{"id":1584,"date":"2022-05-17T19:59:59","date_gmt":"2022-05-17T19:59:59","guid":{"rendered":"https:\/\/blog.praxilabs.com\/?p=1584"},"modified":"2025-10-11T22:26:38","modified_gmt":"2025-10-11T22:26:38","slug":"20-oxidation-reduction-examples","status":"publish","type":"post","link":"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/","title":{"rendered":"Most Famous Oxidation and Reduction Reactions Explained with 20+ Examples"},"content":{"rendered":"<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Chemistry is the branch of science where interactions and reactions between elements, atoms, electrons, molecules, and many other particles, is mainly considered and studied.<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/p>\n<p><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\">One of the most famous reactions widely abundant and occurring in chemistry, and in our day-to-day life, is the topic of this article: the process of oxidation and reduction and their reactions.<br \/>\n<\/span><span style=\"font-weight: 400;\">Here, we will discuss the nature of these reactions, their definitions, the <\/span><span style=\"font-weight: 400;\">difference between oxidation potential and reduction potential, and the <\/span><span style=\"font-weight: 400;\">difference between oxidizing agents and reducing agents, in addition to giving oxidation vs. reduction examples to clearly comprehend the process\u2026 Let\u2019s start!<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><strong><a class=\"maxbutton-3 maxbutton\" href=\"https:\/\/praxilabs.com\/\"><span class='mb-text'>try Oxidation and Reduction Reactions at Praxilabs for FREE<\/span><\/a><\/strong><\/span><\/p>\n<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_82_2 counter-hierarchy ez-toc-counter ez-toc-light-blue ez-toc-container-direction\">\r\n<div class=\"ez-toc-title-container\">\r\n<p class=\"ez-toc-title\" style=\"cursor:inherit\">Table of Contents<\/p>\r\n<span class=\"ez-toc-title-toggle\"><\/span><\/div>\r\n<nav><ul class='ez-toc-list ez-toc-list-level-1 ' ><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Oxidation_and_Its_Historical_Definition\" >Oxidation and Its Historical Definition<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Oxidation_Definition\" >Oxidation Definition<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Oxidation_reactions_may_involve_many_forms_as_follows\" >Oxidation reactions may involve many forms, as follows:<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#What_is_Oxidation_Mechanism\" >What is Oxidation Mechanism?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Examples_of_Oxidation_Reactions\" >Examples of Oxidation Reactions<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-6\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Reduction_Definition\" >Reduction Definition<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-7\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Reduction_Mechanism\" >Reduction Mechanism<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-8\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Examples_of_Reduction_Reactions\" >Examples of Reduction Reactions<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-9\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Identifying_Oxidizing_and_Reducing_Agents\" >Identifying Oxidizing and Reducing Agents<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-10\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Oxidation_and_Reduction_Demystified_Your_FAQs_Answered\" >Oxidation and Reduction Demystified: Your FAQs Answered<\/a><ul class='ez-toc-list-level-3' ><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-11\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#What_are_the_4_types_of_oxidation-_reduction_reactions\" >What are the 4 types of oxidation- reduction reactions?<\/a><ul class='ez-toc-list-level-4' ><li class='ez-toc-heading-level-4'><a class=\"ez-toc-link ez-toc-heading-12\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Combination\" >Combination<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-4'><a class=\"ez-toc-link ez-toc-heading-13\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Decomposition\" >Decomposition<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-4'><a class=\"ez-toc-link ez-toc-heading-14\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Displacement\" >Displacement<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-4'><a class=\"ez-toc-link ez-toc-heading-15\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#_Disproportionation\" >\u00a0Disproportionation<\/a><\/li><\/ul><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-16\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#What_is_oxidation_vs_reduction_reactions_in_organic_chemistry\" >What is oxidation vs reduction reactions in organic chemistry?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-17\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#What_are_examples_of_oxidation\" >What are examples of oxidation?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-18\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#How_can_a_reaction_be_both_oxidation_and_reduction\" >How can a reaction be both oxidation and reduction?