High Quality (and Safe) Copper Plating

Can I plate [insert your metal here] with copper?
It depends. Some metals are compatible, while others are not; the latter are referred to as "dissimilar metals." In the accompanying table borrowed from RFI, you'll find information regarding potential galvanic reactions that may lead to corrosion. This table also indicates which metals can be plated and which cannot. Generally, a lower absolute value indicates greater compatibility. If you are attempting to plate a metal that is deemed incompatible, it may require an intermediate plating of nickel or another metal. For instance, aluminum should be coated with nickel prior to copper plating. You can refer to my nickel plating guide here: link.

How do I plate non-conductive objects?
Initially, you must convert them into conductive materials. This can be achieved using conductive paints, conductive glues, or even metal leaf (such as gold leaf), assuming the coating material is not water-soluble. My personal experience with this process is limited, so I encourage you to experiment and share your findings with me for broader reference.

How much voltage/current do I need?
The goal is to use as little as possible. Lower voltage and current yield better results. At minimum, 0.5V DC is required for copper plating. A C or D cell battery can provide satisfactory results. If higher voltages are unavoidable, consider placing the electrolyte in a large container and maximizing the distance between your electrodes; as the distance increases, so will the resistance of the circuit, thereby reducing the current.

Can I use copper chloride or another electrolyte instead of making it with vinegar?
Yes, you can. I prefer to create my own chemicals, but you can find root kill (which comes in green crystals) at a local hardware store for a reasonable price.

Can I use other acids instead of acetic acid (vinegar)?
Yes, but caution is advised. This instruction is directed towards non-chemists, and other acids can be significantly more hazardous, potentially releasing toxic chemicals into the environment. Unless you hold a formal chemistry degree, I advise against experimenting with other chemicals.

Is plating coins illegal?
I want to clarify that my use of coins is solely for their universal availability and cost-effectiveness for small experiments. The copper and nickel content makes them suitable for such undertakings. This is not a dedicated "how to plate coins" guide; rather, coins serve as convenient and recognizable materials for experimentation.

From my understanding, it is legal to plate coins as long as you: 1) Do not remove metal with the intent to sell it, 2) Do not attempt to pass them off as something other than their original value (for instance, a copper plated dime remains worth 10 cents), and 3) Do not deface the coins maliciously. However, keep in mind that this understanding is personal; verify this information with a reliable source to confirm accuracy.

Why are you using a 6V lantern battery when citing that lower voltages are better?
The quality of plating between 0.5V DC and 6V DC is relatively similar; however, the plating time is significantly reduced with 6V DC. If you prefer lower voltages, you can achieve this by widening the distance between your anode and cathode, as the electrolyte acts as a variable resistor, creating more resistance. Good lantern batteries maintain their effectiveness for considerable time due to their parallel internal connections, providing consistent results despite usage.

Can I plate Aluminum?
I would advise against it. Aluminum is one of those metals that does not plate well. Instead, for a corrosion-resistant finish on aluminum, consider anodizing to create a robust clear oxide layer. If you desire a colored finish, there are dyes available that can stain the oxide layer, similar to techniques used by companies like Apple for their iPods.

Can I use copper plating to prevent steel parts from rusting?
No, absolutely not. Several issues arise with this approach: 1) Copper can develop a patina (essentially rust) which may peel away, exposing the base metal underneath to corrosion, and 2) When copper interacts with iron in steel and is immersed in water, it catalyzes rusting in steel parts. An experiment involving a copper piece in saltwater with steel will quickly demonstrate this accelerated rusting.

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