Chemguide: Support for CIE A level Chemistry

Learning outcome 11.2

Group 17 (previously Group 7)

The chemical properties of the halogen elements and the hydrogen halides

Learning outcome 11.2.1

This statement is about the reactivity of the halogens as oxidising agents.

Before you go on, you should find and read the statement in your copy of the syllabus.

Reactions between halogens and other halide ions

This is covered on the page halogens as oxidising agents.

You only need the first part of this page - the descriptions, the equations and the trend. You do not need the explanations. You can also ignore the reference to fluorine.

It is important that you remember what you have read on this page.

Other redox reactions illustrating the same trend

The important reactions are those you have already read about. However, the teachers' support material also mentions two other sets of reactions as well. Since these aren't specifically mentioned by the syllabus, you probably don't need to remember these, but they could come up in a question asking you to draw some conclusions from given information.

Reactions with iron

If you pass chlorine gas over hot iron, the iron burns to form iron(III) chloride.

This is a rapid reaction (the iron burns), and the iron has been oxidised to an iron(III) compound - in other words, from an oxidation state of zero in the iron metal to an oxidation state of +3 in the iron(III) compound.

Note:  If you have forgotten about oxidation states (oxidation numbers), it is essential that you revise them before you go on with this topic. There are several places where you will need them in Group 17 chemistry. You will find them discussed in Section 6.

If you pass bromine vapour over hot iron, a similar but slightly less vigorous reaction happens, this time producing iron(III) bromide.

Again the iron has been oxidised from an oxidation state of zero to +3.

However, the reaction between hot iron and iodine vapour only produces iron(II) iodide, and is much less vigorous.

This time, the iodine is only capable of oxidising the iron as far as the +2 oxidation state.

Reactions with sodium thiosulfate solution

These are much more complicated, and I am only including this because it has information you might need if you come across the reaction between sodium thiosulfate solution and iodine as a titration.

It isn't easy to see that an oxidation has happened here, but something must be being oxidised because the iodine is being reduced from an oxidation state of zero to -1. (If you can't see this, then you must go to the page mentioned in the last green box.)

The element (apart from iodine) whose oxidation state is changing is the sulfur. You need to work out the oxidation states of the sulphur in the sodium thiosulfate and the sodium tetrathionate.

In the sodium thiosulfate, the oxidation state of the sulphur is +2. In the sodium tetrathionate, it is +2.5. There has been a small oxidation of the sulphur.

Note:  If you can't get these answers, then go back and and look again at Section 6.

Don't worry about the fractional oxidation state in the sodium tetrathionate. This an average of the oxidation states of the various sulfur atoms involved.

The reactions between sodium thiosulfate and chlorine or bromine are totally different, and the sulfur-containing product this time is sodium sulfate, Na2SO4.

The oxidation state of the sulfur in this is +6 - a much more major oxidation than that with the iodine.

I am not going to give you the equations for these other two reactions, because some students will waste time trying to learn them. Because these reactions are not specifically mentioned by the syllabus, and are just some out of many possible other reactions, you shouldn't be asked to give them in an exam.

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© Jim Clark 2020