Which element is oxidized, and which is reduced in the following reactions? (b) 3 Fe1NO3221aq2 + 2 Al1s2¡3 Fe1s2 + 2 Al1NO3231aq2

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.

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 identifying which elements are oxidized and reduced in a reaction. For example, in the reaction provided, determining the oxidation states of iron (Fe) and aluminum (Al) will clarify which element undergoes oxidation and which undergoes reduction.

Half-Reactions

Half-reactions are a way to separate the oxidation and reduction processes in a redox reaction. Each half-reaction shows either the loss of electrons (oxidation) or the gain of electrons (reduction) for a specific species. By writing the half-reactions for the given reaction, one can easily identify the oxidized and reduced elements, facilitating a clearer understanding of the overall reaction.