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47 Cards in this Set
- Front
- Back
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Classification of Solids
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1.Ionic (strongest)
2. Covalent Network 3. Metallic 4. Molecular Polar 5. Molecular Nonpolar (weakest) |
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Melting Point
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temp @ which s-->l
greater force, higher mpt |
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boiling pt
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temp @ which l-->g
greater force, higher bpt |
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molar heat of fusion
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quantity of heat to change from 1 mole s-->l
greater force, higher molar heat of fus |
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molar heat of vaporization
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quantity of heat to change from 1 mole l-->g
greater force, higher molar heat of vap |
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vapor pressure
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an indication of the tendency to evaporate l-->g @ surface of a liquid
greater force, lower VP (how easy is it to evaporate) |
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soluble
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dissolving mol solute in L of solvent= total soln
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miscible
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solute and solvent combine in any proportion
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like dissolves like
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ionic/molecular polar= soluble in POLAR solvents
molecular nonpolar=soluble in NONPOLAR solvents |
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Kinetic Molecular Theory of Gases (KMT)
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1. distance btw gas particles is large
2. gases are in random, rapid motion constantly 3. Kinetic energy determined by temp 4. molecules collide w/each other and energy is transferred 5. gases take up no volume |
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Dalton's Law of Partial Pressure
Collecting gas over H20 |
Ptotal= Pa+Pb+Pc+...
Ptotal= Pgas+ PH20 |
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vapor pressure
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the pressure exerted by a vapor (gas produced by evaporation) in a closed container
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volatile/nonvolatile
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volatile: evaporates easily, high vapor pressure
nonvolatile: evaporates slowly, low VP |
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Vapor Pressure and Temperature
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high temp, high VP
(temp increases, KE increases, collide more often, easier to escape the liquid phase) |
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Ideal Gas Law
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PV=nRT
(P and V inversely related) (V and T directly related) (V and n directly related) (T and P directly related) |
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@ STP
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standard temp (273 K) and pressure (1 atm= 760 mmHg)
1 mol= 22.4 L |
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Density @ STP
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Dstp= MM/22.4 L
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thermodynamics
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changes in energy that accompany chemical rxns and phase changes
"will a reaction occur?" |
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Heat
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flow of energy- energy which is transmitted from one substance/object to another
only exists when being transferred always flow from high temp to low temp |
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Calorimetry
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quantifying heat
transfer of heat during chem or physical change= Q Q=mCAT |
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enthalpy
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total stored energy in a substance (H)
measure H by change in enthalpy (AH)- amount of heat released/absorbed to/from surroundings nature favors - enthalpy (exo) |
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entropy
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disorder of a substance
+ increase in disorder - decrease in disorder nature favors + entropy |
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2 ways to look at entropy
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phases
moles (# of moles) |
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Spontaneous
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a process that proceeds on its own once initiated, transfers free energy from system-->surroundings
"will this rxn occur?" nature favors SPON |
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Gibb's free energy
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ability to do useful work
G=gives max. amount work obtainable from spon rxn -AG: SPON +AG: NON SPON |
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Collision Theory
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describes the effect of various factors of the rate of a rxn
1. molecules or atoms must collide in order to react (# of collisions) 2. not all collisions result in rxn (effectives of collisions) |
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How does temp. affect rate of rxn?
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higher temp, higher rate
*affects # of collisions- greater probability of colliding *affect effectiveness of collisions- if more KE, more easy to get over activation energy |
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How does concentration affect rate of rxn?
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higher [ ], higher rate
affects the # of collisions |
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how does surface area affect the rate of a rxn?
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greater surface area, higher rate
affects the # of collisions |
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How does a catalyst affect the rate of a rxn?
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catalyst=substance that increases the rate of a rxn by decreasing/lowering the activation energy (not consumed in rxn)
affects effectiveness of rxn |
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Activated complex
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transition state btw reactants and products
(at top of hump in energy diagrams) |
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Dynamic Equilibrium
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rxn continues to occur @ equal rates in opposite directions
*rate forward=rate reverse |
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Keq
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changes w/rxn
independent of initial concentration only changes w/temp don't include solids and liquids in Keq expression |
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Le Chatelier's Principle
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a rxn will partially relieve a stress by shifting the rxn to re-establish equilibrium
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titration/neautralization
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acid + base --> salt + water
MaVa = MbVb |
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strong acids
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HNO3
H2SO4 HCl (completely dissociate) |
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strong bases
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NaOH
LiOH RbOH KOH (completely dissociate) |
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weak acids
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*concentrations of react. do not equal concentration of prod.
*omit x from initial weak acid* Ka |
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Redox
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Oxidation: lose e-
reduction: gain e- redox=transfer of e- during a chem rxn (all rxns except PDR and ABDR) |
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oxidizing agent/reducing agent
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what was reduced/what was oxidized
*agents come from reactant side |
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Galvanic cells
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device that is used to generate electricity through the use of a SPON rxn
E cell= + (SPON) diagonal rule **higher the voltage=reduced metal don't multiply the volts 2 beakers, salt bridge, no battery |
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electron flow for all cells
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electrons always flow from anode to cathode
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how to measure the rate @ which the charge is transferred
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1 amp= 1C/sec
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voltage
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measures the potential for the electron to flow
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Plating cell
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*metal at anode always plated onto the cathode
*anode always at positive terminal of battery *only 1 metal (become ox and red) *battery |
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cathode
anode |
reduced- gain e-
oxidized- lose e- |
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electrolytic cell
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an external source of electricity that causes an otherwise NON SPON rxn to occur
*ions vs. H20 *@ Anode: anion- vs. H20 (ox form)- 1st box on SRP table *@cathode: cation+ vs H20 (red form)- 2nd box *the ion/H20 closes to zero wins!! battery, 2 inert electrodes |
