GCSE Chemistry (Triple) AQA
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107 topics in 12 modules
☑️ Atomic Structure and the Periodic Table 13 topics
- Atomic Structure: Atoms
- Atomic Structure: Elements
- Atomic Structure: Compounds
- Atomic Structure: Chemical Equations
- Atomic Structure: Mixtures and Chromatography
- Atomic Structure: Distillation
- Atomic Structure: History of the Atom
- Atomic Structure: Electronic Structure
- The Periodic Table
- The Periodic Table: Metals and Non-Metals
- The Periodic Table: Group 1
- The Periodic Table: Group 7
- The Periodic Table: Group 0
☑️ Crude oil, hydrocarbons and alkanes 11 topics
- Overview of Crude Oil: Properties, Extraction and Significance
- Fractional Distillation: Principal and Process
- Understanding Hydrocarbons: Definition and Types
- Alkanes: Definition, Properties and Examples
- Structural Formulas and Molecular Formulas in Hydrocarbons
- General Formula of Alkanes and Its Interpretation
- Homologous Series and Isomers in Hydrocarbons
- Combustion Reactions of Alkanes
- Implications of Uncontrolled Combustion of Hydrocarbons: Air Pollution
- Introduction to the Petrochemical Industry: Use of Alkanes and Crude Oil
- Environmental Concerns and Sustainable Practices Related to the Use of Crude Oil and Hydrocarbons
☑️ Isotopes 11 topics
- Introduction to Isotopes
- The concept of Stable and Unstable Isotopes
- How Isotopes are Formed
- Definition of Isotopic Mass and Atomic Number
- Differences and Similarities among Isotopes
- Chemical behaviour of Isotopes
- Uses of Isotopes: Medical and Industrial Applications
- Radioactive Decay and Isotopes
- Calculation of Relative Isotopic Mass
- Risks and Safety Measures Around Radioactive Isotopes
- Environmental Impact of Using Isotopes
☑️ Bonding, Structure and Properties of Matter 12 topics
- Matter: Formation of Ions
- Matter: Ionic Bonding
- Matter: Ionic Compounds
- Matter: Covalent Bonding
- Matter: Simple Molecular Substances
- Matter: Polymers
- Matter: Giant Covalent Structures
- Matter: Carbon Allotropes
- Matter: Metallic Bonding
- Matter: States of Matter
- Matter: Changing State
- Matter: Nanoparticles
☑️ Quantitative Chemistry 8 topics
- Quantitative Chemistry: Relative Formula Mass
- Quantitative Chemistry: The Mole
- Quantitative Chemistry: Conservation of Mass
- Quantitative Chemistry: Limiting Reactants
- Quantitative Chemistry: Gases and Solutions
- Quantitative Chemistry: Concentration Calculations
- Quantitative Chemistry: Atom Economy
- Quantitative Chemistry: Percentage Yield
☑️ Chemical Changes 8 topics
- Chemical Changes: Acids and Bases
- Chemical Changes: Titrations
- Chemical Changes: Strong and Weak Acids
- Chemical Changes: Reactions of Acids
- Chemical Changes: The Reactivity Series
- Chemical Changes: Separating Metals from Metal Oxides
- Chemical Changes: Redox Reactions
- Chemical Changes: Electrolysis
☑️ Energy Changes 6 topics
- Energy Changes: Exothermic Reactions
- Energy Changes: Endothermic Reactions
- Energy Changes: Bond Energies
- Energy Changes: Cells
- Energy Changes: Batteries
- Energy Changes: Fuel Cells
☑️ The Rate and Extent of Chemical Change 6 topics
- Rates of Reactions
- Factors Affecting Rates of Reactions
- Measuring Rates of Reactions
- Finding Reaction Rates from Graphs
- Rates of Reactions: Reversible Reactions
- Le Chatelier's Principle
☑️ Organic Chemistry 9 topics
- Organic Chemistry: Hydrocarbons
- Organic Chemistry: Fractional Distillation
- Organic Chemistry: Crude Oil
- Organic Chemistry: Alkenes
- Organic Chemistry: Addition Polymers
- Organic Chemistry: Alcohols
- Organic Chemistry: Carboxylic Acids
- Organic Chemistry: Condensation Polymers
- Organic Chemistry: Naturally Occurring Polymers
☑️ Chemical Analysis 7 topics
- Chemical Analysis: Purity
