ElectroChemistry 06 : Electrolysis OR ElectroChemical Cell : Introduction - Product at Electrode

Sure, I can help with that. Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction ("redox") reaction.

A redox reaction is a kind of chemical reaction in which the oxidation states of atoms are changed. Any such reaction involves both a reduction process and a complementary oxidation process, two key concepts involved with electron transfer processes.

Electrolysis is an electrochemical process in which electrical energy is the driving force of chemical reactions. Substances are decomposed, by passing a current through them, into simpler substances when an electric current is passed through them in solution or molten form.

An electrochemical cell is a device capable of either generating electrical energy from chemical reactions or using electrical energy to cause chemical reactions. The electrochemical cells which generate an electric current are called voltaic cells or galvanic cells and those that generate chemical reactions, via electrolysis for example, are called electrolytic cells.

In terms of the products at the electrode, it depends on the specific reactions occurring. In a simple electrolytic cell using sodium chloride, for example, the products would be sodium at the cathode and chlorine gas at the anode.

1. At the anode (where oxidation occurs), chloride ions lose electrons to become chlorine gas. This is represented by the half-reaction: 2Cl- -> Cl2 + 2e-

2. At the cathode (where reduction occurs), sodium ions gain electrons to become sodium atoms. This is represented by the half-reaction: Na+ + e- -> Na

I hope this helps! Let me know if you have any other questions.