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

Electrochemical reactions are vital to many processes in technology and the human body and involve the transfer of electrons from one chemical species to another. These reactions are called reduction-oxidation reactions or redox reactions.
When a species loses electrons, it undergoes oxidation, and we say that it is oxidized. When a species gains electrons, it has undergone reduction, and we say that it is reduced. In an electrochemical galvanic cell, redox reactions occur spontaneously, which generate electrical energy. However, in an electrolytic cell, electrical energy is applied, which causes the redox reactions to occur.
An electrolytic cell consists of the reaction solution called the electrolyte, which contains any chemical species that are oxidized or reduced as well as ions needed to enable electron flow. The electrolytic cell has two metal electrodes that are immersed in the electrolytic solution. An external circuit connects the two electrodes, which completes the circuit and enables us to apply voltage or current.
The applied current or voltage is what causes the electrochemical reaction to take place. The oxidation half-reaction occurs at the anode, and the reduction half-reaction occurs at the cathode. To help you differentiate between the two, remember the phrase &#39;red cat,&#39; which stands for &#39;reduction at cathode&#39;.
But how do we determine which electrode is which? We can use the standard reduction potential of the metal electrodes, which is a measure of the metal&#39;s tendency to lose electrons. The higher the reduction potential, the more likely it is for the metal to be reduced.
Let&#39;s say we place a silver electrode and a copper electrode in an electrolytic cell and apply current. The silver electrode has a higher reduction potential, so it is reduced and acts as the cathode. The copper electrode has a lower reduction potential, so it is oxidized and acts as the anode.
One use of electrolytic cells is to perform electroplating, which is a reaction where one metal is oxidized and then reduced onto the surface of another metal. Since the anode is the metal doing the plating, in our example of silver and copper, the silver electrode is plated with a thin layer of copper.
In this lab, you&#39;ll assemble an electrolytic cell and perform the electroplating process by plating a brass key with copper.