<\/a><ul class='ez-toc-list-level-4' ><li class='ez-toc-heading-level-4'><a class=\"ez-toc-link ez-toc-heading-19\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/05\/17\/20-oxidation-reduction-examples\/#Example_of_Redox_Reactions\" >Example of Redox Reactions<\/a><\/li><\/ul><\/li><\/ul><\/li><\/ul><\/nav><\/div>\r\n<h2><span class=\"ez-toc-section\" id=\"Oxidation_and_Its_Historical_Definition\"><\/span><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 14pt;\"><b>Oxidation and Its Historical Definition<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">In case you are a fan of oxygen-based cleansers, or you are thankful for the sterilizing power of hydrogen peroxide products, then you must thank \u201coxidation.\u201d On the other hand, you can blame oxidation, if you ever have dealt with a rusty car or a toss out browned fruit.<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><span style=\"font-weight: 400;\">Oxidation is a process that can start spontaneously or artificially; it is helpful at times and very destructive at others.<\/span><\/span><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-5053 size-full\" src=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-2.webp\" alt=\"oxidation in the form of car rust\" width=\"515\" height=\"400\" srcset=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-2.webp 515w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-2-300x233.webp 300w\" sizes=\"auto, (max-width: 515px) 100vw, 515px\" \/><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The very classical example of oxidation is when iron interacts and combines with oxygen to form the iron oxide, or the famous reddish or orangish component: <\/span><b>rust.<br \/>\n<\/b><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>On PraxiLabs you can find different <\/b><a href=\"https:\/\/praxilabs.com\/en\/virtual-labs\"><b>virtual labs<\/b><\/a><b> simulations accessible anytime and anywhere. <\/b><a href=\"https:\/\/praxilabs.com\/en\/sign-up\"><b>Subscribe and Get Started NOW!<\/b><\/a><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">In this example, iron is said to be oxidized into rust, where the chemical reaction is given by:<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><strong>2 Fe + O<sub>2 \u2192 <\/sub>Fe<sub>2<\/sub>O<sub>3<\/sub><\/strong><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The older definition of the oxidation process was defined when oxygen or any other electronegative element was added to a compound. This very basic understanding was originating because <\/span><b>oxygen <\/b><b>(<\/b><b>O<\/b><sub><b>2<\/b><\/sub><b>)<\/b><span style=\"font-weight: 400;\"> was the <\/span><b>first<\/b><span style=\"font-weight: 400;\"> oxidizing agent to be known.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Later on, oxidation\u2019s definition was widened to include other types of chemical reactions that do not necessarily contain oxygen. Nevertheless, oxygen\u2019s addition to a compound meets the criteria of electron loss perfectly, in parallel with an increase in the oxidation state.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Oxidation_Definition\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Oxidation Definition<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p style=\"text-align: left;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Nowadays, the term <\/span><i><span style=\"font-weight: 400;\">oxidation <\/span><\/i><span style=\"font-weight: 400;\">is not looked at to be only oxygen-related, but it is looked at as a whole process that does not have to include oxygen. Rather, <\/span><b>oxidation<\/b><span style=\"font-weight: 400;\"> is defined as:<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cthe loss of electrons during a reaction by a molecule, atom, or ion.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Not all elements have the same tendency to lose or gain electrons. Some elements, i.e., metals, including magnesium, iron, and sodium, are easily oxidized, whereas the nonmetals like, chlorine, nitrogen, and oxygen, are not easily oxidized, and they are more reluctant to lose their electrons.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Oxidation_reactions_may_involve_many_forms_as_follows\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Oxidation reactions may involve many forms, as follows:<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<ol>\n<li style=\"font-weight: 400; text-align: left;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong>Addition of oxygen<br \/>\n<\/strong><strong><span style=\"font-weight: 400;\">C + <\/span><span style=\"font-weight: 400;\">O<\/span><sub><span style=\"font-weight: 400;\">2 \u2192 <\/span><\/sub><span style=\"font-weight: 400;\">CO<\/span><sub><span style=\"font-weight: 400;\">2 <\/span><\/sub><span style=\"font-weight: 400;\">(oxidation of carbon)<\/span><\/strong><\/span><\/li>\n<li><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong>Addition of an electronegative element<br \/>\n<\/strong><span style=\"font-weight: 400;\">Fe + S \u2192 <\/span><span style=\"font-weight: 400;\">FeS (oxidation of iron)<br \/>\n<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong>Removal of an electropositive element<br \/>\n<\/strong>2 KI + H<sub>2<\/sub>O<sub>2<\/sub> <span style=\"font-weight: 400;\">\u2192 <\/span>I<sub>2 <\/sub>+ 2 KOH (oxidation of iodide)<\/span><\/li>\n<li aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong>Removal of hydrogen<br \/>\n<\/strong>H<sub>2<\/sub>S + Br<sub>2<\/sub> \u2192 2 HBr + S (oxidation of sulfide)<\/span><\/li>\n<\/ol>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Another important definition is the <\/span><b>oxidizing agent, <\/b><span style=\"font-weight: 400;\">which is:<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201ca substance that accepts, gains, or receives an electron from a reducing agent.