Galvanic Corrosion

Galvanic Corrosion Is a Chemical Process That Is Well Understood

Close-up of a rusty pipe, New York City, New York State, USA
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Over 200 years ago, the British naval frigate Alarm lost its copper sheeting due to the rapid corrosion of the iron nails used to fasten the copper to the hull. This rapid corrosion occurred because of a chemical process called galvanic corrosion.

Galvanic corrosion can only occur when two electrochemically different metals are close to one another and also submerged in an electrolytic liquid (such as salt water).

When this occurs, the metals and the electrolyte create a galvanic cell. The cell has the effect of corroding one metal at the expense of the other.

In the case of the Alarm, the iron was corroded at the expense of the copper. Just two years after attaching the copper sheets, the iron nails that were used to hold the copper to the ship's underside were already severely corroded, causing the copper sheets to fall off.

How Galvanic Corrosion Works

Metals and metal alloys all possess different electrode potentials. Electrode potentials are a relative measure of a metal's tendency to become active in a given electrolyte. The more active, or less noble, a metal is the more likely it is is to form an anode (positively charged electrode) in an electrolytic environment. The less active, or nobler a metal is, the more likely it is to form a cathode (negatively charged electrode) when in the same environment.

The electrolyte acts as a conduit for ion migration, moving metal ions from the anode to the cathode. The anode metal, as a result, corrodes more quickly than it otherwise would, while the cathode metal corrodes more slowly and, in some cases, may not corrode at all.

In the case of Alarm, the metal of greater nobility (copper) acted as a cathode, while the lesser noble iron acted as an anode.

Iron ions were lost at the expense of the copper, ultimately resulting in the rapid deterioration of the nails.

How to Protect Against Galvanic Corrosion

With our current understanding of galvanic corrosion, metal-hulled ships are now fitted with 'sacrificial anodes', which play no direct role in the ship's operation, but serve to protect the structural components of the vessel. Sacrificial anodes are often made of zinc and magnesium, metals with very low electrode potentials. As sacrificial anodes corrode and deteriorate they must be replaced.

In order to understand what metal will become an anode and which will act as a cathode in electrolytic environments, we must understand the metals' nobility or electrode potential. This is generally measured with respect to the Standard Calomel Electrode (S.C.E.).

A list of metals, arranged according to electrode potential (nobility) in flowing seawater can be seen in the table below.

It should also be pointed out that galvanic corrosion does not only occur in water. Galvanic cells can form in any electrolyte, including moist air or soil, and chemical environments.

Galvanic Series In Flowing Sea Water

Steady State ElectrodeMaterial Potential, Volts
(Saturated Calomel Half-Cell)
Graphite+0.25
Platinum+0.15
Zirconium-0.04
Type 316 Stainless Steel (Passive)-0.05
Type 304 Stainless Steel (Passive)-0.08
Monel 400-0.08
Hastelloy C-0.08
Titanium-0.1
Silver-0.13
Type 410 Stainless Steel (Passive)-0.15
Type 316 Stainless Steel (Active)-0.18
Nickel-0.2
Type 430 Stainless Steel (Passive)-0.22
Copper Alloy 715 (70-30 Cupro-Nickel)-0.25
Copper Alloy 706 (90-10 Cupro-Nickel)-0.28
Copper Alloy 443 (Admiralty Brass)-0.29
G Bronze-0.31
Copper Alloy 687 (Aluminum Brass)-0.32
Copper-0.36
Alloy 464 (Naval Rolled Brass)-0.4
Type 410 Stainless Steel (Active)-0.52
Type 304 Stainless Steel (Active)-0.53
Type 430 Stainless Steel (Active)-0.57
Carbon Steel-0.61
Cast Iron-0.61
Aluminum 3003-H-0.79
Zinc-1.03

Source: ASM Handbook, Vol. 13, Corrosion of Titanium and Titanium Alloys, p. 675.