Extraction of iron on a match head!
Introduction
Students reduce iron(III) oxide with carbon on a match head to produce iron in this small scale example of metal extraction. The experiment can be used to highlight aspects of the reactivity series.
Read our standard health & safety guidance
Lesson organisation
This experiment can easily be carried out on an individual basis by students. The experiment itself is very quick to do provided that the apparatus and chemicals are already set out around the laboratory.
Apparatus and Chemicals
Eye protection
Each student (or pair of students) will need:
Match (non-safety) (see note 1)
Tongs (crucible tongs)
Weighing boat (small white plastic ones are ideal)
Spatula
Students will also need access to:
Bunsen burner
Heat resistant mat
Magnet (e.g. bar magnet)
Iron(III) oxide powder (Low hazard) (see note 2)
Sodium carbonate powder (Irritant) (see note 2)
Water (see note 2)
Technical notes
Iron(III) oxide powder (Low hazard). Refer to CLEAPSS Hazcard 55A.
Sodium carbonate (Irritant). Refer to CLEAPSS Hazcard 95A.
1 The experiment works best with non-safety matches. These are often referred to as 'strike anywhere' matches and have a pinkish-red head.
2 Small amounts (a few spatula measures are sufficient) of each of the powders can be provided in, for example, Petri dishes or watch glasses. Groups of students can share the chemicals. The water can be provided in a small beaker.
Procedure
a Dip the head of a match in water to moisten it.
b Roll the damp match head first in sodium carbonate powder, then in iron(III) oxide powder.
c Hold the match in a pair of tongs. Put the head of the match into a blue Bunsen flame (air-hole open). The match will flare and burn. Do not allow the match to burn more than half way along its length.
d Allow the match to cool for about 30 seconds.
e Use a spatula to crush the charred part of the match into a small plastic weighing boat.
f Move a magnet around under the weighing boat – some of the small particles will move around in the weighing boat following the track of the magnet. Do not dip the magnet into the particles directly, unless you have first wrapped the magnet in cling film – any pieces of iron will stick to the magnet and will be difficult to clean off.
Teaching notes
A simple equation for the reaction would be:
Iron(III) oxide + carbon → iron + carbon dioxide
2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g)
Carbon is more reactive than iron. The iron oxide is reduced by the carbon (the oxygen is removed) to form metallic iron.
The sodium carbonate fuses easily and brings the iron oxide into close contact with the carbon.
Health & Safety checked, June 2007
Web Links
Teachers.tv. KS3/4 Science - Banging Chemistry: Fast and Furious
Updated 21 Feb 2008Average rating: 
3 out of 5
Your reviews
Thank you very mcuh. This is great.
Submitted by: PMcCormack on 17 November 2008
I've used this, it's simple and the kids loved it.
Submitted by: Debbie on 26 March 2009
This is a good but simple tool for learning the extraction of iron!!
Submitted by: Kelvin on 13 August 2009
Rubbish, do it properly, large scale!!
Submitted by: dd on 1 February 2010
Likely to mislead without further explanation.
Give students the 'simple equation', then ask where the carbon comes from - since none is added with the iron oxide.
I suspect most will say "from the sodium carbonate", thinking it is decomposed during the reaction.
Others may suggest "from the match head", though this is less likely with pink heads than dark safety matches.
A short diversion into history will help. Remind them that iron was originally extracted from iron ore using (wood) charcoal.
Since some students may know that magnetite is iron oxide, it may be worth testing the Fe2O3 to show that it is not magnetic at the start.
Submitted by: Mike Tingle on 8 April 2009