In the reaction `4Fe+3O_(2)rarr4Fe^(3+)+6O^(2-)`
Which of the following statements is incorrect?

Options

A. it is a redox reaction
B. metallic iron acts as a reducing agent
C. `O_(2)` acts as an oxidising agent
D. metallic iron is reduced to `Fe^(3+)`

Explanation

To determine which statement is incorrect regarding the reaction \(4Fe + 3O_2 \rightarrow 4Fe^{3+} + 6O^{2-}\), we will analyze the oxidation states of the elements involved and identify the roles of the reactants and products in the reaction.

### Step-by-Step Solution:

1. **Identify the Oxidation States:**
- In the reactants:
- Iron (Fe) is in its elemental form, so its oxidation state is \(0\).
- Oxygen (O) in \(O_2\) is also in its elemental form, so its oxidation state is \(0\).
- In the products:
- The iron ion \(Fe^{3+}\) has an oxidation state of \(+3\).
- The oxide ion \(O^{2-}\) has an oxidation state of \(-2\).

2. **Determine Changes in Oxidation States:**
- Iron (Fe) changes from \(0\) to \(+3\), indicating that it has lost electrons. This process is called oxidation.
- Oxygen (O) changes from \(0\) to \(-2\), indicating that it has gained electrons. This process is called reduction.

3. **Identify the Redox Nature of the Reaction:**
- Since oxidation (loss of electrons) and reduction (gain of electrons) are occurring simultaneously, this reaction is classified as a redox reaction.

4. **Identify the Reducing and Oxidizing Agents:**
- The species that is oxidized (loses electrons) acts as the reducing agent. Here, iron (Fe) is oxidized to \(Fe^{3+}\), so it is the reducing agent.
- The species that is reduced (gains electrons) acts as the oxidizing agent. Here, oxygen (\(O_2\)) is reduced to \(O^{2-}\), so it is the oxidizing agent.

5. **Evaluate the Statements:**
- **Statement A:** "Metallic ion acts as reducing agent." - This is correct because metallic iron donates electrons.
- **Statement B:** "O2 acts as an oxidizing agent." - This is correct because \(O_2\) accepts electrons.
- **Statement C:** "Metallic iron is reduced to Fe3+." - This is incorrect because metallic iron is oxidized to \(Fe^{3+}\).
- **Statement D:** "O2 is reduced to O2-." - This is correct because \(O_2\) gains electrons.

### Conclusion:
The incorrect statement is **C: "Metallic iron is reduced to Fe3+"** because metallic iron is actually oxidized to \(Fe^{3+}\).