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Or, more briefly,<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cAny substance that oxidizes another substance.\u201d<\/span><\/i><\/span><\/p>\n<p style=\"text-align: left;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">In the four previously mentioned examples, the oxidizing agents are: <\/span><span style=\"font-weight: 400;\">O<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">, S, <\/span><span style=\"font-weight: 400;\">Br<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">, <\/span><span style=\"font-weight: 400;\">H<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">O<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">.<\/span><\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"What_is_Oxidation_Mechanism\"><\/span><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 14pt;\"><b>What is Oxidation Mechanism?<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Oxidation occurs in stages, and it results in a change in the properties of the atom or the compound that is being oxidized. For example, when iron experiences oxidation, it is transformed into a brittle, reddish powder, and it loses its stiffness and structurally-sound metal nature. This happens as a consequence of the process of losing electrons.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">To visually imagine what happens clearly, this following diagram illustrates what happens to an iron atom as it is oxidized. It starts to carry a charge once it is oxidized. This charge is:<\/span><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Not only one, but <\/span><b>3 charges, <\/b><span style=\"font-weight: 400;\">and<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Positive, as it lost <\/span><b>3 <\/b><span style=\"font-weight: 400;\">electrons.<\/span><\/span><\/li>\n<\/ol>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">This is chemically denoted by (3+) sign written as a superscript to the right of the iron (Fe) symbol. Iron is an effortlessly oxidized element; that is, iron&#8217;s exposure to oxygen and moisture is important and is always preferred. As long as oxygen is abundant, iron will keep losing its electrons.<\/span><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-5054 size-full\" src=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-3.webp\" alt=\"oxidation mechanism in iron metal explained with illustration\" width=\"544\" height=\"386\" srcset=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-3.webp 544w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-3-300x213.webp 300w\" sizes=\"auto, (max-width: 544px) 100vw, 544px\" \/><\/p>\n<p>&nbsp;<\/p>\n<p style=\"text-align: center;\"><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><a class=\"maxbutton-3 maxbutton\" href=\"https:\/\/praxilabs.com\/en\/virtual-chemistry-lab\"><span class='mb-text'>Try oxidation reduction at our virtual chemistry labs<\/span><\/a> \u00a0<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Examples_of_Oxidation_Reactions\"><\/span><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 14pt;\"><b>Examples of Oxidation Reactions<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Many reactions are considered as great examples of oxidation reactions, such as:<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\">The reaction between hydrogen and fluorine to give out hydrofluoric acid, that is given by:<br \/>\n<\/span><\/span><strong>H<sub>2 <\/sub>+ F<sub>2 \u2192 <\/sub>2 HF <\/strong><span style=\"font-weight: 400;\">This reaction can be better understood if it is written in terms of two half reactions, like:<br \/>\n<\/span><strong>H<sub>2<\/sub> \u2192 2 H<sup>+<\/sup>+ 2 e<sup>&#8211;<\/sup><br \/>\n<\/strong><strong>F<sub>2 <\/sub>+ 2e<sup>&#8211;<\/sup> \u2192 2 F<\/strong><sup><span style=\"font-weight: 400;\"><strong>&#8211;<\/strong><br \/>\n<\/span><\/sup><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\">It is easily noticed that this reaction does not have any oxygen atoms in any of its parts.<\/span><\/span><\/span><\/li>\n<li aria-level=\"1\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\">The interaction between copper and silver is a great example of electrochemical reactions, where:<br \/>\n<\/span><\/span><span style=\"font-weight: 400;\">Cu (s) + 2 <\/span><span style=\"font-weight: 400;\">Ag<\/span><sup><span style=\"font-weight: 400;\">+ <\/span><\/sup><span style=\"font-weight: 400;\">(aq) \u2192 <\/span><span style=\"font-weight: 400;\">Cu<\/span><sup><span style=\"font-weight: 400;\">2+ <\/span><\/sup><span style=\"font-weight: 400;\">(aq) + 2 Ag (s)<\/span><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\">Here, a wire of copper is placed into a silver ions solution, where electrons transfer from the copper metal to the silver ions. As a consequence, copper is oxidized by releasing its ions into the solution, and silver whiskers grow onto the copper wire.