Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (a) HClO(aq) → Cl₂(g)

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Identify the oxidation states of the elements in the reactants and products.

For HClO, assign oxidation states: H is +1, O is -2, and Cl is +1.

For Cl_2, assign oxidation states: each Cl is 0.

Determine the change in oxidation state for Cl: from +1 in HClO to 0 in Cl_2.

Since the oxidation state of Cl decreases, this half-reaction is a reduction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction involves the gain of electrons, leading to a decrease in oxidation state. These processes are often summarized by the mnemonic 'OIL RIG' (Oxidation Is Loss, Reduction Is Gain).

Oxidation States

Oxidation states (or oxidation numbers) are assigned to atoms in a compound to indicate their degree of oxidation or reduction. They help in tracking electron transfer during chemical reactions. For example, in HClO, chlorine has an oxidation state of +1, which changes to 0 in Cl2, indicating that chlorine is being reduced as it gains electrons.

Half-Reactions

Half-reactions are equations that show either the oxidation or reduction process separately. They are useful for balancing redox reactions and understanding the electron transfer involved. In the given half-reaction, identifying whether it is an oxidation or reduction helps in classifying the overall reaction and balancing it appropriately.

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