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21.10: End of Chapter Key Terms

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Sep 4, 2024
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- 21.9: End of Chapter Activity
- Back Matter

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Physical and Chemical Reactions Key Terms

Physical Change: A change in which the form of matter is altered but one substance is not transformed into another, such as changes in state (solid, liquid, gas), shape, or size.
Chemical Change: A change that results in the formation of one or more new substances with different chemical properties and compositions, often involving a chemical reaction.
Chemical Reaction: A process in which substances (reactants) undergo chemical changes to form new substances (products), involving the breaking and forming of chemical bonds.
Reactants: The starting materials in a chemical reaction that undergo change to form products.
Products: The new substances formed as a result of a chemical reaction.
Law of Conservation of Mass: A principle stating that mass is neither created nor destroyed in a chemical reaction; the mass of the reactants equals the mass of the products.
Exothermic Reaction: A chemical reaction that releases energy to the surroundings, usually in the form of heat.
Endothermic Reaction: A chemical reaction that absorbs energy from the surroundings, usually in the form of heat.
Activation Energy: The minimum amount of energy required to initiate a chemical reaction.
Catalyst: A substance that increases the rate of a chemical reaction without being consumed in the process, by lowering the activation energy.
Inhibitor: A substance that decreases the rate of a chemical reaction or prevents it from occurring.
Chemical Equilibrium: A state in which the forward and reverse reactions occur at equal rates, resulting in no net change in the concentrations of reactants and products.
Reversible Reaction: A chemical reaction in which the products can react to reform the reactants.
Irreversible Reaction: A chemical reaction in which the products cannot easily reform the reactants.
Precipitate: An insoluble solid that forms and separates from a solution during a chemical reaction.
Synthesis Reaction: A type of chemical reaction in which two or more substances combine to form a more complex product (A + B → AB).
Decomposition Reaction: A type of chemical reaction in which a single compound breaks down into two or more simpler substances (AB → A + B).
Single Replacement Reaction: A type of chemical reaction in which one element replaces another element in a compound (A + BC → AC + B).
Double Replacement Reaction: A type of chemical reaction in which the ions of two compounds exchange places in an aqueous solution to form two new compounds (AB + CD → AD + CB).
Combustion Reaction: A chemical reaction in which a substance combines with oxygen, releasing energy in the form of heat and light, and producing carbon dioxide and water (usually).
Oxidation: The process in which a substance loses electrons during a chemical reaction.
Reduction: The process in which a substance gains electrons during a chemical reaction.
Redox Reaction: A chemical reaction involving the transfer of electrons from one substance to another, comprising both oxidation and reduction processes.
Chemical Bond: The attractive force that holds atoms or ions together in a compound.
Covalent Bond: A chemical bond formed by the sharing of electron pairs between atoms.
Ionic Bond: A chemical bond formed by the electrostatic attraction between oppositely charged ions.
Bond Energy: The amount of energy required to break one mole of bonds in a substance.
Reaction Rate: The speed at which a chemical reaction occurs, often measured as the change in concentration of reactants or products per unit time.
Concentration: The amount of a substance in a given volume, typically expressed in moles per liter (Molarity, M).
Temperature: A measure of the average kinetic energy of particles in a substance, affecting the reaction rate.
Pressure: The force exerted per unit area, influencing the reaction rate of gases.
Surface Area: The total area of the exposed surface of a solid, affecting the reaction rate.
Equilibrium Constant (K): A numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction.
Le Chatelier’s Principle: A principle stating that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract the change.
Reaction Mechanism: The step-by-step sequence of elementary reactions by which overall chemical change occurs.
Intermediate: A species that appears in some steps of a reaction mechanism but not in the net equation.
Transition State: A high-energy state during a chemical reaction where old bonds are breaking and new bonds are forming.
Chemical Kinetics: The study of the rates of chemical processes and the factors that affect them.
Energy Profile Diagram: A graphical representation of the energy changes that occur during a chemical reaction.

Physical and Chemical Reactions Key Terms

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