Section 1
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Alcohol
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Date created
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Cards (73)
Section 1
(50 cards)
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
Strong Base+ Water
KOH+ H2O= K + OH
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
Weak Acid + Water
Same as strong acid + water, but only 5% dissociates
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
Metallic Bond
Delocalized electrons (intramolecular)
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
Weak Base + Water
NH3+ H2O= NH4+ OH
Arrhenius Acids and Bases
Acid: Produces H30 by releasing H Base: Produces OH by releasing OH
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
Hybridization
http://image.tutorvista.com/cms/images/44/hybridization-table.JPG
Volatile Solutions
Some non electrolytes that vaporize easily (some alcohols and ethers)
Boiling point elevation
As particles increase, boiling temperature increases m=molality i=individual particles k=constant
Strong Acid + Water
HCL+H2O= H + Cl H+H20= H3O
Covalent Bond
Sharing of electrons between two nonmetal ions (intramolecular)
Solubility of Ionic Compounds
Solubility Rules Increased temperature= increased solubility
Strong Bases
LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2
Acid + Base
Salt + H2O
Ionic Bond
Transfer of electrons from cation to anion (intramolecular)
Alkyne
Suffix: yne Naming: Same as Alkene
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
Nonvolatile Solutions
Non electrolytes: Covalently bonded (sugars) Electrolytes: ionic compounds (salts)
Henry's Law
Used to determine solubility of a gas
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
Metal Oxide + Water
Base Al2O3+H2O= Al(OH)3
Sigma Bonds vs. Pi Bonds
Double bond: 1 sigma, 1 pi bond Triple bond: 1 sigma, 2 pi bonds
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
% Yield vs. % Error
Percent Yield: Actual Yield/Percent Yield Percent Error: (Experimental-Theoretical)/ Theoretical
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
Volatile
Evaporates with extreme ease
Reducing Agent vs. Oxidizing Agent
Reducing Agent: Is the ion that is oxidized Oxidizing Agent: the ion that is reduced
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.
Oxidation vs. Reduction
Oxidation: the loss of electrons/atom increases in oxidation number Reduction: the gain of electrons/oxidation number decreases
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)
Lewis Acids and Bases
Acid: Electron pair acceptor Base: Electron pair donor
Nonmetal + Oxygen
Nonmetal Oxide C+O2=CO2
Nonmetal Oxide+ Water
Acid CO2 + H2O ---> H2CO3
Le Chatelier's Principle
When a stress is applied to a reaction at equilibrium, the reaction will shift to reduce that stress.
State Symbols
Solid (s) Liquid (l) Gas (g) Precipitate (s) Solution (aq)
Metal Oxide + Nonmetal Oxide
Salt
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
Reaction Types
Single Displacement Double Displacement Combustion Decomposition Synthesis
Bronsted-Lowry Acids and Bases
Acid: Donates a proton Base: Accepts a proton
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
Metal + Oxygen
Metal Oxide 4Al+3O2=2Al2O3
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
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
Freezing point depression
As particles increase, freezing temperature decreases m=molality i=individual particles k=constant
Electron Configuration
Basically, use electrons to write it out S level: 2 electrons P level: 6 electrons D level: 10 electrons
Strong Acids
HCl HBr HI HClO3 HClO4 H2SO4 HNO3
Section 2
(23 cards)