Electrochemistry Mind Map

A galvanic or voltaic cell is an electrochemical cell in which a spontaneous redox reaction converts chemical energy into electrical energy.

For any cell notation, read the left half-cell as anode and the right half-cell as cathode unless the question gives a different convention. Link oxidation with anode and reduction with cathode before writing reactions.

Standard electrode potential is the potential of an electrode measured under standard conditions relative to the standard hydrogen electrode, whose potential is assigned zero volts.

Before substitution, identify cathode as the half-cell with higher reduction potential. Do not mechanically take left minus right unless the cell notation has already been confirmed.

The Nernst equation relates the electrode potential or cell EMF to concentration, pressure, temperature, and reaction quotient for a redox reaction.

Write the balanced cell reaction before writing Q. This prevents most concentration-ratio and electron-number errors.

Conductivity is the conductance of an electrolyte solution of unit length and unit cross-sectional area, while molar conductivity is the conductance due to all ions produced by one mole of electrolyte in solution.

Always check the units of kappa and concentration before substitution. Most numerical errors in this topic are unit-conversion errors.

Electrolysis is the use of electrical energy to drive a non-spontaneous chemical reaction, and Faraday's laws relate the amount of substance deposited or liberated to the quantity of electricity passed.

For numerical questions, write the half-reaction first. The number of electrons in that half-reaction decides the mole ratio between electrons and product.

Batteries and fuel cells are electrochemical devices that supply electrical energy through redox reactions, while corrosion is an unwanted electrochemical oxidation process of metals.

For application questions, mention the redox role first, then the device condition: rechargeable for secondary cells, continuous reactant supply for fuel cells, and moisture plus oxygen for corrosion.