Class 11 Chemistry Redox Reactions Balancing of Redox reactions

Balancing of Redox reactions

There are two ways of balancing Redox reactions:

  • Oxidation number method
  • Half equation method

Oxidation method: The steps to be followed-

  1. Write the skeletal equation of reactants and products.
  2. Indicate the oxidation number of all the elements involved in the reaction.
  3. Calculate the increase or decrease in oxidation number per atom. Also, identify the oxidizing and reducing agents.
  4. Multiply the formula of oxidizing agent and reducing agent by suitable integers, so as to equalize the total increase or decrease in oxidation number as calculated in step c.
  5. Balance all atoms other than H and O.
  6. Finally balance H and O atoms by adding water molecules using hit and trial method.
  7. In case of Ionic reactions:
  • For acidic medium
  • First balance O atoms by adding water molecules to the deficient side.
  • Balance H+ ions to the side deficient in H atoms.
  • For Basic medium
  • First balance oxygen atom by adding water molecules to the deficient side.
  • Then to balance hydrogen, add water molecules equal to the number of deficiency of H atoms.
  • Also add equal number of OH- ions to opposite side of the equation.

Example: Permagnate ion reacts with bromide ion in basic medium to give manganese dioxide and Bromate ion .

Step1: the skeletal ionic equation is :

MnO4- (aq) +Br- (aq) ---> MnO2 +BrO3-

Step 2: assign oxidation numbers for Mn and Br


Step3: calculate the increase and decrease in oxidation number and make the change equal :


Step: 4 as the reaction occurs in basic medium, and the ionic charges are not equal on both sides, add 2OH- ions on the right to make it equal.


Step5: finally count the hydrogen atoms and add appropriate number of water molecules on the left side to achieve balanced Redox reaction.


Half reaction method or Ion electron method

  1. Write the skeletal equation and indicate the oxidation number of all the elements which occur in skeletal equation
  2. Find out the species that are oxidized and reduced.
  3. Split the skeletal equation into two half reactions: oxidation half reaction and reduction half reaction
  4. Balance the two-half equation separately by rules described below:
  • In each half reaction first balance the atoms of element that has undergone a change in oxidation number.
  • Add electrons to whatever side is necessary to make up the difference in oxidation number in each half reaction.
  • Balance the charge by adding H+ ions, if the reaction occurs in acidic medium .For basic medium, add OH- ions if the reaction occurs in basic medium.
  • Balance oxygen atoms by adding required number of water molecules to the side deficient in oxygen atoms
  • In the acidic medium, H atoms are balanced by adding H + ions to the side deficient in H atoms.
  • However, in the basic medium H atoms are balanced by adding water molecules equal to number to H atoms deficient.
  • Add equal number of OH- ions to opposite side of equation.
  • The two half reactions are then multiplied by suitable integers .so that the total number of electrons gained in half reaction becomes equal to total number of electrons lost in another half reaction.
  • Then the two half reactions are added up.
  • To verify the balancing, check whether the total charge on either is equal or not.

Example: Let us consider the skeletal equation:

Fe2+ + Cr2O72- -->  Fe3+ +Cr3+

Step 1: Separate the equation in to two halves:

Oxidation half reaction: Fe--> Fe3+

 Reduction half reaction: Cr2O72-  -->    Cr3+

Step 2: Balance the atoms other than hydrogen and oxygen in each half reaction individually. Here the oxidation half reaction is already balanced with respect to Fe atoms .For the reduction half reaction, we multiply the Cr3+ by 2 to balance Cr atoms.

Step 3: For reactions occurring in acidic medium, add water molecules to balance oxygen atoms and hydrogen ions are balanced by adding H atoms. Thus, we get:

Cr2O72- + 14 H+  +  6e- --> 2 Cr3+ + 7H2O

Step 4: Add electrons to one side of the half reaction to balance the charges .if needed make the number of electrons equal in two half reactions by multiplying one or both half reaction by suitable coefficient.

The oxidation half reaction is thus written again to balance the charge .Now in the reduction half reaction there are 12 positive charges on the left hand side and only 6 positive charge on right hand side .Therefore, we add six electrons to left hand side .

Cr2O72- + 14 H+  +  6e- --> 2 Cr3+ + 7H2O

To equalize the number of electrons in both reactions, we multiply oxidation half reaction by 6 and write as:

6Fe2+  -->  6Fe3+ +6e-

Step 5: We add the two half reactions to achieve the overall reaction and cancel the electrons on each side .This give us net ionic equation:

6Fe2+  + Cr2O72- + 14 H+ -->    2Cr3++6Fe3+ +7H2O

Step6: Verify that the equation contains the same type and number of atoms and the same charges on both sides of the equation. This last check reveals that the equation is fully balanced with respect to number atoms and the charges.

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