Name: redox reactions and half-reaction balancing
Uploaded: 2020-09-24T15:06:52.000Z
Duration: 2 min 58 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.3

Balancing Redox Equations

Como é que uma bateria fornece eletricidade para operar dispositivos móveis, porque é que um abacate cortado fica castanho ou o metal enferruja debaixo de água, estes processos são originados por tipos específicos de reações químicas que envolvem a transferência de elétrons de um átomo para outro. O átomo que perde elétrons é oxidado, enquanto o átomo que ganha elétrons é reduzido. Estas reações são chamadas de reações de oxidação-redução ou redox e são caracterizadas por alterações no estado de oxidação para um ou mais reagentes.A interação entre o magnésio e o ácido clorídrico concentrado é um exemplo de uma reação redox. Aqui, o magnésio é oxidado a 2 íons de magnésio, e os prótons são reduzidos a gás de hidrogénio. As equações químicas simples podem ser facilmente equilibradas.No entanto, como a maioria das equações redox são complexas, o número de elétrons perdidos e ganhos deve ser justificado. Ao equilibrar as equações redox, é essencial observar a lei de conservação da massa. A quantidade de cada elemento e qualquer ganho ou perda de elétrons deve estar equilibrada em ambos os lados da reação;assim, se um reagente é reduzido, outro deve ser oxidado.O método das meias-reações é utilizado para equilibrar as equações redox com sucesso. Consideremos a reação de permanganato com oxalato. Para soluções ácidas aquosas, atribui-se os estados de oxidação e divide-se a reação na sua componente de semirreações.Depois, equilibra-se cada semirreação omitindo o hidrogénio e o oxigénio. Aqui, o manganês já está equilibrado, mas o oxalato precisa de um coeficiente de dois;segundo, equilibra-se os átomos de oxigénio com a adição de moléculas de água;e terceiro, equilibram-se os átomos de hidrogénio adicionando prótons sempre que necessário. Equilibram-se as cargas adicionando elétrons.Uma vez que o manganês é reduzido, são adicionados cinco elétrons no lado do reagente. Em contrapartida, o oxalato é oxidado;assim, são adicionados dois elétrons no lado do produto. Multiplicam-se as semirreações por um número inteiro por isso o número de elétrons adicionados é igual.Por último, acrescentam-se e simplificam-se as meias-reações equilibradas Cancelando as espécies em ambos os lados para obter uma reação redox equilibrada. Para soluções aquosas básicas, o procedimento é semelhante, mas inclui um passo adicional. Aqui, é adicionado um número igual de íons de hidroxilo a ambos os lados da reação para neutralizar os prótons antes de somar as semirreações equilibradas.

