Electroplating uses electrolysis to deposit a thin layer of metal on another substance. The item to be plated is used as one electrode. Copper, silver, tin and chromium are often applied to surfaces in this way.
Electroplating is also known as electrode position. As the name suggests, the process involves depositing material using an electric current. This process results in a thin layer of metal being deposited onto the surface of a work-piece called the substrate. Electroplating is primarily used to change the physical properties of an object. This process can be used to give objects increased wear resistance, corrosion protection or aesthetic appeal, as well as increased thickness.
While electroplating may seem like advanced technology, it is actually a centuries-old process. The very first electroplating experiments occurred in the earth 18th century, and the process was officially formalized by Brugnatelli in the first half of the 19th century. After Brugnatelli’s experiments, the electroplating process was adopted and developed across Europe. As manufacturing practices advanced over the next two centuries through the Industrial Revolution and two world wars, the electroplating process also evolved to keep up with demand, resulting in the process Sharretts Plating Company uses today.
The electroplating process uses an electric current to dissolve metal and deposit it onto a surface. The process works using four primary components:
Anode: The anode, or positively charged electrode, in the circuit is the metal that will form the plating.
Cathode: The cathode in the electroplating circuit is the part that needs to be plated. It is also called the substrate. This part acts as the negatively charged electrode in the circuit.
Solution: The electrodepositing reaction takes place in an electrolytic solution. This solution contains one or more metal salts, usually including copper sulfate, to facilitate the flow of electricity.
Power source: Current is added to the circuit using a power source. This power source applies a current to the anode, introducing electricity to the system.
Once the anode and cathode are placed in solution and connected, the power supply supplies a direct current (DC) to the anode. This current causes the metal to oxidize, allowing metal atoms to dissolve in the electrolyte solution as positive ions. The current then causes the metal ions to move to the negatively charged substrate and deposit onto the piece in a thin layer of metal.
As an example, consider the process of plating gold onto metal jewelry. The gold plating metal is the anode in the circuit, while the metal jewelry is the cathode. Both are placed in solution and DC power is supplied to the gold, which dissolves in solution. The dissolved gold atoms then adhere to the surface of the base metal jewelry, creating a gold coating.
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