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| 6669025982 | State Symbols | Solid (s) Liquid (l) Gas (g) Precipitate (s) Solution (aq) | 0 | |
| 6669025983 | Real Gas vs. Ideal Gas | Ideal: low pressure, high temperature, don't have any attraction or repulsion between each other Real: high pressure, low temperature, has few attractions between them | 1 | |
| 6669025984 | Oxidation vs. Reduction | Oxidation: the loss of electrons/atom increases in oxidation number Reduction: the gain of electrons/oxidation number decreases | 2 | |
| 6669025985 | Arrhenius Acids and Bases | Acid: Produces H30 by releasing H Base: Produces OH by releasing OH | 3 | |
| 6669025986 | Conjugate Acid and Conjugate Base | On the opposite side of the reaction, the conjugate acid is formed from the base and the conjugate base is formed from the acid. Makes Acid/C. Base and Base/C. Acid pairs. | 4 | |
| 6669025987 | Covalent Bond | Sharing of electrons between two nonmetal ions (intramolecular) | 5 | |
| 6669025988 | Ionic Bond | Transfer of electrons from cation to anion (intramolecular) | 6 | |
| 6669025989 | Metallic Bond | Delocalized electrons (intramolecular) | 7 | |
| 6669025990 | Experimental Yield vs. Theoretical Yield | Experimental Yield: How much of a product is actually created Theoretical Yield: According to accurate calculations, how much product is supposed to be created | 8 | |
| 6669025991 | Polar vs. Nonpolar Molecules | Polar: electrons not easily shared, molecule has partial positive or partial negative charges at poles Nonpolar: electrons easily shared, no part of molecule is distinctly positive or negative | 9 | |
| 6669025992 | Le Chatelier's Principle | When a stress is applied to a reaction at equilibrium, the reaction will shift to reduce that stress. | 10 | |
| 6669025993 | IMF Forces | Order= Strongest to Weakest Ion-Dipole: Dipole= polar covalent compound H-Bonding: Bonds with F,O, or N Dipole-Dipole Bonds: two polar molecules Ion-Induced Bonds: Ion forces nonpolar molecule to have a temporary dipole Induced-Dipole Bonds: Polar+nonpolar London Dispersion Forces: Induced-Induced (two nonpolar ions) | 11 | |
| 6669025994 | Hybridization | http://image.tutorvista.com/cms/images/44/hybridization-table.JPG | 12 | |
| 6669025995 | Solubility Rules | Soluble Ionic Compounds 1. All group 1 compounds and ammonium are soluble 2. All nitrates (NO3), acetates (C2H3O2), and most perchlorates (ClO4) are soluble 3. All Chlorides, Bromides, and Iodides are soluble EXCEPT for Ag, Pb, Cu, and Hg. All Fluorides are soluble except for Pb and Group 2 4. All sulfates (SO4) are soluble except for Ca, Sr, Ba, Ag, and Pb. Insoluble Ionic Compounds 1. All metal hydroxides are insoluble except for group 1 and large members of group 2 2. All carbonates (CO3) and phosphates (PO4) are insoluble except for Group 1 and NH4 3. All sulfides are insoluble except for group 1, group 2, and NH4 | 13 | |
| 6669025996 | Reducing Agent vs. Oxidizing Agent | Reducing Agent: Is the ion that is oxidized Oxidizing Agent: the ion that is reduced | 14 | |
| 6669025997 | Bronsted-Lowry Acids and Bases | Acid: Donates a proton Base: Accepts a proton | 15 | |
| 6669025998 | Lewis Acids and Bases | Acid: Electron pair acceptor Base: Electron pair donor | 16 | |
| 6669025999 | Limiting Reactant vs. Excess Reactant | LR: The substance that is completely used up in a reaction XR: The substance that has some left over after all of the LR is used | 17 | |
| 6669026000 | % Yield vs. % Error | Percent Yield: Actual Yield/Percent Yield Percent Error: (Experimental-Theoretical)/ Theoretical | 18 | |
| 6669026001 | Electron Configuration | Basically, use electrons to write it out S level: 2 electrons P level: 6 electrons D level: 10 electrons | 19 | |
