AQA GCSE Combined Science Chemistry Paper 1 Higher Tier Checklist

Overview and Reference Material

• Target Examination: AQA GCSE Combined Science 9-1 Higher Tier Chemistry Paper 1.

• Core Resource: The sub-topics and content refer specifically to the "AQA GCSE Combined Science 9-1 Higher complete revision and practice book" (ISBN: $978-1-382-00487-9$).

• Additional Resources: QR codes provided within the source material lead to BBC Bitesize topic pages for digital review.

• Higher Tier Designation: Content marked with HT is specifically for Higher Tier candidates and is not required for Foundation Tier students.

Topic: Atomic Structure and the Periodic Table

C1: The Atom

• Development of the Model of the Atom (Page 184): History of atomic theory, spanning from ancient concepts to modern quantum mechanics.

• Atoms and Particles (Page 185): Fundamental particles including protons, neutrons, and electrons.

• Drawing Atoms (Page 185): Representing atomic structure through electron shells and Bohr models.

• Elements and Compounds (Page 185): Distinguishing between pure substances consisting of one type of atom and substances formed from multiple elements chemically bonded.

• Isotopes (Page 185): Atoms of the same element with the same number of protons but different numbers of neutrons.

• Mixtures (Page 185): Combinations of substances that are not chemically joined and can be separated by physical means.

C4: The Periodic Table

• Development of the Periodic Table (Page 214): Evolution from Newlands' Octaves to Mendeleev’s table and the modern version based on atomic number.

• Sub-atomic Discoveries (Page 214): How the discovery of sub-atomic particles influenced the organization of the Periodic Table.

• Group 0 (Page 214): Properties and trends of the Noble Gases.

• Group 1 Elements (Page 215): Overview of the Alkali Metals.

• Group 1 Properties (Page 215): Physical and chemical characteristics of alkali metals.

• Group 7 Elements (Page 215): Overview of the Halogens.

• Group 7 Reactivity (Page 215): Trends in reactivity as you move down the group.

• Group 7 Displacement (Page 215): Reactions where a more reactive halogen displaces a less reactive one from its salt.

Topic: Bonding, Structure, and Properties of Matter

C2: Covalent Bonding

• Particle Model (Page 194): Fundamental understanding of particles in different states of matter.

• Covalent Bonding (Page 194): The sharing of electron pairs between non-metal atoms.

• Covalent Structures (Page 194): Identification of simple molecular and giant covalent structures.

• Covalent Structures Properties (Page 195): Explanation of melting points, boiling points, and electrical conductivity related to structure.

• Graphite (Page 195): A giant covalent structure of carbon with layers and delocalized electrons.

• Fullerenes (Page 195): Carbon molecules with hollow shapes, such as buckyballs and nanotubes.

• Graphene (Page 195): A single layer of graphite with unique properties.

C3: Ionic Bonding, Metallic Bonding, and Structure

• Ions (Page 204): Atoms that have gained or lost electrons to become charged.

• Ionic Bonding (Page 204): Electrostatic attraction between oppositely charged ions.

• Giant Ionic Lattice (Page 204): The regular repeating arrangement of ions in an ionic compound.

• Formulae (Page 204): Determining the chemical formulas of ionic compounds.

• Melting Points (Page 204): High melting points of ionic compounds due to strong electrostatic forces.

• Conductivity (Page 204): Why ionic compounds conduct electricity only when molten or in aqueous solution.

• Metals (Page 205): Bonding involving an array of positive ions in a sea of delocalized electrons.

• Malleability, Conductivity, and Melting Points (Page 205): Physical properties explained by metallic bonding.

• Alloys (Page 205): Mixtures of metals that are typically harder than pure metals due to distorted layer structures.

Topic: Quantitative Chemistry

C5: Quantitative Chemistry

• Conservation of Mass (Page 224): The principle that no atoms are lost or made during a chemical reaction.

• Decrease in Mass (Page 224): Explanations for mass loss, often due to gas escaping a non-enclosed system.

• Increase in Mass (Page 224): Explanations for mass gain, often due to a gaseous reactant (like oxygen) being incorporated into a solid.

• Balancing Symbol Equations (Page 224): Ensuring the number of atoms for each element is the same on both sides of the equation.

• State Symbols (Page 224): Use of $(s)$, $(l)$, $(g)$, and $(aq)$.

• Formula Mass (Page 224): Calculating relative formula mass ($M_r$).

