"Redox is a type of chemical reaction in which the oxidation states of substrate change."
A chemical reaction in which there is a transfer of electrons between two species.
Oxidation and Reduction Reactions: Chemical reactions that involve the transfer of electrons from one substance to another.
Redox Half-Reactions: A chemical equation that describes the oxidation or reduction of a single reactant or product.
Reducing and Oxidizing Agents: A substance that donates or accepts electrons, respectively, in a redox reaction.
Redox Potential: The tendency of a substance to undergo oxidation or reduction.
Galvanic Cells: An electrochemical device that converts chemical energy into electrical energy using redox reactions.
Standard Reduction Potentials: The standard potential (measured in volts) of a redox reaction, used to determine the feasibility of a reaction.
Electrolytic Cells: An electrochemical device that uses electrical energy to drive a non-spontaneous redox reaction.
Faraday's Laws of Electrolysis: Laws that describe the relationship between the amount of substance produced or consumed during electrolysis and the amount of electricity used.
Nernst Equation: An equation that relates the equilibrium redox potential to the concentration of reactants and products.
Corrosion: The deterioration of materials due to redox reactions with the environment.
Oxidation-reduction reaction: A chemical reaction in which the oxidizing agent loses electrons and the reducing agent gains electrons.
Combustion: A type of redox reaction in which a substance reacts with oxygen to release energy.
Corrosion: A redox reaction that occurs when an oxidizing agent slowly attacks and weakens a metal.
Photosynthesis: A process in which plants convert carbon dioxide and water into glucose using sunlight energy.
Respiration: A process in which the body converts glucose into energy and produces carbon dioxide and water.
Electroplating: A process in which a metal object is coated with a thin layer of another metal using electricity.
Batteries: Devices that use redox reactions to generate electricity by converting chemical energy into electrical energy.
Fuel cells: Similar to batteries, fuel cells produce electricity from chemical reactions and are used in electric vehicles and power plants.
Metal extraction: Redox reactions are used to extract metals from ores. For example, iron can be extracted from hematite using a redox reaction with carbon monoxide.
Rusting: A type of corrosion that occurs when iron reacts with oxygen and water to form iron oxide.
"Oxidation is the loss of electrons or an increase in the oxidation state."
"Reduction is the gain of electrons or a decrease in the oxidation state."
"There are two classes of redox reactions."
"Only one (usually) electron flows from the atom being oxidized to the atom that is reduced."
"This type of redox reaction is often discussed in terms of redox couples and electrode potentials."
"An atom transfers from one substrate to another."
"For example, in the rusting of iron, the oxidation state of iron atoms increases as the iron converts to an oxide, and simultaneously the oxidation state of oxygen decreases as it accepts electrons released by the iron."
"Although oxidation reactions are commonly associated with the formation of oxides, other chemical species can serve the same function."
"In hydrogenation, C=C (and other) bonds are reduced by transfer of hydrogen atoms."
"Oxidation state refers to the state of an atom regarding the loss or gain of electrons."
"Electrons play a crucial role in redox reactions, with their loss or gain determining the oxidation or reduction of a substance."
"The oxidation state of iron atoms increases as the iron converts to an oxide."
"The oxidation state of oxygen decreases as it accepts electrons released by the iron."
"The main difference is that in electron-transfer redox reactions, only one electron flows, while in atom transfer redox reactions, an atom is transferred."
"Redox reactions find applications in various fields, including energy production, corrosion prevention, and chemical synthesis."
"A common everyday example of a redox reaction is the process of burning wood, where the carbon in wood undergoes oxidation, releasing energy."
"Reduction is defined as the gain of electrons by a substance."
"The redox couple of Fe2+/Fe3+ is often used to explain electron transfers in redox reactions."
"Electrode potentials provide a measure of the propensity of a substance to undergo oxidation or reduction."