While every effort has been made to follow citation style rules, there may be some discrepancies. Please refer to the appropriate style manual or other sources if you have any questions. Show Select Citation Style Copy CitationShare Share Share to social media Facebook Twitter URL https://www.britannica.com/science/oxidation-reduction-reactionGive Feedback External Websites Feedback Corrections? Updates? Omissions? Let us know if you have suggestions to improve this article (requires login). Feedback Type Your Feedback Submit FeedbackThank you for your feedback Our editors will review what you’ve submitted and determine whether to revise the article. External Websites
print Print Please select which sections you would like to print:
verifiedCite While every effort has been made to follow citation style rules, there may be some discrepancies. Please refer to the appropriate style manual or other sources if you have any questions. Select Citation Style Copy CitationShareShare Share to social media Facebook Twitter URL https://www.britannica.com/science/oxidation-reduction-reactionFeedbackExternal Websites Feedback Corrections? Updates? Omissions? Let us know if you have suggestions to improve this article (requires login). Feedback Type Your Feedback Submit FeedbackThank you for your feedback Our editors will review what you’ve submitted and determine whether to revise the article. External Websites
Alternate titles: redox reaction By Maynard V. Olson Last Updated: Nov 24, 2022 Edit History Table of ContentsRelated Topics:electrochemical reaction combustion oxidation number reduction biological oxidation...(Show more) See all related content → Summary Read a brief summary of this topicoxidation-reduction reaction, also called redox reaction, any chemical reaction in which the oxidation number of a participating chemical species changes. The term covers a large and diverse body of processes. Many oxidation-reduction reactions are as common and familiar as fire, the rusting and dissolution of metals, the browning of fruit, and respiration and photosynthesis—basic life functions. Major classificationsMost oxidation-reduction (redox) processes involve the transfer of oxygen atoms, hydrogen atoms, or electrons, with all three processes sharing two important characteristics: (1) they are coupled—i.e., in any oxidation reaction a reciprocal reduction occurs, and (2) they involve a characteristic net chemical change—i.e., an atom or electron goes from one unit of matter to another. Both reciprocity and net change are illustrated below in examples of the three most common types of oxidation-reduction reactions. Oxygen-atom transferCarbon reacts with mercury(II) oxide (a compound in which mercury has a bonding capacity expressed as +2; see below Oxidation-state change) to produce carbon dioxide and mercury metal. This reaction can be written in equation form: Carbon, receiving oxygen, is oxidized; mercury(II) oxide, losing oxygen, undergoes the complementary reduction; and the net change is the transfer of two oxygen atoms from mercury(II) oxide units to a carbon atom. Britannica Quiz Types of Chemical ReactionsHydrogen-atom transferHydrogen atoms are transferred from hydrazine, a compound of nitrogen and hydrogen, to oxygen in the following reaction: Hydrazine, losing hydrogen, is oxidized to molecular nitrogen, while oxygen, gaining hydrogen, is reduced to water. Get a Britannica Premium subscription and gain access to exclusive content. Subscribe Now Electron transferZinc metal and copper(II) ion react in water solution, producing copper metal and an aqueous (denoted by aq) zinc ion according to the equation With the transfer of two of its electrons, the zinc metal is oxidized, becoming an aqueous zinc ion, while the copper(II) ion, gaining electrons, is reduced to copper metal. Net change is the transfer of two electrons, lost by zinc and acquired by copper. Because of their complementary nature, the oxidation and reduction processes together are referred to as redox reactions. The reactant that brings about the oxidation is called the oxidizing agent, and that reagent is itself reduced by the reducing agent. In the examples given above, mercury(II) oxide, oxygen, and the copper(II) ion are oxidizing agents, and carbon, hydrazine, and zinc are the reducing agents. What is known as the reducing agent?In chemistry, a reducing agent (also known as a reductant, reducer, or electron donor) is a chemical species that "donates" an electron to an electron recipient (called the oxidizing agent, oxidant, oxidizer, or electron acceptor).
What is the reducing agent in combustion of glucose?For example, consider the overall reaction for aerobic cellular respiration: C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)The oxygen (O2) is being reduced, so it is the oxidizing agent. The glucose (C6H12O6) is being oxidized, so it is the reducing agent.
Is CO2 used as reducing agent?The oxidant which cannot act as a reducing agent is carbon dioxide CO2 as C atom is in its highest oxidation state and cannot increase its oxidation state.
|
