Redox Reactions and Electrochemistry

• Redox Reaction: Involves the transfer of electrons between chemical species, characterized by oxidation and reduction processes.

Half Reaction

• Represents either the oxidation or the reduction part of a redox reaction, examined separately.

Oxidation

• The loss of electrons by a species during a chemical reaction.

Electrochemistry

• The study of redox reactions and the phenomena of electron transfer.

Disproportionation Reaction

• A reaction where a single species undergoes both oxidation and reduction simultaneously.

Reduction

• The gain of electrons by a species during a chemical reaction.

LEO

• Acronym for "Loss of Electrons is Oxidation," a mnemonic to remember oxidation.

GER

• Acronym for "Gain of Electrons is Reduction," a mnemonic to remember reduction.

Oxidizing Agent (OA)

• The species that facilitates oxidation in a reaction by accepting electrons.

Reducing Agent (RA)

• The species that facilitates reduction in a reaction by donating electrons.

Non-Redox Reaction

• A reaction in which no electron transfer occurs between the reactants.

Change in State

• Indicates a redox reaction when ions are formed.

Ionic Compounds

• Compounds formed through the transfer of electrons, resulting in the creation of ions.

Spectators

• Species or ions that are present in a reaction but do not participate in the electron transfer process.

Water Formation

• The combination of H+ and OH- ions to produce H2O molecules.

Oxidation Half Reaction

• Characterized by electrons appearing as products in the reaction.

Reduction Half Reaction

• Characterized by electrons appearing as reactants in the reaction.

Forward Reaction

• The reaction direction that leads to the formation of products from reactants.

Spontaneous Reactions

• Reactions that proceed without the need for additional energy input.

Non-Spontaneous Reactions

• Reactions that require external energy to occur.

Strongest Oxidizing Agent (SOA)

• Located at the top left of a redox table.

Strongest Reducing Agent (SRA)

• Located at the bottom right of a redox table.

Spontaneity Rule

• Used to determine whether a reaction will proceed without any external energy input.

Half-Cell Reaction

• Represents either the oxidation or reduction process occurring at an electrode in electrochemistry.

Primary Standard

• A substance available in a stable and pure state, can be directly used to prepare a standard solution.

Voltaic Cells

• Electrochemical cells that produce energy through spontaneous chemical reactions.

Electrolytic Cells

• Electrochemical cells that require energy to drive non-spontaneous reactions.

Electrolyte

• An aqueous solution containing ions that enables electrical conduction.

Electrode

• A solid electrical conductor that boosts redox reactions.

Half Cell

• An electrode immersed in an electrolyte solution where redox reactions occur.

Cathode

• The positive electrode where reduction occurs in an electrochemical cell.

Anode

• The negative electrode where oxidation occurs in an electrochemical cell.

Phase Boundary

• The separation between the solid electrode and the liquid electrolyte in a cell.

Salt Bridge

• A component used to maintain electrical neutrality within electrochemical cells.

Porous Cup

• A container that allows ion movement between solutions without the use of a salt solution.

Cell Potential

• The difference in reduction potentials between two half-cells, determining the voltage of the cell.

Corrosion

• A redox reaction where a metal returns to its ore state.

Oxide Coating

• A protective layer formed on metals that preserves the remaining metal from corrosion.

Iron Corrosion

• A specific spontaneous reaction of iron with water and oxygen.

Rust

• Iron (III) oxide hydrates that are formed as a result of iron corrosion.

Flaking

• The detachment of rust from iron, exposing fresh iron to further corrosion.

Protective Coatings

• Barriers applied to metals to prevent contact with oxygen and water, thus preventing corrosion.

Galvanization

• The process of coating iron with zinc to protect it from corrosion.

Cathodic Protection

• Preventing iron degradation by making it the cathode in an electrochemical cell.

Impressed Current

• The method of electrically forcing electron flow through iron to prevent corrosion.

Sacrificial Anode

• A stronger reducing agent connected to iron to protect it from degradation by corroding instead.

Electric Cell

• A device that converts chemical energy into electrical energy.

Explore redox reactions involving electron transfer, oxidation, and reduction. Understand half-reactions, electrochemistry, disproportionation, and the roles of oxidizing and reducing agents, along with LEO and GER mnemonics.