When writing oxidation or reduction half reactions, always place the correct number of electrons on the side with the largeroxidation 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 theequation.1) MgMg2+2) H₂→ 2H*3) Cu²+ → Cuº4) 2Br→ Br₂⁰5) Al6) Cu*→ Cu→ A1³+

Balanced each reaction by placing correct number of electrons ---

(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

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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