Name: electroplating with electrolytic cells
Uploaded: 2020-03-26T07:22:26.000Z
Duration: 2 min 52 s
Channel: JoVE

电化学反应对技术和人体的许多过程至关重要，涉及电子从一种化学物质转移到另一种化学物质。这些反应称为还原-氧化反应或氧化还原反应。
当一个物种失去电子时，它会发生氧化，我们说它被氧化了。当一个物质获得电子时，它就经历了还原，我们说它被还原了。在电化学原电池中，氧化还原反应自发发生，从而产生电能。然而，在电解槽中，施加了电能，这会导致氧化还原反应的发生。
电解槽由称为电解质的反应溶液组成，其中包含任何被氧化或还原的化学物质以及实现电子流动所需的离子。电解槽有两个浸入电解液中的金属电极。外部电路连接两个电极，从而完成电路并使我们能够施加电压或电流。
施加的电流或电压是导致发生电化学反应的原因。氧化半反应发生在阳极，还原半反应发生在阴极。为了帮助您区分两者，请记住短语"红猫"，它代表"阴极还原"。
但是我们如何确定哪个电极是哪个呢？我们可以使用金属电极的标准还原电位，这是衡量金属失去电子趋势的指标。还原电位越高，金属被还原的可能性就越大。
假设我们将一个银电极和一个铜电极放入电解槽中并施加电流。银电极具有较高的还原电位，因此它被还原并充当阴极。铜电极具有较低的还原电位，因此它被氧化并充当阳极。
电解槽的一种用途是进行电镀，这是一种金属被氧化然后还原到另一种金属表面的反应。由于阳极是进行电镀的金属，因此在我们的银和铜示例中，银电极上镀有一层薄薄的铜。
在本实验中，您将组装电解槽，并通过在黄铜键上镀铜来执行电镀过程。

电解槽

电化学
电化学是化学的一个分支，用于描述和测量电能与化学变化之间的关系。电化学反应涉及电子从一种物质到另一种物质的运动。如果反应是自发的，则会产生电流。如果反应不是自发的，则可以通过施加电流来驱动。
在电化学中，关键反应是氧化还原反应，称为氧化还原反应。氧化还原反应由两个半反应组成;氧化，称为还原剂的物质失去电子，还原，称为氧化剂的物质获得电子。氧化还原反应总是成对发生，并改变相关分子中原子的氧化态。记住这种关系的一种简单方法是通过气动 OIL-RIG: Oxidation Is Losing – Reduction Is Gaining。
<h4>电化学电池</h4>
电化学池用于测量或诱导电化学反应。它由几个组件组成:一个包含反应溶液的腔室、两个导电电极、一个导电电解质溶液和一个外部电路。电化学电池有两种类型。一种是电解槽，它使用电能来驱动非自发反应。在这种类型的电池中，电能由外部电源提供。
另一种类型的电池是原电池，它使用自发的电化学反应来产生电能。这两个电极称为阳极和阴极，它们通过外部电路连接。反应室充满电解质，可促进离子在电极之间通过。在原电池中，盐桥允许离子在包含电极的电解液之间流动，从而完成电路。在电解池中，没有盐桥，因为电极通常位于相同的电解溶液中。
还原反应发生在阴极，而氧化反应发生在阳极。这是使用助记词"Red Cat"来记住的，这意味着 reduction 发生在 cathode。
<h4>电解槽</h4>
电解槽通常有一个反应室，其中包含电解质溶液。电解质通常是含有离子或溶解盐的水溶液。电解质中的离子促进离子和电子在溶液中的运动。
当施加外部电压时，电解质中的离子被吸引到带相反电荷的电极上。这是两个半反应发生的地方。阳极在氧化过程中失去电子，而阴极在还原过程中获得电子。
电镀是一种利用电解槽的工艺。电镀是将一种金属沉积在电极表面（通常是另一种金属）的过程。英国科学家迈克尔·法拉第（法拉第常数就是以他的名字命名的）证明了电镀带电离子和电流之间的摩尔关系。看看银的特定半反应:
Ag+ + 1e- → Ag
需要一摩尔电子，由外部电流提供，才能将一摩尔银阳离子还原成固体银。因此，半反应化学计量法可以确定用于已知电子量的电镀材料的量。回想一下，电不是根据电子的摩尔数来测量的，而是以库仑为单位的，库仑以法国工程师查尔斯-奥古斯丁·德·库仑 （Charles-Augustin de Coulomb） 的名字命名。一库仑是在 1 秒间隔内以 1 安培电流通过电路的电量，这是基于基本电荷的原理，或单个电子携带的电荷。因此，法拉第的发现可以将电流与电镀阳离子镀层的摩尔数联系起来:
F = eNA
F 是法拉第常数，e 是以库仑表示的基本电荷，NA 是阿伏加德罗数。因此，法拉第常数表示为每摩尔的库仑数，值为 96485 库仑/摩尔。我们如何根据电流确定转移到阳极的电子摩尔数？使用电荷 Q 和库仑的定义:
<img src="/CDNSource/lm/labs/53/53_Concepts_3.jpg">
电荷等于以安培 （I） 为单位的电流乘以允许电流流动的时间（以秒为单位）。通过将 Q 除以法拉第常数，法拉第常数的单位为每摩尔的库仑:
<img src="/CDNSource/lm/labs/53/53_Concepts_4.jpg">
这个方程允许我们计算电子的摩尔数，从而确定电镀阳离子的还原量。
在电镀中，金属由阳极板或覆盖物组成，阴极位于一层薄金属中。镀金属的量取决于施加的电流量以及可用的电镀阳离子的摩尔数。外部电源（如电池）感应电子从阳极流向阴极，以及从电池的正极流向负极。
例如，考虑一个带有铜电极的电解槽，黄铜键作为第二个电极，硫酸铜水溶液作为电解质。在这里，电解液中的铜和铜电极被电镀到黄铜键上。
为了使铜金属沉积在黄铜键上，固体铜电极必须被氧化以形成铜离子。然后，电极和电解液中的铜阳离子从溶液中还原出来，在黄铜键上形成固体铜。
Cu2+ + 2e- → Cu（s）
反应的电子从电池的负极端子接收。因此，还原反应发生在黄铜键处，而氧化反应发生在铜电极处。浓缩和酸化的硫酸铜溶液增加溶解度;因此，溶液浓度越高，电阻越低，电流越高。反过来，更高的电流允许更多的铜离子电镀到黄铜键上。
一些金属比其他金属更容易失去电子。物质的标准电极电位 （E°） 是物质失去电子趋势的量度。还原电位最高的金属失去电子的倾向最高;因此，它首先被电镀。
<h4>引用</h4>
<ol>
	<li style="font-size:17px">Kotz， J.C.， Treichel Jr， P.M.， Townsend， J.R. （2012）.化学和化学反应性。加利福尼亚州贝尔蒙特:Brooks/Cole，圣智学习。</li>
	<li style="font-size:17px">Silberberg， M.S. （2009）.化学:物质和变化的分子性质。马萨诸塞州波士顿:麦格劳·希尔。</li>
</ol>

