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British education is renowned for concerning itself with the development of the whole personality.

In the British education system, students are taught to learn by questioning, problem-solving and creative thinking rather than by the mere retention of facts, hence giving them analytical and creative thinking skills that they will need in the working world. A variety of teaching and assessment methods designed to develop independent thought as well as a mastery of the subject matter is used.

The National Curriculum of England has a clearly defined series of academic and other objectives at every level. mydrasa focuses on Key stage 3 (Year 7-9), Key stage 4 IGCSE/GCSE (Year 10-11) and Key stage 5 A-Level (Year 12-13).

mydrasa added subjects related to Key stage 4 to Year 9, and added subjects related to Key stage 5 to Year 11 for student preparation.

IGCSE stands for the "International General Certificate of Secondary Education". It is a program leading to externally set, marked and certificated examinations from the University of Cambridge. Any student who takes an IGCSE subject will be gaining a qualification that is recognized globally.

The exam boards covered under the International GCSE are Cambridge, Edexcel, and Oxford AQA.

SUbjects

Subjects

Oxford AQA - Chemistry - 9202

  • Overview
  • Chapters

Chemistry 9202 is a basic course of chemistry. It is a pre-requisite for the advanced Chemistry course. The content contains a broad range of topics that are designed to engage students whilst providing the knowledge and understanding required for progression to Level 3 qualifications.

