Write a balanced ionic equation to describe the oxidation of iodide `(I^-)` in by permanganate `(MnO_(4)^(-))` ion in basic solution to yield molecular iodine `(l_2)` and manganese (IV) oxide `(MnO_2)`.
Strategy : We are given the formulas for two reactants and two prodcts. We use these to write the skeletal ionic equatin. We construct and balance the appropriate half-reactions using the rules just described. Then we add the half -reactions and eliminate common terms.

Explanation

To write a balanced ionic equation for the oxidation of iodide ions (I^-) by permanganate ions (MnO4^-) in a basic solution, we will follow these steps:

### Step 1: Write the skeletal ionic equation
The reactants are iodide ions (I^-) and permanganate ions (MnO4^-), and the products are molecular iodine (I2) and manganese(IV) oxide (MnO2). The skeletal equation can be written as:

\[ \text{I}^- + \text{MnO}_4^- \rightarrow \text{I}_2 + \text{MnO}_2 \]

### Step 2: Identify oxidation and reduction half-reactions
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