**Considering the following net ionic equation:**\[ M_x + Fe^{2+} \rightarrow M_x^{2+} + Fe \]The species oxidized is ___ and the oxidizing agent is ___.**Choices:**- ○ **M\_x, M\_x**- ○ **M\_x, Fe^{2+}**- ○ **Fe, Fe^{2+}**- ● **Fe^{2+}, M\_x**In this equation, a metal \( M_x \) reacts with \( Fe^{2+} \) ions, resulting in the oxidation of \( M_x \) to \( M_x^{2+} \) and the reduction of \( Fe^{2+} \) to elemental iron \( Fe \). **Note:**- **Oxidized Species:** A species that loses electrons and increases its oxidation state. In this reaction, \( Fe^{2+} \) is getting oxidized.- **Oxidizing Agent:** A substance that brings about the oxidation of another by being reduced itself. Here, \( M_x \) is the oxidizing agent as it gets oxidized.

Mg + Fe+2 → Mg+2 + Fespecies loss electrons are oxidation. Mg - 2e- → Mg+2 The species oxidized is Mg and the oxidizing agent is Fe+2. Fe+2 gains electrons to oxidize Mg so Fe+2 is the oxidizing agent.

Answered: Considering the following net ionic…

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Chemistry

Considering the following net ionic eauation: Mg+ Fe Mg+ Fe the species axidized isand the oxidizing agent is O ME ME O ME F O Fe:ME

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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