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Galvanization: Corrosion protection for ferrous metals

Why choose galvanized steel over stainless steel?

December 13, 2018

Square hollow rods are pulled shining out of a bath of silvery liquid during hot-dip galvanization
Hot-dip galvanization is used to coat steel with zinc alloy.

Ferrous metals, which contain iron, comprise 90% of the world’s metal manufacture. Iron is dense, strong when mixed with carbon, plentiful, and easy to refine, so is an excellent and dependable material for many industrial and structural applications. However, iron and many of its alloys—such as steel—are also highly prone to corrosion in the presence of air and water. Protecting against corrosion is an important consideration when designing a structure out of ferrous metal. Sometimes, the protection can come from the material properties of the alloy; stainless steels, for example, have chromium and sometimes elements like molybdenum added to provide the material a chemical protection against corrosion. Yet these additions can change mechanical properties and are not always the most cost-effective choice. Sometimes, a sealant is used to provide corrosion protection. Powder coating, paint, and oil treatments are all common and easily understood options. Galvanization is another common, but somewhat less well understood, seal used on ferrous metals.

What is galvanization?

Galvanization is a process in which zinc coatings are applied to steel or iron, creating a barrier that protects the ferrous metal from corrosion. The layer of zinc works physically, by blocking water and air from reaching the steel’s surface, and it works chemically, by offering cathodic protection.

Galvanization is usually done at high heat. Although a zinc layer can be added through painting or electroplating, either of these only create a thin layer: a shiny, brightly pretty surface only 3 microns thick. A topical application like this is vulnerable in outdoor applications where corrosion resistance is important.

True galvanization happens at high heat, and relies on the chemical interaction between zinc, oxygen, and carbon dioxide. The three react at temperature to create a dark grey zinc carbonate layer that is typically 50 microns thick and much more durable in outdoor locations.

Two pulleys on a crane ready to lower a steel grid with rows of rods hanging to be dipped into molten zinc
Galvanized metal is corrosion resistant and durable in many normal conditions.

Hot-dip galvanization

Hot-dip galvanization is the most common form of zinc galvanizing. In this method, steel or iron parts are cleaned of debris and mill scale and then are lowered into a zinc or zinc-alloy bath at a temperature near 840°F. The steel is left in the bath until it comes up to the same temperature, after which it is lifted and cooled. This cooling can be done quickly or slowly, depending on the intended look of the final product.

Galvannealing is the process of galvanizing in a zinc bath that has an addition of aluminum. While the metal is still hot, the entire product is heat treated, causing the formation of several strata of zinc-iron alloys. The addition of aluminum and the heat treatment after gives the resulting steel better weldability. Galvannealed steel will generally develop a reddish-rust-like patina but not corrode the way unprotected ferrous alloys corrode.

Dry galvanizing

A less common method for zinc galvanization is dry galvanizing. This process is also known as Sherardizing, named for the metallurgist Sherard Cowper-Coles, who developed the method. In this technique, small steel parts are heated in a closed rotating drum, along with zinc dust and sand, until the temperature and tumble cause the zinc to fuse chemically to the surface of the steel. The part is then quenched. It is often used for small parts and ones with inner surfaces that might be unreached by hot-dip.

A sheet of galvanized steel is covered in large leaf-like spangles of dark grey, light grey, and silver
Spangle, a visible flower- or feather-like metal grain, is characteristic of galvanized steel.

Spangle

One of the traditionally recognizable features of galvanized steel is the spangle on its surface. All metal freezes in crystalline forms, like a series of snowflakes packed tightly together. For most metals, this crystalline grain is too small to see, or the grain boundaries are not obvious without etching. Zinc-alloy galvanization allows people to see the crystallization pattern that forms during the freezing of the metal.

Spangle shape and size can give a hint to the cooling conditions after hot-dip galvanizing. In many cases, the more slowly the surface freezes, the larger the crystal grains, often evidencing feather- or leaf-like shapes. A quick quenching to colder temperatures can lead to smaller, more regular, or boxier grain.

