6.10: End of Chapter Key Terms
- Page ID
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)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.