This document provides an overview of electrochemistry, including definitions of key terms like oxidation, reduction, oxidizing agent, and reducing agent. It discusses different types of electrochemical cells and batteries, how they work, and examples like zinc-copper cells. Standard reduction potentials and how to calculate cell voltages are explained. Methods for balancing redox reactions are also covered.

1. ELECTROCHEMISTRY Chapter 18 SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

10. Anode Cathode Basic Concepts of Electrochemical Cells

14. Terms Used for Voltaic Cells

17. TABLE OF STANDARD REDUCTION POTENTIALS 2 To determine an oxidation from a reduction table, just take the opposite sign of the reduction! E o (V) Cu 2+ + 2e- Cu +0.34 2 H + + 2e- H 0.00 Zn 2+ + 2e- Zn -0.76 oxidizing ability of ion reducing ability of element

20. E o for a Voltaic Cell Cd --> Cd 2+ + 2e- or Cd 2+ + 2e- --> Cd Fe --> Fe 2+ + 2e- or Fe 2+ + 2e- --> Fe All ingredients are present. Which way does reaction proceed?

23. Charging a Battery When you charge a battery, you are forcing the electrons backwards (from the + to the -). To do this, you will need a higher voltage backwards than forwards. This is why the ammeter in your car often goes slightly higher while your battery is charging, and then returns to normal. In your car, the battery charger is called an alternator. If you have a dead battery, it could be the battery needs to be replaced OR the alternator is not charging the battery properly.

29. H 2 as a Fuel Cars can use electricity generated by H 2 /O 2 fuel cells. H 2 carried in tanks or generated from hydrocarbons