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109 Cards in this Set
- Front
- Back
volume
|
the total amount of space taken up of a container
(in Liters, L) |
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temperature
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energy of gas particles
(Kelvin, K) |
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pressure
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collision of gas particles w/ container
(in atmospheres- atms) |
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moles
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number of gas particles
(mol, n) |
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Boyle's Law
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P and V are inversely proportional
Pi x Vi = Pf x Vf |
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Charles' Law
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T and V are directly proportional
Vi/Ti = Vf/Tf |
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Avogadro's Law
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relationship between n & V
n/v = constant |
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molar volume of a gas
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amt of space a gas will occupy @ STP
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___torr = ___ atm
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760 torr = 1 atm
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Dalton's Law of Partial Pressure
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the overall pressure of a mixture of gases is equal to the sum of the pressures for the individual gases
Ptot = P1+P2+P3 |
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solubility
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maximum amount of solute that be dissolved in a solvent
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saturated
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maximum amt of solute dissolved in solvent
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how are solubility and temperature related for solids?
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solubility of solids increases with increasing temperature.
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unsaturated solution
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less than the maximum amount of solute is dissolved in the solvent
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how are solubility and T related for gases?
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solubility decreases w/ increasing T. increases with increasing P
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concentration
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amount of solute in a given amt of solvent
|
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Molarity (M)
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mols solute
--------------- L solution |
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3 steps for making solution from a solid
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1. calculate the # of grams needed
2. measure out the solid and addit to the volumetric flask 3. add water to the line- total V |
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3 steps for making solution from stock solution
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1) calculate the volume of stock solution needed
2) measure stock solution and add to volumetric flask 3) add solvent to the line |
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dilution equal equasion
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M1 x V1 = M2 x V2
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vapor pressure
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pressure due to evaporation of solvent particles
liquid <----> gas |
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dynamic equilibrium (for gas/liquid)
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same amt of liquid particles becoming a gas as of gas particles becoming a liquid
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boiling temperature
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100.0 C. temp when vapor pressure = atmospheric pressure
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colligative properties
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properties that depend on the quantity of solute present not the identity (it doesn't matter WHAT just HOW MUCH solute)
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boiling point elevation
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bp of a solution is higher than the bp of a pure solvent
aka >100.0 C |
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freezing point depression
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fp of a soln is lower than the freezing pt of a pure solvent
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bp equasion
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BPsoln = BPsolvent + change in Tb
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fp equasion
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FPsoln = FPsolv - change in Tf
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molality (m)
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mol solute
--------------- kg solvent |
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change in T depends on...
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1) identity of solvent (k)
2) molality of solute (conc) |
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change in Tf equation
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[delta]Tf = i x Kf x m
i = number of ions the substance breaks into |
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change in Tb equation
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[delta]Tb = i x Kb x m
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kinetics
|
the study of rxn rates
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reaction mechanism
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series of steps to go from reactants to product
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substitution rxn
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one atom/group of atoms replaces another
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find the change in the energy of a reaction (equation)
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[delta]Hrxn = [delta]H( bonds broken) - [delta]H(bonds formed)
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relationship between forward and reverse enthalpy changesq
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[delta]Hforward = -[delta]Hreverse
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transition state
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structure(s) in between reactants and product
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bond enthalpy
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energy required to break a bond
always + |
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enthalpy
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the amount of energy available
|
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Collision theory (3)
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in order for a rxn to occur, molecules
1) must collide 2) w/ the proper orientation 3) and sufficient energy |
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catalyst
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a molecule/compound that speeds upa rxn that is not consumed in the rxn
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ezymes
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biological catalysts
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how do enzymes work? (2)
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1) lowering activation energy
2) &/or orienting molecules |
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concentration and rate relationship
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a higher conc of solute increases the rate
|
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rate law
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equation used to describe the effect of concentration on rate
rate = k[A]^x *[B]^y |
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Hess's Law
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if a series of rxns can be added to give an overall rxn, then the energies of the rxns can be added to give the energy of the overall rxn
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how to do Hess's Law probs (3 steps)
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1. flip rxns as needed to organize the rxns to be added so that the reactnats are on the reactant side & products are on the product side (location of compounds match the overall equasion)
2. make coeffiecients in the rxns to be added match the coefficients in the overall rxn by muliplying by same # 3. add rxns together |
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average rate
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change in conc over a period of time
[delta][A] -------------- [delta]t |
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instantaneous rate
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how the conc is changing at a specific time
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inital rate
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instantaneous rate at the beginning of a rxn
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what can rate laws not be determined by?
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rate laws cannot be determined by stoichiometry. only get it by experiment
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reaction orders
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tells how a change in specific conc affects the rate
|
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ORDERS: 0
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0th: x=0
--2x => no change in rate --4x => no change in rate |
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ORDERS: 1
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1st: x=1
--2x conc => 2x rate --4x conc => 4x rate |
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ORDER: 2
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2nd: x= 2
change in conc has a squared change in rate --2x conc =>4x rate --4x conc =>16x rate |
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rate law- determining
2 main steps |
1) determine rxn orders
--choose 2 experiments where only 1 conc changes 2) determine the rate constant --plugging in experimental values |
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rxn mechanics
|
a series of steps that occur to get from reactants to products
--sum of the steps in a mechanism must give the overall rxn -only valid if it matches the experimental rate law |
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rate determining step
|
slowest step in a rxn.