电化学
电化学是化学的一个分支，用于描述和测量电能与化学变化之间的关系。...

Education

教育

JoVE Lab Manual

Chemistry

化学

Electrolytic Cells

electroplating with electrolytic cells

Electrochemistry links electrical energy with chemical change, and electrolytic cells show how electricity can drive a nonspontaneous reaction. In these reactions, electrons move from one species to another. The key chemistry is a redox reaction, or oxidation-reduction reaction, which happens in two half-reactions.

Oxidation is the loss of electrons, and reduction is the gain of electrons. The substance that loses electrons is the reducing agent, and the substance that gains electrons is the oxidizing agent. Redox reactions always occur in pairs and change the oxidation state of the atoms involved. A simple memory aid is OIL-RIG: oxidation is losing, reduction is gaining.

An electrochemical cell is used to measure or cause electrochemical reactions. It includes a reaction chamber, two conductive electrodes, a conductive electrolyte, and an external circuit. The two main types are electrolytic cells and galvanic cells. An electrolytic cell uses outside electrical energy to drive a nonspontaneous reaction, while a galvanic cell uses a spontaneous reaction to produce electrical energy. The electrodes are the anode and cathode, and the reaction at the cathode is reduction while the reaction at the anode is oxidation. This is often remembered with “Red Cat,” which means reduction occurs at the cathode.

Electrolytic cells usually have one reaction chamber filled with an electrolyte solution. The electrolyte is often an aqueous solution with ions or dissolved salts. These ions help charge move through the solution. When voltage is applied, ions move toward the electrode with the opposite charge, and the two half-reactions occur there. The anode loses electrons during oxidation, and the cathode gains electrons during reduction.

A major use of an electrolytic cell is electroplating. In electroplating, one metal is deposited as a thin layer on the surface of another electrode. Michael Faraday showed the link between the charge of the ions being plated and the electrical current. For silver, the half-reaction is Ag+ + 1e- -&gt; Ag, so one mole of electrons reduces one mole of silver cations to solid silver. This means half-reaction stoichiometry can be used to calculate how much plating occurs for a known amount of charge.