<\/span><\/span><\/span><\/span><\/li>\n<li style=\"text-align: left;\" aria-level=\"1\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\">The reaction between magnesium and oxygen to give out <a href=\"https:\/\/praxilabs.com\/en\/3d-simulations\/test-for-magnesium-radical-virtual-lab-chemistry-simulation\">magnesium radical<\/a> oxide is one example of oxidation where oxygen is conspicuous in the equation. That is to say: <\/span><strong>2 Mg (s) + O<sub>2 <\/sub>(g) \u2192 2 MgO (s)<\/strong><\/span><\/li>\n<\/ol>\n<h2><span class=\"ez-toc-section\" id=\"Reduction_Definition\"><\/span><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 14pt;\"><b>Reduction Definition<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The counter process to that of oxidation is known as <\/span><b>reduction, <\/b><span style=\"font-weight: 400;\">and rationally speaking, it is the process of gaining electrons. Reduction is defined as:<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cThe gain of electrons during a reaction by a molecule, atom, or ion.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The historical perspective of reduction was viewed as if it is a process where hydrogen, or any electropositive element, is added.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Reduction_Mechanism\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Reduction Mechanism<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\">Reduction mechanism is not any different than that of the oxidation. Here, and instead of losing electrons as it is the case with oxidation, elements gain electrons, and the compound is said to be <\/span><i><span style=\"font-weight: 400;\">reduced<\/span><\/i><span style=\"font-weight: 400;\">.<br \/>\n<\/span><span style=\"font-weight: 400;\">Also, changes happen to the properties of the atom or the compound that is being reduced.<\/span><\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Examples_of_Reduction_Reactions\"><\/span><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 14pt;\"><b>Examples of Reduction Reactions<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">This may involve many forms, as follows:<\/span><\/p>\n<ol>\n<li><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\">Addition of hydrogen<br \/>\n<\/span><strong>N<sub>2 <\/sub>+ 3 H<sub>2<\/sub> \u2192 2 NH<sub>3 <\/sub><\/strong><span style=\"font-weight: 400;\">(reduction of nitrogen)<\/span><\/span><\/li>\n<li><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\">Addition of electropositive element<br \/>\n<\/span><\/span><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\"><strong>SnCl<sub>2 <\/sub>+ 2 HgCl<sub>2<\/sub> \u2192 SnCl<sub>4 <\/sub>+ HgCl<sub>2 <\/sub><\/strong><span style=\"font-weight: 400;\">(reduction of mercuric oxygen)<\/span><\/span><\/span><\/span><\/li>\n<li><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\">Removal of oxygen<br \/>\n<strong>ZnO + C \u2192 <\/strong><span style=\"font-weight: 400;\"><span style=\"font-weight: 400;\"><strong>Zn + CO<\/strong> (reduction of zinc oxide)<\/span><\/span><\/span><\/li>\n<li><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\">Removal of electronegative element<br \/>\n<\/span><strong>2 FeCl<sub>3 <\/sub>+ H<sub>2<\/sub> \u2192 2 FeCl<sub>2 <\/sub><\/strong><span style=\"font-weight: 400;\"><strong>+ 2 HCl<\/strong> (reduction of ferric chloride)<\/span><\/span><\/li>\n<\/ol>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Again, the <\/span><b>reduction agent <\/b><span style=\"font-weight: 400;\">is important to be defined as follows:<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201ca substance that gives, loses, or donates an electron from an oxidizing agent.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Or, more briefly,<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cAny substance that oxidizes another substance.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The reduction agents in the previous examples are: <\/span><span style=\"font-weight: 400;\">H<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">, <\/span><span style=\"font-weight: 400;\">HgCl<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">, and C.<\/span><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\"><a href=\"https:\/\/praxilabs.com\/en\/blog\/2021\/03\/16\/applications-of-redox-titration\/\">Oxidation and reduction<\/a> are two simultaneous processes that occur together, and they result in a very famous reaction, known as: <\/span><b>redox reaction. <\/b><span style=\"font-weight: 400;\">In which, the atoms or the compounds gain and lose electrons simultaneously at the same time.<\/span><\/span><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-5055 size-medium\" src=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-4-300x218.webp\" alt=\"Illustration of redox reaction\" width=\"300\" height=\"218\" srcset=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-4-300x218.webp 300w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/08\/Most-Famous-Oxidation-and-Reduction-Reactions-4.webp 768w\" sizes=\"auto, (max-width: 300px) 100vw, 300px\" \/><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><a href=\"https:\/\/praxilabs.com\/en\/sign-up\"><strong>Join PraxiLabs for FREE, and enjoy your oxidation-reduction simulation!<\/strong><\/a><\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Identifying_Oxidizing_and_Reducing_Agents\"><\/span><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 14pt;\"><b>Identifying Oxidizing and Reducing Agents<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">An Oxidizing agent is a substance that accepts, gains, or receives an electron from a reducing agent.