This vocabulary is taken from Chapter 14 of _Chemistry: The Central Science - AP* Edition_.
Terms : Hide Images
| The area of chemistry concerned with the speeds, or rates, at which chemical reactions occur. | ||
| The decrease in concentration of a reactant or the increase in concentration of a product with time. | ||
| The reaction rate at a particular time as opposed to the average rate over an interval of time. | ||
| The light absorbed by a substance (A) equals the product of its molar absorptivity constant (a), the path length through which the light passes (b), and the molar concentration of the substance (c). In other words, A = abc. | ||
| An equation that related the reaction to the concentrations of reactants (and surroundings of products also). | ||
| A constant of proportionality between the reaction rate and the concentrations of reactants that appear in the rate law. | ||
| The power to which the concentration of a reactant is raised in a rate law. | ||
| The sum of the reaction orders of all the reactants appearing in the rate expression. | ||
| A reaction in which the reaction rate is proportional to the concentration of a single reactant, raised to the first power. | ||
| A reaction in which the overall reaction order (the sum of the concentration term exponents) in the rate law is 2. | ||
| The time required for the concentration of a reactant substance to decrease to half its initial value; the time required for half of a sample of a particular radioisotope to decay. | ||
| A model of reaction rates based on the idea that molecules must collide to react. | ||
| The minimum energy needed for reaction; the height of the energy barrier to formation of products. | ||
| The particular arrangement of atoms found at the top of the potential-energy barrier as a reaction proceeds from reactants to products. | ||
| An equation that relates the rate constant for a reaction to the frequency factor, the activation energy, and the temperature. | ||
| A term in the Arrhenius equation that is related to the frequency of collision and the probability that the collisions are favorably oriented for reaction. | ||
| A detailed picture, or model, of how the reaction occurs; that is, the order in which bonds are broken and formed and the changes in relative positions of the atoms as the reaction proceeds. | ||
| A process in a chemical reaction that occurs in a single event or step. | ||
| The number of molecules that participate as reactants in an elementary reaction. | ||
| An elementary reaction that involves one molecule. | ||
| An elementary reaction that involves two molecules. | ||
| A rare elementary reaction that involves three molecules. | ||
| A substance formed in one elementary step of a multi-step mechanism and consumed in another; it is neither the reactant nor the product of the overall reaction. | ||
| The slowest elementary step in a reaction mechanism. | ||
| A substance that changes the speed of a chemical reaction without itself undergoing a permanent chemical change in the process. | ||
| A catalyst that is in the same phase as the reactant substances. | ||
| A catalyst that is a different phase from that of the reactant substances. | ||
| The binding of molecules to a surface | ||
| A protein molecule that acts to catalyze specific biochemical reactions. | ||
| A substance that undergoes a reaction at the active site in an enzyme. | ||
| The specific site on a heterogeneous catalyst or an enzyme where catalysis occurs. | ||
| A model of enzyme action in which the substrate molecule is pictured as fitting rather specifically into the active site on the enzyme. |
