IGCSE EXTENDED CHEMISTRY METALS – METALS MASTER CHEAT SHEET

Rusting

The slow oxidation of iron in the presence of water and oxygen, resulting in hydrated iron(III) oxide.

Galvanising

The process of coating iron or steel with zinc to prevent rusting through barrier and sacrificial protection.

Blast Furnace

A method for extracting iron from its ore, involving the reduction of iron oxides using coke and limestone.

Reactivity Series

A ranking of elements based on their tendency to lose electrons and form positive ions.

Oxidation

Gain of oxygen or loss of electrons.

Reduction

Loss of oxygen or gain of electrons.

Displacement Reaction

A reaction where a more reactive metal displaces a less reactive metal from its salt solution.

Slag

A waste product composed mainly of calcium silicate that is formed during the extraction of iron.

Alloy

A mixture of a metal with other elements, which generally has improved properties.

Sacrificial Protection

A method of preventing corrosion where a more reactive metal corrodes instead of the protected metal.

Malleable

A property of metals that allows them to be hammered into shapes.

Ductile

A property of metals that allows them to be drawn into wires.

Empirical Formula

The simplest ratio of the elements in a compound.

Water + Oxygen + Iron = Rust

The conditions required for iron to rust, summarized as 'WOW'.

Zn²⁺ ions

The ions formed from zinc during galvanising that protect iron from oxidising.

First step in iron extraction.

C + O₂ → CO₂. Coke burns, producing heat.

Second step in iron extraction.

CO₂ + C → 2CO. Carbon monoxide is formed.

Main reaction in the iron extraction process.

Fe₂O₃ + 3CO → 2Fe + 3CO₂. This step extracts iron.

Fourth step in the iron extraction process.

CaCO₃ → CaO + CO₂. This involves limestone decomposition.

Fifth step in the iron extraction process.

CaO + SiO₂ → CaSiO₃ (slag). This removes sand impurities.