Atoms and Elements: Represented by symbols in the periodic table.
Compounds: Substances with two or more different atoms chemically bonded (e.g., H2O).
Mixtures: Combinations of elements/compounds not chemically bonded (e.g., air).
Filtration: Separates solids from liquids.
Distillation: Separates liquids based on boiling points.
States of Matter
Solid: Particles vibrate in fixed positions.
Liquid: Particles move past each other.
Gas: Particles far apart and move randomly.
State Changes: Physical processes; no new substances are made.
State Symbols: (s) solid, (l) liquid, (g) gas, (aq) aqueous.
Atomic Theories
JJ Thompson: Plum pudding model.
Ernest Rutherford: Nucleus discovery.
Niels Bohr: Electron shells.
James Chadwick: Neutrons.
The Periodic Table
Atomic Number: Number of protons.
Mass Number (RAM): Protons + Neutrons.
Isotopes: Same element, different neutrons.
Arrangement: Based on atomic number and properties.
Electron Configuration
Electrons fill shells: Each shell has a maximum capacity (2, 8, 8, 2).
Transition metals have complex configurations.
Chemical Bonding
Metallic Bonding: Delocalized electrons around a lattice.
Ionic Bonding: Metal donates electrons to nonmetals.
Ionic compounds form crystal lattices and conduct electricity when liquid.
Covalent Bonding: Nonmetals share electrons.
Simple covalent have low melting points; giant covalent (e.g., diamond) have high melting points.
Molecular Ions: E.g., hydroxide (OH-).
Quantitative Chemistry
Conservation of Mass: Mass is conserved in reactions.
Relative Atomic/Formular Mass: Sum of atomic masses.
Moles: Measure of substance amount.
Equation: Moles = Mass/RAM.
Chemical Changes
Reactivity Series: Metals compared for reactivity.
Displacement: More reactive metal displaces less reactive.
Reduction/Oxidation (Redox): OIL RIG - Oxidation Is Loss, Reduction Is Gain of electrons.
Acids and Bases: Neutralization results in salt and water.
Energy Changes
Exothermic: Releases energy (e.g., combustion).
Endothermic: Absorbs energy.
Energy Profiles: Show energy changes in reactions.
Triple Only
Nanoparticles: High surface-to-volume ratio, significant in reactions.
Titrations: Determine concentrations in solutions.
Electrolysis: Splits compounds using electricity; metals purified/extracted.
Fuel Cells: Use hydrogen and oxygen to produce electricity.
Conclusion
This summary provides an overview of key concepts for AQA GCSE Chemistry Paper 1. Understanding these foundational principles is crucial for success in the exam.