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Electrochemical Cell
An apparatus that uses a redox reaction to produce electrical energy or uses electrical energy to cause a chemical reaction.
Salt Bridge
A pathway constructed to allow positive and negative ions to move from one solution to another.
Voltaic Cell
A type of electrochemical cell that converts chemical energy into electrical energy by a spontaneous redox reaction
Anode
In an electrochemical cell, the electrode where oxidation takes place.
Cathode
In an electrochemical cell, the electrode where reduction takes place
Reduction Potential
The tendency of a substance to gain electrons
Battery
One or more electrochemical cells in a single package that generates electrical current.
Dry Cell
An electrochemical cell that contains a moist electrolytic paste inside a zinc shell.
Primary Batteries
A type of battery that produces electric energy by redox reactions that are not easily reversed, delivers current until the reactants are gone, and then is discarded.
Secondary Batteries
A rechargeable battery that depends on reversible redox reactions.
Corrosion
The loss of metal that results from an oxidation-reduction reaction of the metal with substances in the environment
Electrolysis
The process that uses electrical energy to bring about a chemical reaction
Electrolytic Cell
An electrochemical cell in which electrolysis occurs
Galvanizing
The process in which an iron object is dipped into molten zinc or electroplated with zinc to make the iron more resistant to corrosion.
Redox Reactions
An oxidation-reduction reaction.
Oxidation
The loss of electrons from the atoms of a substance; increases an atom’s oxidation number.
Reduction
The gain of electrons by the atoms of a substance; decreases an atom’s oxidation number.
Oxidizing Agent
The substance that oxidizes another substance by accepting its electrons.
Reducing Agent
The substance that reduces another substance by losing electrons.
Oxidation-number Method
the technique that can be used to balance more difficult redox reactions, based on the fact that the number of electrons transferred from atoms must equal the number of electrons accepted by other atoms.
Species
Any kind of chemical unit involved in a process.
Half Reaction
One of two parts of a redox reaction — the oxidation half, which shows the number of electrons lost when a species is oxidized, or the reduction half, which shows the number of electrons gained when a species is reduced.
Electrochemical Processes
The conversion of chemical energy into electrical energy and the conversion of electrical energy into chemical energy are known as these processes.
Hydrochloric Acid
HCl
Nitric Acid
HNO3
Sulfuric acid
H2SO4
Phosphoric Acid
H3PO4
Acetic Acid
HC2H3O2
Carbonic Acid
H2CO3
Potassium Hydroxide
KOH
Sodium Hydroxide
NaOH
Calcium Hydroxide
Ca(OH)2
Arrhenius Acid
Acids are compounds containing hydrogen that ionize to yield hydrogen ions (H+) in aqueous solution.
Arrhenius Base
Bases are compounds that ionize to yield hydroxide ions (OH-) in aqueous solution.
Monoprotic Acid
Contain one ionizable hydrogen.
Diprotic Acid
Contain two ionizable hydrogen.
Triprotic Acid
Contain three ionizable hydrogen.
Bronsted-Lowry Acid
A model of acids and bases in which an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor.
Bronsted-Lowry Base
A hydrogen ion acceptor.
Conjugate Base
The species produced when an acid donates a hydrogen ion to a base.
Conjugate Acid
The species produced when a base accepts a hydrogen ion from an acid.
Self-Ionization of water
The reaction in which two water molecules react to give ions.
Titration
The process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration.
Standard solution
A solution of known concentration used in carrying out a titration.
Endpoint
The point at which the indicator that is used in a titration changes color.
Equivalence point
The point at which the moles of H+ ions from the acid equals moles of OH- ions from the base.
Buffer
A solution that resists changes in pH when limited amounts of acid or base are added.
Buffer Capacity
The amount of an acid or base a buffer solution can absorb without a significant change in pH.
Titrant
A solution of known concentration used to titrate a solution of unknown concentration; also called the standard solution.
Buret
A buret is a precisely marked glass cylinder. It measures the volumes of reacting solutions.
Physical Equilibrium
Occurs when there is no net change in a physical system and no new substances are formed.
Reversible Reaction
A reaction that can take place in both the forward and reverse directions; leads to an equilibrium state where the forward and reverse reactions occur at equal rates and the concentrations of reactants and products remain constant.
Chemical Equilibrium
The state in which forward and reverse reactions balance each other because they occur at equal rates.
Closed System
A system where only the exchange of energy occurs but the exchange of matter is not.
Le Chatelier's Principle
States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.
Heterogeneous Equilibrium
A state of equilibrium that occurs when the reactants and products of a reaction are present in more than one physical state.
Common Ion Effect
The lowering of the solubility of a substance by the presence of a common ion.
Homogeneous Equilibrium
A state of equilibrium that occurs when all the reactants and products of a reaction are in the same physical state
Law of Chemical Equilibrium
States that at a given temperature, a chemical system may reach a state in which a particular ratio of reactant and product concentrations has a constant value.
Solubility Product Constant
Ksp, which is an equilibrium constant for the dissolving of a sparingly soluble ionic compound in water
Precipitate
A solid produced during a chemical reaction in a solution
Dynamic Equilibrium
Occurs in reversible reactions where products and reactants are formed at such a rate that neither of their concentrations change.
Equilibrium Constant
Keq, is the numerical value that describes the ratio of product concentrations to reactant concentrations, with each raised to the power corresponding to its coefficient in the balanced equation.
Reaction Rate
The change in concentration of a reactant or product per unit time, generally calculated and expressed in moles per liter per second.
Collision Theory
States that atoms, ions, and molecules must collide in order to react.
Activation Energy
The minimum amount of energy required by reacting particles in order to form the activated complex and lead to a reaction.
Activated Complex
A short-lived, unstable arrangement of atoms that can break apart and re-form the reactants or can form products; also sometimes referred to as the transition state.
Homogeneous Catalyst
A catalyst that exists in the same physical state as the reaction it catalyzes.
Heterogeneous Catalyst
A catalyst that exists in a different physical state than the reaction it catalyzes.
Reaction Order
For a reactant, describes how the rate is affected by the concentration of that reactant.
Complex Reaction
A chemical reaction that consists of two or more elementary steps.
Instantaneous Rate
The slope of the straight line tangent to the curve at a specific time
Reaction Mechanism
The complete sequence of elementary steps that make up a complex reaction.
Intermediate
A substance produced in one elementary step of a complex reaction and consumed in a subsequent elementary step.
Rate-Determining Step
The slowest elementary step in a complex reaction; limits the instantaneous rate of the overall reaction.
Inhibitor
A substance that slows down the reaction rate of a chemical reaction or prevents a reaction from happening.