Here's a breakdown:
* Reduction: The process of gaining electrons.
* Oxidation: The process of losing electrons.
* Cathode: The electrode where reduction occurs.
* Anode: The electrode where oxidation occurs.
Key points to remember:
* Electrons flow from the anode to the cathode.
* In a galvanic (voltaic) cell, the cathode is the positive electrode. This is because electrons are flowing towards it from the anode.
* In an electrolytic cell, the cathode is the negative electrode. This is because an external power source forces electrons to flow towards it.
Example:
In a simple battery, the cathode is often made of a metal like copper. During the battery's operation, copper ions from the electrolyte solution gain electrons at the cathode, reducing them to copper metal. This is represented by the following half-reaction:
Cu²⁺(aq) + 2e⁻ → Cu(s)
