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✅ Atomic Structure & Periodic Table
✅ Bonding, Structure & Properties
✅ Quantitative Chemistry
✅ Chemical Changes
✅ Energy Changes
🧱 1. Atomic Structure & the Periodic Table
🔬 Structure of the Atom
Protons = +1 charge
Neutrons = 0
Electrons = −1
Key facts:
Atomic number = protons
Mass number = protons + neutrons
Isotopes = same element, different neutrons
⚛️ Electronic Structure
Electrons fill shells: 2, 8, 8…
Reactivity depends on outer shell electrons
📊 Periodic Table
Groups to know:
Group 1 → more reactive down group
Group 7 → less reactive down group
Group 0 → unreactive
🔗 2. Bonding, Structure & Properties
🧲 Types of Bonding
Ionic Bonding
Metal + non-metal
Electrons transferred → ions
Covalent Bonding
Non-metals share electrons
Metallic Bonding
Positive ions + delocalised electrons
🧊 Properties of Structures
Type Key Properties
Ionic High mp, conducts when molten
Simple molecular Low mp, no conduction
Giant covalent Very strong, high mp
Metals Conduct electricity
🧮 3. Quantitative Chemistry
⚖️ Key Equations (MUST KNOW)
Moles:
moles=
Mr
mass
Concentration:
concentration=
volume
moles
Gas volume:
1 mole gas = 24 dm³
🧪 Required Practical: Making Salts
Methods:
Acid + metal
Acid + alkali (titration)
Crystallisation steps:
Evaporate
Cool
Filter
⚡ 4. Chemical Changes
🔥 Reactivity Series
8
Key ideas:
More reactive metal displaces less reactive
Metals + acids → salt + hydrogen
⚡ Electrolysis
Molten:
Metal → cathode
Non-metal → anode
Aqueous:
Hydrogen may form instead of metal
🧪 Required Practical: Electrolysis
Identify gases formed
Write half equations
🌡️ 5. Energy Changes
🔥 Exothermic vs Endothermic
Exothermic:
Releases energy
Temperature increases
Endothermic:
Takes in energy
Temperature decreases
💥 Bond Energy Calculations
Energy change=energy in−energy out
🧠 MOST IMPORTANT THINGS TO MEMORISE
✅ Definitions:
Isotope
Ionic bond
Covalent bond
Exothermic / Endothermic
✅ Equations:
Moles
Concentration
Energy change
✅ Required practicals:
Making salts
Electrolysis
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