Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (d) SbCl₄^-(aq) → SbCl₆^-(aq)

Verified step by step guidance

1. Identify the oxidation states of the central atom (Sb) in both the reactant and the product.
2. In SbCl_4^- (aq), determine the oxidation state of Sb by considering the oxidation state of Cl as -1.
3. In SbCl_6^- (aq), determine the oxidation state of Sb by considering the oxidation state of Cl as -1.
4. Compare the oxidation states of Sb in the reactant and product to determine if it has increased or decreased.
5. If the oxidation state of Sb increases, it is an oxidation reaction; if it decreases, it is a reduction reaction.

Key Concepts

Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between species. 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 always coupled, meaning that when one species is oxidized, another must be reduced.

Oxidation States

Oxidation states (or oxidation numbers) are a way to keep track of electron transfer in redox reactions. Each element in a compound is assigned an oxidation state based on its electron configuration and bonding. Understanding how to assign oxidation states is crucial for identifying which species is oxidized and which is reduced in a half-reaction.

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 context of the given question, analyzing the half-reaction allows us to determine whether the species is gaining or losing electrons, thus classifying it as oxidation or reduction.