Chapter 1: Introduction

• Electrochemical cells consist of an anode (oxidation) and cathode (reduction) connected by a wire.

  • Electrons flow from anode to cathode spontaneously due to energy difference.

• Voltage difference is the electrical energy difference between electrodes, measured in volts.

  • Volt defined as energy required to impart 1 joule to 1 coulomb charge.

• Cell potential (e subcell) is the electromotive force of the cell.

• Standard cell potential (E naught) is for 1 molar solutions at 25 degrees c.

• Relationship between delta g, equilibrium constant k, and standard free energy discussed.

Chapter 2: Half Cell Potential

• Equilibrium constant (kth) related to free energy of the system.

• Half cell potential measures energy of electrons in an electrochemical reaction.

• Half cell potential associated with standard reduction potentials.

• Standard reduction potentials measured relative to standard hydrogen electrode.

Chapter 3: Energy Of Electrons

• Standard reduction potentials indicate electron energy levels.

• More positive potentials indicate stronger oxidizing agents, more negative for reducing agents.

• Spont