| 6669026002 | Sigma Bonds vs. Pi Bonds | Double bond: 1 sigma, 1 pi bond Triple bond: 1 sigma, 2 pi bonds | 20 | |
| 6669026003 | Metal + Oxygen | Metal Oxide 4Al+3O2=2Al2O3 | 21 | |
| 6669026004 | Metal Oxide + Water | Base Al2O3+H2O= Al(OH)3 | 22 | |
| 6669026005 | Nonmetal + Oxygen | Nonmetal Oxide C+O2=CO2 | 23 | |
| 6669026006 | Nonmetal Oxide+ Water | Acid CO2 + H2O ---> H2CO3 | 24 | |
| 6669026007 | Metal Oxide + Nonmetal Oxide | Salt | 25 | |
| 6669026008 | Acid + Base | Salt + H2O | 26 | |
| 6669026009 | Reaction Types | Single Displacement Double Displacement Combustion Decomposition Synthesis | 27 | |
| 6669026010 | Strong Acid + Water | HCL+H2O= H + Cl H+H20= H3O | 28 | |
| 6669026011 | Weak Acid + Water | Same as strong acid + water, but only 5% dissociates | 29 | |
| 6669026012 | Strong Base+ Water | KOH+ H2O= K + OH | 30 | |
| 6669026013 | Weak Base + Water | NH3+ H2O= NH4+ OH | 31 | |
| 6669026014 | Strong Acids | HCl HBr HI HClO3 HClO4 H2SO4 HNO3 | 32 | |
| 6669026015 | Strong Bases | LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2 | 33 | |
| 6669026016 | Solubility of Ionic Compounds | Solubility Rules Increased temperature= increased solubility | 34 | |
| 6669026017 | Solubility of Molecular Compounds | Likes dissolve likes rule (polar dissolved in polar, nonpolar dissolves in nonpolar) Increased polarity means increased solubility in water Decreased polarity means increased solubility in hexane | 35 | |
| 6669026018 | Solid-Liquid Solubility | Unsaturated Solutions: rate of solute dissolving is greater than rate of recrystallization Saturated Solutions: Rate of solute dissolving equal to rate of recrystallization Super Saturated: Rate of solute dissolving is lower than rate of recrystallization | 36 | |
| 6669026019 | Gas-Liquid Solubility | Gases are often mixed with liquids such as water Temperature effects: as temperature increases, solute decreases Pressure effects: as pressure increases, solute increases | 37 | |
| 6669026020 | Henry's Law | Used to determine solubility of a gas |  | 38 |
| 6669026021 | Boiling point elevation | As particles increase, boiling temperature increases m=molality i=individual particles k=constant |  | 39 |
| 6669026022 | Freezing point depression | As particles increase, freezing temperature decreases m=molality i=individual particles k=constant |  | 40 |
| 6669026023 | Volatile | Evaporates with extreme ease | 41 | |
| 6669026024 | Raoult's Law | The vapor pressure of a solvent above the solution decreases when a solute is dissolved in the solvent CHECK NOTES FOR THESE EQUATIONS It's under Vapor Pressure early in the year There's like three different equations for three different types of solutions | 42 | |
| 6669026025 | Nonvolatile Solutions | Non electrolytes: Covalently bonded (sugars) Electrolytes: ionic compounds (salts) | 43 | |
| 6669026026 | Volatile Solutions | Some non electrolytes that vaporize easily (some alcohols and ethers) | 44 | |
| 6669026027 | Hydrocarbons | Methane: CH4 Ethane: C2H6 Propane: C3H8 Butane: C4H10 Pentane: C5H12 Hexane: C6H14 Heptane: C7H16 Octane: C8H18 Nonane: C9H20 Decane: C10H22 Saturated hydrocarbons: Contain only SP3 hybridization, carbon-carbon single bonds, so basically every one above Unsaturated Hydrocarbons: Contain at least one carbon-carbon double bond or triple bond of cycloalkanes | 45 | |
| 6669026028 | Alkene | Suffix: -ene Naming: 1. Name longest carbon chain that contains double bond 2. Number from end nearer the double bond 3. Give location and name of each substituent as a prefix |  | 46 |
| 6669026029 | Alkyne | Suffix: yne Naming: Same as Alkene |  | 47 |
