Here's a breakdown:

* Anode: The electrode where oxidation occurs (loss of electrons).

* Cathode: The electrode where reduction occurs (gain of electrons).

The specific reactions happening at each electrode depend on the type of electrochemical cell:

* Galvanic Cells (Battery): These cells convert chemical energy into electrical energy.

* The anode is the negative electrode, and the cathode is the positive electrode.

* The oxidation reaction at the anode provides electrons that flow through an external circuit to the cathode, where they are used in the reduction reaction.

* Electrolytic Cells: These cells use electrical energy to drive non-spontaneous chemical reactions.

* The anode is the positive electrode, and the cathode is the negative electrode.

* An external power source pushes electrons from the anode to the cathode, forcing the oxidation and reduction reactions to occur.

In summary:

Electrochemical cells are designed to separate oxidation and reduction reactions to generate electrical energy (galvanic cells) or drive non-spontaneous chemical reactions (electrolytic cells). These reactions happen at the electrodes: the anode for oxidation and the cathode for reduction.