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">A reducing agent is a substance that gives, loses, or donates an electron from an oxidizing agent.<\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">For i<\/span>dentifying oxidizing and reducing agents<span style=\"font-weight: 400;\">:<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Break the reaction down into a net ionic equation and then into half-reactions.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The substance that loses electrons is being oxidized and is the reducing agent.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The substance that gains electrons is being reduced and is the oxidizing agent.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">For more clarification, let\u2019s take an example:<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">When chlorine gas is bubbled into a solution of sodium bromide, a reaction occurs which produces aqueous sodium chloride and bromine. Determine what is being oxidized and what is being reduced. Identify the oxidizing and reducing agents.<\/span><\/p>\n<p><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><strong>Cl2(g)+2NaBr(aq)\u21922NaCl(aq)+Br2(l)<\/strong><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Break the reaction down into a net ionic equation and then into half-reactions.<\/span><\/p>\n<p><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><strong>Cl2(g)+2Na+(aq)+2Br\u2212(aq) -\u2192 2Na+(aq)+2Cl\u2212(aq)+Br2(l)<\/strong><\/span><\/p>\n<p><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\"><strong>Cl2(g)+2Br\u2212(aq) \u21922Cl\u2212(aq)+Br2(l)<\/strong> (net ionic equation)<\/span><span style=\"font-weight: 400;\">\u00a0<\/span><\/span><\/p>\n<p><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><b>Reduction<\/b><span style=\"font-weight: 400;\">: <strong>Cl2(g)+2e\u2212\u21922Cl\u2212(aq)<\/strong><\/span><span style=\"font-weight: 400;\">\u00a0<\/span><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Oxidation<\/b><span style=\"font-weight: 400;\">: <strong>2Br\u2212(aq)\u2192Br2(l)+2e\u2212<\/strong><\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The Cl2 is being reduced and is the oxidizing agent.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The Br\u2212 is being oxidized and is the reducing agent.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Another example:<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Write the following reaction in the form of half-equations. Identify each half-equation as an oxidation or a reduction. Also identify the oxidizing agent and the reducing agent in the overall reaction<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><strong>Zn+2Fe3+\u27f6Zn2++2Fe2+<\/strong><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Answer<\/b><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The half-equations are<\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong>Zn\u27f6<\/strong><span style=\"font-weight: 400;\"><strong>Zn2++2e\u2212<\/strong> \u00a0 \u00a0 oxidation\u2014loss of electrons<\/span><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong>2e\u2212+2Fe3+\u27f6<\/strong><span style=\"font-weight: 400;\"><strong>2Fe2+<\/strong> \u00a0 reduction\u2014gain of electrons<\/span><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Zinc has been oxidized; the oxidizing <\/span><i><span style=\"font-weight: 400;\">agent<\/span><\/i><span style=\"font-weight: 400;\"> must be the other reactant, namely, iron(III).<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Iron(III) ions have been reduced; the zinc must be the reducing agent.<\/span><\/p>\n<p><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 12pt;\"><span style=\"font-weight: 400;\">Source : <\/span>Libretexts (2022) <i>8.2: Oxidizing and reducing agents<\/i>, <i>Chemistry LibreTexts<\/i>. Available at: https:\/\/chem.libretexts.org\/Bookshelves\/Introductory_Chemistry\/Chemistry_for_Changing_Times_(Hill_and_McCreary)\/08%3A_Oxidation_and_Reduction\/8.02%3A_Oxidizing_and_Reducing_Agents (Accessed: 28 July 2024).<\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Note<\/b><span style=\"font-weight: 400;\">: For identifying reduced and oxidized Elements, you should know that the elements that lose electrons are said to be oxidized, while the elements that gain electrons are said to be reduced.<\/span><\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Oxidation_and_Reduction_Demystified_Your_FAQs_Answered\"><\/span><span style=\"font-family: tahoma, arial, helvetica, sans-serif; font-size: 14pt;\">Oxidation and Reduction Demystified: Your FAQs Answered<\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<h3><span class=\"ez-toc-section\" id=\"What_are_the_4_types_of_oxidation-_reduction_reactions\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>What are the 4 types of oxidation- reduction reactions?<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>There are 4 types of oxidation-reduction reactions (Redox Reactions):<\/b><\/span><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Combination Reactions.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Decomposition Reactions.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Displacement Reactions.