LCCC Mr. Hiner's Chem 2 Final
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| Intermolecular Forces | Fixed- keeps shape when placed in a container, Indefinite- takes the shape of the container
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| Solid Intermolecular Forces | very strong forces, particles are packed close together and can only vibrate and are incompressible
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| Liquid Intermolecular Forces | particles are packed close together but have the ability to move from place to place, and are incompressible
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| Gas Intermolecular Forces | cohesive, complete freedom of motion and aren't held together, but flow and no shape and can't be compressed
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| State of Matter | Depends on: The amount of kinetic energy the particles possess, the strength of attraction between molecules
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| Gas Kinetic Energy | their kinetic energy overcomes the attractive forces between molecules
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| Forces of Attraction | the particles are attracted to each other by electrostatic forces (strength varies, depends on kinds of particles)
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| Specific Heat (c) | amount of energy needed to raise 1 gram of water 1 degree Celcius
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| Q=mc(delta T) | heating of a substance
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| Q=mQf Heat of fusion(Qf) | Heat of fusion= 79.7cal/gm or 334kJ/kg
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| Q=mQvap Heat of Vaporization(Qvap) | Heat of Vaporization=539 cal/gm or 2260kJ/kg
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| Heating Water | 100 cal/gm or 418.6 kJ/kg to heat water 0 degrees --> 100 degrees
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| Intermolecular Attractions | attractive forces between opposite charges, H bonding especially strong
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| London Dispersion Forces | nonpolar molecules-very weak
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| Dipole-Dipole | polar molecules, strong alignment
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| H-bonding | O-H, N-H, F-H
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| Ion-Dipole Forces | In a mixture, ions from an ionic compound are attracted to the dipole in polar molecules.
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| Viscosity | resistance of a liquid to flow, raising temperature reduces viscosity
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| Capillary Action | is the ability of a liquid to flow up a thin tube
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| Super Critical Fluid | A point at which you get one state (liquid and gas blur)
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| Boiling Point | the temperature at which the vapor pressure equals external atmosphere pressure
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| Dynamic Equilibrium | rate of evaporation=rate of condensation
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| Heat of Vaporization | the amount of heat energy required to vaporize one mole of the liquid
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| Vapor Pressure and Temperature | as the temperature increases, the vapor pressure increases, increasing the temperature increases number of molecules escaping a liquid
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| Clausis-Clapeyron Equation | ln(P2/P1)=(Hvap/R)((1/T1)-(1/T2))
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| Crystalline Solids | particles are in highly ordered arrangements
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| Amorphous Solids | no particular order in the arrangement of particles
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| Ionic Crystals | ions pack themselves so as to maximize the attractions and minimize repulsions
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| Homogeneous Solutions | A mixture of two or more substances
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| Solvent | majority component of a solution
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| Solute | minority component of a solution
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| Soluble | when a solute dissolves in a solvent
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| Entropy | measure of randomness
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| Solubility | the maximum amount of solute that can be dissolved in a given amount of solvent (temperature dependent)
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| Lattice Energy | attractive forces between ions
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| Saturated Solutions | the solvent holds as much solute as is possible at that temperature
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| Unsaturated Solutions | less solute than can dissolve in the solvent at that temperature is dissolved in the solvent
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| Henry's Law | Sg=kPg, Sg=solubility of gas, k=Henry's Law Constant, Pg=partial pressure of gas above liquid, (S1/P1)=(S2/P2)
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| Concentration | amount of solute in a given amount of solution
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| Part of a whole | amount of solute in a given amount of solution
%=(amount of solute/ amount of solution) x 100
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| Molarity | M=(mass of solute)/((Molar Mass)(V of solution in liters))
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| Molality | m=(moles of solute)/(mass of solvent in kilograms)
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| Mole Fraction | Xa=moles of solute/total number of moles
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| Density | D=M/V
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| Colligative Properties | vapor pressure of a solvent above a solution is lower than the vapor pressure of the pure solvent
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| Raoult's Law | P solvent in solution= X solvent (pressure of gas at standard conditions)
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| Boiling Point Elevation | Delta Tb=Kb(m) Kb=molal boiling point Delta Tb=added to the normal boiling point
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| Freezing Point Elevation | Delta Tf=Kf(m)
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| Van't Hoff Effect | Delta Tf=Kf(mi) mi=number of particles in an electrolyte
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| Osmosis | is the flow of solvent from a solution of low concentration into a solution of high concentration
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| Semipermeable Membrane | allows solvent to flow through it, but not solute
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| Osmotic Pressure | amount of pressure needed to keep osmotic flow from taking place, II=MRT
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| Isotonic | exerts the same osmotic pressure as body fluids such as red blood cells (RBCs)
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| Hypertonic | has a lower solute concentration than RBCs, water goes out of cells by osmosis
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| Hypotonic | has higher solute concentration than RBCs, water goes out of cells by osmosis
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| Colloids | have medium-size particles, cannot be filtered, can be seperated by semipermeable membrane
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| Suspensions | very large particles, settle out, can be filtered, must be stirred to stay suspended
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| Soaps | Ionic heads (hydrophilic), nonpolar tails (hydrophobic)
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| Reaction Rate | the speed of a chemical reaction
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| Rate | how much a quantity changes in a given period of time
Rate=change of something/delta t
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| Rate Equation | Rate=-1/a delta A/delta t=etc.
