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90 Cards in this Set
- Front
- Back
accuracy
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closeness of measurements to the correct or accepted value of the quantity measured
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anion
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a negative ion
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anode
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electrode where oxidation takes place
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atom
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smallest unit of mass of an element that maintains the properties of that element
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atomic mass unit
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unit of mass that is exactly 1/12 the mass of a carbon-12 atom
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atomic number
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number of protons in the nucleus of each atom of an element
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auogadro's law
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equal volumes of gasses at the same temperature and pressure contain equal numbers of molecules
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barometer
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device used to measure atmospheric pressure
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boiling point
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temperature at which the equilibrium vapor pressure of a liquid equals the atmospheric pressure
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Boyle's law
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volume of a fixed mass of gas varies inversely with pressure at constant temperature
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catalyst
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substance that changes the rate of a chemical reaction without itself being permanently consumed
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cathode
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electrode where reduction takes place
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cation
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positive ion
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Charles' law
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volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature
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chemical
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any substance that has a definite composition
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chemical change
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a change in which one or more substances are converted into different substances
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chemical equation
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a representation with symbols and formulas of the identities and relative amounts of the reactants and products in a chemical unchanged
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chemical property
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ability of a substance to undergo a charge that transforms it into a different substance
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chemical reaction
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reaction in which one or more substances are converted into a different substance.
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chemistry
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the study of the composition, structure and properties of matter and the changes it undergoes
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coefficient
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small whole number that appears in front of a formula in a chemical equation
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composition reaction
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reaction in which 2 or more substances combine to form a new compound
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combustion reaction
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reaction in which a substance combines with oxygen, releasing a large amount of energy in the form of light and heat
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compound
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substance that is made from the atoms of 2 or more elements that are chemically bonded
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concentration
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measure of the amount of solute in a given amount of solvent or solution
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covalent bonding
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chemical bond resulting from the sharing of an e- pair between 2 atoms
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Dalton's law of partial pressure
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total pressure of a mixture of gases is equal to the sum of the partial pressures of component gases
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decomposition reaction
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reaction in which a single compound produces 2 or more simpler substances
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density
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ratio of mass to volume or mass divided by volume
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derived unit
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unit that is a combination of SI base units
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diatomic molecule
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molecule containing only 2 atoms
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ductility
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ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire
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elastic collision
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collision between gas particles and between gas particles and container wall in which there is no loss of kinetic energy
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electrode
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conductor used to establish electrical contact with a nonmetallic part of a circuit, such as an electrolyte
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electron affinity
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energy change that occurs when an e- is acquired by a neutral atom
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electron dot notation
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electron configuration in which only the valence e- of an atom of a particular element are shown, indicated by dots placed around the element's symbol
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element
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pure substance made of only one kind of atom
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empirical formula
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symbols for the elements combined in a compound with subscripts showing the smallest whole number mole ratio of the different atoms in the compound
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equilibrium
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dynamic condition in which 2 opposing changes occur at equal rates in a closed system
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evaporation
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process by which particles escape from the surface of a nonboiling liquid and enter the gas state
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family
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vertical column of the periodic table
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fluid
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substance that can flow and therefore take the shape of its container; a liquid or a gas
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formula mass
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sum of the average atomic masses of all the atoms represented in the formula of any molecule, formula, unit, or ion
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formula unit
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simplest collection of atoms from which an ionic compound's formula can be established
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freezing point
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temperature at which a solid and liquid are in equilibrium at 1 atomic pressure
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frequency
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number of waves that pass a given point in a specific time, usually 1 second
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gas
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state of matter in which a substance has neither definite volume nor definite shape
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gas laws
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simple mathematical relationships between the volume, temperature, pressure, and quantity of gas
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Gay-Lussac's law
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pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temp
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group
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vertical column of the periodic table
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halogen
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1 of the elements of group 17, fluorine, chlorine, bromin, iodine, and astatine
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heterogeneous
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not having a uniform composition throughout
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homogeneous
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having a uniform composition throughout
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hydrogen bonding
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intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
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ideal gas
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imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory
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ion
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atom or group of bonded atoms that has a positive or negative charge
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ionic bonding
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chemical bond resulting from electrical attraction between large numbers of cations and anions
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ionic compound
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compound composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
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isotopes
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atoms of the same element that have different masses
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kinetic-molecular theory
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theory based on the idea that particles of matter are always in motion
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law of conservation of mass
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mass is neither created nor destroyed during ordinary chemical or physical reactions
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law of multiple proportions
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2 or more different compounds are composed of the same 2 elements, then the ratio of the masses of the 2nd element combined with a certain mass of the 1st element is always a ratio of small whole numbers
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law of definite proportions
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chemical compound contains the same proportions by mass regardless of the size of the sample or the source of the compound
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Lewis structure
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formula in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between 2 atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only 1 atomic symbol represent unshared electrons
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limiting reactant
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reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction
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liquid
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state of matter in which the substance has a definite volume but an indefinite shape
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magnetic quantum number
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quantum # that indicates the orientation of an orbital around the nucleus
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malleability
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ability of a substance to be hammered or beaten into thin sheets
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mass
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measure of the amount of matter
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mass number
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total number of protons and neutrons in the nucleus of an isotope
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matter
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anything that has mass and takes up space
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melting
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physical change of a solid to a liquid by the addition of heat
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melting point
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temperature at which a solid becomes a liquid
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metal
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element that is a good conductor of heat and electricity
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metalloid
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element that has some characteristics of metals and some characteristics of nonmetals
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millimeters of mercury
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common units of pressure
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molar mass
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mass of 1 mole of a pure substance
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molarity
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number of moles of solution in 1 liter of solution
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mole
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amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12
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mole ratio
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conversion factor that relates the amounts in a mole of any 2 substances involved in a chemical reaction
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molecular compound
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chemical compound whose simplest units are molecules
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molecular formula
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formula showing the types and numbers of atoms combined in a single molecule of a molecular compound
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molecule
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neutral group of atoms that are held together by covalent bonds
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monatomic ion
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ion formed from a single atom
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noble gas
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group 18 element helium, neon, argon, krypton, xenon, and radon
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nomenclature
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naming system
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nonmetal
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element that is a poor conductor of heat and electricity
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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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percent error
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value calculated by subtracting the experimental value from the accepted value, dividing the difference by the accepted value, and them multiplied by 100.
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percent yield
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ratio of the actual yield to the theoretical yield, multiplied by 100
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