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Disproportionation Reactions.<\/span><\/li>\n<\/ul>\n<h4><span class=\"ez-toc-section\" id=\"Combination\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Combination<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h4>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Combination reactions \u201ccombine\u201d elements to form a chemical compound. As usual, oxidation and reduction occur together.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">For example:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>\u00a02 H2 + O2 \u2192 2 H2O<\/b><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The sum of oxidation states in the reactants is equal to that in the products: 0 + 0 \u2192 (2)(+1) + (-2)<\/span><\/p>\n<h4><span class=\"ez-toc-section\" id=\"Decomposition\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Decomposition<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h4>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Decomposition reactions are the reverse of combination reactions, meaning they involvethe breakdown of a chemical compound into its component elements.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">For example:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">\u00a0<\/span><b>2 H2O \u2192 2 H2 + O2<\/b><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>\u00a0(2)(+1) + (-2) = 0 \u2192 0 + 0<\/b><\/span><\/p>\n<h4><span class=\"ez-toc-section\" id=\"Displacement\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Displacement<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h4>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Displacement reactions, also known as replacement reactions, involve compounds and the \u201creplacement\u201dof elements. They occur as single and double replacement reactions.<\/span><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>A single replacement reaction<\/b><span style=\"font-weight: 400;\"> \u201creplaces\u201d an element in the reactants with another element in the products.<\/span><\/span><\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">For example:<\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Cl2 + 2 NaBr \u2192 2 NaCl + Br2<\/b><span style=\"font-weight: 400;\"> (Cl is reduced and replaces Br, while Br is oxidized)<\/span><\/span><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>A double replacement reaction<\/b><span style=\"font-weight: 400;\"> is similar to a single replacement reaction but involves \u201creplacing\u201d two elements in the reactants with two in the products.<\/span><\/span><\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">For example:<\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Fe2O3 + 6 HCl \u2192 2 FeCl3 + 3 H2O<\/b><span style=\"font-weight: 400;\"> (Fe and H as well as O and Cl trade places)<\/span><\/span><\/p>\n<h4><span class=\"ez-toc-section\" id=\"_Disproportionation\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>\u00a0Disproportionation<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h4>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Disproportionation reactions refer to the reactions of some substances which can be both oxidized and reduced. For example: the reaction of hydrogen peroxide, H2O2, when it is poured over a wound. At first, this might look like a simple decomposition reaction, because hydrogen peroxide breaks down to produce oxygen and water: <\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>2 H2O2 (aq.) \u2192 2 H2O(l) + O2(g)<\/b><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The key to this reaction lies in the oxidation states of oxygen, however. Notice that oxygen is present in the reactant and <\/span><i><span style=\"font-weight: 400;\">both<\/span><\/i><span style=\"font-weight: 400;\"> products. In H2O2, oxygen has an oxidation state of -1. In H2O, its oxidation state is -2, and it has been reduced. In O2,however, its oxidation state is 0, and it has been oxidized. Oxygen has been both oxidized and reduced in the reaction, making this a disproportionation reaction.<\/span><\/span><\/p>\n<h3><span class=\"ez-toc-section\" id=\"What_is_oxidation_vs_reduction_reactions_in_organic_chemistry\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>What is oxidation vs reduction reactions in organic chemistry?<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<table>\n<tbody>\n<tr>\n<td style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Oxidation Reaction<\/b><\/span><\/td>\n<td style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Reduction Reaction<\/b><\/span><\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Oxidation is the loss of electrons during a reaction by a molecule, atom, or ion.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Oxidation is the process by which a carbon atom gains bonds to more electronegative elements, with oxygen being the most common.\u00a0<\/span><\/td>\n<td><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Reduction is the gain of electrons during a reaction by a molecule, atom, or ion.<\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Reduction is a process by which a carbon atom gains bonds to less electronegative elements,<\/span> <span style=\"font-weight: 400;\">with hydrogen being the most common.