Electroplating is a process that uses electric current to reduce dissolved metal cations onto an electrode surface, forming a thin film. Thin films are a layer of material that range in thickness from less than one nanometer to several micrometers. These thin films are used in a wide range of applications, ranging from solar cells to biosensor probes, and provide modified surface properties with minimal change in volume. However, it is essential that the thickness of the thin film is consistent and controllable. There are many different thin film deposition techniques commonly used to controllably deposit thin films, and each has its own benefits and drawbacks. In this video, we will introduce the electroplating technique, and demonstrate how to form a thin film using this method in the laboratory.
Electroplating is performed in a set up like a galvanic cell which consists of two different metals, an anode and a cathode, connected by a salt bridge or porous membrane. These electrochemical cells have oxidation and reduction half-cell reactions that spontaneously occur at each of the metal electrodes, thereby generating electrical current. Electroplating relies on a similar concept. However, it reverses it by supplying current, thereby driving non-spontaneous redox reactions. The anode is made of the metal to be plated and is oxidized, creating dissolved ions. These ions flow through the electrolytic solution, which contains metal salts and other ions which permit the flow of electricity.
The dissolved metal ions are then reduced and plated on the cathode. The electroplating process requires that both the anode and cathode materials are conductive. Thus, metals are typically used. Plating thickness is controlled by varying the duration and strength of the electric current between the electrodes. Increasing either or both of these parameters will result in thicker plating layers. Now that you've learned the basics of electroplating, we will demonstrate the technique by plating a thin film of the dark pigment, Prussian blue, onto a sheet of polyester coded with indium tin oxide, or ITO.
To begin, prepare the Prussian blue solution. Prussian blue is a pigment produced by the oxidation of ferrocyanide salts. Mix 50 milliliters of 0.05 molar hydrochloric acid, 100 milliliters of 0.05 molar potassium hexacyanoferrate (III), and 100 milliliters of 0.05 molar iron (III) chloride hexahydrate. Now, create an anode by wrapping about eight centimeters of Nichrome wire into a tight coil. Prepare the cathode by first cutting the ITO-coated polyester into a five by five centimeter square. Then remove the outer coating that protects the conductive side of the material.
Next build the circuit by connecting the positive terminal of a nine volt battery in series with a 30 kiloohm resistor. Then connect it to the Nichrome anode using an alligator clip. Connect the negative end of the battery to the ITO cathode using an alligator clip. Make sure that the anode and cathode are not touching. Now, lower the cathode and anode into the Prussian blue solution, taking care not to submerge the alligator clips. Hold the setup in the solution for one minute. Then remove and rinse the two electrodes in deionized water. Repeat the process with new ITO electrodes, each submerged for different deposition times and battery voltages.
Now we'll analyze the various films using percent transmission of visible light in the range of 750 to 400 nanometers via UV-VIS spectroscopy. First, perform a background scan using a ITO substrate that has not been coated with Prussian blue. Then, measure the percent-transmission of the Prussian blue coated samples, subtracting the background transmittance from the blank ITO. Now compare the percent transmittance between each of the samples. First, let's take a look at the effective deposition time. These samples were deposited for 30, 60, and 240 seconds. The percent transmittance was lower for samples with longer deposition times, indicating thicker films. Similarly, films deposited at higher voltages showed lower transmittance than those deposited at lower voltages, indicating the formation of thicker films at higher voltages.
Thin films had a wide range of applications in materials engineering and other fields of research. The electroplating technique can be used to pattern micro-scale features and nano-scale thickness onto a surface. Here, researchers spin coated photoresist onto a conductive substrate. And then patterned a microscale lattice using a mesh-patterned mask using UV light. The UV-exposed patterned was then removed using developer solution to reveal a lattice pattern of trenches that reveal the conductive substrate. Copper was then electroplated onto the surface with the metal film forming only on the conductive parts of the substrate and not on the remaining photoresist.
After removal of the remaining photoresist pattern, a lattice of raised metal remained, with a thickness of less than two nanometers. Electroplating can also be used to deposit layers of biological materials on a surface, thereby improving the bio-compatibility of a sensor or probe. Here, a thin film of chitosan was electro deposited onto a patterned gold cathode. Chitosan, a polysaccharide, is soluble below pH 6.3 and insoluble above pH 6.3. Water electrolysis at the cathode induced a local increase in pH, which caused the sol-gel transition of the material, making the deposited film insoluble. This enabled its use as a bio-compatible surface for enzyme adhesion and the development of a glucose sensor.
You have just watched JoVE's introduction to the electroplating of thin films. You should now understand how the electroplating process works, how it is performed in the lab, as well as some applications of this technology. Thanks for watching.
