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29 Cards in this Set
- Front
- Back
Activated Complex
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An unstable, short-lived structure caused by the effective collision of particles.
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Activation Energy
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The minimum amount of kinetic energy particles must possess in order to undergo an effective collision.
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Catalyst
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A substance that increases the rate of a chemical reaction, but is not chemically changed at the end of the reaction.
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Chemical Equation
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A system for using chemical formulas and coefficients to indicate the types and rations of products and reactants involved in a chemical reaction.
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Chemical Reaction
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The conversion of substances into other substances that have different chemical properties.
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Collision Theory
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They hypothesis that in order to react, particles must collide at the proper orientation with more than a minimum amount of kinetic energy, known as the activation energy.
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Concentration
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Amount of a substance per unit of volume; for gases, this is the number of moles of the gas per liter.
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Elementary Process
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One of the steps of a reaction mechanism.
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Endothermic Process
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A process that absorbs heat.
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Energy
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The ability to perform work or to transfer heat.
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Enzyme
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A biological molecule that acts as a catalyst.
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Equilibrium
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A dynamic balance in which the rate of the forward process equals the rate of the reverse process.
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Exothermic Process
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A process that releases heat.
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Intermediate
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A particle thought to be present in the elementary processes of a reaction mechanism. Intermediates do not appear in the balanced equation of the reaction because they are both produced and consumed in the course of the reaction.
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Kinetic Energy
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Energy associated with motion.
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Kinetics
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The study of reaction rates and mechanisms.
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Mole
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6.02 X 10^23
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Order
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For an individual reactant, the exponent of the reactant's concentration in the rate law; for an overall reaction, it is the sum of the exponents of all concentrations in the rate law.
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Potential Energy
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Energy that is stored due to position, chemical bonds, or other factors.
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Product
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A substance resulting from a chemical reaction.
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Rate
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Amount of change per unit of time.
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Rate Constant
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The proportionality in a rate law expression, which is symbolized by k. The rate constant is temperature dependent.
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Rate-Determining Step
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A reaction mechanism's slowest elementary process. This step determines the overall rate of a reaction.
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Rate Law Expression
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A mathematical expression relating the concentrations of reactants to a reaction rate.
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Reactant
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A substance present at the start of a chemical reaction.
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Reactant Mechanism
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The set of elementary processes that describes a chemical reaction at the molecular level.
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Reaction Rate
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The change in concentration of a reactant or product divided by time, normalized by dividing by the stoichiometric coefficient of the reactant or product in the balanced equation.
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Stoichiometry
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The techniques employed for calculating the relationship of the quantities of reactants and products in chemical reactions and for balancing chemical equations.
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Transition State
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The point at which the activated complex exists, as reactants turn into products.
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