Define the terms oxidation and reduction; identify the...

Define the terms oxidation and reduction; identify the reactants oxidized and reduced. Identify each of the following as an oxidation or a reduction: a. $\mathrm{O}_{2}(g)+4 e^{-} \longrightarrow 2 \mathrm{O}^{2-}(a q)$ b. $\mathrm{Ag}(s) \longrightarrow \mathrm{Ag}^{+}(a q)+e^{-}$ c. $\mathrm{Fe}^{3+}(a q)+e^{-} \longrightarrow \mathrm{Fe}^{2+}(a q)$ d. $2 \mathrm{Br}^{-}(a q) \longrightarrow \mathrm{Br}_{2}(l)+2 e^{-}$

Define the terms oxidation and reduction; identify the reactants oxidized and reduced.
Identify each of the following as an oxidation or a reduction:
a. $\mathrm{O}_{2}(g)+4 e^{-} \longrightarrow 2 \mathrm{O}^{2-}(a q)$
b. $\mathrm{Ag}(s) \longrightarrow \mathrm{Ag}^{+}(a q)+e^{-}$
c. $\mathrm{Fe}^{3+}(a q)+e^{-} \longrightarrow \mathrm{Fe}^{2+}(a q)$
d. $2 \mathrm{Br}^{-}(a q) \longrightarrow \mathrm{Br}_{2}(l)+2 e^{-}$

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Key Concepts

Half-Reactions

Half-reactions are a method of breaking down complex redox reactions into separate oxidation and reduction components. Each half-reaction shows either the electron loss (oxidation) or electron gain (reduction), making it easier to analyze and balance the overall redox equations.

Oxidation

Oxidation is the process in which an atom, ion, or molecule loses electrons, leading to an increase in its oxidation state. This concept is fundamental in understanding redox reactions because it identifies the species that undergo electron loss and become oxidized.

Reduction

Reduction is the process in which an atom, ion, or molecule gains electrons, resulting in a decrease in its oxidation state. This is the complement of oxidation in redox reactions, with the species gaining electrons being reduced.

Electron Transfer Mechanism

Redox reactions are characterized by the transfer of electrons from one species to another. The movement of electrons explains the changes in oxidation states that occur during the reaction, highlighting the intrinsic connection between oxidation and reduction processes.

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