Considering the following net ionic equation: Mg + Fe²⁺ $\rightarrow$ Mg²⁺ + Fe
The species that is OXIDIZED is _____,and the OXIDIZING AGENT is _____.

Question

Considering the following net ionic equation: Mg + Fe²⁺ $\rightarrow$ Mg²⁺ + Fe The species that is OXIDIZED is _____,and the OXIDIZING AGENT is _____.

Quizplus · Accepted Answer

In the given net ionic equation, FeS and Mg are the reactants. FeS is reducing agent and hence it gets oxidized. Mg is the oxidizing agent and hence it reduces FeS. Therefore, the species that is oxidized is FeS and the oxidizing agent is Mg. Option B is the correct choice as it correctly identifies both the oxidized species and the oxidizing agent.

Considering the Following Net Ionic Equation: Mg + Fe2+ →\rightarrow→ Mg2+ + Fe the Species That Is OXIDIZED Is _____,And

Considering the Following Net Ionic Equation: Mg + Fe²⁺ $\rightarrow$ Mg²⁺ + Fe
the Species That Is OXIDIZED Is _____,And