<\/span><\/span><\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>There are many forms of oxidation reactions:<\/b><\/span><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Addition of oxygen<\/b><b><br \/>\n<\/b> <span style=\"font-weight: 400;\">C + O<\/span><span style=\"font-weight: 400;\">2 \u2192 <\/span><span style=\"font-weight: 400;\">CO<\/span><span style=\"font-weight: 400;\">2 <\/span><span style=\"font-weight: 400;\">(oxidation of carbon)<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Addition of an electronegative element<\/b><b><br \/>\n<\/b> <span style=\"font-weight: 400;\">Fe + S \u2192 FeS (oxidation of iron)<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Removal of an electropositive element<\/b><b><br \/>\n<\/b> <span style=\"font-weight: 400;\">2 KI + H<\/span><span style=\"font-weight: 400;\">2<\/span><span style=\"font-weight: 400;\">O<\/span><span style=\"font-weight: 400;\">2<\/span><span style=\"font-weight: 400;\"> \u2192 I<\/span><span style=\"font-weight: 400;\">2 <\/span><span style=\"font-weight: 400;\">+ 2 KOH (oxidation of iodide)<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Removal of hydrogen<\/b><b><br \/>\n<\/b> <span style=\"font-weight: 400;\">H<\/span><span style=\"font-weight: 400;\">2<\/span><span style=\"font-weight: 400;\">S + Br<\/span><span style=\"font-weight: 400;\">2<\/span><span style=\"font-weight: 400;\"> \u2192 2 HBr + S (oxidation of sulfide)<\/span><\/span><\/li>\n<\/ol>\n<\/td>\n<td><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>There are many forms of reduction reactions:<\/b><\/span><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Addition of hydrogen<\/b><b><br \/>\n<\/b><span style=\"font-weight: 400;\"> N<\/span><span style=\"font-weight: 400;\">2 <\/span><span style=\"font-weight: 400;\">+ 3 H<\/span><span style=\"font-weight: 400;\">2<\/span><span style=\"font-weight: 400;\"> \u2192 2 NH<\/span><span style=\"font-weight: 400;\">3 <\/span><span style=\"font-weight: 400;\">(reduction of nitrogen)<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Addition of electropositive element<\/b><b><br \/>\n<\/b> <span style=\"font-weight: 400;\">SnCl<\/span><span style=\"font-weight: 400;\">2 <\/span><span style=\"font-weight: 400;\">+ 2 HgCl<\/span><span style=\"font-weight: 400;\">2<\/span><span style=\"font-weight: 400;\"> \u2192 SnCl<\/span><span style=\"font-weight: 400;\">4 <\/span><span style=\"font-weight: 400;\">+ HgCl<\/span><span style=\"font-weight: 400;\">2 <\/span><span style=\"font-weight: 400;\">(reduction of <a href=\"https:\/\/praxilabs.com\/en\/3d-simulations\/test-for-mercuric-radical-virtual-lab-chemistry-simulation\">mercuric radical<\/a> oxygen)<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Removal of oxygen<\/b><b><br \/>\n<\/b> <span style=\"font-weight: 400;\">ZnO + C \u2192 Zn + CO (reduction of zinc oxide)<\/span><\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Removal of electronegative element<\/b><b><br \/>\n<\/b> <span style=\"font-weight: 400;\">2 FeCl<\/span><span style=\"font-weight: 400;\">3 <\/span><span style=\"font-weight: 400;\">+ H<\/span><span style=\"font-weight: 400;\">2<\/span><span style=\"font-weight: 400;\"> \u2192 2 FeCl<\/span><span style=\"font-weight: 400;\">2 <\/span><span style=\"font-weight: 400;\">+ 2 HCl (reduction of ferric chloride)<\/span><\/span><\/li>\n<\/ol>\n<\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Oxidizing agent is <\/b><span style=\"font-weight: 400;\">a substance that accepts, gains, or receives an electron from a reducing agent.<\/span><\/span><\/td>\n<td><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Reduction agent <\/b><span style=\"font-weight: 400;\">is a substance that gives, loses, or donates an electron from an oxidizing agent.<\/span><\/span><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h3><span class=\"ez-toc-section\" id=\"What_are_examples_of_oxidation\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>What are examples of oxidation?<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<ul>\n<li><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">\u00a0Rusting is a form of corrosion of metal. Corrosion occurs due to the degradation of a metal by the action of water (moisture) and air as a result of the metal oxidation. Iron catches rust because it gets oxidized in the presence of air and water to form hydrated iron oxide (Fe2O3.xH2O).<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The iron oxide forms a reddish-brown covering on the metal surface. <strong>4Fe + 3O2 + 2xH2O \u2014&gt; Fe2O3.xH2O<\/strong> (Rust).<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The rancidity happens when fried foods acquire a bad odor and flavor after being exposed to air for a long time.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The respiration\u00a0 is the process that\u00a0 happens inside our bodies, which triggers an oxidation reaction. The food is oxidized during the metabolism cycles to produce the energy we need for our life.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Browning: Oxygen in the air can cause the sliced fruits )such as apple( to brown, a process called enzymic browning which is considered as an oxidation reaction. In the apple cells, phenols and the enzyme phenolase are found, and when exposed to oxygen in the air, for example through slicing, the oxygen causes a reaction (oxidation).