Reactions of the Halogens | A Level Chemistry | OCR, AQA, Edexcel
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The reactions of halogens involve the halogen gaining an electron to achieve a full outer shell. Halogens are found in Group 7 of the periodic table meaning that they have 7 electrons in their outermost shell. This means that when they react, they gain one electron to achieve a full outer shell like noble gases.
The reactivity of halogens decreases as you move down Group 7. Halogens become less reactive as you move down the group as the atomic radius of the element increases which means that the distance between the outer shell of electrons and the nucleus increases. There is a reduced attraction between the nucleus and the outermost shell so it is more difficult to gain an extra electron. This is why the reactivity decreases down the group.
As the halogens become less reactive down the group, their oxidising ability decreases. Remember that oxidation is a gain of electrons. Halogens become less oxidising as you move down the group as it is more difficult to gain an electron.
Displacement reactions are a good test for oxidising ability. The oxidising strength of the halogens can be compared by carrying out displacement reactions involving the halide ions. It is worth to note here that a halide in solution will only be displaced by a halogen that is above it in the periodic table.
Displacement reactions can also be used to identify the halogen present in the solution.
Halogens react with Group 1 and Group 2 metals to form halide salts. Reactions between halogens and Group 1 and Group 2 metals are typical redox reaction with Group 1 and Group 2 metals being oxidised from an oxidation state of 0 to an oxidation state of 1+ and 2+ respectively.
The trend of reactivity of halogen is illustrated by their reactions with hydrogen. Halogens form covalent bonds with hydrogen to form hydrogen halide molecules. As we go down the group the reaction becomes less vigorous.
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