AP | A-Level | IB | NCERT 11 + 12 – FREE NOTES, RESOURCES AND VIDEOS!
IB® (SL and AHL)
YouTube Channel
YouTube Channel
@chemistry.student
S1.1 - Introduction to the particulate nature of matter S1.2 - The nuclear atom S1.3 - Electron configurations S1.4 - Counting particles by mass - The mole S1.5 - Ideal gases S2.1 - The ionic model S2.2 - The covalent model S2.3 - The metallic model S2.4 - From models to materials S3.1 - The periodic table - Classification of elements S3.2 - Functional groups - Classification of organic compounds R1.1 - Measuring enthalpy changes R1.2 - Energy cycles in reactions R1.3 - Energy from fuels R1.4 - Entropy and spontaneity AHL R2.1 - How much? The amount of chemical change R2.2 - How fast? The rate of chemical change R2.3 - How far? The extent of chemical change R3.1 - Proton transfer reactions R3.2 - Electron transfer reactions R3.3 - Electron sharing reactions R3.4 - Electron-pair sharing reactions

R3.2 - Electron transfer reactions

3.2.1 Redox and Oxidation States 3.2.2 Redox Half-Equations 3.2.3 Reactivity and Periodic Trends 3.2.4 Metal + Acid Reaction 3.2.5 Electrochemical Cells 3.2.6 Primary (Voltaic) Cells 3.2.7 Secondary (Rechargable) Cells 3.2.8 Electrolysis 3.2.9 Oxidation of Alcohol 3.2.10 Reduction of Organic Compounds 3.2.11 Reduction of Alkenes and Alkynes 3.2.12 Standard Electrode Potential + Hydrogen Electrode (AHL) 3.2.13 Standard Cell Potential, Ecell (AHL) 3.2.14 ∆G and Ecell (AHL) 3.2.15 Electrolysis of Aqeuous Solutions (AHL) 3.2.16 Electroplating and Electrode Reactions (AHL)

Electroplating and Electrode Reactions HL Only

Specification Reference R3.2.16

Quick Notes

  • Electroplating uses an electrolytic cell to deposit a thin metal layer onto an object.
  • The object to be plated is the cathode (negative electrode).
  • The anode is usually made of the metal being plated.
  • The electrolyte is a solution containing ions of the plating metal.
  • Reduction occurs at the cathode where metal ions gain electrons and are deposited.
  • Oxidation occurs at the anode where metal atoms lose electrons to replenish ions in solution.

Full Notes

Electroplating is a process that uses electrolysis to coat the surface of a metal object with a thin layer of another metal.

It’s widely used for a variety of reasons - such as to improve the appearance or prevent corrosion.

Basic Setup of an Electrolytic Cell for Electroplating

IB Chemistry HL electroplating setup showing cathode as object, silver anode, and electrolyte solution.

Components:

Current flow: Electrons flow from the anode to the cathode via external circuit.

Example: Silver Electroplating

Example Silver Electroplating

Cathode (reduction): Ag+(aq) + e⁻ → Ag(s)
(Silver ions from solution are deposited on the object)

Anode (oxidation): Ag(s) → Ag+(aq) + e⁻
(Silver anode gets smaller and Ag+ replenished in solution)

Net result: A thin layer of silver builds up on the cathode.

Other Common Electroplating Reactions

Summary