)
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transition elements
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the d-block elements which are metals with typical metallic properties
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cation
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a positive ion
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electronegativity
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a measure of the ability of an atom in a chemical compound to attract electrons
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lattice energy
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the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
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nuclear forces
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short-range proton-proton, proton-neutron, and neutron-neutron forces that hold the nuclear particles together
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