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

배터리가 휴대용 장치를 작동하기 위한 전기를 어떻게 제공할까요? 왜 잘린 아보카도는 갈색으로 변하거나 물속에서 금속이 녹이 슬까요? 이러한 과정은 한 원자에서 다른 원자로의 전자 전달과 관련된 특정 유형의 화학 반응에 의해 구동됩니다.

전자를 잃은 원자는 산화되며 전자를 얻는 원자는 환원됩니다. 이러한 반응을 산화 환원 반응이라고 하며 하나 이상의 반응물에서의 산화 상태의 변화로 특징지어집니다. 마그네슘과 농축 염산 사이의 상호작용은 산화환원반응의 가지 예입니다.

이 반응에서 마그네슘은 마그네슘 2 이온으로 산화되고 양성자는 수소 기체로 환원됩니다. 간단한 화학 방정식은 쉽게 균형을 이룰 수 있습니다. 그러나 대부분의 산화환원 방정식은 복잡하므로 손실되고 얻은 전자 수가 해명되어야 합니다.

산화환원 방정식의 균형을 맞출 때 질량 보존 법칙을 준수하는 것이 중요합니다. 각 원소의 양과 전자의 손익은 반응의 양쪽에서 균형을 이루어야 합니다. 따라서 한 반응 물질이 환원하면 다른 반응 물질은 산화되어야 합니다.

산화환원 방정식의 균형을 성공적으로 맞추기 위해 반반응 방법을 사용합니다. 과망간산염과 수산염의 반응을 생각해보세요. 수용성 산성 용액의 경우 산화 상태를 할당하고 반응을 성분 반반응으로 나눕니다.

그리고 나서 수소와 산소를 제외한 각각의 반반응의 균형을 맞춥니다. 여기서, 망간은 이미 균형을 이루었지만 수산염은 계수 2가 있어야 합니다. 산소 원자와 물 분자에 대한 추가적인 균형을 맞춥니다.

셋째, 필요한 곳에 양성자를 추가함으로써 수소 원자의 균형을 이룹니다. 전자를 추가하여 전하의 균형을 맞춥니다. 망간은 환원되었기 때문에 5개의 전자가 반응물 쪽에 추가됩니다.

반대로 수산염은 산화되기 때문에 생성물 측에 두 개의 전자가 추가됩니다. 반반응에 정수를 곱하여 추가된 전자 수가 같도록 합니다. 마지막으로 균형잡힌 산화환원 반응을 얻기 위해 양쪽의 종을 취소함으로써 균형잡힌 반반응을 추가하고 단순화합니다.

염기 수용성 용액의 경우 절차는 유사하지만 한 가지 추가 단계가 포함됩니다. 여기서, 균형의 반반응을 가중하기 전에 양성자를 중화시키기 위해 반응의 양쪽에 같은 수의 수산기 이온을 첨가합니다.

산화환원 방정식의 균형 맞추기

전기화학은 전기 반응과 화학 반응의 상호 변환과 관련된 과학입니다. 이러한 반응을 환원-산화 또는 산화환원 반응이라고 합니다. 이러한 중요한 반응은 하나 이상의 반응물 요소에 대한 산화 상태의 변화로 정의되며 반응물 종 간의 전자 이동과 관련된 반응의 하위 집합을 포함합니다. 한 분야로서의 전기화학은 산화환원 화학의 기본 원리와 산업 규모의 야금 공정부터 전기 자동차용 견고한 충전식 배터리에 이르는 다양한 기술에 대한 충분한 통찰력을 제공하도록 발전했습니다. 전자 이동과 관련된 반응은 전기화학 연구에 필수적이므로 산화환원 화학에 대한 간략한 검토에는 다음이 포함됩니다.

산화수

정의에 따르면, 산화환원 반응은 하나 또는 여러 반응물에 대한 산화수 또는 산화 상태의 변화를 수반합니다. 원소의 산화수는 원자의 전자 환경이 순수 원소의 원자와 어떻게 다른지를 평가한 것입니다. 이 정의에 따르면 원소의 원자는 산화수 0을 갖습니다. 원자의 경우 산화수는 화합물이 이온성인 경우 화합물의 원자 전하와 같습니다. 따라서 분자 내의 모든 원자에 대한 산화수의 합은 분자의 전하와 같습니다.

이온 화합물

단순한 이온 화합물은 원소의 이온 전하와 동일한 산화수를 갖기 때문에 이러한 형식주의의 가장 간단한 예입니다. 염화나트륨(NaCl)은 Na^+ 양이온과 Cl^- 음이온으로 구성되며, 나트륨과 염소의 산화수는 각각 +1과 -1입니다. 불화칼슘(CaF_2)은 Ca^2+ 양이온과 F^- 음이온으로 구성되며, 칼슘과 불소의 산화수는 +2와 -1입니다.

공유결합 화합물

공유 화합물은 형식주의를 사용하는 것이 더 어렵습니다. 물은 극성 공유 O−H 결합을 통해 O 원자에 결합된 두 개의 H 원자로 구성된 공유 결합 화합물입니다. O-H 결합을 만드는 공유 전자는 전기 음성도가 더 높은 O 원자에 더 강하게 끌립니다. 따라서 산소는 원소 산소의 O 원자와 비교하여 부분적인 음전하를 얻습니다. 결과적으로 물 분자의 H 원자는 수소 가스의 수소 원자에 비해 부분적인 양전하를 나타냅니다. 각 물 분자의 부분적인 음전하와 양전하의 합은 0이므로 물 분자는 중성이 됩니다.

