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85 Cards in this Set
- Front
- Back
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molecule
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a neutral group of atoms bonded together
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ionic compounds
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compounds made up of cations and anions (usually a metal and nonmetal)
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monatomic ion
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An atom with a charge consisting of one or more atoms of a single element
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ions
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an atom with a charge
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empirical formula
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a formula with the lowest whole number ratio of elements in a compound
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chemical formula
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indicates number and type of atoms in a substance
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molecular formula
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shows number of atoms in a compound
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polyatomic ions
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a group of atoms with a charge
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binary compound
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compound with 2 elements
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mole
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a unit used in describing amounts of atoms and other small particles
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Avogadro's number
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6.02*10^23
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molar mass
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amount of g/mol in a compound
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STP
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standard temperature pressure
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molar volume
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22.4L/mol
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percent composition
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mass of element/mass of compound x 100
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catalyst
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speeds reactions up
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Synthesis reactions are usually
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1:1:1
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Percent error
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(Actual-Theoretical) / (Theoretical) x100
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Chemical Equation
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uses symbols and numbers to portray a chemical reaction, reactants on the left, products on the right
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Combination Reaction
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A+B -> AB
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Double Replacement Reaction
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AB + CD -> AD + CB
1. Both reactants must be aqueous 2. A solid or liquid must be in the product |
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Precipitate
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Indicator of a chemical reaction, solidification process
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Combustion Reaction
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CH compound reacts with O2 ALWAYS forms CO2 + H2O
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Net Ionic Equation
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Used with double replacement reactions to show main chemicals that react to form a solid or liquid
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Stoichiometry
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Predicting quantities in chemical reactions
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Limiting Reactant, Excess Reactant
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The reactant that is completely used up, the reactant that there is extra of
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Theoretical yield
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Theoretical results attained from an experiment
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Actual yield
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Results attained from an experiment
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Percent Yield
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(Actual Yield / Theoretical Yield) x100
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Kinetic Energy
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Energy of motion
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Vaporization
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Going from liquid to gas (can be boiling or evaporation)
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Evaporation
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Going from any state to a gas, but NOT boiling
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Vapor pressure
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Pressure exerted by a liquid as it evaporates
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Boiling point
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Vapor pressure and atmospheric pressure are the same, all particles in the liquid have the energy to go from a liquid to gas
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Melting point
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Temperature at which a solid goes to a liquid
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Phase diagram
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Shows the temperature and pressure of a substance and the phases in which the substance is in
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Triple point
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All three states are present
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Sublimation
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Solid to gas, no liquid phase
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Law of conservation of energy
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Energy can be neither created nor destroyed, but transferred
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Endothermic process
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Energy absorbed into the system
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Exothermic process
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Energy released to surroundings
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Heat capacity
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Energy required to increase the temperature of an object exactly one degree celsius
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Specific heat
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The amount of energy required to raise the temperature of 1 g of a substance 1 degree celsius
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Calorimetry
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The method used to find how much heat is absorbed/ released in a physical or chemical change
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Calorimeter
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Insulated device used to measure the absorption or release of heat in a physical or chemical change
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Enthalpy
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the heat content of a substance at constant pressure
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Heat of reaction
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heat change in a rxn
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Heat of combustion
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heat change in a combustion reaction
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Molar heat of fusion
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Energy required to melt one mole of a substance
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Molar heat of solidification
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Energy required to freeze one mole of a substance
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Molar heat of vaporization
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Energy required to turn one mole of substance from liquid to gas
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Molar heat of condensation
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Energy required to turn one mole of a substance from gas to liquid
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Molar heat of solution
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Energy required to raise the temperature of one mole of solution one degree celsius
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Kinetics
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Speed
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Dynamic Equilibrium
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Occurs when the forward and reverse actions occur at the same time and no change in concentration occurs
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Collision Theory
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Particles can react if they collide with enough kinetic energy and correct orientation
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Activation Energy
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Energy colliding particles require to start the rxn
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Activated Complex
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Point of molecules' impact
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Le Chatlier's Principle
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When a system is in equilibrium and a change is introduced upon that system, the equilibrium will shift in order to minimize the effect of the change
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Increasing the pressure of a system in equilibrium will shift the equilibrium...
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in the direction of fewer moles
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Increasing the temperature will shift the quilibrium...
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Away from the energy term
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The larger the equilibrium constant...
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the further the reaction goes
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Why does a higher temperature cause a reaction to go faster?
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There are more collisions and thee collisions are of greater energy
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If the equilibrium constant is large...
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More products are made
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Why does a catalyst cause a reaction to proceed faster?
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The activation energy is lowered
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What happens to a catalyst in a reaction?
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It is unchanged
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The following effect the rate of a reaction...
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1. Activation energy
2. Concentration 3. Particle Size 4. Temperature 5. Rate of reaction |
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Boyle's Law
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As pressure increases volume decreases (P1V1 = P2V2)
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Charles' Law
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As volume increases temperature does too (V1/T1 = V2/T2)
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Gay-Lussac Law
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As pressure increases, temperature goes too (P1/T1 = P2/T2)
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Combined Gas Law
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P1V1/T1n1 = P2V2/T2n2
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Ideal Gas Law
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PV = nRT
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R =
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0.0821 L atm/ K mol
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Dalton's Law of Partial Pressures
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Ptot = Pa + Pb
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Effusion
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The passing of a gas through a tiny hole
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Diffusion
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The passing of a gas through a medium
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Graham's law of effusion
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Gasses go from a high pressure area to a low pressure one
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Equation...
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Rate A/Rate B = √MMB / √MMA
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Where A is...
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the faster gas
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Gas particles are not affected by...
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Attractive forces
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All gas particle collisions are...
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elastic
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An ideal gas has...
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1.No attraction for itself
2. No volume (particles) 3. All collisions elastic |
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Units in PV = nRT
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atm, L, mol, K
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When converting something to STP...
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Use 1 atm, 273 K in the combined gas law
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heat of reaction
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ΔH = kJ/mol
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