Examples of Redox Reaction - Displacement of Halogen

Displacement of Halogen From Halide Solution

  1. Halogens are elements in Group 17 of the Periodic Table of Elements. They are fluorine, chlorine, bromine, iodine, astatine.
  2. All halogens tend to accept one electron to form negative ions. For instance,
  3. The ions of halogen are called halide.
  4. The electronegativity of halogens decreases down the group, as shown in the chart below:
    Cl2 + 2e → 2C1-
  1. Halogen which placed higher in group 17
    1. are more electronegative
    2. act as strong oxidising agent
    3. can be reduced easily
  2. The halogen which is at a higher position in group 17 ( more electronegative and reactive) can displace a halogen that is below it (less electronegative and less reactive) from its solution of halide ions.
  3. When the displacement reaction of the halogen occurs:
    1. transfer of electrons from the halide ions which are positioned further down in group 17 to halogens which are positioned further up occurs.
    2. Halogens which are positioned further up in group 17 act as oxidation agents. 
    3. These halogens undergo reduction and are reduced to halide ions. The halide ions which are positioned further down in group 17 act as reducing agents. These ions undergo oxidation and are oxidised to halogens.

Reaction between Chlorine water and Potassium Bromide solution.

  1. A few drops of chlorine water are added to 2 cm³ of potassium bromide solution.
  2. 2 cm³ of tetrachloromethane is then added into the mixture and shaken.
  3. The colour of the tetrachloromethane (the lower layer) is recorded.


The colourless tetrachloromethane turn brown. This indicates that bromine is presence in the solution.

Half Equation:

2Br- → Br2 + 2e
Cl2 + 2e → Cl2

Ionic Equation:

Cl2 +  2Br-  2Cl- + Br2

  1. Chlorine is more electronegative than bromine.
  2. In the reaction, chlorine molecules displaced bromide ions in the solution.
  3. Bromide ion is oxidised by releasing electrons to become bromine.
  4. Chlorine molecule is reduced by receiving electrons from bromide ion.

Oxidising agent: Chlorine
Reducing agent: Bromide

1 comment:

  1. correction for the half equation (Cl2 + 2Cl- → Cl2) to (Cl2 + 2e -> 2Cl-)