equilíbrio de reações redox

A eletroquímica é a ciência envolvida na interconversão de reações elétricas e químicas. Tais reações são chamadas de oxidação-redução, ou reações redox. Estas importantes reações são definidas por mudanças nos estados de oxidação para um ou mais elementos de reagentes e incluem um subconjunto de reações envolvendo a transferência de eletrões entre espécies de reagentes. A eletroquímica como campo evoluiu de forma a fornecer conhecimentos suficientes sobre os princípios fundamentais da química redox e de várias tecnologias, desde processos metalúrgicos à escala industrial até baterias robustas e recarregáveis para veículos elétricos. Como as reações que envolvem a transferência de eletrões são essenciais para o estudo da eletroquímica, uma breve revisão da química redox inclui o seguinte.
Números de Oxidação
Por definição, uma reação redox envolve uma alteração no número de oxidação ou no estado de oxidação de um ou vários reagentes. O número de oxidação de um elemento é uma avaliação de como o ambiente eletrónico dos seus átomos difere em relação aos átomos do elemento puro. Por esta definição, um átomo de um elemento carrega um número de oxidação de zero. Para um átomo, o número de oxidação é igual à carga do átomo no composto se o composto fosse iónico. Assim, a soma dos números de oxidação de todos os átomos em uma molécula é igual à carga da molécula.
Compostos Iónicos
Os compostos iónicos simples são os exemplos mais simples deste formalismo, uma vez que os elementos têm números de oxidação iguais às suas cargas iónicas. O cloreto de sódio, NaCl, é composto por catiões Na+ e aniões Cl−, sendo os números de oxidação para sódio e cloro +1 e −1, respectivamente. O fluoreto de cálcio, CaF2, é composto por catiões Ca2+ e aniões F−, com números de oxidação para cálcio e flúor, +2 e −1.
Compostos Covalentes
Os compostos covalentes são mais desafiantes no uso do formalismo. A água é um composto covalente constituído por dois átomos H ligados a um átomo O através de ligações O−H covalentes polares. Os eletrões partilhados que fazem uma ligação O−H são mais fortemente atraídos pelo átomo O mais eletronegativo. Assim o oxigénio adquire uma carga negativa parcial, em comparação com um átomo de O em oxigénio elementar. Como resultado, os átomos de H em uma molécula de água apresentam carga positiva parcial em comparação com os átomos de hidrogénio em hidrogénio gasoso. A soma das cargas parciais negativas e positivas para cada molécula de água é zero, tornando a molécula de água neutra.
Se a polarização de eletrões partilhados dentro das ligações O−H da água estivesse completa, o resultado seria a transferência completa de eletrões de H para O e a água seria um composto iónico composto por aniões O2− e catiões H+. E assim, os números de oxidação para oxigénio e hidrogénio na água são de −2 and +1, respectivamente. Aplicando esta mesma lógica ao tetracloreto de carbono, CCl4, temos números de oxidação de +4 para carbono e −1 para cloro. No ião nitrato, NO3−, o número de oxidação para o azoto é +5 e para o oxigénio é −2, somando-se para igualar a carga de −1 na molécula:
<img alt="Eq1" src="/files/ftp_upload/11432/11432_Equation_1.png" style="text-align: center; height: 70px;" />
Equilíbrio de Equações Redox
A equação desequilibrada apresentada abaixo descreve a decomposição do cloreto de sódio:
<img alt="Eq2" src="/files/ftp_upload/11432/11432_Equation_2.png" style="text-align: center; height: 48px;" />
Esta reação corresponde ao critério para uma reação redox, uma vez que o número de oxidação para Na diminui de +1 para 0 (passando por redução) e para Cl aumenta de −1 para 0 (passando por oxidação). O caso da equação é facilmente equilibrado pela adição do coeficiente estequiométrico de 2 para NaCl e Na:
<img alt="Eq3" src="/files/ftp_upload/11432/11432_Equation_3.png" style="text-align: center; height: 48px;" />
Reações redox que ocorrem em soluções aquosas são comumente encontradas em eletroquímica e muitas envolvem água ou os iões, H+ (aq) e OH− (aq), quer como reagentes ou como produtos.
Nesses casos, equações que representam reações redox podem ser muito desafiantes para equilibrar apenas por inspecção, e o uso de uma abordagem sistemática conhecida como método de semi-reação é útil. Esta abordagem envolve os seguintes passos:
<ol>
<li>Dividir a equação nos esqueletos das suas semi-reações de oxidação e redução componentes.</li>
<li>Equilibrar cada semi-reação para todos os elementos que não O e H.</li>
<li>Equilibrar cada semi-reação para os átomos de O adicionando moléculas de água na equação conforme necessário.</li>
<li>Equilibrar cada semi-reação para átomos de H adicionando protões na equação conforme necessário.</li>
<li>Finalmente, equilibrar as cargas nos elementos adicionando eletrões conforme necessário.</li>
<li>Multiplicar as semi-reações por qualquer número inteiro necessário para igualar o número de eletrões perdidos na semi-reação de oxidação ao número de eletrões ganhos na semi-reação de redução.</li>
<li>Adicionar ambas as semi-reações e simplificá-las ainda mais, cancelando espécies comuns em ambos os lados da equação.</li>
<li>Se a reação ocorrer em meio alcalino, adicionar iões OH− à equação obtida no passo 7 para neutralizar os protões (adicionados em números iguais a ambos os lados da equação) e simplificar.</li>
<li>Verificar a equação para garantir que as cargas nos átomos estão equilibradas.</li>
</ol>
Este texto é adaptado de  <a href="https://openstax.org/books/chemistry-2e/pages/17-1-review-of-redox-chemistry">Openstax, Chemistry 2e, Chapter 17: Introduction,</a> e <a href="https://openstax.org/books/chemistry-2e/pages/17-1-review-of-redox-chemistry">Openstax, Chemistry 2e, Section17.2: Review of Redox Chemistry</a>.