  • 1: ATOMIC STRUCTURE AND THE PERIODIC TABLE
    1.1: SOLIDS, LIQUIDS AND GASES
    1.1.1: Matter can be classified in terms of the three states of matter
    1.1.2: Evidence for the existence of particles can be obtained from simple experiments
    1.2: A SIMPLE MODEL OF THE ATOM
    1.2.1: All substances are made of atoms
    1.2.2: Atoms of each element are represented by a chemical symbol
    1.2.3: Atoms have a small central nucleus, made of protons and neutrons
    1.2.4: The relative electrical charge
    1.2.5: The number of electrons is equal to the number of protons in the nucleus
    1.2.6: The number of protons in an atom of an element is its atomic number
    1.2.7: Atoms of the same element can have different numbers of neutrons
    1.2.8: Representation of atoms
    1.2.9: Electrons occupy particular energy levels
    1.2.10: The relative masses of protons, neutrons and electrons
    1.2.11: The relative atomic mass of an element
    1.3: THE PERIODIC TABLE
    1.3.1: The periodic table is arranged in order of atomic (proton) number
    1.3.2: Elements in the same group in the periodic table
    1.3.3: The elements in Group 0 of the periodic table are called the noble gases
  • 2: STRUCTURE, BONDING AND THE PROPERTIES OF MATTER
    2.1: CHEMICAL BONDS: IONIC, COVALENT AND METALLIC
    2.1.1: Compounds
    2.1.2: Chemical bonding
    2.1.3: Ion formation
    2.1.4: The elements in Group 1 of the periodic table, the alkali metals
    2.1.5: The elements in Group 7 of the periodic table, the halogens
    2.1.6: An ionic compound is a giant structure of ions
    2.1.7: When atoms share pairs of electrons, they form covalent bonds
    2.1.8: In non-metals, the atoms are held together by covalent bonds
    2.1.9: Metals consist of giant structures of atoms arranged in a regular pattern
    2.1.10: The electrons in the highest energy levels of metal atoms are delocalised
    2.2: HOW BONDING AND STRUCTURE ARE RELATED TO THE PROPERTIES OF SUBSTANCES
    2.2.1: Ionic compounds have regular structures
    2.2.2: When melted or dissolved in water, ionic compounds conduct electricity
    2.2.3: Substances that consist of simple molecules
    2.2.4: Weak forces between the molecules (intermolecular forces)
    2.2.5: Overall electric charge
    2.2.6: Atoms that share electrons can also form giant structures or macromolecule
    2.2.7: Metals conduct heat and electricity because of the delocalised electrons
    2.3: STRUCTURE AND BONDING OF CARBON
    2.3.1: The element carbon can form four covalent bonds
    2.3.2: In diamond, each carbon atom forms four covalent bonds
    2.3.3: In graphite, each carbon atom bonds to three others, forming layers
    2.3.4: In graphite, one electron from each carbon atom is delocalised
    2.3.5: Carbon can also form fullerenes with different numbers of carbon atoms
    2.4: NANOPARTICLES
    2.4.1: Nanoscience refers to structures that are 1–100 nm in size
  • 3: CHEMICAL CHANGES
    3.1: METALS
    3.1.1: Metals are useful materials as they are good conductors of heat and electricity
    3.1.2: An alloy is a mixture of at least two elements
    3.1.3: Copper is useful for electrical wiring and plumbing
    3.2: The reactivity series
    3.2.1: Metals can be arranged in an order of their reactivity
    3.2.2: Displacement reactions involving metals and their compounds in aqueous solution
    3.2.3: Unreactive metals such as gold
    3.2.4: Metals that are less reactive than carbon can be extracted from their oxides
    3.2.5: Metals extracted by electrolysis of molten compounds
    3.2.6: New ways of extracting copper from low-grade ores
    3.2.7: Copper can be obtained from solutions of copper salts by electrolysis
    3.2.8: Copper can be obtained from solutions of copper salts by displacement
    3.2.9: Recycle metals because extracting them uses limited resources
    3.3: Metal carbonates
    3.3.1: The carbonates of magnesium, copper, zinc, calcium and lithium
    3.3.2: Metal carbonates react with acids to produce carbon dioxide, a salt and water
    3.4: ELECTROLYSIS
    3.4.1: When an ionic substance is melted or dissolved in water
    3.4.2: Passing an electric current through ionic substances that are molten
    3.4.3: During electrolysis
    3.4.4: Oxidation and reduction
    3.4.5: At the cathode
    3.4.6: Reactions at electrodes
    3.4.7: Mixture of ions
    3.4.8: Electrolysis is used to electroplate objects
    3.4.9: Aluminium is manufactured by the electrolysis
    3.4.10: The electrolysis of sodium chloride solution produces hydrogen and chlorine
  • 4: CHEMICAL ANALYSIS
    4.1: PURITY AND CHROMATOGRAPHY
    4.1.1: A pure element or compound contains only one substance
    4.1.2: Measures of purity are important in everyday substances
    4.1.3: A mixture consists of two or more elements or compounds
    4.1.4: Paper chromatography can be used to analyse substances present in a solution
    4.1.5: Chromatography involves a stationary and a mobile phase
    4.2: IDENTIFICATION OF COMMON GASES
    4.2.1: A pop is heard when a lighted splint is placed near hydrogen gas
    4.2.2: A glowing splint relights in a test tube of oxygen gas
    4.2.3: Carbon dioxide turns limewater (calcium hydroxide solution) cloudy white
    4.2.4: Ammonia has a characteristic sharp, choking smell
    4.2.5: Chlorine has a characteristic sharp, choking smell
    4.3: IDENTIFICATION OF IONS
    4.3.1: Flame tests can be used to identify metal ions
    4.3.2: Aluminium, calcium and magnesium ions form white precipitates
