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(Remember: Reduction - gaining - electrons on the left, Oxidation - losing - electrons on the right) C) Balance each of the following half reactions by placing the correct number of electrons into the equation. 1) Mg° → Mg²+ 2) H₂ → 2H* 3) Cu²+ → Cuº 4) 2Br → Br₂° 5) Al 6) Cu → Cu →A1³+

(Remember: Reduction - gaining - electrons on the left, Oxidation - losing - electrons on the right) C) Balance each of the following half reactions by placing the correct number of electrons into the equation. 1) Mg° → Mg²+ 2) H₂ → 2H* 3) Cu²+ → Cuº 4) 2Br → Br₂° 5) Al 6) Cu → Cu →A1³+

Chemistry
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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When writing oxidation or reduction half reactions, always place the correct number of electrons on the side with the larger oxidation state. The reaction must also be balanced for mass (the number of atoms) and for charge. (Remember: Reduction - gaining - electrons on the left, Oxidation - losing - electrons on the right) C) Balance each of the following half reactions by placing the correct number of electrons into the equation. 1) Mg Mg2+ 2) H₂ → 2H* 3) Cu²+ → Cuº 4) 2Br → Br₂⁰ 5) Al 6) Cu* → Cu → A1³+
Transcribed Image Text:When writing oxidation or reduction half reactions, always place the correct number of electrons on the side with the larger oxidation state. The reaction must also be balanced for mass (the number of atoms) and for charge. (Remember: Reduction - gaining - electrons on the left, Oxidation - losing - electrons on the right) C) Balance each of the following half reactions by placing the correct number of electrons into the equation. 1) Mg Mg2+ 2) H₂ → 2H* 3) Cu²+ → Cuº 4) 2Br → Br₂⁰ 5) Al 6) Cu* → Cu → A1³+
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