| 6669026030 | Aromatic | Suffix: Benzene Naming: Put name of group before benzene With multiple groups: Ortho (o): 1,2 Meta (m): 1, 3 Para (p): 1, 4 Common Aromatic Compounds CH3: Toluene NH2: Aniline OH: Phenol |  | 48 |
| 6669026031 | Alcohol | Suffix: -ol Naming: Add ending by replacing the -e YOU MUST NUMBER WHERE THE OH IS Classifying: Primary: 1 alkyl group attached Secondary: 2 groups Tertiary: 3 groups |  | 49 |
| 6669026032 | Mercaptan | Suffix: -thiol |  | 50 |
| 6669026033 | Ether | Suffix: -alkoxy Naming: List alkyl names in alphabetical order followed by ether |  | 51 |
| 6669026034 | Aldehyde | Suffix: -al Naming: Add suffix to ending First four common names: 1. form 2. acet 3. propion 4. butyr |  | 52 |
| 6669026035 | Ketone | Suffix: -one Naming: add suffix, carbonyl group indicated by a number |  | 53 |
| 6669026036 | Ester | Suffix: -oate Naming: 1. Contains the names of the alkyl group from the alcohol and the carbon chain from the acid with the suffix |  | 54 |
| 6669026037 | Carboxylic Acid | Suffix: -oic acid Naming: add suffix Common names 1. Formic acid 2. Acetic Acid 3. Propionic acid 4. Butyric Acid |  | 55 |
| 6669026038 | Amine | Suffix: -amine |  | 56 |
| 6669026039 | Amide | Suffix: -amide |  | 57 |
| 6669026040 | Cycloalkanes | Alkane compounds in a cyclical form Use prefix cyclo- to refer |  | 58 |
| 6669026041 | Substituents | Attached to the carbon chain and replace at least one H Methyl: CH3- Ethyl: CH3-CH2- Propyl: CH3-CH2-CH2- Fluoro: F- Chloro: Cl- Bromo: Br- Iodo: I- | 59 | |
| 6669026042 | Naming Alkanes | 1. Write alkane name of longest chain of carbon atoms 2. Number carbon atoms from end nearer branch 3. Give location and name of each substituent (alphabetical order) as a prefix of the main chain | 60 | |
| 6669026043 | Naming cycloalkanes | 1. Substituent placed in front of cycloalkane 2. Number not needed if only one branch 3. If 2 or more substituents are attached, ring is assigned according to which substituent is first alphabetically | 61 | |
| 6669026044 | Cis and Trans Isomers | Cis: Atoms are on the same side of the double bond Trans: atoms are on opposite sites of double bond |  | 62 |
| 6669026045 | KNOW ORGANIC CHEM REACTIONS | So yeah, most synthesize | 63 | |
| 6669026046 | Organic Chem Redox | Oxidation: Increasing C-O bonds or decreasing C-H bonds Reduction: Decreasing C-O bonds or increasing C-H bonds Common Oxidizing Agents: H2Cr2O7 KMO4 HNO3 Cl2, Br2, I2 Common Reducing Agents: H2 Li or Na Sn, Zn, Mg | 64 | |
| 6669026047 | Reaction Rates | Calculating Rate: change in concentration/ change in time (basically it's slope) Control Factors: Concentration, physical state, temperature, catalysts If collision increases, so does reaction rate Given: aA+bB= cC+dD, then rate: (see picture) |  | 65 |
| 6669026048 | Rate Law and Temperature | As temperature increases, the value of K increases. k= rate constant R: energy gas constant (8.31) A: collision frequency factor Ea: Energy of Activation |  | 66 |
| 6669026049 | Endothermic vs. Exothermic | Endo: Heat absorbed H>0 Exo: Heat released H<0 | 67 | |
| 6669026050 | Catalysts | Lowers energy of activation, which increases the rate constant (k) and thus increases rate of reaction of both forward and reverse reactions Yields products more quickly, but the same amount of product |  | 68 |
| 6669026051 | Equilibrium Constant | Reactant favored: K<1 Product Favored: K>1 |  | 69 |
| 6669026052 | Reaction Quotient | At equilibrium, K=Q
If Q |  | 70 |
| 6669026053 | Disturbing a Chemical Equilibrium | 3 ways to disturb equilibrium: 1. Changing temperature 2. Changing concentration of a reactant 3. Changing volume (for systems involving gases) | 71 | |
| 6669026054 | Ka and Pka | As Ka decreases, Pka increases As acidity increases, Ph decreases | 72 |