물의 O-H 결합 내에서 공유 전자의 분극이 완료되면 그 결과 전자가 H에서 O로 완전히 이동하게 되며 물은 O_2^- 음이온과 H^+ 양이온으로 구성된 이온 화합물이 됩니다. 따라서 물 속의 산소와 수소의 산화수는 각각 -2와 +1입니다. 이 동일한 논리를 사염화탄소(CCl_4)에 적용하면 탄소의 경우 +4, 염소의 경우 -1의 산화수가 생성됩니다. 질산염 이온 NO_3^−에서 질소의 산화수는 +5이고 산소의 산화수는 -2입니다. 합하면 분자의 -1 전하와 같습니다.

<img alt="Eq1" src="/files/ftp_upload/11432/11432_Equation_1.png" style="text-align: center; height: 70px;" />

산화환원 방정식의 균형 맞추기

아래 표시된 불균형 방정식은 염화나트륨의 분해를 설명합니다.

<img alt="Eq2" src="/files/ftp_upload/11432/11432_Equation_2.png" style="text-align: center; height: 48px;" />

이 반응은 Na의 산화수가 +1에서 0(환원을 통해)으로 감소하고 Cl의 산화수가 -1에서 0(산화를 통해)으로 증가하므로 산화환원 반응의 기준과 일치합니다. 방정식 사례는 NaCl 및 Na에 대해 화학양론적 계수 2를 추가하여 쉽게 균형을 이룹니다.

<img alt="Eq3" src="/files/ftp_upload/11432/11432_Equation_3.png" style="text-align: center; height: 48px;" />

수용액에서 발생하는 산화환원 반응은 전기화학에서 흔히 볼 수 있으며, 많은 경우 물이나 그 이온, H^+(aq) 및 OH^−(aq)가 반응물 또는 생성물로 포함됩니다.

이러한 경우, 산화환원 반응을 나타내는 방정식은 검사만으로 균형을 맞추는 것이 매우 어려울 수 있으며 반쪽 반응 방법으로 알려진 체계적인 접근 방식을 사용하는 것이 도움이 됩니다. 이 접근 방식에는 다음 단계가 포함됩니다.

<ol>
	<li>방정식을 구성 요소인 골격 산화 및 환원 반쪽 반응으로 나눕니다.</li>
	<li>O와 H를 제외한 모든 원소에 대해 각 반쪽 반응의 균형을 맞춥니다.</li>
	<li>방정식에 필요에 따라 물 분자를 추가하여 O 원자에 대한 각 반쪽 반응의 균형을 맞춥니다.</li>
	<li>방정식에 필요한 대로 양성자를 추가하여 H 원자에 대한 각 반쪽 반응의 균형을 맞춥니다.</li>
	<li>마지막으로 필요에 따라 전자를 추가하여 원소의 전하 균형을 맞춥니다.</li>
	<li>산화 반쪽 반응에서 손실된 전자 수와 환원 반쪽 반응에서 얻은 전자 수를 동일하게 만드는 데 필요한 정수를 반쪽 반응에 곱합니다.</li>
	<li>두 반쪽 반응을 모두 추가하고 방정식의 양쪽에서 공통 종을 제거하여 더욱 단순화합니다.</li>
	<li>반응이 알칼리성 매질에서 발생하는 경우 7단계에서 얻은 식에 OH- 이온을 추가하여 양성자를 중화하고(식의 양쪽에 동일한 수로 추가) 단순화합니다.</li>
	<li>원자의 전하가 균형을 이루고 있는지 방정식을 확인합니다.</li>
</ol>

이 문서는 에서 발췌되었습니다  <a href="https://openstax.org/books/chemistry-2e/pages/17-1-review-of-redox-chemistry">Openstax, Chemistry 2e, Chapter 17: Introduction,</a> and <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>.

전기 화학은 전기 및 화학 반응의 상호 변환과 관련된 과학입니다. 이러한 반응을 환원-산화 또는 ...

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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...

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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...

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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...

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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...

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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...

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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...

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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,...

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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

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PS.PSc.1.2

physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

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

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

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

PS.PSc.1.3

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

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.

PS.PSc.1.4

Ions and Ionic Charges

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

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

PS.PSc.1.5

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 ...

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

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


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

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

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

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

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

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 ...

Nomenclature of Alkynes

Alkynes are unsaturated hydrocarbons characterized by the presence of carbon-carbon triple bonds and have a general formula CnH2n-2. The nomenclature of ...

structure-and-nomenclature-of-alcohols-and-phenols

Structure and Nomenclature of Alcohols and Phenols

Overview 
Alcohols are one of the most important functional groups in organic chemistry. The name of alcohol comes from the hydrocarbon from which it is ...

Structure and Nomenclature of Ethers

Structure and Bonding
Ethers are organic compounds with an ether functional group which is characterized by an oxygen atom connected to two &#8212; ...

IUPAC Nomenclature of Aldehydes

Aldehydes are named based on the systematic nomenclature rules set by the IUPAC. For acyclic aldehydes, the longest carbon chain containing the aldehydic ...

IUPAC Nomenclature of Ketones

Like aldehydes, ketones are named using IUPAC rules; in this case, by replacing &#8220;e&#8221; in the name of the longest hydrocarbon chain with ...

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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