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34 Cards in this Set
- Front
- Back
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solute vs. solvent
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solute: substance being dissolved
solvent: substance doing the dissolving - most abundant substance is the solvent |
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4 factors that affected the rate of a chemical reaction
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1. nature of reactants (ionic = faster)
2. concentration of reactants (more collisions) 3. temperature (more energy = increased speed) 4. catalysts = speeds up chemical reactions without being active or used up |
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soluable vs. insoluable
miscible vs. immiscible |
soluable: does dissolve
insoluable: does not dissolve liquids only- miscible: does dissolve immiscible: doesn't dissolve |
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solubility
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maximum amount of solute with a given amount of solvent at a given temperature and pressure
temperature increases - particles move faster, bonds weaken gases - decrease solubility by heating gas until it leaves the solution |
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Reaction mechanism
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series of steps a reaction gas goes through
slowest step - rate determining step |
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Collision theory
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must collide head on at the right angle with enough force
usually involves two particles |
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properties of acids and bases
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acids: hydrogen, sour, stings/burns, red paper, 0-6 pH, produces co2 when reacting with carbonate and h2 when reacting with metals, and when reacting with phenolphaline it is clear
bases: bitter, slippery, hydroxide (OH), does not react with metals or carbonates, blue paper, 8-14 pH, and turns pink/magenta when reacts with pheolphaline |
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saturated solution
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solubility is reached at a given temperature and pressure
-will not be clear -the amount left over of the solute will stay at the bottom because it can't be dissolved anymore |
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molarity
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M = moles of solute/L of solution
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colloid
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.001 im - 1.0 um
doesn't settle no filter heterogenous lights scatters (tyndall effect) examples: toothpaste, milk, paint, glue |
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percent composition
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1. determine molar mass of compound
2. divide each element's mass by total mass of compound 3. multiply by 100 |
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predict products
precipitate reaction |
-2Na+F2 -> 2NaF
-double displacement reaction; solids formed from two reacting liquid ionic solutions; eventually will settle -only if substance formed is higher on the chart |
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pH scale
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0,1,2 = strong acid
3,4,5,6 = weak acid 7 = neutral (water) 8,9,10,11 = weak base 12,13,14 = strong base logarithmic scale - jump from one number to the next with a change by the power of 10 |
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strong bases vs. weak bases
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strong base: higher pH, shifts to the right and only makes molecules to ions (Free moving ions) and conductivity is better
weak base: shifts both ways because it goes from ions to molecules randomly |
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4 types of solids
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metallic: metals, atoms, metallic bonding, loses 1-4 valence electrons, goes from soft to hard, low to high b.p. and m.p., and conducts
ionic: salts, positive and negative ions, electrostatic attraction, hard/brittle, high m.p. and b.p., dissolves, and conducts molecular: organic compound, atoms/molecules, hydrogen boding, dipole-dipole, dispersion, soft, low m.p. and b.p., does not conduct, and is insoluable covalent network: diamonds, graphite, silicon, quartz, atoms, covalent bonds, strong, high m.p. and b.p., poor conductivity, and insoluable |
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8 properties of water
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-HOH
-pH = 7 -bent shape -polar (positive and negative ends of the molecule) -most abundant substance on Earth -exists as a liquid at room temperature -very high specific heat (has to absorb and release lots of energy to change temperature) -ice molecules form circular shapes -bends light (refraction) -universal solvent |
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phase changes
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solid - liquid: melting
solid - gas: sublimation gas - liquid: condensation/vaporization gas - solid: depositio |
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mercury level in thermometer goes down when in ice because...
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-mercury atoms give energy to colder water
-atoms move slowly -collide with force and contract/come together -thermometer level goes down |
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kinetic theory of matter
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1. all matter is made of particles and these particles have mass
2. particles experience constant random motion 3. collisions keep going and going (perfectly eleastic) 4. particles have higher energies at higher temperatures and lower energy at lower temperatures; more massive particles will move slower then less massive particles |
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empirical formula
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formula for a compoudn with the simplest ratio of elements
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mole
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-chemical quantity
-6.02 X 10 ^23 -22.4 L -molar mass in grams |
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exothermic vs. endothermic
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exothermic: hot, releases heat energy
endothermic: cold, absorbs heat energy -products of reaction have more energy then reactants |
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types of reactions
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double displacement: ab+cd -> ad+bc
combustion: ab+cd->co2+h20 synthesis: a+b->ab |
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Le Chatelier's Principle
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-when stressing a system by changing temperature, pressure or concentration, the system will undo what has been done to it
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chemical equilibrium
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rate of forward reaction equals the reate of the reverse reaction; the concentration of all substances are cosntant
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how do you know a reaction has occured?
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energy change, color change, gas emitted
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representative particle
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-smallest portion of a substance that still maintains its original properties
-ionic compound = formula unit -molecular compound = molecule -atom = element |
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when gases produce pressure...
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they bump into each other and into the walls of their container
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Boyle's Law
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inverse relationship
pressure and volume of a gase are proprtionate to each over P1V1 = P2V2 |
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Charle's Law
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direct relationship (when pressure is constant)
volume increass when temperature increases V1/T1=V2/T2 |
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combined gas law
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P1V1/T1 = P2V2/T2
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Ideal gas law
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PV = nRT
R = PV/nT R = 8.31 |
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identifying molar mass
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MM = dRT/P
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5 properties of a solution
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1. one substance dissolved in another substance
2. uniform throughout 3. particles can't be seen 4. can't be flitered 5. particles don't settle |
