Terms : Hide Images
| 7267444967 | aqueous solution | a solution in which the water is the dissolving medium | 0 | |
| 7267444968 | solution | homogeneous mixture of two or more substances | 1 | |
| 7267444969 | solvent | substance present in the greatest quantity and the one the dissolves the other substances | 2 | |
| 7267444970 | solute | the substances in a solution that are being dissolved (of the least quantity) | 3 | |
| 7267444971 | dissociation | the separation into component ions that occurs when an ionic compound dissolves | 4 | |
| 7267444972 | electrolyte | a substance whose aqueous solutions contain ions, commonly with ionic compounds | 5 | |
| 7267444973 | nonelectrolyte | a substance that does not form ions in solution, commonly molecular compounds | 6 | |
| 7267444974 | solvation | process that helps stabilize the ions in solution and prevents the cations and anions from recombining; this process is symbolized by aq in reactions and causes ions to become dispersely uniform throughout a solution | 7 | |
| 7267444975 | strong electrolytes | solutes that exist in solution completely or nearly completely as separate ions; fully or almost fully dissociate; in chemical equations, represented by a full arrow | 8 | |
| 7267444976 | weak electrolytes | solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions; do not completely dissociate; in a chemical equation, represented by two half arrows | 9 | |
| 7267444977 | chemical equilibrium | balance that produces a state in which the relative numbers of each type of ion or molecule in the reaction are constant over time | 10 | |
| 7267444978 | precipitation reaction | reaction that results in the formation of an insoluble product | 11 | |
| 7267444979 | precipitate | an insoluble solid formed by a reaction in solution | 12 | |
| 7267444980 | solubility | amount of substance that can be dissolved in a given quantity of solvent at the given temperature (at a given temperature) | 13 | |
| 7267444981 | insoluble | A substance is described as ______ if they have a solubility less than 0.01 mol/L | 14 | |
| 7267444982 | metathesis reaction | Ax + By -> Ay + Bx; these reactions include both single and double replacement reactions | 15 | |
| 7267444983 | molecular equation | an equation that shows the complete chemical formulas of the reactants and products without indicating ionic behavior |  | 16 |
| 7267444984 | complete ionic equation | an equation written with all strong soluble electrolytes shown as ions |  | 17 |
| 7267444985 | spectator ions | ions that appear in identical forms among both the reactants and products of a complete ionic equation | 18 | |
| 7267444986 | net ionic equation | an equation for a reaction in solution showing only those particles that are directly involved in the chemical change |  | 19 |
| 7267444987 | acid | substance that ionizes in aqueous solutions to form hydrogen ions, thereby increasing the concentration of H+(aq) ions; often called proton donors | 20 | |
| 7267444988 | monoprotic acids | acids that yield one H+ per molecule of acid ex) HCl, HNO3 | 21 | |
| 7267444989 | diprotic acids | acids that yield two H+ per molecule of acid ex) H2SO4 | 22 | |
| 7267444990 | base | substance that accepts (reacts with) H+ ions and produce hydroxide ions (OH-) when they dissolve in water; there are common ____s that do not contain hydroxide, however, like NH4 | 23 | |
| 7267444991 | strong acids | acids that are strong electrolytes (completes ionized in solution) | 24 | |
| 7267444992 | strong bases | bases that are strong electrolytes (completely ionized in solution) | 25 | |
| 7267444993 | strong acids | HCl, HBr, HI, HClO3, HClO4, HNO3, H2SO4 | 26 | |
| 7267444994 | strong bases | All Group 1A metal hydroxides (LiOH, NaOH, KOH, RbOH, CsOH) and heavy Group 2A metal hydroxides (Ca(OH)2, Sr(OH)2, Ba(OH)2) | 27 | |
| 7267444995 | weak acids | acids that are weak electrolytes (partly ionize in solution) | 28 | |
| 7267444996 | weak bases | bases that are weak electrolytes (partly ionize in solution) | 29 | |
| 7267444997 | neutralization reaction | the reaction that occurs when a solution of an acid and a solution of a base are mixed | 30 | |
| 7267444998 | salt | any ionic compound whose cation comes from a base and whose anion comes from an acid; ____ and water are the products of neutralization reactions | 31 | |
| 7267444999 | oxidation-reduction (redox) reaction | reaction in which electrons are transferred between reactants | 32 | |
| 7267445000 | oxidation | loss of electrons by a substance | 33 | |
| 7267445001 | reduction | gain of electrons by a substance, and therefore increase in negative charge | 34 | |
| 7267445002 | oxidation number | either the actual charge of a monatomic ion or the hypothetical charge assigned to an atom in a neutral molecule or charged species | 35 | |
| 7267445003 | 0 | oxidation number of elemental ions | 36 | |
| 7267445004 | charge of the ion | oxidation number for monatomic ions | 37 | |
| 7267445005 | displacement reaction | reactions in which the ion in solution is displaced/replaced through oxidation of an element |  | 38 |
| 7267445006 | activity series | list of metals arranged in order of decreasing ease of oxidation; active metals are top and noble metals bottom; any metal on the list can be oxidized by the ions of elements below it |  | 39 |
| 7267445007 | concentration | term used by scientists to designate the amount of solute dissolved in a given quantity of solvent or solution | 40 | |
| 7267445008 | molarity | the concentration of a solution expressed as the number of moles in a liter of solution (mol/L) | 41 | |
| 7267445009 | dilution | process in which solutions of lower concentrations can be obtained by adding water | 42 |
