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

K12 Standards

north-carolina-k-12-science-standard-course-of-study

NC K-12 Science Standard Course of Study

9-12

Physical Science

Matter and its Interactions

PS.PSc.2.3

Balancing Redox Equations

Bir pil, taşınabilir cihazları çalıştırmak için nasıl elektrik sağlar? Neden kesilmiş bir avokado kahverengiye döner veya su altındaki metal paslanır? Bu süreçler, bir atomdan diğerine elektron transferini içeren belirli kimyasal reaksiyon türleri tarafından yönlendirilir.Elektron kaybeden atom oksitlenirken, elektron kazanan atom indirgenir. Bu reaksiyonlara oksidasyon indirgeme veya redoks reaksiyonları adı verilir ve bir veya daha fazla reaktan için oksidasyon durumundaki değişikliklerle karakterize edilir. Magnezyum ve konsantre hidroklorik asit arasındaki etkileşim, bir redoks reaksiyonunun bir örneğidir.Burada magnezyum magnezyum 2 iyonlarına oksitlenir ve protonlar hidrojen gazına indirgenir. Basit kimyasal denklemler kolaylıkla dengelenebilir. Bununla birlikte, çoğu redoks denklemi karmaşık olduğundan, kaybedilen ve kazanılan elektron sayısı gerekçelendirilmelidir.Redoks denklemlerini dengelerken, kütlenin korunumu yasasına uymak önemlidir. Her bir elementin miktarı ve herhangi bir elektron kazancı veya kaybı reaksiyonun her iki tarafında dengelenmelidir;bu nedenle, bir reaktan indirgenirse, diğeri oksitlenmelidir. Redoks denklemlerini başarılı bir şekilde dengelemek için yarı reaksiyonlar yöntemi kullanılır.Permanganatın oksalat ile reaksiyonunu düşünün. Sulu asidik çözeltiler için, oksidasyon durumlarını belirleyin ve reaksiyonu bileşen yarı reaksiyonlarına bölün. Ardından, hidrojen ve oksijeni atlayarak her bir yarı tepkimeyi dengeleyin.Burada manganez zaten dengelidir, ancak oksalatın iki katsayısına ihtiyacı vardır;ikinci olarak, oksijen atomlarını su molekülleri ilavesiyle dengeleyin;ve üçüncü olarak, gerektiğinde proton ekleyerek hidrojen atomlarını dengeleyin. Elektron ekleyerek yükleri dengeleyin. Manganez indirgendiğinden, reaktan tarafına beş elektron eklenir.Tersine, oksalat oksitlenir;böylece ürün tarafına iki elektron eklenir. Yarım tepkimeleri bir tamsayı ile çarpın, böylece eklenen elektron sayısı eşit olur. Son olarak, dengeli bir redoks reaksiyonu elde etmek için her iki taraftaki türleri iptal ederek dengeli yarı reaksiyonları ekleyin ve basitleştirin.Bazik sulu çözeltiler için prosedür benzerdir ancak bir ek adım içerir. Burada, dengeli yarı reaksiyonları tamamlamadan önce protonları nötralize etmek için reaksiyonun her iki tarafına eşit sayıda hidroksil iyonu eklenir.

redoks denklemlerinin dengelenmesi

Elektrokimya, elektriksel ve kimyasal reaksiyonların dönüşümünde yer alan bilimdir. Bu tür reaksiyonlara redüksiyon-oksidasyon veya redoks reaksiyonları denir. Bu önemli reaksiyonlar, bir veya daha fazla reaktan element için oksidasyon durumlarındaki değişikliklerle tanımlanır ve reaktan türleri arasında elektron transferini kapsayan bir reaksiyon alt kümesini içerir. Bir alan olarak Elektrokimya, redoks kimyasının temel ilkeleri ve endüstriyel ölçekli metalurjik işlemlerden elektrikli araçlar için sağlam, şarj edilebilir pillere kadar çeşitli teknolojiler hakkında yeterli bilgi vermek için gelişmiştir. Elektron transferini içeren reaksiyonlar Elektrokimya çalışması için gerekli olduğundan, redoks kimyasının kısa bir incelemesi aşağıdakileri içerir.
 
 Oksidasyon Numaraları
 
 Tanım olarak, bir redoks reaksiyonu, bir veya daha fazla reaktan için oksidasyon sayısında veya oksidasyon durumunda bir değişim içerir. Bir elementin oksidasyon sayısı, atomlarının elektronik ortamının saf elementin atomlarına kıyasla nasıl farklılaştığının bir değerlendirmesidir. Bu tanımla, bir elementteki bir atom, sıfır oksidasyon numarası taşır. Eğer bileşik, iyonik olsaydı, bir atom için oksidasyon sayısı bileşikteki atomun yüküne eşittir. Bu nedenle, bir moleküldeki tüm atomlar için oksidasyon sayılarının toplamı molekülün yüküne eşittir.
 
 İyonik Bileşikler
 
 Basit iyonik bileşikler, bu formalizmin en basit örnekleridir, çünkü elementler iyonik yüklerine eşit oksidasyon sayılarına sahiptir. Sodyum klorür, NaCl, Na+ katyonlarından ve Cl− anyonlarından oluşur, sodyum ve klor için oksidasyon sayıları sırasıyla +1 ve −1'dir. Kalsiyum florür, CaF2, kalsiyum ve florin, +2 ve −1 için oksidasyon numaraları ile Ca+2 katyonları ve F− anyonlarından oluşur.
 