<\/span><\/li>\n<li><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The interaction between copper and silver is a great example of electrochemical reactions, where:<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><span style=\"font-weight: 400;\"> Cu (s) + 2 Ag<\/span><span style=\"font-weight: 400;\">+ <\/span><span style=\"font-weight: 400;\">(aq) \u2192 Cu<\/span><span style=\"font-weight: 400;\">2+ <\/span><span style=\"font-weight: 400;\">(aq) + 2 Ag (s) . <\/span>Here, a wire of copper is placed into a silver ions solution, where electrons transfer from the copper metal to the silver ions. As a consequence, copper is oxidized by releasing its ions into the solution, and silver whiskers grow onto the copper wire.<\/span><\/li>\n<\/ul>\n<ul>\n<li><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Combustion reactions. For example, Bunsen burners which are used in the school lab use methane (a hydrocarbon) as fuel, which burns with oxygen in the air (oxidation reaction).<\/span><\/li>\n<\/ul>\n<h3><span class=\"ez-toc-section\" id=\"How_can_a_reaction_be_both_oxidation_and_reduction\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>How can a reaction be both oxidation and reduction?<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The reaction can be both oxidation and reduction in case of redox reactions,<\/span><span style=\"font-weight: 400;\"> which <\/span><span style=\"font-weight: 400;\">is a type of chemical reaction that involves a transfer of electrons between two species.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">In redox reactions, oxidation and reduction are two simultaneous processes that occur together, and the atoms or the compounds gain and lose electrons simultaneously at the same time.<\/span><\/p>\n<h4><span class=\"ez-toc-section\" id=\"Example_of_Redox_Reactions\"><\/span><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Example of Redox Reactions<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h4>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">In the reaction between hydrogen and fluorine, hydrogen is being oxidized and fluorine is being reduced:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>H2 + F2 \u2192 2 HF<\/b><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">This reaction is spontaneous and releases 542 kJ per 2 g of hydrogen because the H-F bond is much stronger than the weak, high-energy F-F bond. We can write this overall reaction as two half-reactions:<\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>The oxidation reaction:<\/b><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>H2 \u2192 2 H+ + 2 e\u2212<\/b><\/span><\/p>\n<p><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>And the reduction reaction:<\/b><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>F2 + 2 e\u2212 \u2192 2 F\u2212<\/b><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">Elements, even in molecular form, always have an oxidation state of zero. In the first half-reaction, hydrogen is oxidized from an oxidation state of zero to an oxidation state of +1. In the second half-reaction, fluorine is reduced from an oxidation state of zero to an oxidation state of \u22121.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">When adding the reactions together, the electrons are canceled and the ions combine to form hydrogen fluoride:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>2 H+ + 2 F\u2212 \u2192 2 HF<\/b><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\">The overall reaction is<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>H2 + F2 \u2192 2 HF<\/b><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>PraxiLabs provides <\/b><b>virtual experiments simulations<\/b><b> in analytical chemistry..\u00a0 <\/b><a href=\"https:\/\/praxilabs.com\/en\/sign-up\"><b>Create a free account now <\/b><\/a><b>and try our simulations that you can access anytime and anywhere to perform a variety of chemistry experiments.<\/b><\/span><\/p>\n","protected":false},"excerpt":{"rendered":"<p>Chemistry is the branch of science where interactions and reactions between elements, atoms, electrons, molecules, and many other particles, is mainly considered and studied. One of the most famous reactions widely abundant and occurring in chemistry, and in our day-to-day life, is the topic of this article: the process of oxidation and reduction and their &hellip;<\/p>\n","protected":false},"author":11,"featured_media":4521,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_lmt_disableupdate":"no","_lmt_disable":"no","footnotes":""},"categories":[3],"tags":[],"class_list":["post-1584","post","type-post","status-publish","format-standard","has-post-thumbnail","","category-chemistry"],"modified_by":"Muhamed Elmesery","_links":{"self":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts\/1584","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/users\/11"}],"replies":[{"embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/comments?post=1584"}],"version-history":[{"count":26,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts\/1584\/revisions"}],"predecessor-version":[{"id":5422,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts\/1584\/revisions\/5422"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/media\/4521"}],"wp:attachment":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/media?parent=1584"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/categories?post=1584"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/tags?post=1584"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}