Sure! Let's analyze the given half-reaction step-by-step to determine what is taking place.
The half-reaction provided is:
[tex]\[ Fe \longrightarrow Fe^{2+} + 2e^{-} \][/tex]
1. Identifying the Species:
- [tex]\( Fe \)[/tex] represents a neutral iron atom.
- [tex]\( Fe^{2+} \)[/tex] represents an iron ion with a charge of +2.
- [tex]\( 2e^{-} \)[/tex] represents two electrons.
2. Understanding Electron Transfer:
- The neutral iron atom [tex]\( Fe \)[/tex] is transformed into an iron ion [tex]\( Fe^{2+} \)[/tex].
- In this process, the iron atom loses electrons.
3. Oxidation vs. Reduction:
- Oxidation refers to the loss of electrons.
- Reduction refers to the gain of electrons.
Given that [tex]\( Fe \)[/tex] is losing 2 electrons to become [tex]\( Fe^{2+} \)[/tex], it is undergoing oxidation.
4. Agent Identification:
- An oxidizing agent is something that causes another substance to be oxidized and is itself reduced.
- A reducing agent is something that causes another substance to be reduced and is itself oxidized.
In this reaction, iron [tex]\( (Fe) \)[/tex] is losing electrons, hence it is being oxidized.
5. Best Statement:
- Let's now analyze the possible statements given:
- Iron is being reduced.
- This is incorrect because reduction involves gaining electrons, but iron is losing electrons.
- Iron is being oxidized.
- This is correct because iron is indeed losing electrons.
- Iron is gaining electrons.
- This is incorrect because iron is losing electrons, not gaining them.
- Iron is an oxidizing agent.
- This is incorrect because iron itself is oxidized; an oxidizing agent would be reduced.
Hence, the correct statement that best describes what is taking place in this half-reaction is:
Iron is being oxidized.
