Applicable for A-Level, IB, DSE, AP-Level Exams

Atomic Structure    Stoichiometry    Bonding    Energetics    Kinetics    Equilibria    Redox    Group 2    Group 7    Alkanes    Alkenes and Alcohols    Organic Analysis    Thermodynamics    Kinetics 2    Equilibrium Constant Kp    Electrode Potentials & Cells    Acids, Bases & Buffer    Periodicity    Transition Metals    Inorganic Compounds in Acqeous Solutions    Optical Isomerism    Aldehydes & Ketones    Carboxylic Acids & Derivatives    Aromatic Chemistry    Amines    Polymers    Amino Acids, Proteins & DNA    Organic Synthesis    NMR    Chromatography   

Electrode Potentials & Cells

Electrode Potentials

Electrochemical cells can be made from 2 different metals dipped in salt solutions of their own ions and connected by a wire. Electrons flow due to oxidation on one electrode and reduction in another electrode. The electrode the electrons flow to is the positive electrode and the electrode the electrons flow from is the negative electrode.

When drawing the conventional representation of cells, it is important to draw the more negative elctrode potential on the left and the less negative on the right. The left one being the half cell that is oxidised (i.e. lost electrons to the positive electrode).

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Commercial Applications of Electrochemical Cells

Commercial applicaions of electrochemical cells include lithium ion batteries, rechargeable cells as well as a more environmentally-friendly hydrogen-oxygen fuel cell.

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