Alloys and rusting
In a nutshell
Alloys are compounds which are made up of two or more elements, one of these being a metal. Rusting is the process of the oxidation of a metal, there are a variety of ways to protect alloys and metals from rusting including galvanisation and sacrificial protection to name a few.
Alloys
Definition
Alloys are a mixture of two or more elements where at least one of the elements is a metal. Alloys are useful because pure compounds such as copper, iron and aluminium are too soft on their own and require mixing with other compounds to meet the standards of everyday use.
Alloy | Element one | Element two |
Steel | Iron | Carbon |
Bronze | Copper | Tin |
Brass | Copper | Zinc |
Example
Iron on its own is too soft and easily deformed under stress. However, with the addition of carbon it becomes a perfect construction material by increasing is strength and ability to resist deformation under stress.
Rusting
Rusting is an oxidation reaction, electrons are lost in this reaction. Both air and water are required for rusting to occur. Rusting occurs to both iron and steel as well as other metals.
iron + oxygen + water → hydrated iron (III) oxide iron → iron ion + 3 electrons Fe(s) → Fe3+(aq) + 3e−
Aluminium is protected from rusting due to a protective layer of aluminium oxide, preventing further rusting. Iron and steel rusting tends to flake off which further exposes the iron and steel.
| CONDITIONS | APPEARANCE |
1. | Air and water | Rust develops |
2.
| Air without water | No rust develops |
3.
| Water without air | No rust develops |
How to prevent rusting
There are several ways to prevent rusting, these methods include but are not limited to: oiling, galvanisation, painting and sacrificial protection.
Sacrificial protection
Sacrificial protection is when a more reactive metal is used to protect a less reactive metal and become oxidised. This then forms a layer around the less reactive metal protecting it from air and water.
Galvanisation
Galvanisation involves adding a layer of zinc over iron, therefore protecting it. Since zinc is more reactive than iron it gets oxidised and forms a layer preventing iron from being oxidised. This is a form of sacrificial protection.