For each of the following oxidation-reduction reactions,...

For each of the following oxidation-reduction reactions, identify which element is oxidized and which is reduced. a. $\mathrm{Mg}(s)+\mathrm{Br}_{2}(l) \rightarrow \mathrm{MgBr}_{2}(s)$ b. $2 \mathrm{Na}(s)+\mathrm{S}(s) \rightarrow \mathrm{Na}_{2} \mathrm{~S}(s)$ c. $\mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \rightarrow \mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g)$ d. $6 \mathrm{~K}(s)+\mathrm{N}_{2}(g) \rightarrow 2 \mathrm{~K}_{3} \mathrm{~N}(s)$

For each of the following oxidation-reduction reactions, identify which element is oxidized and which is reduced.
a. $\mathrm{Mg}(s)+\mathrm{Br}_{2}(l) \rightarrow \mathrm{MgBr}_{2}(s)$
b. $2 \mathrm{Na}(s)+\mathrm{S}(s) \rightarrow \mathrm{Na}_{2} \mathrm{~S}(s)$
c. $\mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \rightarrow \mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g)$
d. $6 \mathrm{~K}(s)+\mathrm{N}_{2}(g) \rightarrow 2 \mathrm{~K}_{3} \mathrm{~N}(s)$

Key Concepts

Redox Reactions

Redox reactions combine oxidation and reduction processes in a single chemical event, characterized by the transfer of electrons between chemical species. Grasping the nature of redox reactions is fundamental for analyzing and balancing reactions where electron transfer is involved.

Oxidizing and Reducing Agents

These are the substances that facilitate redox reactions by respectively gaining or losing electrons. An oxidizing agent causes another species to oxidize by being reduced itself, while a reducing agent causes reduction by being oxidized. This concept is crucial for understanding the roles different reactants play in a redox process.

Oxidation Numbers

Assigning oxidation numbers to atoms in compounds allows chemists to keep track of electron transfer during reactions. This systematic method aids in identifying changes in oxidation states, helping to pinpoint which elements are oxidized or reduced.

Oxidation

This concept refers to the process in which an atom, molecule, or ion loses electrons, resulting in an increase in its oxidation state. Recognizing oxidation helps in identifying which species in a chemical reaction is undergoing an electron loss.

Reduction

Reduction is the complementary process to oxidation, occurring when an atom, molecule, or ion gains electrons, leading to a decrease in its oxidation state. Understanding reduction is key for determining which species in a reaction is accepting electrons.

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