Reaction of zinc with iodine
Class practical or demonstration
This experiment involves the
synthesis of a metal salt by direct reaction of a metal and a non-metal. powder is added to a solution of Zinc in iodine ethanol. An exothermic redox reaction occurs, forming , which can be obtained by evaporating the solvent. zinc iodide
Zn + I
2 → ZnI 2
The experiment can be extended to show the
decomposition of a compound into its elements by electrolysing the zinc iodide.
This experiment can be used to illustrate the differences between metallic and non-metallic elements and their reaction to form a compound – a metal salt – with new properties.
The reaction can be easily reversed using electrolysis to decompose the compound back into its elements. These are easily recognisable from their distinctive appearances.
Both parts of the experiment can be done either as demonstrations or as class experiments. Each part should take about 10 mins as a demonstration; longer as a class experiment.
Each group (or demonstration) requires:
Test-tubes (100 x 16 mm), 3
Measuring cylinder (10 cm
Small filter funnel
Weighing boat or suitable container for zinc powder
For the extension work:
Beaker (100 cm
Pair of graphite electrodes mounted in a rubber bung
Electrical leads and crocodile clips
Source of 3–6 V DC, either battery or power supply
Torch bulb in a suitable holder
Chemicals are for one demonstration or one group of students:
Iodine (HARMFUL), about 0.5 g (Note 1)
Zinc powder (HIGHLY FLAMMABLE), about 0.5 g (Note 2)
Ethanol (HIGHLY FLAMMABLE) or IDA (Industrial Denatured Alcohol) (HIGHLY FLAMMABLE, HARMFUL) about 5 cm 3
For the extension work:
Distilled water, about 20 cm
hydrochloric acid, 1 M or sulfuric acid, 1 M (IRRITANT), about 20 cm 3
Refer to Health & Safety and Technical notes section below for additional information.
Health & Safety and Technical notes
Read our standard health & safety guidance
Wear eye protection.
Iodine, I 2(s), (HARMFUL, DANGEROUS FOR THE ENVIRONMENT) - see CLEAPSS Hazcard.
Zinc powder, Zn(s), (HIGHLY FLAMMABLE, DANGEROUS FOR THE ENVIRONMENT) - see CLEAPSS Hazcard.
Ethanol, C 2H 5OH(l), (HIGHLY FLAMMABLE or HIGHLY FLAMMABLE and HARMFUL if using IDA) - see CLEAPSS Hazcard.
Zinc iodide, ZnI 2(s), (IRRITANT) - see CLEAPSS Hazcard.
hydrochloric acid, HCl(aq) or dilute sulfuric acid, H 2SO 4(aq) (IRRITANT) - see CLEAPSS Hazcards.
The solid iodine should be powdered by grinding in a mortar in a fume cupboard. For a class experiment a stoppered test-tube containing 0.5 g of powdered iodine should be supplied to each group of students. 1
For a class experiment each group of students should be supplied with a pre-weighed sample of 0.5 g zinc powder in a weighing boat or a test-tube. 2
Synthesis of zinc iodide
Measure out 5 cm a
3 of ethanol using a measuring cylinder. Place a thermometer in the ethanol and record the temperature.
Add the ethanol to 0.5 g of powdered iodine in a test-tube. Stir carefully, using the thermometer, to dissolve the iodine. The solution should be dark brown. Note the temperature. b
When all the iodine has dissolved, slowly add the zinc powder using a spatula and stir the mixture with the thermometer. The temperature should rise, indicating an exothermic reaction. When the reaction is finished, the colour of the iodine should have faded and excess zinc will be left. If not, add further small amounts of zinc powder and stir until the brown colour due to iodine has gone. c
Filter the solution into another test-tube. Using a teat pipette, transfer a few drops of the filtrate on to a watchglass and allow the solvent to evaporate. This can be speeded up by placing the watchglass on a beaker containing some hot water. Zinc iodide will be left as a white solid. d
Pour the remainder of the solution containing the zinc iodide into a 100 cm a
3 beaker. Add about 20 cm 3 of distilled water and stir to mix.
Clamp the bung carrying the two graphite electrodes over the beaker, so that the bottoms of the electrodes are immersed as far as possible in the solution. It may be easier just to rest the bung in the beaker so that the electrodes touch the bottom. b
Using the leads and crocodile clips, connect the electrodes and the bulb in series and then to the power supply as shown in the diagram on this page. The bulb should glow to show that the circuit is complete, and that electrolysis is occurring. c
If the bulb does not glow, raise the bung out of the solution and check the connections by touching both electrodes at once with a metal spatula. If the bulb lights up, put the electrodes back into the solution. If there is still no indication of electrolysis, add a small amount of zinc iodide from the watchglass to the solution and stir. Repeat until the bulb starts to glow. d
Allow electrolysis to continue for a few minutes. Note any changes occurring around the electrodes in the solution – a brown colour (due to iodine) should develop in the solution around the positive electrode. There may be some effervescence at the negative electrode. e
Disconnect the power supply. Lift the electrodes out of the solution. Wash them under a tap. The bottom of the negative electrode should be covered with a silver-grey layer of zinc metal. f
The zinc deposit can be tested (and removed) by immersing the tip of the electrode in a little dilute acid. It reacts and dissolves, giving off a colourless gas (hydrogen).
This reaction shows the synthesis of a compound from two elements, each with their own distinctive appearance and properties. (A practical worksheet could involve drawing up a table of properties (type of element, appearance, and so on) for each of the elements and the compound formed.)
The reaction can also be used to illustrate the direct reaction of a typical metal and non-metal. It is one of the few reactions of the halogens (Group 17) with a metal that students can do safely themselves.
A useful extension of this experiment is the decomposition, by electrolysis, of the compound formed back into its elements.
Health & Safety checked, 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