Equilíbrio de Reações Redox

A eletroquímica é a ciência envolvida na interconversão de reações elétricas e químicas. Tais reações são chamadas de redução-oxidação, ou ...

Education

JoVE Core

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Electrochemistry

Eletroquímica

KEY TERMS AND CONCEPTS

TERMOS-CHAVE E CONCEITOS

redox reactions and half-reaction balancing

Redox reactions involve electron transfer and changes in oxidation number. In electrochemistry, these reactions connect chemical changes with electrical energy. They also power technologies such as industrial metal processing and rechargeable batteries used in electric vehicles.

Oxidation number is a way to track how an atom's electronic environment changes compared with the pure element, where the oxidation number is zero. For a simple ionic compound, the oxidation number matches the ion charge. Sodium chloride has Na at +1 and Cl at -1, and calcium fluoride has Ca at +2 and F at -1.

Covalent compounds need a closer look because electrons are shared. In water, the O-H bonds are polar, so oxygen pulls shared electrons more strongly than hydrogen does. That gives oxygen an oxidation number of -2 and hydrogen +1. The same idea gives carbon +4 and chlorine -1 in carbon tetrachloride, and nitrogen +5 with oxygen -2 in the nitrate ion, which adds up to the ion's -1 charge.

A simple redox example is the decomposition of sodium chloride. Sodium changes from +1 to 0, so it is reduced. Chlorine changes from -1 to 0, so it is oxidized. The equation is balanced by placing a coefficient of 2 in front of NaCl and Na.

Redox reactions in aqueous solution are often harder to balance because water, H+ ions, or OH- ions can appear as reactants or products. A systematic half-reaction method helps. First, split the equation into oxidation and reduction half-reactions. Then balance all elements except O and H, add water for oxygen, add protons for hydrogen, and add electrons to balance charge. After that, multiply the half-reactions so the electrons lost and gained are equal, add them together, and cancel species that appear on both sides.

If the reaction occurs in an alkaline medium, add OH- ions to neutralize the protons and simplify the equation. Finish by checking that both atoms and charge are balanced. This method gives a clear path for balancing redox equations in electrochemistry.

Redox Reactions and Half-Reaction Balancing

redox-reactions-and-half-reaction-balancing

balancing redox equations

Redox reactions involve electron transfer and changes in oxidation number. In electrochemistry, these reactions connect chemical changes with electrical energy. They also power technologies such as industrial metal processing and rechargeable batteries used in electric vehicles. Oxidation number is a way to track how an atom's electronic environment changes compared with the pure element, where the oxidation number is zero. For a simple ionic compound, the oxidation number matches the ion...

electromotive force

Cell Voltage and Electron Flow

Electric current is the flow of electric charge through a conducting medium or a solution. In wires, that charge is carried by electrons. In some solutions, ions can also move and carry charge. When electrons move through a wire, they produce an electric current. This idea connects to redox reactions, where electrons are lost and gained. In the spontaneous reaction between zinc and copper ions, zinc is oxidized to zinc ions. Copper ions are reduced to solid copper. Even so, this direct...

voltaic/galvanic cells

Galvanic Cells and Battery Reactions

Galvanic cells use spontaneous redox reactions to produce electric current. A common example is a disposable AA battery, which powers devices by turning chemical energy into electrical energy. Another example is a copper wire placed in silver nitrate solution, where the solution slowly turns bright blue and a grey solid forms on the wire. In the copper and silver reaction, copper is oxidized and silver ions are reduced. Copper forms cuprous ions, which give the solution its blue color. At the...

standard electrode potentials

Using Electrode Potentials to Predict Reactions

Electrode potentials help predict whether a redox reaction will happen on its own. A redox reaction involves electron transfer. In electrochemistry, the measured value is called cell potential or cell voltage. It shows the energy linked to charge transfer and is measured in volts, where 1 volt equals 1 joule per coulomb. A single half-cell cannot be measured by itself because electron transfer needs both a donor and a receiver. For that reason, scientists measure the difference between two...

cell potential and free energy

Redox Cell Potential, ΔG°, and K

Redox cell potential connects chemical energy, free energy change, and the equilibrium constant in an electrochemical cell. In these reactions, chemical energy is converted into electrical energy. That link helps predict whether a reaction is spontaneous and how far it may proceed. Thermodynamics is the study of how heat and other forms of energy are related. In an electrochemical cell, cell potential can also reflect oxidizing strength or reducing strength. A similar idea appears in acid-base...

