Identify each of the following as an oxidation or a...

Identify each of the following as an oxidation or a reduction: a. $\mathrm{Na}^{+}(a q)+e^{-} \longrightarrow \mathrm{Na}(s)$ b. $\mathrm{Ni}(s) \longrightarrow \mathrm{Ni}^{2+}(a q)+2 e^{-}$ c. $\mathrm{Cr}^{3+}(a q)+3 e^{-} \longrightarrow \mathrm{Cr}(s)$ d. $2 \mathrm{H}^{+}(a q)+2 e^{-} \longrightarrow \mathrm{H}_{2}(g)$

Identify each of the following as an oxidation or a reduction:
a. $\mathrm{Na}^{+}(a q)+e^{-} \longrightarrow \mathrm{Na}(s)$
b. $\mathrm{Ni}(s) \longrightarrow \mathrm{Ni}^{2+}(a q)+2 e^{-}$
c. $\mathrm{Cr}^{3+}(a q)+3 e^{-} \longrightarrow \mathrm{Cr}(s)$
d. $2 \mathrm{H}^{+}(a q)+2 e^{-} \longrightarrow \mathrm{H}_{2}(g)$

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Key Concepts

Oxidation

Oxidation is defined as the process where a chemical species loses electrons, resulting in an increase in its oxidation state. This concept is central to redox reactions, where the species undergoing oxidation releases electrons that are subsequently accepted by another species.

Reduction

Reduction is the process in which a chemical species gains electrons, leading to a decrease in its oxidation state. In any redox reaction, the species that accepts electrons is reduced, functioning as the complement to the species undergoing oxidation.

Electron Transfer

Electron transfer is a fundamental aspect of redox reactions, where electrons are moved from one species to another. This transfer is critical because the number of electrons lost in oxidation must equal the number of electrons gained in reduction, ensuring charge balance in the overall reaction.

Half-Reactions

Half-reactions are used to break down complex redox reactions into two separate equations—one for oxidation and one for reduction. Each half-reaction shows either the loss or gain of electrons, thereby simplifying the analysis and balancing of redox processes.

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