Chemistry Unit 10 Kinetics and Equilibrium (Jones - TJHSST)

Vocabulary

Collision Theory

proposes that atoms, molecules, or ions must collide in order to react

Transition State

associated with activated complex, can form prodcuts or reform reactants

Activation Energy

Minimum amount of energy needed to form activated complex

Instantaneous Rate

Reaction Rate calculated by finding slope of line tangent to curved plot of \[reactant\] = f(time) at specific instant in time

Rate Law

Quantitative relationship between reaction rate and reactant concentrations

Specific Rate Constant (k)

characteristic constant associated with reaction at given temperature

Inhibitor

species that decelerates reaction rates

Complex Reaction

multi-step reaction that consists of two or more elementary steps

reactive intermediate

species produced in one elementary step of mechanism and then consumed in subsequent elementary step of same mechanism

catalyst

species that speeds up reaction rates and is recycled

Reaction Order

Defines how reaction rate depends on concentration on certain reaction

Reaction Mechanism

complete sequence of elementary steps in multi-step reaction (Mechanism = Pathway)

Rate - Determining Step

Slowest or “Bottleneck” elementary step in multi-step reaction