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. $$ \begin{array}{l}{\text { a. } 6 \mathrm{Na}(s)+\mathrm{N}_{2}(g) \rightarrow 2 \mathrm{Na}_{3} \mathrm{N}(s)} \\ {\text { b. } \mathrm{Mg}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{MgCl}_{2}(s)} \\ {\text { c. } 2 \mathrm{Al}(s)+3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{AlBr}_{3}(s)} \\ {\text { d. } 4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)}\end{array} $$

For each of the following oxidation–reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced.
$$
\begin{array}{l}{\text { a. } 6 \mathrm{Na}(s)+\mathrm{N}_{2}(g) \rightarrow 2 \mathrm{Na}_{3} \mathrm{N}(s)} \\ {\text { b. } \mathrm{Mg}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{MgCl}_{2}(s)} \\ {\text { c. } 2 \mathrm{Al}(s)+3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{AlBr}_{3}(s)} \\ {\text { d. } 4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)}\end{array}
$$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Redox Reactions

Redox reactions involve the transfer of electrons between chemical species. In these reactions, one substance undergoes oxidation (loses electrons) while another undergoes reduction (gains electrons). These reactions are fundamental in chemistry and are crucial in processes such as combustion, metabolism, and corrosion.

Oxidation

Oxidation refers to the process in which a species loses electrons during a chemical reaction, leading to an increase in its oxidation state. It is one half of the redox process and is often accompanied by a corresponding reduction in another species.

Reduction

Reduction is the gain of electrons by a chemical species, thereby decreasing its oxidation state. It complements oxidation in redox reactions, and the electron lost by the oxidized species is gained by the reduced species.

Oxidation State Assignment

The concept of oxidation states is used to keep track of electron transfers in chemical reactions. By assigning oxidation numbers to atoms, chemists can determine which species are oxidized and which are reduced in a reaction, providing a systematic way to analyze electron flow.

Transcript

Please give Ace some feedback