Name: electron transfer in redox
Uploaded: 2019-03-11T09:21:00.000Z
Duration: 1 min 24 s
Channel: JoVE

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ESS.EES.3.1

Redox Reactions

- [Verteller] Tijdens oxidatiereductie, of redoxreacties, worden elektronen overgedragen tussen atomen. De molecuul die een elektron doneert is geoxideerd. De molecuul die een elektron ontvangt is gereduceerd.

Het heeft een minder positieve lading. Als neutrale natrium- en chlooratomen ionen worden verliest natrium een elektron, het is geoxideerd. en chloor krijgt een elektron, het is gereduceerd.

Tevens wordt het molecuul dat een elektron doneert de reducerende agens genoemd. Waarbij het molecuul dat het elektron ontvangt de oxiderende agens is. Natrium is geoxideerd, dus dat is de reducerende agens. Chloor is gereduceerd, dus dat is de oxiderende agens.

redoxreacties

Oxidatie-reductie- of redoxreacties omvatten de overdracht van elektronen van het ene molecuul of atoom naar het andere. Wanneer een atoom een elektron verkrijgt, moet een ander atoom een elektron afstaan. Dit betekent dat oxidatie en reductie altijd gelijktijdig plaatsvinden. Omdat redoxreacties in paren optreden, wordt het atoom dat wordt geoxideerd het reductiemiddel genoemd, en het atoom dat wordt gereduceerd het oxidatiemiddel of de oxidant. Een eenvoudige manier om de definities van oxidatie en reductie te onthouden, is via de uitdrukking OIL-RIG, wat staat voor: Oxidation Is Losing– De Reductie neemt toe (elektronen).

Oxidatietoestanden

Een redoxreactie verandert de oxidatietoestanden van atomen. De oxidatietoestand of het oxidatiegetal verwijst naar de lading die een atoom zou hebben als al zijn bindingen met andere elementen puur ionisch waren. Het bepalen van veranderingen in de oxidatiegetallen van atomen in de reactanten kan helpen vaststellen of een reactie een oxidatie-reductiereactie is.

Bij de reactie tussen natrium en chloor, waarbij natriumchloride wordt gevormd, wordt natrium geoxideerd en chloor gereduceerd.

<img alt="Equation1" src="/files/ftp_upload/10671/Equation_1.svg" style="text-align: center; height: 13px;" />

Om het proces beter te begrijpen, is het nuttig om de reactie van elke stof afzonderlijk te bekijken in de vorm van halfreacties:

<img alt="Equation2" src="/files/ftp_upload/10671/Equation_2.svg" style="text-align: center; height: 13px;" />

<img alt="Equation3" src="/files/ftp_upload/10671/Equation_3.svg" style="text-align: center; height: 13px;" />

Deze vergelijkingen tonen aan dat Na-atomen elektronen verliezen, waardoor hun oxidatiegetal verandert van 0 naar +1. Tegelijkertijd winnen Cl-atomen (in Cl2-moleculen) elektronen, waardoor hun oxidatiegetal verandert van 0 naar -1.

Onvolledige overdracht van elektronen

Een redoxreactie kan niet alleen optreden bij de volledige overdracht van elektronen, maar ook wanneer de verdeling van elektronen binnen een covalente binding verandert.Een voorbeeld hiervan is de reactie tussen methaan en zuurstof, waarbij koolstofdioxide en water worden gevormd. In methaan zijn de elektronen gelijk verdeeld tussen koolstof en waterstof. In koolstofdioxide daarentegen is de koolstof gedeeltelijk positief, omdat zuurstof elektronen sterker aantrekt dan koolstof. Hierdoor verliest koolstof elektronen en wordt geoxideerd, terwijl zuurstof elektronen wint en wordt gereduceerd.

Deze tekst is aangepast van <a href="https://openstax.org/books/chemistry-2e/pages/4-2-classifying-chemical-reactions">Openstax, Chemistry 2e, Section 4.2: Classifying Chemical Reactions.</a>

Redoxreacties

Oxidation-reduction or redox reactions involve the transfer of electrons from one molecule or atom to another. When an atom gains an electron, another ...

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electron transfer in redox

Redox reactions are chemical reactions that involve electron transfer between atoms or molecules. When one particle gains electrons, another must lose them at the same time. That is why oxidation and reduction always happen together.

The two roles in a redox reaction are linked. The atom that is oxidized acts as the reducing agent, or reductant. The atom that is reduced acts as the oxidizing agent, or oxidant. A simple way to remember the ideas is OIL-RIG, which means oxidation is losing electrons and reduction is gaining electrons.

Redox reactions also change oxidation states, or oxidation numbers. An oxidation state is the charge an atom would have if all of its bonds were purely ionic. Checking whether oxidation numbers change in the reactants can help identify a redox reaction.

A sodium and chlorine reaction makes this idea clear. Sodium is oxidized, and chlorine is reduced to form sodium chloride. The process can be shown with half-reactions, which separate the fate of each reactant. In these equations, sodium goes from an oxidation number of 0 to 1+, while chlorine in Cl2 goes from 0 to 1-.

Electron transfer is not always complete. A redox reaction can also happen when the sharing of electrons changes in a covalent bond. Methane and oxygen can react to form carbon dioxide and water. In methane, electrons are shared equally between carbon and hydrogen, but in carbon dioxide the carbon is partially positive because oxygen pulls electrons more strongly. In that reaction, carbon dioxide is oxidized and oxygen is reduced.

Electron Transfer in Redox

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Learn how redox reactions move electrons, change oxidation states, and use half-reactions to track sodium, chlorine, methane, and oxygen.

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Electron Transfer in Redox

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