Chemistry
Atomic structure, bonding, periodic table, reactions, thermochemistry, acids & bases, equilibrium, kinetics, and industrial chemistry — all 13 exam topics.
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Your Chemistry Progress
Complete all 13 topics. Each has full notes, key formulas, and 8 quick-fire MCQs.
Topics
1. Structure of Atom
Sub-atomic particles, atomic models, electronic configuration, isotopes.
2. Chemical Bonding
Ionic, covalent, metallic, hydrogen bonds. Polar vs non-polar.
3. Elements, Compounds & Mixtures
Classification of matter, separation techniques, colloids vs solutions.
4. Periodic Table
Groups, periods, periodic trends, key group properties.
5. States of Matter & Gas Laws
Solid, liquid, gas; changes of state; Boyle's, Charles's, ideal gas law.
6. Thermochemistry
Exo/endothermic, enthalpy, Hess's Law, Q = mcΔT.
7. Environmental Chemistry
Air & water pollution, greenhouse effect, ozone layer, acid rain.
8. Mole, Molarity & Solutions
Mole concept, Avogadro's number, molarity, colligative properties.
9. Acids & Bases
Arrhenius, Brønsted-Lowry, Lewis theories, pH scale, neutralisation.
10. Equilibrium
Le Chatelier's principle, equilibrium constant Kc, reversible reactions.
11. Chemical Reactions
Reaction types, redox (OIL RIG), balancing equations, precipitation.
12. Industrial & Electrochemistry
Haber process, Contact process, electrolysis, galvanic cells, fractional distillation.
13. Chemical Kinetics
Rate of reaction, collision theory, activation energy, factors affecting rate.
Important Values to Memorise
6.022 × 10²³
Avogadro's Number (per mole)
22.4 L/mol
Molar volume of gas at STP
18 g/mol
Molar mass of H₂O
58.5 g/mol
Molar mass of NaCl
98 g/mol
Molar mass of H₂SO₄
44 g/mol
Molar mass of CO₂
4.18 J/g°C
Specific heat capacity of water
450°C, 200 atm
Haber process conditions (iron catalyst)
pH 7
Neutral solution at 25°C
R = 8.314 J/mol·K
Universal gas constant
1869
Mendeleev's Periodic Table
1987
Montreal Protocol — phased out CFCs
Key Formulas at a Glance
| Formula | Meaning |
|---|---|
| n = m / M | Moles = Mass ÷ Molar Mass |
| M = n / V | Molarity = moles ÷ volume (litres) |
| PV = nRT | Ideal Gas Law |
| P₁V₁ = P₂V₂ | Boyle's Law (constant T) |
| V₁/T₁ = V₂/T₂ | Charles's Law (constant P) |
| pH = −log[H⁺] | pH from hydrogen ion concentration |
| Q = mcΔT | Heat energy = mass × specific heat × ΔT |
| Kc = [products]/[reactants] | Equilibrium constant expression |
Famous Chemists
⚛️
John Dalton (1808)
Atomic theory — atoms are indivisible, indestructible spheres
🔋
J.J. Thomson (1897)
Discovered electron — plum pudding model
🥇
Ernest Rutherford (1911)
Gold foil experiment — discovered the nucleus
🌀
Niels Bohr (1913)
Planetary model — electrons in fixed energy levels
📊
Dmitri Mendeleev (1869)
Periodic table by atomic mass; predicted missing elements
🔢
Avogadro
Avogadro's number = 6.022 × 10²³ particles per mole
⚡
Michael Faraday
Laws of electrolysis — mass deposited ∝ charge passed
⚖️
Le Chatelier
Principle of equilibrium shift under applied stress
💧
Arrhenius
Acids produce H⁺, bases produce OH⁻ in water
🧪
Brønsted & Lowry
Acid = proton donor, Base = proton acceptor