CHE1143_13MW_Alfaro

Foundations of Electrochemistry00:00:22

Explanation of half-cells, where oxidation (loss of electrons) and reduction (gain of electrons) occur simultaneously. Key concepts include the wire connection for electron flow and the salt bridge for charge balance.

Redox Reactions00:01:35

Detailed overview of the redox reaction, utilizing the mnemonics OIL (Oxidation Is Loss) and RIG (Reduction Is Gain) to identify how electrons are transferred between half-reactions to form a balanced overall chemical reaction.

Galvanic Cells00:03:52

Description of galvanic (voltaic) cells, which generate electricity spontaneously. These are the fundamental principles behind various batteries, featuring negative anodes and positive cathodes.

Electrolytic Cells00:05:15

Introduction to electrolytic cells, which require an external power source to drive non-spontaneous chemical reactions. These cells operate in reverse of galvanic cells, with flipped electrode charges.

Calculating Standard Electrode Potential00:06:49

Explanation of E-not values used to predict cell voltage. By subtracting the anode potential from the cathode potential, engineers can determine the total voltage of a system, demonstrated with a copper-zinc cell example resulting in 1.10V.