Which of the following is an oxidation half-reaction?Group of answer choicesO + 4H + 4e 2HOCl + 2e 2ClFe + e FeSn Sn + 2e PreviousNext

To determine which of the given reactions is an oxidation half-reaction, we need to identify the reaction where there is an increase in oxidation state, which typically involves the loss of electrons.

1. Break Down the Problem

We examine each reaction to see if it involves the loss of electrons:

1. O + 4H + 4e → 2HOCl
2. 2Cl + 2e → Fe
3. Sn → Sn + 2e
4. Fe + e → Fe

2. Relevant Concepts

• Oxidation Half-Reaction: A reaction that results in the loss of electrons, thereby increasing the oxidation state of an element.

3. Analysis and Detail

• Reaction 1: O + 4H + 4e → 2HOCl

  • The oxygen is gaining electrons; it’s a reduction reaction.

• Reaction 2: 2Cl + 2e → Fe

  • Chlorine is gaining electrons, making it a reduction half-reaction.

• Reaction 3: Sn → Sn + 2e

  • This looks incorrect as it appears to have no change in oxidation state; it should be analyzed further to ensure context.

• Reaction 4: Fe + e → Fe

  • Here iron is gaining electrons; thus, it's not an oxidation.

4. Verify and Summarize

We need to note that the reactions generally depict either oxidation or reduction and are usually listed with their correct states.

Final Answer

From the given options, none of the listed half-reactions are properly written oxidation reactions, as the first three indicate reductions. The closest interpretation that suggests an increase in oxidation state (for clarity, if Sn were to represent Sn → Sn²⁺ + 2e as a correct formatting) could suggest an oxidation. However, if the original context included that formatting, it would suggest that the Sn reaction is the oxidation half-reaction. This needs correct validation of the stated half-reactions.