**Question:**Identify the species being oxidized and reduced in the following reaction: \[ \text{Cr}^+ + \text{Sn}^{4+} \rightarrow \text{Cr}^{3+} + \text{Sn}^{2+} \]**Options:**- ○ \(\text{Cr}^+: \text{reduced}, \text{Sn}^{4+}: \text{oxidized}\)- ○ Neither is being oxidized or reduced- ● \(\text{Cr}^+: \text{oxidized}, \text{Sn}^{4+}: \text{reduced}\) (Correct choice)**Explanation:**To determine which species is oxidized and which is reduced, examine the changes in oxidation states: - **Oxidation** involves an increase in oxidation state. Here, \(\text{Cr}^+\) becomes \(\text{Cr}^{3+}\), indicating that chromium is oxidized.- **Reduction** involves a decrease in oxidation state. Here, \(\text{Sn}^{4+}\) becomes \(\text{Sn}^{2+}\), indicating that tin is reduced.The correct answer is that \(\text{Cr}^+\) is oxidized and \(\text{Sn}^{4+}\) is reduced.

Oxidation process involves the loss of electrons Reduction process involves the gain of electrons

Identify the species being oxidized and reduced in the following reaction: Cr* + Sn4+- 3++Sn2+ O Crt: reduced, Sn4*: oxidized Neither is being oxidized or reduced O Cr*: oxidized, Sn4*: reduced

Identify the species being oxidized and reduced in the following reaction: Cr* + Sn4+- 3++Sn2+ O Crt: reduced, Sn4: oxidized Neither is being oxidized or reduced O Cr: oxidized, Sn4*: reduced

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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