- Chemical Analysis: Formulations
- Chemical Analysis: Paper Chromatography
- Chemical Analysis: Tests for Gases
- Chemical Analysis: Tests for Anions
- Chemical Analysis: Test for Cations
- Chemical Analysis: Flame Emission Spectroscopy
☑️ Atmosphere Chemistry 5 topics
- Atmosphere Chemistry: The Evolution of the Atmosphere
- Atmosphere Chemistry: Greenhouse Gases
- Atmosphere Chemistry: Climate Change
- Atmosphere Chemistry: Carbon Footprints
- Atmosphere Chemistry: Air Pollution
☑️ Using Resources 11 topics
- Using Resources: Ceramics, Composites and Polymers
- Using Resources: Properties of Materials
- Using Resources: Corrosion
- Using Resources: Finite Resources
- Using Resources: Renewable Resources
- Using Resources: Reuse and Recycling
- Using Resources: Life Cycle Assessments
- Using Resources: Potable Water
- Using Resources: Waste Water Treatment
- Using Resources: The Haber Process
- Using Resources: NPK Fertilisers
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GCSE Chemistry (Triple) AQA Revision Content
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GCSE Chemistry (Triple) AQA - Atomic Structure and the Periodic Table - Atomic Structure: Atoms Content Preview
Atomic Structure and the Periodic Table
Atomic Structure: Atoms
Understanding Atoms
- An atom is the smallest part of an element that can exist, typically around a hundred millionth of a centimetre across.
- Every atom is made of three fundamental particles: protons, neutrons, and electrons.
- The nucleus at the centre of the atom contains the protons and neutrons.
- The electrons move in energy levels around the nucleus, also known as electron shells.
Atomic Number & Mass Number
- The atomic number (Z) of an atom is the number of protons in its nucleus. It gives the identity of the atom.
- The mass number (A) is the total number of protons and neutrons in the nucleus.
- An atom is neutral because it contains equal numbers of protons (positively charged) and electrons (negatively charged).
Isotopes & Ionisation
- Isotopes are atoms of the same element with different numbers of neutrons, and hence different mass numbers.
- Isotopes of an element have identical chemical reactions because they have the same electron arrangement.
- Ionisation occurs when an atom gains or loses electrons, becoming an ion. Positive ions (cations) form by losing electrons, negative ions (anions) form by gaining electrons.
Atomic Model Evolution
- The atomic model has changed as scientists have discovered new information.
- JJ Thomson’s 'Plum Pudding' Model discovered that atoms contain electrons. However, he believed these were embedded in a sphere of positive charge.
- Rutherford's Alpha Particle Scattering Experiment showed that most of the atom is empty space with a tiny, dense, positive nucleus.
- Niels Bohr improved Rutherford's model by placing electrons in specific orbits, or energy levels. The modern atomic model was based on Bohr's work.
Using Mass Spectrometry
- Mass spectrometry can be used to find relative isotopic abundance and identify elements.
- This method supports theories about atomic structure and isotopes.
- It helps to calculate the relative atomic mass of an element from the relative abundances of its isotopes.
Understanding Energy Levels
- Electrons fill the energy levels in a specific order – from lower to higher.
- Each energy level can hold only a certain number of electrons: 2 in the first level and generally 8 in the others.
- Electron configuration (distribution of electrons in energy levels) affects the chemical properties of atoms.
Question: What differentiates isotopes of the same element from each other, and how does this difference however, not affect their chemical reactions?
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