• Ratios and Moles [HT] (Page 224): Calculating the number of moles using mass and molar mass.

• The Avogadro Constant [HT] (Page 224): The number of particles in one mole: $6.02 \times 10^{23}$.

• Using Balanced Equations [HT] (Page 225): Calculating masses of reactants or products based on stoichiometry.

• Excess and Limiting Reactants [HT] (Page 225): Identifying the reactant that is completely consumed and limits the amount of product formed.

• Concentrations (Page 225): Calculating concentration in $g/dm^3$ or $mol/dm^3$.

Topic: Chemical Changes

C6: Reactions of Metals

• Reactions of Metals (Page 234): General observations when metals react with water or acids.

• Reactivity Series (Page 234): The arrangement of metals based on their tendency to form positive ions.

• Metal Extraction (Page 234): Methods for obtaining metals from ores based on their position in the reactivity series (e.g., carbon reduction).

• Reduction and Oxidation (Page 234): Definitions in terms of oxygen gain/loss.

• Displacement Reactions (Page 235): More reactive metals replacing less reactive metals in compounds.

• Reactivity and Ions (Page 235): The relationship between metal atoms and the formation of cations.

• Ionic Equations [HT] (Page 235): Equations showing only the species that change in a reaction.

• Steps for Writing an Ionic Equation [HT] (Page 235): Procedural guide to removing spectator ions.

• Half Equations [HT] (Page 235): Describing what happens to each reactant during a redox process.

• Reduction and Oxidation: Electrons [HT] (Page 235): Definitions in terms of electron transfer (OIL RIG: Oxidation Is Loss, Reduction Is Gain).

C7: Reaction of Acids

• Acids and Alkalis (Page 244): Characterizing substances by pH and ion presence ($H^+$ and $OH^-$).

• Logarithmic Scales (Page 244): The relationship between pH change and the concentration of hydrogen ions.

• Indicators (Page 244): Substances used to determine pH (e.g., universal indicator, litmus).

• Strong and Weak Acids [HT] (Page 244): Distinction based on the degree of ionization in aqueous solution.

• Concentrated and Dilute Acids (Page 244): Distinction based on the amount of acid molecules dissolved in a specific volume of water.

• Salts (Page 245): Ionic compounds formed when the hydrogen in an acid is replaced by a metal or ammonium ion.

• Reactions of Acids (Page 245): Reactions with metals, bases, alkalis, and carbonates.

• Redox (Page 245): Involvement of reduction and oxidation in acid reactions.

• Alkalis and Base (Page 245): Bases are metal oxides/hydroxides; alkalis are water-soluble bases.

• Crystallisation (Page 245): Process of obtaining solid salt crystals from a solution.

C8: Electrolysis

• Electrolysis (Page 254): Decomposition of a liquid/solution using electricity.

• Electrolysis of Molten Compounds (Page 254): Breaking down simple ionic salts in liquid form.

• Half Equations [HT] (Page 254): Representation of electron loss at the anode and electron gain at the cathode.

• Electrolysis of Aqueous Solutions (Page 254): Determination of products based on the reactivity of water ions ($H^+$ and $OH^-$).

• Products at the Anode [Equations Part = HT] (Page 254): Identifying if oxygen or a halogen is produced.

• Products at the Cathode [Equations Part = HT] (Page 254): Identifying if hydrogen or a metal is produced.

• Electrolysis of Aluminum Oxide (Page 255): The industrial extraction of Aluminum using cryolite and carbon electrodes.

Topic: Energy Changes

C9: Energy Changes

• Energy Changes (Page 264): Classification of reactions as exothermic or endothermic.

• The Surroundings (Page 264): Measuring temperature changes in the environment to determine energy transfer.

• Reaction Profiles (Page 264): Diagrams showing activation energy ($E_a$) and the relative energies of reactants and products.

• Bonds – Breaking and Making [HT] (Page 265): Breaking bonds is endothermic; making bonds is exothermic.

• Bond Calculations [HT] (Page 265): Using bond energies to calculate the overall enthalpy change of a reaction.

Required Practicals

• Making Salts (Page 247): Preparation of a pure, dry sample of a soluble salt from an insoluble oxide or carbonate.

• Electrolysis of Aqueous Solutions (Page 257): Observing and identifying the products of the electrolysis of various salt solutions.

• Investigating Temperature Changes in Reacting Solutions (Page 267): Measuring the variables affecting the energy change of reactions such as neutralization.