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| Polarimetry | measures the change in the degree of rotation of plane polarized light caused by one of the components over time
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| Spectrophotometry | this measures the amount of light of a particular wavelength absorbed by one component over time
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| Catalyst | affect speed of reaction without being consumed
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| The Rate Law | Rate=k[A]^n
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| Zero Order | rate is always the same/don't change rate
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| First Order | rate is directly proportional to reactant concentration
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| Second Order | rate is directly proportional to the square of the reactant concentrations/ double concentration=quadruple the rate
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| Integrated Rate Laws | zero=line, drop down, first=straight sloped line, slight bow, Second=bent line, big bow
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| Zeroth Order | [A]=-kt+[A]initial
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| First Order Half Life | 0.693/rate
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| First Order | ln([At]/[Ao])=-kt
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| Second Order | 1/[A]=kt+(1/[A]initial)
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| Second Order Half Life | 1/k[Ao]
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| Activation Energy (Ea) | minimum amount of energy required for reaction
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| Activation Energy Equation | ln(k2/k1)=(Ea/R)((1/T1)-(1/T2))
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| Mechanism | sequence of events that are a road map of bond breaking and making
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| Le Chatelier's Principle | If a system at equilibrium is disturbed by a change in temperature, pressure, or the concentration of one of the components it will shift its equilibrium to counteract the effect of disturbance
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| Arrhenius Acid | a substance that when dissolved in water, increases the concentration of hydrogen ions
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| Arrhenius Base | a substance that when dissolved in water, increasing the concentration of hydroxide ions
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| Bronsted-Lowry | acid=proton donor/must have a removable protein, base=proton acceptor/must have pair of nonbonding electrons
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| Lewis Acid | species that can form a covalent bond by accepting an electron pair
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| Lewis Base | an electron pair donator
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| Acids | strong acids completely dissociate, weak acids don't
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| Kw | Kw=Ka x Kb, Kw=1.0x10^-14
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| Equilibrium Expression | Kc=[H3O+][OH-]
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| pH | pH=-log[H3O+] pH=pKa+log([base]/[acid])
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| pOH | pOH=-log[OH-]
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| pKa | pKa=-log[Ka]
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| Salt Anions | bases that can react with water in a hydrolysis reaction to form OH- and the conjugate acid
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| Salt Cations | with acidic protons will lower the pH of a solution, most metal cations when hydrated in solution also lower the pH
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| Buffers | resist changes in pH when an acid or base is added
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| Equivalence Point | where stiochiometric equality
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| End Point | where indicator changes color and allows you to end titration
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| Common-Ion Effect | If one of the ions in a solution equilibrium is already dissolved in the solution, the equilibrium will shift to the left and the solubility of the salt will decrease
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| First Law of Thermodynamics | Energy cannot be created nor destroyed. Therefore total energy of the universe is a constant.
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| Spontaneous Processes | are those that can proceed without any outside intervention, processes spontaneous forward are not reverse
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| Irreversible Processes | cannot be undone by exactly reversing the change to the system
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| Entropy Equation | S=entropy Delta S=Sfinal-Sinitial S-klogW
Delta S= Delta Hvap/T
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| Second Law of Thermodynamics | Entropy of universe increases for spontaneous processes, but doesn't change for reversible processes
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| Third Law of Thermodynamics | The entropy of a pure crystalline substance at absolute zero is 0
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| Gibb's Free Energy | Delta G= Delta H- T Delta S
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| Voltaic Cells | In spontaneous oxidation-reduction (redox) reactions, electrons are transferred and energy is released
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| Electromotive Force (emf) | the potential difference between the anode and cathode in a cell Wmax=-nFEcell
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| Oxidizing and Reducing Agents | The strongest oxidizers have the most positive reduction potentials and vice versa
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| Free Energy | Delta G=-nFE Ecell=(0.592)logK/n
E=E(circle)-(0.0592/n)logQ
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| Radioactive Decays | Alpha, Beta, Gamma,Electron Capture (K-capture), Positron Emmission
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| Alpha Decay | mass number decrease by 4, atomic number decrease by 2
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| Beta Decay | mass number stays the same, atomic number increase by 1
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| Positron Emmission | mass number stays the same, atomic number decrease by 1
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| Gamma Decay | gives off m (meta) in decay
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| Electron Capture (K-Capture) | proton meets electron to make neutron
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| Nuclear Kinetics | Nuclear transmutation is a first order process
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| Nuclear Rate | Rate=kNt Nt=number of radionuclei at any time
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| Curie | 1 Curie=3.7x10^10 nuclei/s
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