Which element is oxidized and which is reduced in each of the following reactions? (b)

Verified step by step guidance

1. Identify the oxidation states of each element in the reactants and products.
2. Determine the change in oxidation state for each element from reactants to products.
3. The element whose oxidation state increases is oxidized.
4. The element whose oxidation state decreases is reduced.
5. Summarize which element is oxidized and which is reduced based on the changes in oxidation states.

Key Concepts

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 always occur simultaneously in a redox reaction, where one species is oxidized and another is 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 oxidation states helps identify which elements are oxidized and reduced during a reaction, as the changes in these states indicate the flow of electrons.

Half-Reactions

Half-reactions are a method of breaking down redox reactions into two separate equations: one for oxidation and one for reduction. This approach allows for a clearer understanding of the electron transfer process. By analyzing half-reactions, students can easily identify which species are oxidized and reduced, facilitating the balancing of redox equations.