Electricity is measured in coulombs, not in moles of electrons. One coulomb is the amount of electricity that passes through a circuit with 1 ampere of current in 1 second. Faraday’s constant connects these ideas. It is equal to the elementary charge times Avogadro’s number, and it has a value of 96485 coulombs per mole. The electrical charge is found by multiplying current, I, by time in seconds, and dividing Q by Faraday’s constant gives the moles of electrons transferred.

This relationship shows how current controls electroplating. The amount of metal plated depends on the current applied and on how much electroplating cation is available. An external power source, such as a battery, pushes electrons from the anode to the cathode and from the positive terminal to the negative terminal on the battery. In a copper plating example, a copper electrode, a brass key, and aqueous copper sulfate are used. Copper from the electrode and from the solution is deposited onto the brass key.

For copper to coat the key, the solid copper electrode must first be oxidized to copper ions. Then copper cations in the solution are reduced to solid copper on the brass key, following Cu2+ + 2e- -&gt; Cu(s). The electrons come from the negative terminal of the battery. So the brass key is the site of reduction, and the copper electrode is the site of oxidation. A concentrated and acidified copper sulfate solution increases solubility, lowers resistance, and raises the current, which allows more copper to plate onto the key.

Some metals lose electrons more easily than others. The standard electrode potential, E°, measures a substance’s tendency to lose electrons. In electroplating, the metal with the highest reduction potential has the highest tendency to lose electrons, so it is plated first.

Electroplating with Electrolytic Cells

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Oxidation States in Redox Reactions

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Solubility in Water and Other Solvents

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metal flame emission

Flame Test Metal Color Clues

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balmer series

Hydrogen Emission Lines

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Absorbance Spectra and Beer-Lambert Analysis

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Reaction Order and Rate Constants

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Reaction Rate, Arrhenius, and Catalysts

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galvanic cells

Battery Power from Redox Reactions

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electrolytic cells

Electrochemistry links electrical energy with chemical change, and electrolytic cells show how electricity can drive a nonspontaneous reaction. In these reactions, electrons move from one species to another. The key chemistry is a redox reaction, or oxidation-reduction reaction, which happens in two half-reactions. Oxidation is the loss of electrons, and reduction is the gain of electrons. The substance that loses electrons is the reducing agent, and the substance that gains electrons is the...

proper lab notebook keeping

Recording a Reproducible Lab Experiment

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basic organic chemistry techniques

Organic Lab Glassware and Safe Handling

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melting points

How Impurities Change Melting Points

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boiling points

Boiling Point and Vapor Pressure

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recrystallization

Purifying Crystals by Solubility

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extraction

Separating Mixtures with Solvent Extraction

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simple distillation

Separating Liquids by Boiling Point

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steam distillation

Steam Distillation and Low-Boiling Separation

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thin-layer chromatography

TLC Separation by Polarity

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column chromatography

Separating Mixtures by Polarity

Column chromatography separates compounds in an organic chemistry lab by using differences in physical properties. It is especially useful for microscale separations when less than 10 grams of material is available for analysis. The method can separate a mixture based on solubility, polarity, hydrophobicity, size, and charge. Any chromatography system has three main parts: the stationary phase, the mobile phase, and the sample mixture. In column chromatography, the stationary phase is usually...

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Soap Formation from Triglycerides

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Luminol Chemiluminescence in Forensics

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Ester Formation and Everyday Fragrances

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identification of unknown aldehydes and ketones

identification-of-unknown-aldehydes-and-ketones

Carbonyl Tests for Aldehydes and Ketones

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chemistry

Comprehensive, curriculum-focused videos for both instructors and students in introductory chemistry lab courses.

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Learn how electrolytic cells drive electroplating, move electrons through redox reactions, and use Faraday’s constant to calculate plated metal.

Electroplating with Electrolytic Cells | JoVE K12

通过这段 3 分钟的教师指南，准备教授 电解槽。涵盖 JoVE Lab Manual 上 Chemistry 实验的关键准备步骤。

Chemistry 中的 电解槽 教师准备 - 2.2K+ 观看次数 | JoVE Lab Manual

在这段 9 分钟的学生实验流程视频中，逐步学习 电解槽 的操作步骤。属于 JoVE Lab Manual 上的 Chemistry 系列。

Chemistry 中的 电解槽 学生实验流程 - 12K+ 观看次数 | JoVE Lab Manual

Electroplating with Electrolytic Cells

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