For each of the following oxidation–reduction reactions of...

For each of the following oxidation–reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. $$ \begin{array}{l}{\text { a. } 3 \mathrm{Zn}(\mathrm{s})+\mathrm{N}_{2}(g) \rightarrow \mathrm{Zn}_{3} \mathrm{N}_{2}(\mathrm{s})} \\ {\text { b. } \mathrm{Co}(s)+\mathrm{S}(s) \rightarrow \cos (s)} \\ {\text { c. } 4 \mathrm{K}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{K}_{2} \mathrm{O}(s)} \\ {\text { d. } 4 \mathrm{Ag}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Ag}_{2} \mathrm{O}(s)}\end{array} $$

For each of the following oxidation–reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced.
$$
\begin{array}{l}{\text { a. } 3 \mathrm{Zn}(\mathrm{s})+\mathrm{N}_{2}(g) \rightarrow \mathrm{Zn}_{3} \mathrm{N}_{2}(\mathrm{s})} \\ {\text { b. } \mathrm{Co}(s)+\mathrm{S}(s) \rightarrow \cos (s)} \\ {\text { c. } 4 \mathrm{K}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{K}_{2} \mathrm{O}(s)} \\ {\text { d. } 4 \mathrm{Ag}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Ag}_{2} \mathrm{O}(s)}\end{array}
$$

Key Concepts

Oxidation

Oxidation is the process in a chemical reaction where an element loses electrons, leading to an increase in its oxidation state. This concept is fundamental in redox reactions as it helps determine which species is undergoing oxidation by tracking the change in the number of electrons before and after the reaction.

Reduction

Reduction is the complementary process to oxidation, involving the gain of electrons by an element. In a redox reaction, reduction is identified by a decrease in the oxidation state of a species, which gains electrons during the course of the reaction.

Oxidation States

Oxidation states are numbers assigned to elements in compounds that indicate their degree of oxidation or reduction. By comparing the oxidation states of elements in reactants and products, it is possible to identify which elements have been oxidized (increase in oxidation state) and which have been reduced (decrease in oxidation state).

Electron Transfer

Electron transfer refers to the movement of electrons from one atom or molecule to another during a chemical reaction. This transfer is the underlying mechanism of oxidation and reduction, with one species losing electrons and another gaining them, forming the basis for redox processes.

Redox Reaction Identification

Redox reaction identification involves determining the changes in oxidation states of the reacting species to establish which one loses electrons (oxidized) and which one gains electrons (reduced). This systematic approach is crucial in understanding and predicting the behavior of both metals and nonmetals in these reactions.

Transcript

Please give Ace some feedback