Dilute HCI oxidises metallic Fe to `Fe^(2+)`.

Explanation

To determine whether the statement "Dilute HCl oxidizes metallic Fe to Fe²⁺" is true or false, we can analyze the reaction step by step.

### Step 1: Understanding the Reactants
- **Metallic Iron (Fe)**: Iron in its elemental form has an oxidation state of 0.
- **Dilute Hydrochloric Acid (HCl)**: This is a strong acid that dissociates in water to produce H⁺ and Cl⁻ ions.

### Step 2: Reaction of Iron with Hydrochloric Acid
When metallic iron reacts with dilute hydrochloric acid, the general reaction can be represented as:
\[ \text{Fe} + \text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2 \uparrow \]

### Step 3: Identifying the Products
- **FeCl₂**: This is iron(II) chloride, where iron has an oxidation state of +2.
- **H₂**: Hydrogen gas is released during the reaction.

### Step 4: Analyzing Oxidation States
- **Before Reaction**: Iron (Fe) has an oxidation state of 0.
- **After Reaction**: In FeCl₂, iron has an oxidation state of +2.
- **Chlorine (Cl)** in HCl is at -1 and remains at -1 in FeCl₂.

### Step 5: Determining Oxidation and Reduction
- **Oxidation**: The process where an element loses electrons and increases its oxidation state. Here, Fe goes from 0 to +2, indicating oxidation.
- **Reduction**: The process where an element gains electrons and decreases its oxidation state. In this case, H⁺ ions from HCl are reduced to H₂ gas.

### Conclusion
Since iron is oxidized from an oxidation state of 0 to +2, the statement "Dilute HCl oxidizes metallic Fe to Fe²⁺" is **True**.

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