Redox reactions
Redox Reactions
Redox reactions (pronounced: /ˈriːdɒks/), also known as oxidation-reduction reactions, are a type of chemical reaction that involve a transfer of electrons between two species. The term "redox" comes from two concepts involved with electron transfer: reduction and oxidation.
Etymology
The term "redox" is a portmanteau of the words "reduction" and "oxidation". The concept of redox reactions dates back to the late 18th century with the work of Antoine Lavoisier on the nature of chemical reactions, but the term itself was coined in the 1920s.
Oxidation
In the context of a redox reaction, oxidation (pronounced: /ɒksɪˈdeɪʃən/) is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. The term comes from the Greek word for "sharp", referring to the pungent smell of oxygen gas produced by some reactions.
Reduction
Reduction (pronounced: /rɪˈdʌkʃən/) in a redox reaction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion. The term is derived from the Latin word "reducere", meaning "to lead back".
Related Terms
- Oxidizing agent: A substance that has the ability to oxidize other substances, meaning it causes them to lose electrons.
- Reducing agent: A substance that has the ability to reduce other substances, meaning it causes them to gain electrons.
- Half-reaction: Either the oxidation or reduction reaction component of a redox reaction.
- Electrochemistry: The study of chemical reactions that involve the movement of electrons.
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