the nernst equation

Cell Potential Under Changing Conditions

Cell potential changes when a redox reaction does not run at standard conditions. Standard cell potentials connect with standard free energy change, ΔG°, and the equilibrium constant K, but those relationships only hold at 1 M concentration, 298 K, and 1 atmosphere. A zinc(II) and tin(II) redox cell with E°cell = +0.291 V and ΔG° = −56.2 kJ is spontaneous under those standard conditions. As a cell discharges, the reactant concentration changes and the cell potential steadily drops. Many redox...

concentration cells

Cell Potential from Concentration Differences

Concentration cells are voltaic cells that use two almost identical half-cells. The half-cells use the same electrode and the same half-reaction. They differ only in the concentration of one redox species, so the cell potential depends on that concentration difference. In a concentration cell, the Nernst equation can be used to find the cell potential. For the zinc example shown, the calculated cell potential is positive. A positive cell potential means the overall reaction is spontaneous. <br...

batteries and fuel cells

Primary, Rechargeable Batteries and Fuel Cells

Batteries and fuel cells are galvanic cells that supply electrical power for many applications. They range from tiny button batteries in wristwatches to large systems that can provide backup energy to municipal power grids. Some are primary cells, which are single-use and cannot be recharged. Others are secondary cells, which use reversible reactions and can be charged again by an external power source. A common primary battery is the dry cell. It uses zinc as both the container and the anode,...

corrosion

Rusting and Metal Protection

Corrosion is the natural breakdown of metals through electrochemical reactions. It can appear as rust on iron, tarnish on silver, or a blue-green patina on copper. In each case, the metal is oxidized. Some corrosion products can protect the surface, while others keep damaging the metal. Rusting is the harmful type of corrosion seen in iron. It happens when iron is exposed to oxygen and water. A galvanic cell forms on the iron surface, and this drives oxidation at the anodic region and...

electrolysis

Electrolysis in Batteries and Metal Production

Electrolysis uses electrical energy to drive a nonspontaneous redox reaction. In a galvanic cell, a spontaneous redox reaction does electrical work on the surroundings by sending electrons through an external circuit. In electrolysis, an external circuit does work on the redox system by applying a voltage large enough to force the reaction in the opposite direction. This process is used in several real-world settings. Recharging a battery is one example, because an outside power source drives...

key terms and concepts

Learn how oxidation numbers, redox changes, and the half-reaction method help balance redox equations in aqueous and alkaline solutions.

Redox Reactions and Half-Reaction Balancing | JoVE K12

chemistry

JoVE Core - Química dá vida a conceitos gerais de química usando vídeos de animação fáceis de entender. Além disso, nos vídeos Cientistas em ação, demonstramos experimentos de pesquisa clássicos e originais realizados atualmente por cientistas em laboratórios em todo o mundo.

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IPC.8

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Tennessee Academic Standards

Matter and Its Interactions

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Balancing Chemical Equations and Reaction Outcomes

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Physical Properties of Matter

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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Carry out investigations to compare physical and chemical properties of matter.

PS.PSc.1.3

The Atomic Theory of Matter

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Subatomic Particles

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The Bohr Model

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Emission Spectra

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The de Broglie Wavelength

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The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

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Ions and Ionic Charges

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Use models to compare representations of atoms, ions, and isotopes.

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The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

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Atomic Radii and Effective Nuclear Charge

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Ionic Radii

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Ionization Energy

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Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


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Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.PSc.1.6

Types of Chemical Bonds

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Covalent Bonding and Lewis Structures

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Bonding in Metals

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Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Nomenclature of Alkanes

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Nomenclature of Alkenes

The IUPAC naming system for alkenes replaces -an- with -en- in the corresponding parent alkanes. Accordingly, a simple alkene replaces the -ane suffix of ...

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Structure and Nomenclature of Ethers

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IUPAC Nomenclature of Aldehydes

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IUPAC Nomenclature of Ketones

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IUPAC Nomenclature of Carboxylic Acids

IUPAC names of carboxylic acids are systematically derived following a few rules discussed below.
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Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Redox Reactions and Half-Reaction Balancing

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