Permanganate (VII) ion,  in basic solution oxidises iodide ion, I^- to produce molecule iodine (I₂) and manganese (IV) oxide (MnO₂). Write a balanced ionic equation to represent redox reaction. 

The skeleton ionic equation is

1. Write the oxidation and reduction half-reactions by observing the changes in oxidation number and writing these separately. 
             Oxidation half reaction:
                -1               0
                I^-(aq)    I₂(s)
              Reduction half reaction:
                +7               +4
               
2. Balance the oxidation half reaction
(i) Balance 1 atoms by multiplying I^- by 2
                       -1                  0
                       
(ii) Add 2 electrons towards R.H.S. to balance the charges on iodine atoms
                     
3. Balancing the reduction half reaction
    (i) Add 3 electrons towards L.H.S. to balance the charge on Mn
                     
     (ii) Balance O atoms by adding two H₂O molecules towards R.H.S.
             
     (iii) Balance H atoms by adding four H⁺ towardS
      L.H.S.
               
Since the reaction takes place in a basic solution, therefore for four H⁺ ions, we add four OH^- ions to both sides of the equation.

[Balanced reduction half reaction]
4. Multiply balanced oxidation half-reaction by 3 and balanced reduction half-reaction by 2 and add both the half reactions.

This is a balanced equation.