To analyze what happens to iron in this chemical reaction, let's break down the process step-by-step.
The given chemical reaction is:
[tex]\[ \text{Cu}^{2+}_{(\text{aq})} + \text{Fe}_{(\text{s})} \rightarrow \text{Cu}_{(\text{s})} + \text{Fe}^{2+}_{(\text{aq})} \][/tex]
### Step 1: Identify Initial and Final Oxidation States of Iron
- Initially, iron ([tex]\(\text{Fe}\)[/tex]) is in solid form with an oxidation state of 0 (metallic iron).
- In the product side, iron is in the form of [tex]\(\text{Fe}^{2+}_{(\text{aq})}\)[/tex], which indicates it has an oxidation state of +2.
### Step 2: Determine Electron Transfer
The change in oxidation state from 0 to +2 means that iron has lost electrons. Specifically:
- Loss of two electrons corresponds to the transition:
[tex]\[ \text{Fe} \rightarrow \text{Fe}^{2+} + 2e^- \][/tex]
### Step 3: Clarify the Changes that Occur:
1. Iron has lost two electrons:
- True. Iron in the reaction went from an oxidation state of 0 to +2. This change means iron lost two electrons.
2. Iron experienced an increase in oxidation state:
- True. The oxidation state increased from 0 to +2.
3. Iron has been oxidized:
- True. Oxidation involves the loss of electrons, and since iron lost electrons, it has been oxidized.
4. Iron has been reduced:
- False. Reduction involves the gain of electrons. Since iron lost electrons, it was not reduced; it was oxidized.
### Conclusion
Based on the analysis, the correct options are:
- Iron has lost two electrons.
- Iron experienced an increase in oxidation state.
- Iron has been oxidized.
- Iron has not been reduced.
The final answer to the question is:
Iron has lost two electrons, iron experienced an increase in oxidation state, iron has been oxidized, iron has not been reduced.
