| Question | Answer |
| steps for balancing redox reactions in basic solutions | Same as balacing in acid PLUS: 8. Add OH- ions to cancel H+. 9. Reduce H2O again |
| steps for balancing redox reactions in acidic solution | 1. Divide into 1/2 reactions. 2. Balance for any element other than H or O. 3. Balance each for O by adding H2O. 4. Balance for H by adding H+. 5. Balancing for charge by adding e-. 6. Multiply 1/2 reactions by integer to cancel e-. 7. Cancel like items on reactant and product sides |
| reducing agent | Electron donor. Oxidized |
| oxidizing agent | Electron acceptor. Reduced |
| reduction | Gain of Electrons |
| oxidation | Loss of Electrons |
| how to find oxidation states | Atom in elemental state = 0. Monoatomic ion = charge. Peroxides, O = -1 |
| oxidation states | Way to keep track of electrons in redox reactions. Sum of oxidation states 0 for neutral compounds |
| endpoint | Point where indicator actually changes color |
| equivalence point / stoichiometric point | Point in titration where enough titrant has been added to react exactly with analyte |
| titration | Delivery of measure volume of solution of known concentration |
| volumetric analysis | Determining amount of certain substance by titration |
| neutralization reaction | Acid-base reaction. When base reacts exactly with acid, acid has been neutralized |
| base | Proton acceptor |
| acid | Proton donor |
| stoichiometry of precipitation reactions | Convert all quantities to moles and then use coefficients of balanced equation to assemble appropriate mole ratios. If reactants mixed, determine limiting reactant. Same principals apply to reactions that take place in solutions. Always right down species present in solution |
| net ionic equation | Includes only solution components directly involved in chemical reaction. No spectator ions |
| spectator ions | Ions that do not participate directly in reaction |
| complete ionic equation | Better represents actual forms of the reactants and products in solution. All substances that are strong electrolytes represented as ions. Reveals that only some ions participate in reaction |
| formula equation | Shows reactants and products of reaction, Not a correct picture of what actually occurs in solution |
| finding a precipitate | In virtually every case, when solid containing ions dissolves in water, ions separate. Move around independently. 1. Compound produced must have 0 net charge, contain both anions and cations. 2. Must compounds only 1 type of cation and 1 anion. Whichever of products more soluble becomes solution. Least soluble = precipitate. Solubilities of ionic substances. Slightly soluble interchangeable with insoluble. Focus on actual components of solution before any reaction occurs then figure out how these components will react with each other |
| precipitate | Solid formed, must know identities of reactants and products |
| precipitation reaction | 2 solutions mixed, insoluble substance sometimes forms. Solid forms separate from solution |
| types of solution reactions | Precipitation reactions, Acid-base reactions, Oxidation-reduction reactions |
| M1V1 = M2V2 | The same as moles of solute constant. Always holds up in dilution |
| dilution | Water added to achieve molarity desired from stock solution. Moles of solute after dilution = moles of solute before dilution. Typically 2 types of glassware: Pipet, Volumetric flask |
| standard solution | Solution whose concentration is accurately known |
| molarity (M) | Moles of solute per volume of solution, in liters. M = molarity = moles of solute / liters of solution |
| Must know 2 things to perform stoichiometric calculations | 1. Nature of reaction (Exact forms the chemicals take when dissolved) 2. Amounts of chemicals (concentrations) |
| nonelectrolytes | No current. No ions. C2H5OH |
| weak bases | NH3 |
| weak acids | Dissociates (ionizes) only to a slight extent in aqueous solutions |
| weak electrolytes | Conduct only a small current. Relatively few ions. Exhibit small degree of ionization in water. Acetic acid, HC2H3O2. Non-acidic Hydrogens written later in the formula. Reaction happens in both directions- Double arrows |
| Strong bases | Contain OH-. Become cation + OH- |
| Strong acids | Virtually every molecule ionizes. HCl, HNO3, H2SO4. Sulfuric acid-- 2 H+'s per molecule, but only 1 H+ ionizes |
| acids | Substances that produce H+ ions when dissolved in water. Polar nature of water causes them to ionize |
| Strong electrolytes | Conduct electricity well. Readily produce ions. Completely ionized |
| electrical conductivity | Ability to conduct an electric current. Arises from presence of ions. Extent to which solution can conduct an electric current depends directly on the number of ions present |
| solute | dissolver |
| "Like dissolves like" | Polar dissolves polar, nonpolar dissolves nonpolar |
| Solubility | Varies between substances. Depends on relative attractions of ions for each other. Depends on attractions of ions for water molecules |
| hydration | Positive ends attracted to negative other molecules and vice versa. Ionic substances dissolve in water by breaking down into individual cations and anions |
| polar molecule | unequal charge distribution |
| δ symbol | indictates partial charge |
| Describe the H2O molecule | Ability to dissolve many substances. Bent (V-shape). Covalent bonds between O and H's. O more electronegative than H, attracts more e-. O -, H+ |
| aqueous solutions | Solutions in which water is the dissolving medium (solvent) |
46 cards - created nov 15, 3:56pm