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AP Chemistry
forgotten facts
| Term | Definition |
|---|---|
| Addition/Subtraction SigFigs | line up decimal points, last sig fig is column in which all digits in column are significant |
| Multiplication/Division SigFigs | same number of sig figs as factor with fewest sig figs |
| Naming binary ionic compounds | cation + anion" ide" |
| roman numerals in naming compounds | represent charge of transition metal |
| naming covalent compounds | prefix of first element name (except mono) + first element + prefix of second element + second element"ide" |
| Coulombic Attraction determinants | charge difference, distance between attracted particles |
| Microwave spectroscopy | molecular rotation |
| infrared spectroscopy | molecular vibrations and types of bonds (double, single, triple) |
| uv spectroscopy | electron transitions between energy levels |
| ionization energy exceptions | Be has higher ionization energy than B N has higher ionization energy than O |
| Electron affinity | energy change when an atom gains an electron; elements that are more likely to gain electrons have greater electron affinities |
| high melting point | strong bond |
| ionic compound structure | lattice, brittle, transferred electrons |
| covalent compound structure | discrete, independent molecule, shared electrons |
| Metallic compound structure | conduct electricity, flexible bonds, delocalized electrons |
| Interstitial alloy | atoms of different radii, higher density than pure metal, less malleable |
| Substitutional alloy | atoms of same radii, density between two different pure metals, still malleable |
| sigma bond | single bond, stronger than pi bond |
| pi bond | added to sigma bond to form double and triple bonds, prevents rotation around bonds |
| bond order | calculated by averaging bond orders in a molecule, higher bond order means stronger bond and more stable molecule |
| covalent network solids | diamond, graphite (soft), SiO2, SiC, boron nitride BN |
| ideal gas law | molecules do not interact with each other, weaker IMF's mean more ideal gas (particles slide pass each other because of KE) |
| Acid or Water first? | Always add ACID to WATER just like you otter :) |
| how soluble will something be? | based on IMF's. H2O can hydrogen bond with itself so things that only do LDF will dissolve in other things that can only do LDF |
| ionization rules | no solid liquid or gas; ionic compound solutions and ammonium ionize; strong acids ionize |
| strong acids | HCl, HBr, HI, HNO3, HClO4, H2SO4 |
| percent error | (experimental - theoretical) / theoretical |
| percent yield | experimental / theoretical |
| will products dissolve? | sodium, potassium, ammonium, and nitrate compounds will be aqueous and ionize |
| H2CO3 | automatically forms H2O and CO2 |
| oxidation state exceptions | O in peroxide is -1, H when bonded to metals is -1 |
| Combustion of Hydrocarbons | produces CO2 and H2O (combustion is redox with oxygen |
| decomposition of Hydrogen Peroxide | 2H2O2 produces 2H2O and O2 |
| Determinants of Reaction Rates | Concentration, Surface Area, Temperature (KE), Catalysts |
| enthalpy of Fusion/Vaporization | Multiply enthalpy of Fusion/Vaporization by number of mols |
| enthalpy equation | enthalpy = -q / mol rxn |
| bond enthalpies | bond energies of bonds broken are positive (endothermic), bond energies of bonds that are formed are negative (exothermic) |
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