 Kovalent Bileşikler
 
 Kovalent bileşikler formalizm kullanımında daha zordur. Su, polar kovalent O−Hbağları yoluyla bir O atomuna bağlanmış iki H atomundan oluşan kovalent bir bileşiktir. Bir O−H bağı oluşturan paylaşılan elektronlar, daha elektronegatif O atomuna daha güçlü bir şekilde çekilir. Böylece oksijen, elementel oksijendeki bir O atomuna kıyasla kısmi bir negatif yük kazanır. Sonuç olarak, bir su molekülündeki H atomları, hidrojen gazındaki hidrojen atomlarına kıyasla kısmi bir pozitif yük sergiler. Her su molekülü için kısmi negatif ve pozitif yüklerin toplamı sıfırdır, bu da su molekülünü nötr hale getirir.
 
 O−H su bağları içindeki paylaşılan elektronların polarizasyonu tamamlansaydı, sonuç elektronların H'den O'ya tamamen aktarılması ve suyun O2− anyonları ve H+ katyonlarından oluşan iyonik bir bileşik olması gerekirdi. Ve böylece, sudaki oksijen ve hidrojen için oksidasyon sayıları sırasıyla −2 ve +1'dir. Aynı mantığı karbon tetraklorür, CCl4'e uygulamak, karbon için +4 ve klor için −1 oksidasyon sayıları verir. Nitrat iyonunda, NO3−, azot için oksidasyon sayısı +5'tir ve oksijen için −2'dir, moleküldeki −1 yüküne eşittir:
 
 <img alt="Eq1" src="/files/ftp_upload/11432/11432_Equation_1.png" style="text-align: center; height: 70px;" />
 
 Redoks Denklemlerinin Dengelenmesi
 
 Aşağıda gösterilen dengesiz denklem, sodyum klorürün ayrışmasını açıklar:
 
 <img alt="Eq2" src="/files/ftp_upload/11432/11432_Equation_2.png" style="text-align: center; height: 48px;" />
 
 Bu reaksiyon, bir redoks reaksiyonu kriterine karşılık gelir, çünkü Na için oksidasyon sayısı +1'den 0'a düşer (indirgeme geçirilerek) ve Cl için −1'den 0'a yükselir (oksidasyon geçirilerek). Denklem durumu, NaCl ve Na için 2 stokiyometrik katsayısı eklenerek kolayca dengelenir:
 
 <img alt="Eq3" src="/files/ftp_upload/11432/11432_Equation_3.png" style="text-align: center; height: 48px;" />
 
 Sulu çözeltilerde meydana gelen redoks reaksiyonları elektrokimyada yaygın olarak görülür ve birçoğu reaktan veya ürün olarak su veya iyonları, H+ (aq) ve OH− (aq) içerir.
 
 Bu durumlarda, redox reaksiyonlarını temsil eden denklemler sadece dengelemek için çok zor olabilir ve yarı reaksiyon yöntemi olarak bilinen sistematik bir yaklaşımın kullanımı yardımcı olur. Bu yaklaşım aşağıdaki adımları içerir:
 <ol>
 <li>Denklemi bileşen iskelet oksidasyon ve indirgeme yarı reaksiyonlarına bölün.</li>
 <li>Her yarı reaksiyonu O ve H dışındaki tüm elementler için dengeleyin.</li>
 <li>Denklemde gerektiği gibi su molekülleri ekleyerek O atomları için her yarım reaksiyonu dengeleyin.</li>
 <li>Denklem için gerekli olan protonları ekleyerek H atomları için her yarım reaksiyonu dengeleyin.</li>
 <li>Son olarak, gerektiğinde elektron ekleyerek elementler üzerindeki yükleri dengeleyin.</li>
 <li>Yarı reaksiyonları, oksidasyon yarı reaksiyonunda kaybedilen elektron sayısını, indirgeme yarı reaksiyonunda kazanılan elektron sayısına eşitlemek için gereken herhangi bir tamsayı ile çarpın.</li>
 <li>Her iki yarı reaksiyonu da ekleyin ve denklemin her iki tarafındaki ortak türleri çıkararak daha da basitleştirin.</li>
 <li>Reaksiyon alkali bir ortamda gerçekleşirse, protonları nötralize etmek için Adım 7'de elde edilen denkleme OH iyonları ekleyin (denklemin her iki tarafına eşit sayıda eklenir) ve basitleştirin.</li>
 <li>Atomlar üzerindeki yüklerin dengelendiğinden emin olmak için denklemi kontrol edin.</li>
 </ol>
 
 Bu metin bu kaynaklardan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/17-1-review-of-redox-chemistry"">Openstax, Chemistry 2e, Chapter 17: Introduction,</a> ve <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>.

Redoks Denklemlerinin Dengelenmesi

Elektrokimya, elektriksel ve kimyasal reaksiyonların birbirine dönüştürülmesinde yer alan bilimdir. Bu tür reaksiyonlara indirgeme-oksidasyon denir veya ...

Education

JoVE Core

Chemistry

Kimya

Electrochemistry

Elektrokimya

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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

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Matter and Its Interactions

CHEM1.PS1.2

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balancing-chemical-equations-and-reaction-outcomes

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PS.PSc.1.3

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PS.PSc.1.4

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PS.PSc.1.5

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PS.PSc.1.6

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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

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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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