Rust

Chemical reactions

The oxidation of iron metal

Iron metal is relatively unaffected by pure water or by dry oxygen. As with other metals, a tightly adhering oxide coating, a passivation layer, protects the bulk iron from further oxidation. Thus, the conversion of the passivating iron oxide layer to rust results from the combined action of two agents, usually oxygen and water. Other degrading solutions are sulfur dioxide in water and carbon dioxide in water. Under these corrosive conditions, iron(III) species are formed. Unlike iron(II) oxides, iron(III) oxides are not passivating because these materials do not adhere to the bulk metal. As these iron(III) compounds form and flake off from the surface, fresh iron is exposed, and the corrosion process continues until all of the iron(0) is either consumed or all of the oxygen, water, sulfur dioxide in the system are removed or consumed.^[2]

Chemical reactions associated with rusting

The rusting of iron is an calcium chloride) on the corrosion of automobiles. The key reaction is the reduction of oxygen:

O₂ + 4 e^- + 2 H₂O → 4 OH^-

Because it forms pH. Providing the electrons for the above reaction is the oxidation of iron that may be described as follows:

Fe → Fe²⁺ + 2 e⁻

The following redox reaction also occurs in the presence of water and is crucial to the formation of rust:

2 Fe²⁺ + 0.5 O₂ → 2 Fe³⁺ + O²⁻

Additionally, the following multistep acid-base reactions affect the course of rust formation:

Fe²⁺ + 2 H₂O ⇌ Fe(OH)₂ + 2 H⁺

Fe³⁺ + 3 H₂O ⇌ 2 Fe(OH)₃ + 3 H⁺

as do the following dehydration equilibria:

Fe(OH)₂ ⇌ FeO + H₂O

Fe(OH)₃ ⇌ FeO(OH) + H₂O

2 FeO(OH) ⇌ Fe₂O₃ + H₂O

From the above equations, it is also seen that the corrosion products are dictated by the availability of water and oxygen. With limited dissolved oxygen, iron(II)-containing materials are favoured, including FeO and black hydroxides and oxides of iron to precipitate a variety of Ca-Fe-O-OH species.

Rust prevention

Rust is permeable to air and water, therefore the interior iron continues to corrode. Rust prevention thus requires coatings that preclude rust formation. zinc.

An important approach to rust prevention entails sacrificial anode.

Several other methods are available to control corrosion and prevent the formation of rust, colloquially termed rustproofing:

• electrode potential, commonly zinc or magnesium. The electrode alone does not react in water but only provides electrons that are otherwise provided by the iron.

• Bluing is a technique that can provide limited resistance to rusting for small steel items, such as firearms; for it to be successful, water-displacing oil is rubbed onto the blued steel.

• Rust formation can be controlled with paint, that isolate the iron from the environment. Large structures with enclosed box sections, such as ships and modern automobiles, often have a wax-based product (technically a "slushing oil") injected into these sections. Such treatments also contain rust inhibitors. Covering steel with concrete provides protection to steel by the high pH environment at the steel-concrete interface.

Economic impact

Main article: Corrosion

Rust is associated with degradation of iron-based tools and structures. As rust has higher volume than the originating mass of iron, its buildup can also cause failure by forcing apart adjacent parts — a phenomenon known as "rust smacking." Similarly corrosion of concrete-covered steel and iron can cause the concrete to spall, creating structural problems.

References

1. ^ Interview, David Des Marais.
2. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
3. ^ Hubert Gräfen, Elmar-Manfred Horn, Hartmut Schlecker, Helmut Schindler "Corrosion" Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH: Weinheim, 2002. DOI: 10.1002/14356007.b01_08

See also

• WD-40
• Cosmoline
• Weathering steel