Chemistry is the study of matter, its composition, structure, properties,
and the changes it undergoes. Both JAMB and WAEC test students on theoretical knowledge,
problem-solving skills, and practical applications. Mastering Chemistry requires understanding
basic principles, practicing calculations, and familiarizing yourself with laboratory techniques.

1. Structure of the Atom

– Subatomic particles: protons, neutrons, and electrons.
– Atomic number, mass number, and isotopes.
– Electronic configuration, orbitals, and periodic table arrangement.

Example Question: The electronic configuration of sodium is 1s² 2s² 2p⁶ 3s¹.

2. Chemical Bonding

– Types: ionic, covalent, metallic bonds.
– Properties of compounds depending on bond type.
– Intermolecular forces: van der Waals forces, hydrogen bonding.

Example: Which of these has hydrogen bonding? Answer: NH₃.

3. States of Matter

– Kinetic theory of gases and assumptions.
– Gas laws: Boyle’s law, Charles’s law, and the Ideal Gas Law (PV=nRT).
– Differences between solids, liquids, and gases.

Example Calculation: A gas at 2 atm and 300 K is heated to 600 K at constant volume.
New pressure = 4 atm.

4. Stoichiometry and Mole Concept

– Mole and Avogadro’s number.
– Balancing equations.
– Limiting reagents, percentage yield, and empirical formula.

Example: 10 g of CaCO₃ decomposes to give CO₂ at STP.
Moles = 0.1, Volume = 2.24 dm³.

5. Periodic Table and Periodicity

– Arrangement in groups and periods.
– Trends in atomic radius, ionization energy, electronegativity.
– Properties of alkali metals, halogens, and noble gases.

6. Chemical Reactions

– Types: combination, decomposition, single displacement, double displacement, redox reactions.
– Energy changes: exothermic and endothermic reactions.
– Factors affecting reaction rate: temperature, catalysts, concentration, surface area.

7. Acids, Bases and Salts

– Definitions (Arrhenius, Bronsted-Lowry, Lewis).
– Strong and weak acids and bases.
– Neutralization and titration calculations.
– Preparation of salts and uses.

Example: Calculate pH of 0.01M HCl.
[H+] = 0.01, pH = 2.

8. Organic Chemistry

– Hydrocarbons: alkanes, alkenes, alkynes.
– Functional groups: alcohols, carboxylic acids, esters, amines.
– Nomenclature according to IUPAC rules.
– Reactions: substitution, addition, combustion, esterification.

Example: Which hydrocarbon decolourizes bromine water? Answer: Alkenes.

9. Electrochemistry

– Electrolysis of molten and aqueous solutions.
– Faraday’s laws of electrolysis and calculations.
– Electrochemical cells, Daniell cell, batteries.
– Applications in industry: electroplating, purification of metals.

10. Industrial Chemistry

– Manufacture of ammonia (Haber process).
– Manufacture of sulphuric acid (Contact process).
– Manufacture of sodium hydroxide, soap, glass, and cement.
– Environmental impact of industrial processes.

11. Practical Chemistry (WAEC Focus)

– Identification of gases: O₂ (glows splint), CO₂ (limewater), H₂ (pops with flame), NH₃ (turns red litmus blue), Cl₂ (bleaches litmus).
– Qualitative analysis of cations: Na⁺, Ca²⁺, Fe²⁺, Fe³⁺, Cu²⁺.
– Qualitative analysis of anions: SO₄²⁻, NO₃⁻, Cl⁻, CO₃²⁻.
– Acid-base titration procedures and calculations.

12. Exam Tips

1. Practice past JAMB and WAEC questions regularly.
   2. Pay attention to calculations in stoichiometry, gas laws, and mole concepts.
   3. Revise practical chemistry experiments, observations, and inferences.
   4. Manage time wisely: attempt simple questions first.
   5. Stay calm, confident, and disciplined during exams.

Conclusion

To succeed in JAMB and WAEC Chemistry, students must develop a solid
understanding of theory, practice problem-solving daily, and become familiar with laboratory
procedures. Consistency, discipline, and smart study habits will ensure excellent performance.