Activation Energy: The minimum energy required for effective collisions to occur.
Activated Complex(es): An unstable arrangement of atoms that represents the maximum potential energy.
Average Rate: the average rate of change of a function over a given interval
Catalysts: reduce the activation energy…so it takes less energy for the reaction to happen.
Chemical Kinetics: the study and discussion of chemical reactions with respect to reaction rates, effect of various variables, re-arrangement of atoms, formation of intermediates etc.
Chemical system: The set of reactants and products undergoing energy transformations.
Collision Theory: explains how chemical reactions occur and why reaction rates differ for different reactions.
Elementary Step: a step involving one, two or three entity collisions
Endothermic: A chemical system that absorbs energy from its surroundings
Exothermic: A chemical system that releases energy from its surroundings
Heat: Amount of heat energy transferred between substances, systems or surroundings. When a reaction occurs, heat is transferred between substances, systems and surroundings.
Instantaneous Rate: the rate of change at a particular moment.
Rate of Reaction: the speed at which a chemical reaction proceeds.
Rate determining step: the slowest step in a reaction mechanism
Reaction intermediates: a substance produced in one elementary step and used up in another reaction (i.e. not in the final equation)
Reaction Mechanism: a series of elementary steps that give the overall equation
Potential Energy Diagrams: A potential energy diagram is a graphical representation of the energy transferred during a physical or chemical change.
Temperature: A measure of the average kinetic energy of the particles in a sample
Thermal energy: The energy available from a substance as a result of its motion of its molecules. For example, when you burn your foods, you break down sugars into carbon dioxide, water, ATP and thermal energy (heat). The SI unit for measuring work and all forms of energy is the Joule (J).
Activated Complex(es): An unstable arrangement of atoms that represents the maximum potential energy.
Average Rate: the average rate of change of a function over a given interval
Catalysts: reduce the activation energy…so it takes less energy for the reaction to happen.
Chemical Kinetics: the study and discussion of chemical reactions with respect to reaction rates, effect of various variables, re-arrangement of atoms, formation of intermediates etc.
Chemical system: The set of reactants and products undergoing energy transformations.
Collision Theory: explains how chemical reactions occur and why reaction rates differ for different reactions.
Elementary Step: a step involving one, two or three entity collisions
Endothermic: A chemical system that absorbs energy from its surroundings
Exothermic: A chemical system that releases energy from its surroundings
Heat: Amount of heat energy transferred between substances, systems or surroundings. When a reaction occurs, heat is transferred between substances, systems and surroundings.
Instantaneous Rate: the rate of change at a particular moment.
Rate of Reaction: the speed at which a chemical reaction proceeds.
Rate determining step: the slowest step in a reaction mechanism
Reaction intermediates: a substance produced in one elementary step and used up in another reaction (i.e. not in the final equation)
Reaction Mechanism: a series of elementary steps that give the overall equation
Potential Energy Diagrams: A potential energy diagram is a graphical representation of the energy transferred during a physical or chemical change.
Temperature: A measure of the average kinetic energy of the particles in a sample
Thermal energy: The energy available from a substance as a result of its motion of its molecules. For example, when you burn your foods, you break down sugars into carbon dioxide, water, ATP and thermal energy (heat). The SI unit for measuring work and all forms of energy is the Joule (J).