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| 10997708865 | stoichiometry | the area of study that examines that quantities of substances involved in chemical reactions | 0 | |
| 10997714163 | chemical reaction | a process by which one or more substances are converted to other substances | 1 | |
| 10997719173 | chemical equations | use chemical formulas to symbolically represent chemical reactions | 2 | |
| 10997753847 | balanced chemical equation | has an equal number of atoms of each element on each side of the arrow | 3 | |
| 10997793751 | g,l,s,aq | are all symbols used to designate the physical state of each reactant and product | 4 | |
| 10997863834 | decomposition reaction | one reactant changes to two or more products | 5 | |
| 10997881369 | combustion reaction | involves oxygen, often from air, reacting with hydrocarbons or other organic molecules containing carbon, hydrogen, and oxygen to produce carbon dioxide and water. | 6 | |
| 10997927785 | avogadro's number | 6.02 X 10^23 of atoms in that element | 7 | |
| 10997937434 | a mole | the amount of matter that contains 6.02 X 10^23 atoms, ions, molecules, or formula units | 8 | |
| 10997947705 | molar mass | the mass in grams of one mole of that substance. to calculate: add the atomic mass of all the atoms in its formula | 9 | |
| 10997970166 | molar road |  | 10 | |
| 10998021025 | percentage composition | the percentage by man contributed by each element in the compound % composition= 100 x (molar mass of element x subscript for element) / (molar mass of substance) | 11 | |
| 10998047747 | empirical forumla | expresses the simplest ratio of atoms in the formula. can be calculated from the percentage composition. | 12 | |
| 10998056819 | molecular formula | tells exactly how many atoms are in one molecule of the compound | 13 | |
| 10998071957 | ionic compounds | often form crystal structures called hydrates by acquiring one or more water molecules per formula unit | 14 | |
| 10998078972 | stoichometry | the quantities of substances involved in chemical reactions | 15 | |
| 10998096767 | limiting reactant | the reactant that is completely consumed in a chemical reaction. limits the amount of products formed | 16 | |
| 10998103432 | excess reactant | some is left unreacted when the limiting reactant is completely consumed | 17 | |
| 10998114345 | theoretical yield | the quantity of product that is calculated to form | 18 | |
| 10998119646 | actual yield | the amount of product actually obtained and is usually less than the theoretical yield | 19 | |
| 10998126129 | percent theoretical yield | related the actual to the theoretical yield percent theoretical yield= (actual yield) / (theoretical yield) x 100 | 20 | |
| 10998145546 | solution | a homogenous picture of two or more substances | 21 | |
| 10998148553 | solvent | the dissolving medium, usually the substance present in the greatest quantity in a solution | 22 | |
| 10998153948 | aqueous solution | solutions in which water is the solvent | 23 | |
| 10998164895 | solutes | other substances in the solution | 24 | |
| 10998167736 | electrolyte | a substance whose aqueous solution contains ions. the solution conducts electricity because the ions are free to migrate throughout the solution | 25 | |
| 10998180219 | strong electrolyte | substances that exist in solution, completely ionized. ionic compounds and some molecular compounds called strong acids are strong electrolytes | 26 | |
| 10998194825 | strong acids | can react readily with metals | 27 | |
| 10998198566 | strong bases | dissociate completely | 28 | |
| 10998204391 | weak electrolytes | exist mostly as molecules in solution. molecular compounds called weak acids and weak bases are weak electrolytes. | 29 | |
| 10998218517 | ionic compounds | are always strong electrolytes if they're on the chart | 30 | |
| 10998226929 | nonelectrolyte | a substance that does not form ions in solution and its solution does not conduct electricity. usually consists of a molecular compound, which when dissolved in water, usually consists of intact, un-ionized molecules. | 31 | |
| 10998255566 | precipitate | an insoluble solid formed by a reaction in solution | 32 | |
| 10998292804 | complete ionic equation | if the soluble strong electrolytes are shown as ions write it as a complete ionic equation | 33 | |
| 10998413576 | spectator ions | ions that appear in identical form among both reactants and products of a complete ionic equation | 34 | |
| 10998455138 | net ionic equation | omits spectator ions because they do not change from reactants to products | 35 | |
| 10998468171 | the cations and anions that generally DO NOT form precipitates are | ammonium: NH4+ sodium: Na+ potassium: K+ nitrate: NO3- | 36 | |
| 10998485194 | general rules for writing net ionic equations | 1. write all the reactants that are indicated to be solids, liquids, or gasses 2. rewrite the formulas of the aqueous reactants, omitting the spectator ions (NH4+, Na+, K+, NO3-) 3. predict and write the product 4. if necessary, use ions to balance the mass and charge. then balance using coefficients. check to see if the charges are balanced. | 37 | |
| 10998541012 | acids | substances that ionize in quests solution to form H+ ions | 38 | |
| 10998545703 | bases | substances that react with H+ ions | 39 | |
| 10998554174 | strong acids and strong bases are strong electrolytes | the completely ionize in solutions | 40 | |
| 10998727442 | neutralization reaction | water is usually a product. because strong-acids and bases are strong electrolytes, their ions are usually spectator ions in acid-base reactions. | 41 | |
| 10999460821 | ionic compounds | containing carbonate, sulfite, or sulfide ions produce gases when they react with acids | 42 | |
| 10999474863 | metal carbonates and metal hydrogen carbonates | react with acids to produce carbon dioxide gas and water | 43 | |
| 10999488653 | oxidation-reduction reactions | also called redox reactions are reactions that transfer electrons between reactants oxidation: losing negative charge and gaining positive charge reduction: gained negative charge and losing positive charge | 44 | |
| 10999527819 | oxidation | is the loss of electrons, becomes more positive | 45 | |
| 10999537503 | reduction | the gain of electrons, becomes more negative | 46 | |
| 10999587837 | metals | also react with metal ions to exchange electrons | 47 | |
| 10999816431 | activity series | a list of metals arranged in order of decreasing ease of oxidation | 48 | |
| 10999854984 | oxidation state | also called oxidation number. A positive or negative whole number assigned to an element in a chemical formula based on set formal rules. used to track electron transfer in redox reactions. | 49 | |
| 10999914183 | a solution | a homogeneous mixture consisting of a solvent and one or more solutes | 50 | |
| 10999927090 | concentration | the amount solute dissolved in a given amount of solvent or solution | 51 | |
| 10999943552 | molar concentration | also called molarity. the number of moles of solute dissolved in a liter of solution molarity= moles of solute/volume of solution in liters | 52 | |
| 10999993497 | dilution | adding water to a solution decreases the molar concentration of each substance in the solution by a factor called the dilution factor. a ratio of the original volume to the new volume old volume/new volume | 53 | |
| 11000115769 | solution stoichiometry | involved calculations that relate moles of reactants and products to the volumes of solutions of their molar concentrations. | 54 | |
| 11000150253 | titration | an analytical technique used to determine the unknown concentration of a solution by reacting it with a solution of known concentration called a standard solution. Equivalence point of the titration is the only point at which the moles of a substance dissolved in the unknown solution completely react with the moles of a substance in the standard solution. | 55 |