-determines the rate for the entire rxn |
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intermediates
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substance made in the step & used in a later step
=> doesn't appear in overall equation |
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dynamic equilibrium
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rate of forward rxn = rate of reverse rxn
-rxn doesnt stop, but the conc of reactants & prod.s stop changing |
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Keq =
|
Keq = Kfor [products]
---------- = --------------- Krev [reactants] |
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what phases are included in Keq?
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aqueous (aq)
gas (g) NOT solids (s) liquids (l) |
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when is Keq product/reactant favored?
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if Keq <1 then it is a reactant favored rxn
if Keq>1 it is a product favored rxn |
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Le Chatelier's Principle
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if a rxn at equilibrium is distrubed then the rxn will shift to minimize the effect of the disturbance & reachieve equilibrium
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adding products?
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shift to left-reactants
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removing reactants?
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shifts left-reactants
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remove products?
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shifts right- products
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add reactants?
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shifts right-products
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GAS EQ
decrease V = increase P |
shift to side w/ fewer moles of gas
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GAS EQ
increase V = decrease P |
shift to side with more moles of gas
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[delta]H = + (positive)
heat/energy as a ______ |
reactant.
increase T, shift to right, K will get bigger decrease T, shift to left, K will get smaller |
|
[delta]H = - (negative)
heat/energy as a ____ |
product
increase T, shift to left, K will get smaller. decrease T, shift to right, K will get bigger |
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q = mc[delta]T
variables? |
q=heat (J)
m=mass (g) c=specific heat capacity (J/g x degrees Celsius) [delta]T=change in temp (K or C) |
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specific heat capacity
|
energy required to raise the temp of 1g of a substance by 1`C
|
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1st law of thermodynamics (law of cons. of energy)
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energy cannot be created or destroyed therefore
q(hot) = --q(cold) |
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to find [delta]Hrxn
(3 steps) |
1) q(water) q=mc[delta]T
2) q(rx) q(rxn)=--q(water) 3) [delta]Hrxn = q(rxn) -------------- n (limit.react.) |
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electrolytes
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dissolve in H2O and produce ions
-conduct electricity --ionic compounds |
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non-electrolytes
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dissolve in H2O but no ions
-doesn't conduct electricity --covalent compounds |
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strong electrolyte
|
completely dissociates
product favored |
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weak electrolyte
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partially dissociates
reactant favored |
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7 strong acids
|
1) HCl - hydro chloric acid
2) HBr - hydrobromic acid 3) HI - hydroiodic acid 4) HNO3 - nitric acid 5) H2SO4 - sulfuric acid 6) HClO4 - perchloric acid 7) HClO3 - chloric acid |
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3 defining aspects of ACIDS
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1. sour taste
2. turns litmus red 3. reacts w/ metal to produce H2 |
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3 defining aspects of BASES
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1. bitter taste
2. turns litmus blue 3. aqueous solutions feel slippery |
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Arrhenius def. acid
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produces H+ ions in H20
|
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Arrhenius def. bases
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produces OH- ions in H20
|
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strong bases?
|
group 1 hydroxides
soluble hydroxides group 2 (Ca, Sr, Ba) |
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monoprotic acids
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--lose 1 H+
(all strongs acids but H2SO4) |
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diprotic acids
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lose 2 H+
(only H2SO4) |
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pH
|
measure of the amt of H+
pH = --log[H+] |
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Kw ?
|
the auto-ionization constant for water
|
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buffers
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solns that resist a change in pH
composed of a conjugate acid/base pair |
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radioactivity
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spontaneous emissions of energy &/or particles from the nucleus
|
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e- capture
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the nucleus snags an electron from 1 of lower energy orbitals
particle as a reactant |
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gamma radiation
|
high energy radiation
causes no change to the nucleus usually accompanies another type of decay |
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polymers
|
long chain of molecules made of smaller molecules
|
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monomers
|
small molecules that react to form long chains
|
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addition polymers
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monomers bond together to make one chain
|
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condensation polymers
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polymerization creates a small molecule as a byproduct
|
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what 5 things affect rxn rate?
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rate, k, Ea, orientation, concentration
|
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Bronsted-Lowry def. acid
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anything that donates a proton
|
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Bronsted-Lowry def. base
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anything that accepts a proton
|
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Kw =
|
[OH-] x [H3O+]
10^-7 |
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intermolecular forces def. &
3 types? |
attraction between molecules
1) London Dispersion forces- nonpolar molecules 2) dipole-dipole forces - polar molecules 3) hydrogen bonding (VERYstrong, but not a bond) |
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London Dispersion Forces
|
condensed states are formed by (the domino effect) attraction of e- in other molecules to the instantaneous dipole
|
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instantaneous dipole
|
momentary uneven distribution of e-
|
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dipole-dipole
|
uneven sharing of e- creating partial charges
attraction of partial charges on polar molecules |
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hydrogen bonding
|
-very strong dipole force
-NOT a bond -must have an H bonded to an N, O, F -attracted to a N,O,F in another molecule |
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kinetic molecular theory of gases
(4) |
1. the V of a gas molecule is small compared to the distance between molecules
2. gases experience no IMFs --gases neither attract nor repel each other 3. gases are in constant, rapid, random motion & their collisions are elastic 4. the average kinetic energy of a gas is proportional to its T (K) |