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29 Cards in this Set
- Front
- Back
Electrolyte
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A substance that conducts a current when dissolved in water
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Solvated
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Surrounded by water molecules
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Molecular Equation
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Shows all reactants and products as if they were intact, undissolved compounds
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Total Ionic Equation
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Shows all soluble substances dissociated into ions
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Net Ionic Equation
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Shows the actual chemical change (elimination of spectator ions)
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Precipitation Reaction
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Two soluble ionic compounds react to form and insoluble produce (precipitate)
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Metathesis Reaction
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Double-Displacement Reaction
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Oxidation-Reduction (Redox) Reaction
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Reaction with a net movement of electrons from one reactant to the other. Driving force is from the reactant with less attraction for electrons to the reactant with more attraction for electrons.
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Electron Transfer
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Behavior in a redox reaction that forms and ionic compound
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Electron Shift
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Behavior in a redox reaction that results in a polar molecule
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Boyle's Law
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Volume and Pressure
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Charles's Law
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Volume and Temperature
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Avogadro's Law
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Volume and Moles
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Mole Fraction
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One component's fraction of moles in a mixture
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Root-Mean-Square Speed
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(3RT/M)^(1/2)
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Rate of Effusion or Diffusion
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Rate1/Rate2 = (Molarity2/Molarity1)^(1/2)
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van der Waals Equation
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Adjusts pressure up and volume down to account for intermolecular attraction and molecular volume.
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Thermodynamics
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The study of heat and its transformations
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E
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Internal Energy
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Heat
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q; energy transfer due to difference in TEMPERATURE
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Work
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w; transfer of energy by force
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Law of Conservation of Energy (First Law of Thermodynamics)
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The total energy of the universe in constant
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Pressure-Volume Work
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Type of work in which a volume changes against an external pressure
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State Function
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A property dependent only on the current state of the system, NOT the path the system took to get to that state
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Enthalpy
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H; At constant pressure, this eliminates the need to consider PB work. E + PV
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Heat of Reaction
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H(final) - H(initial)
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Heat Capacity
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The quantity of heat required to change the temperature of 1 GRAM of a substance by 1 K
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Heat absorbed or released (formula)
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q = c * m * change in T
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Thermochemical Equation
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A balanced equation that states the heat of reaction
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