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

Identify each of the following as an oxidation or a reduction: (7.6) a. $\mathrm{Zn}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Zn}(s)$ b. $\mathrm{Al}(s) \longrightarrow \mathrm{Al}^{3+}(a q)+3 e^{-}$ c. $\mathrm{Pb}(s) \longrightarrow \mathrm{Pb}^{2+}(a q)+2 e^{-}$ d. $\mathrm{Cl}_{2}(g)+2 e^{-} \longrightarrow 2 \mathrm{Cl}^{-}(a q)$

Identify each of the following as an oxidation or a reduction: (7.6)
a. $\mathrm{Zn}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Zn}(s)$
b. $\mathrm{Al}(s) \longrightarrow \mathrm{Al}^{3+}(a q)+3 e^{-}$
c. $\mathrm{Pb}(s) \longrightarrow \mathrm{Pb}^{2+}(a q)+2 e^{-}$
d. $\mathrm{Cl}_{2}(g)+2 e^{-} \longrightarrow 2 \mathrm{Cl}^{-}(a q)$

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

Oxidation

Oxidation is the chemical process in which a substance loses electrons, leading to an increase in its oxidation state. This process is crucial in redox reactions and is often observed in half-reactions where electrons appear on the products side.

Reduction

Reduction is the chemical process in which a substance gains electrons, resulting in a decrease in its oxidation state. It is the counterpart to oxidation and is identified in half-reactions by the appearance of electrons on the reactants side.

Half-Reactions

Half-reactions are simplified chemical equations that separately display the oxidation and reduction processes occurring in a redox reaction. They help in balancing the overall reaction by focusing on the electron transfer events within each process.

Electron Transfer

Electron transfer is the underlying mechanism in redox reactions where electrons are moved from one species to another. This concept is essential for understanding how oxidation (electron loss) and reduction (electron gain) occur, and it plays a key role in many chemical and biological systems.

Transcript

Please give Ace some feedback