5.111SC | Fall 2014 | Undergraduate

Principles of Chemical Science

Unit IV: Transition Metals & Oxidation-Reduction Reactions

Lecture 26: Chemical and Biological Oxidations

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Image excerpted from Lecture 26 Notes 

  1. Relationship between Cell Potential and Gibbs Free Energy
  2. Meaning of Standard Reduction Potentials
  3. Nernst Equation

Lecture Video

Viewers are introduced to agents of oxidation and agents of reduction. Are oxidizing agents really that bad for you? Hear from Professor John Essigmann about the double-edged sword that is oxidation-reduction. Oxidizing agents can protect us from disease but can also damage our genetic material. Friend or foe, you decide.

Lecture Notes

Notes for Lecture 26 (PDF)

Clicker Questions

Lecture 26 Clicker Questions (PDF)

Textbook Reading

Galvanic and Electrolytic Cells Sections 13.6–13.12 Sections 12.6–12.12

Linking Oxidation To DNA Damage

John Essigmann describes how oxidation reactions in our bodies are both essential for life and responsible for cell damage that can potentially lead to cancer. John’s research focuses on studying how cells respond to toxins that cause oxidative damage to DNA.

John Essigmann’s Personal Story

John Essigmann describes how an early industry experience doing real science pushed him to pursue a career as a professor and professional scientist. He also realizes that the Scientific Method is a framework that can be applied to better understanding questions in the real world.

Problems and Solutions

Problems for Lecture 26 (PDF)

Solutions for Lecture 26 (PDF)

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Fall 2014
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