electrolytic cells

Electrochemistry
Electrochemistry is a branch of chemistry that describes and measures the relationship between electrical energy and a chemical change. Electrochemical reactions involve the movement of electrons from one species to another. If the reaction is spontaneous, it can result in a generated current. If the reaction is not spontaneous, it can be driven by the application of current.
In electrochemistry, the key reaction is the oxidation-reduction reaction, called a redox reaction. The redox reaction is composed of two half-reactions; oxidation, where a substance known as the reducing agent loses electrons, and reduction, where a substance known as the oxidizing agent gains electrons. Redox reactions always occur in pairs and change the oxidation states of the atoms in the molecules involved. An easy way to remember this relationship is through the pneumatic OIL-RIG: Oxidation Is Losing &#8211; Reduction Is Gaining.
<h4>Electrochemical Cells</h4>
An electrochemical cell is used to measure or induce electrochemical reactions. It consists of several components: a chamber containing the reaction solution, two conductive electrodes, a conductive electrolyte solution, and an external circuit. There are two types of electrochemical cells. One is the electrolytic cell, which uses electrical energy to drive a nonspontaneous reaction. In this type of cell, electrical energy is supplied from an external power source.
The other type of cell is the galvanic cell, which uses a spontaneous electrochemical reaction to generate electrical energy. The two electrodes are called the anode and cathode, and they are connected by an external circuit. The reaction chamber is filled with an electrolyte, which promotes the passage of ions between electrodes. In a galvanic cell, a salt bridge completes the circuit by allowing the flow of ions between the electrolytic solutions containing the electrodes. In an electrolytic cell, there is no salt bridge as the electrodes are typically in the same electrolytic solution.
The reduction reaction occurs at the cathode, while the oxidation reaction occurs at the anode. This is remembered using the mnemonic &#8220;Red Cat,&#8221; which means that reduction occurs at the cathode.
<h4>Electrolytic Cells</h4>
Electrolytic cells typically have one reaction chamber, which contains the electrolyte solution. The electrolyte is usually an aqueous solution containing ions or dissolved salts. The ions in the electrolyte promote the movement of ions and electrons through the solution.
When an external voltage is applied, ions in the electrolyte are attracted to the electrode with the opposite charge. This is where the two half-reactions occur. The anode loses electrons during oxidation, while the cathode gains electrons during reduction.
Electroplating is a process that utilizes an electrolytic cell. Electroplating is a process in which one metal is deposited on the surface of an electrode, typically another metal. British scientist Michael Faraday, for whom the Faraday constant is named after, demonstrated the molar relationship between the electroplating charged ion and the electrical current. Looking at the specific half-reaction for silver:
Ag+ + 1e- &#8594; Ag
It takes one mole of electrons, supplied by an external current, to reduce one mole of silver cations into solid silver. Therefore, half-reaction stoichiometry can determine the amount of the electroplating material utilized for a known quantity of electrons. Recall that electricity is not measured based on the moles of electrons but rather in coulombs, named after the French engineer Charles-Augustin de Coulomb. One coulomb is the quantity of electricity passing through an electrical circuit with 1 ampere of current over a 1-second intervale, which is based on the principle of elementary charge, or the charge a single electron carries. Faraday&#8217;s discovery can therefore relate electrical current to the number of moles the electroplating cation plated:
F = eNA
F is the Faraday constant, e is the elementary charge expressed in coulombs, and NA is Avogadro&#8217;s number. Therefore, Faraday&#8217;s constant is expressed as the number of coulombs per mole and has a value of 96485 coulombs per mole. How can we determine the number of moles of electrons transferred to the anode based on the current? Using the electrical charge Q and the definition of a coulomb:
<img src="/CDNSource/lm/labs/53/53_Concepts_3.jpg" alt="Electrical formula: Q=I&#215;t, charge calculation equation, physics educational content." data-altupdatedat="1761830439000" />
The electrical charge is equal to the current in amps (I) multiplied by the time in seconds that the current was allowed to flow. By dividing Q by the Faraday constant, which has the units of coulombs per mole:
<img src="/CDNSource/lm/labs/53/53_Concepts_4.jpg" alt="Electrochemical equation, mole calculation: moles of electrons = Q/F, formula representation." data-altupdatedat="1761830439000" />
This equation allows us to calculate the number of moles of electrons and thus determine how much of the electroplating cation was reduced.
In electroplating, the metal comprises the anode plates, or covers, the cathode in a thin layer of metal. The amount of metal plated is dependent on the amount of current applied as well as the number of moles of the electroplating cation available. An external power source, such as a battery, induces the flow of electrons from the anode to the cathode, and from the positive terminal to the negative terminal on the battery.
For example, consider an electrolytic cell with a copper electrode, a brass key acting as the second electrode, and an aqueous solution of copper sulfate as the electrolyte. Here, copper from the electrolyte and the copper electrode is plated onto the brass key.
For the copper metal to be deposited on the brass key, the solid copper electrode must be oxidized to form copper ions. Then, the copper cations from both the electrode and electrolyte are reduced from the solution to form solid copper on the brass key.
Cu2+ + 2e- &#8594; Cu(s)
The electrons for the reaction are received from the negative terminal of the battery. Thus, the reduction reaction occurs at the brass key, while the oxidation reaction occurs at the copper electrode. The concentrated and acidified copper sulfate solution increases solubility; therefore, the higher the concentration of the solution, the lower the resistance and the higher the current. In turn, a higher current allows more plating of the copper ions onto the brass key to occur.
Some metals have a greater tendency than others to lose electrons. The standard electrode potential (E&#176;) of a substance is the measure of the tendency of a substance to lose electrons. The metal with the highest reduction potential has the highest tendency to lose electrons; thus, it is electroplated first.
<h4>References</h4>
<ol>
	<li style="font-size:17px">Kotz, J.C., Treichel Jr, P.M., Townsend, J.R. (2012). Chemistry and Chemical Reactivity. Belmont, CA: Brooks/Cole, Cengage Learning.</li>
	<li style="font-size:17px">Silberberg, M.S. (2009). Chemistry: The Molecular Nature of Matter and Change. Boston, MA: McGraw Hill.</li>
</ol>

Electrolytic Cells

Electrochemistry
Electrochemistry is a branch of chemistry that describes and measures the relationship between electrical energy and a chemical change. ...

Education

JoVE Lab Manual

Chemistry

Scheikunde

Elektrolytische cellen

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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Electroplating with Electrolytic Cells

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