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40 Cards in this Set
- Front
- Back
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stoichiometry
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the area of study that examines the quantities of substances consumed and produced in chemical reactions
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reactants
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represented on the left of the arrow in a chemical formula
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products
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represented on the right of the arrow in a chemical formula
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combination reactions
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a process in which two reactants form to make one product
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decomposition reaction
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a process in which a single reactant forms two or more products
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combustion reaction
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a process in which a hydrocarbon or a related compound reacts with o2 to co2 and h2o
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formula weight
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sum of the atomic weights of the atoms in a formula
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molecular weight
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refers to the formula weight if the formula is a molecular formula
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mole
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avogadros number of formula units of that substance
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Avogadros number
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6.022 x 10^23
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molar mass
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the mass of a mole of atoms, molecules, or ions
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limiting reactant
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consumed in a reaction
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theoretical yield
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quantity of product calculated to form when all of the limiting reagent reacts
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percent yield
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compares the actual and theoretical yields
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exchange reaction
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AgNO3(aq) + KCl(aq) ====> AgCl(s) + KNO3(aq)
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molecular equation
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equation showing the complete chemical formulas of the reactants and products
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complete ionic equation
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an equation written with all soluble strong electrolytes shown as ions
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spectator ions
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ions that appear in identical forms among both the reactants andproducts of a complete ionic equation
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net ionic equation
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when spectator ions are omitted from the equation
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stong acids
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acids that are strong electrolytes
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strong bases
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bases that are strong electrolytes
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weak acids
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acids that are weak electrolytes
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weak bases
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bases that are weak electrolytes
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neutralization
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occurs when a solution of an acid and a solution of a base are mixed
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salt
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ionic compound whose cation comes from a base and whose anion comes from an acid
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oxidation reduction reaction
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process in which electrons are transferred between reactants
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oxidation
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loss of electrons by a substance
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reduction
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the gain of electrons by a substance
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elemental form
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when the oxidation number is always zero
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oxidation number of oxygen
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-2
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oxidation number of hydrogen
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+1
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oxidation number of fluorine
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-1
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the sum of the oxidation numbers
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zero
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displacement reactions
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when the ion in solution is displaced or replaced through oxidation of an element
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activity series
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a list of metals arranged in order of decreasing ease of oxidation
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concentration
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used to designate the the amount of solute dissolved in a given quantity of solvent or quantity of solution
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dilution
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adding water to a solution
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titration
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combinding a sample of the solution with a reagent solution of known concentration
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indicatiors
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used to determine when the equalivalents point of the titration has been reached
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solvent
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the component of the solution that is in greater quantity
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