Magnesium is weighed and then heated in a crucible. It reacts with oxygen to produce the oxide. It can be shown that there has been an increase in mass. The results can be used to find the formula of magnesium oxide and two methods are described for doing so.
The practical activity takes around 30-45 minutes, depending on the competence of the class. Students should all be standing and should wear eye protection. Students with long hair should tie it back.
It is a good idea for students to practice lifting the lid on and off the crucible and the crucible off the pipe clay triangle before they start. This has the added bonus of checking that all the tongs are functioning correctly.
To enable students to light their Bunsen burners they will need access to matches or lighters. Alternatively, light one or two Bunsen’s around the room and students can light their own using a splint.
The most significant hazard in this experiment is the hot apparatus. Warn students that it will take some time to cool down.
For classes with shorter attention spans, the final step of heating to constant mass could be omitted.
Per pair or group of students:
Crucible with lid
Pipe clay triangle
Heat resistant mat
Emery paper (optional)
Balance (2 d.p.)
Magnesium ribbon, about 10-15 cm
Refer to Health & Safety and Technical notes section below for additional information.
Health & Safety and Technical notes
Wear eye protection.
Magnesium ribbon, Mg(s) - see CLEAPSS Hazcard. Fresh, clean magnesium is best for this experiment. If the magnesium is tarnished then emery or sand paper will be required to clean it.
a Cut a piece of magnesium about 10-15 cm long. If it is looking tarnished or black then clean it using the emery paper. Twist it into a loose coil.
b Weigh the crucible with the lid (mass 1) and then the magnesium inside the crucible with the lid (mass 2).
c Set up the Bunsen burner on the heat resistant mat with the tripod. Place the pipe clay triangle over the tripod in a ‘star of David’ formation, ensuring that it is secure. Place the crucible containing the magnesium in the pipe clay triangle and put the lid on.
d Light the Bunsen burner and begin to heat the crucible. It is best to start with a gentle blue flame, but you will need to use a roaring flame (with the air hole fully open) to get the reaction to go.
e Once the crucible is hot, gently lift the lid with the tongs a little to allow some oxygen to get in. You may see the magnesium begin to flare up. If the lid is off for too long then the magnesium oxide product will begin to escape. Don’t let this happen.
f Keep heating and lifting the lid until you see no further reaction. At this point, remove the lid and heat for another couple of minutes. Replace the lid if it appears that you are losing some product.
g Turn off the Bunsen burner and allow the apparatus to cool.
h Re-weigh the crucible with lid containing the product (mass 3).
i Heat the crucible again for a couple of minutes and once again allow to cool. Repeat this step until the mass readings are consistent. This is called ‘heating to constant mass.’
Students should have recorded the following masses:
- (mass 1) Crucible + lid
- (mass 2) Crucible + lid + magnesium
- (mass 3) Crucible + lid + product
This should allow them to calculate the mass of the mass of the magnesium (mass 2) - (mass 1) and the mass of the product (mass 3) - (mass 1). They could also calculate the increase in mass (mass 3) - (mass 2), which corresponds to the mass of oxygen.
The equation is:
Magnesium + oxygen → magnesium oxide
2Mg + O2 → 2MgO.
Students sometimes get unconvincing results to this experiment. It is worth evaluating what they have done as there are several reasons why their results may be disappointing:
- the magnesium oxide product may escape as they lift the lid
- not all the magnesium may have reacted (the product may still look a bit grey rather than white)
- they may have prodded the product with their splint so not all of it got weighed (more common than you might expect!)
- not tareing the balance correctly for one of the weighings
- having the magnesium coiled too tightly so that not all of it reacts
Finding the formula of magnesium oxide
To find the formula of magnesium oxide, students will need the mass of the magnesium and the mass of the oxygen. They will also require the relative atomic masses. Magnesium is 24 and oxygen is 16.
They should divide mass by the atomic mass for each element. The gives the number of moles of each.
Having done this for both elements, they should find the ratio between the two by dividing them both by the smallest number.
The ratio should be close to 1:1 as the formula of magnesium oxide is MgO.
Mass magnesium = 2.39 g
Mass magnesium oxide = 3.78 g
So mass oxygen = 1.39 g
Number moles Mg = 2.39/24 = 0.0995
Number moles O = 1.39/16 = 0.0868
Divide by the smallest to give the ratio aprox. 1 Mg: 1O
This would suggest a formula of MgO, which is the correct formula.
Students will need the mass of the magnesium and the mass of oxygen which has combined with it. You will need a copy of the graph below for the class.
All students plot their masses of magnesium and oxygen onto the graph. The majority of the class’ results should fall on or near the line representing the formula MgO, a 1:1 ratio. This helps to show clearly any anomolous results and should help to convince students who are disappointed by a 1:1.25 ratio, for instance, that the correct formula really is MgO.
Health & Safety checked, August 2016
This Practical Chemistry resource was developed by the Nuffield Foundation and the Royal Society of Chemistry.
© Nuffield Foundation and the Royal Society of Chemistry
Page last updated October 2015
This is a resource from the Practical Chemistry project, developed by the Nuffield Foundation and the Royal Society of Chemistry. This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. Practical Chemistry activities accompany Practical Physics and Practical Biology.
The experiment is also part of the Royal Society of Chemistry’s Continuing Professional Development course: Chemistry for non-specialists