A lot of the most eye-catching spangle, historically, has been created with small amounts of lead or tin in the zinc alloy. These additions allow the dendrite-like creation of the grains—the process of freezing that encourages feather-like shapes stretch across the surface. The development of lead-free galvanization has created zinc coatings that freeze from the steel up. These lead-free alloys may create rounder spangles that can be smaller than .5mm across. The interplay between alloy and freezing conditions means that a skilled galvanizer can influence the size and shape of spangle in the final product.

A morning glory leaf pokes through the hole in a rusted galvanized steel wall
Galvanic corrosion means that zinc oxidizes before steel: when it is gone, the steel will rust.

Galvanic corrosion and a sacrificial anodes

The galvanization process is not just a matter of creating a shell of zinc around the metal to create a physical barrier. If it were, other metals might be used. Rather, zinc protects through a chemical process called “cathodic protection.”

When two metals with very dissimilar electrical potentials are placed together in an electrolyte bath, they begin to act as an anode and cathode in an electrochemical reaction, creating a current. The most “active” of the two metals, the anode, will corrode more quickly than it would if it were alone, because it offers up electrons. The electron-stripped molecules within this anode are chemically unstable, and seek to form stable molecules with chemicals in the environment, producing oxides and other products of corrosion. Batteries use this form of galvanic corrosion to generate current.

Metals are classed by their reactivity in an anodic index. Gold, the most inert or passive of the metals, is used as the reference material. All other metals are given a number that represents their voltage when in an electrolyte bath with gold. This index is the basis for the galvanic scale, which sorts metals from most passive to most active.

Galvanic Scale
Most Cathodic/Passive

Gold
Silver
Nickel
Copper
Brass, bronze
Tin
Lead
Mild steel, cast iron
Aluminum
Zinc
Magnesium
Beryllium

Most Anodic/Active

Avoid placing different metals together unless they’re close on the galvanic scale.

In galvanization, zinc, an anodic metal, covers steel or iron. It works as a sealant, yet if there are any pin-holes in the covering, the electrochemical sacrifice of zinc means that it will corrode first, as the more active of the two metals. This property of a more anodic metal protecting a more cathodic one is used purposefully on boat hulls, which, submerged in sea water, are at risk of corrosion. These sacrificial anodes, also just called zincs, are usually bolted to a hull. Often, zinc parts are included in a design of a propeller or other device.

Zinc sacrifices quickly, but not too quickly, in the presence of iron. Looking at the galvanic scale, it is clear aluminum, magnesium, and beryllium might also be “more active” and therefore protective. However, aluminum is harder to bond to steel, more expensive, and is too close on the anodic index to function as well as a sacrificial anode. On the other side, magnesium would dissolve much faster, and additionally may be more reactive in many environments. Zinc also has the benefit of being protective against organic or bacterial breakdown. Beryllium is rare, expensive, and very unstable.

The galvanized metal roof of a building shows white rust where moisture has collected
“White rust” is zinc hydroxide: the red rust accumulating on the girders is an iron oxide.

Finishing the metal

White-rust can form on galvanized steel as the zinc breaks down into zinc hydroxide. This “rust” is indeed the product of zinc corrosion, but in normal conditions it happens at a much slower rate than unprotected steel oxidizes. In order to help slow this process even further, sometimes the galvanized metal is oiled, or occasionally chromium passivated, to create a final sealing layer. This oily or passivated metal cannot be painted or otherwise finished, but in many climates will look good for decades and stay structurally sound for even longer. Galvanized steel is useful for oiled working parts that might see paint quickly worn away.

In applications where the aesthetic of paint or powder-coat is preferred, galvanized steel can be left uncoated. Yet most often an item is either galvanized or painted, not both, to maintain the cost-savings of each approach.

Galvanized steel vs aluminum vs stainless steel

Galvanization is a cost-effective way to help protect metal that will be exposed to the elements. Aluminum and stainless steel are also used for applications that need strong, corrosion-resistant metal. They are better choices for cookware, utensils, and health-care, as too much zinc can be toxic, and both acids and heat might mobilize the zinc. In places where galvanized steel’s dull grey spangle is not ideal, they present a shinier, more adaptable aesthetic.

Yet aluminum and stainless each cost more, and their mechanical properties are not identical to steel. For applications where mechanical properties, aesthetic, or metal weight are important, more expensive materials might be the optimal choice. In other places, where standard steel’s functionality is desired, the galvanization process is ideal for weatherproofing at low cost.

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