    4.3.3: Copper(II), iron(II) and iron(III) ions form coloured precipitates
    4.3.4: Carbonates react with dilute acids to form carbon dioxide
    4.3.5: Halide ions in solution produce precipitates with silver nitrate solution
    4.3.6: Sulfate ions in solution produce a white precipitate
  • 5: ACIDS, BASES AND SALTS
    5.1: THE PROPERTIES OF ACIDS AND BASES
    5.1.1: Metal oxides and hydroxides are bases
    5.1.2: Acids react with bases to form salts
    5.1.3: Salt produced in any reaction between an acid and a base or alkali
    5.1.4: Ammonia dissolves in water to produce an alkaline solution
    5.1.5: A solution of calcium hydroxide in water (limewater) reacts with carbon dioxide
    5.1.6: Hydrogen ions and hydroxide ions
    5.1.7: In neutralisation reactions
    5.2: PREPARATION OF SALTS
    5.2.1: Soluble salts can be made from acids
    5.2.2: Salt solutions can be crystallised to produce solid salts
    5.2.3: Insoluble salts can be made by mixing appropriate solutions of ions
  • 6: QUANTITATIVE CHEMISTRY
    6.1: CONSERVATION OF MASS
    6.1.1: Chemical reactions can be represented by word equations or by symbol equations
    6.1.2: Information about the states of reactants
    6.1.3: No atoms are lost or made during a chemical reaction
    6.1.4: The masses of reactants and products can be calculated
    6.1.5: It is not always possible to obtain the calculated amount of a product
    6.2: USE OF AMOUNT OF SUBSTANCE IN RELATION TO MASSES OF PURE SUBSTANCES
    6.2.1: The relative formula mass (Mr) of a compound
    6.2.2: The percentage by mass of an element in a compound
    6.2.3: The empirical formula of a compound
    6.3: THE MOLE CONCEPT
    6.3.1: The relative formula mass of a substance
    6.3.2: One mole contains 6.02 X 10 23 atoms or molecules
    6.4: MOLAR CONCENTRATIONS
    6.4.1: The concentration of a solution is related to the mass of the solute
    6.4.2: The volumes of acid and alkali solutions
    6.4.3: The concentration of the other reactant
    6.4.4: The molar gas volume at room temperature
  • 7: TRENDS WITHIN THE PERIODIC TABLE
    7.1: GROUP PROPERTIES
    7.1.1: The elements in Group 1 of the periodic table
    7.1.2: The further down the group an element is, the more reactive the element
    7.1.3: The elements in Group 7 of the periodic table
    7.1.4: In Group 7
    7.1.5: A more reactive halogen can displace a less reactive halogen
    7.1.6: The trends in reactivity within groups in the periodic table
    7.2: TRANSITION METALS
    7.2.1: Transition metals are those in the centre of the periodic table
    7.2.2: Compared with the elements in Group 1
  • 8: THE RATE AND EXTENT OF CHEMICAL CHANGE
    8.1: RATE OF REACTION
    8.1.1: The rate of a chemical reaction
    8.1.2: Reacting particles collide with each other and with sufficient energy
    8.1.3: Increasing the temperature increases the speed of the reacting particles
    8.1.4: Increasing the pressure of reacting gases
    8.1.5: Increasing the concentration of reactants
    8.1.6: Increasing the surface area of solid reactants
    8.1.7: Catalysts change the rate of chemical reactions
    8.1.8: Catalysts are important in increasing the rate of chemical reactions
    8.2: FACTORS AFFECTING EQUILIBRIUM
    8.2.1: When a reversible reaction occurs in a closed system
    8.2.2: The relative amounts of all the reacting substances at equilibrium
    8.2.3: If the temperature is raised
    8.2.4: In gaseous reactions
    8.2.5: The optimum conditions in industrial processes
    8.3: PRODUCTION OF AMMONIA AND SULFURIC ACID
    8.3.1: The raw materials for the Haber process are nitrogen and hydrogen
    8.3.2: Ammonia is a raw material in the production of fertilizers
    8.3.3: The purified gases are passed over a catalyst of iron
    8.3.4: Sulfuric acid is produced industrially using the contact process
    8.4: REDOX REACTIONS
    8.4.1: Oxidation and reduction by gain and loss of oxygen
    8.4.2: Oxidation by the loss of electrons and reduction as gain of electrons
    8.4.3: Redox reaction
  • 9: ENERGY CHANGES
    9.1: EXOTHERMIC AND ENDOTHERMIC REACTIONS
    9.1.1: When chemical reactions occur, energy is transferred to or from the surroundings
    9.1.2: An exothermic reaction is one that transfers energy to the surroundings
    9.1.3: An endothermic reaction is one that takes in energy from the surroundings
    9.1.4: The products of the reaction can react to produce the original reactants
    9.2: CALCULATING AND EXPLAINING ENERGY CHANGE
    9.2.1: The relative amounts of energy released when substances burn
    9.2.2: Energy is normally measured in joules (J) or kilojoules (kJ)
    9.2.3: The amount of energy produced by a chemical reaction in solution
    9.2.4: Simple energy level diagrams
    9.2.5: During a chemical reaction
    9.2.6: In an exothermic reaction
    9.2.7: In an endothermic reaction
    9.2.8: Catalysts provide a different pathway for a chemical reaction
    9.3: CHEMICAL CELLS AND FUEL CELLS
    9.3.1: A chemical cell produces a potential difference
    9.3.2: Fuel cells produce electricity through the reaction of a fuel with oxygen
  • 10: ORGANIC CHEMISTRY
    10.1: CARBON COMPOUNDS AS FUELS :Crude oil
    10.1.1: Crude oil is a mixture of a very large number of compounds
    10.1.2: Compounds in crude oil are hydrocarbons
    10.1.3: The many hydrocarbons in crude oil may be separated into fractions
    10.2: Hydrocarbons
    10.2.1: Most of the hydrocarbons in crude oil are saturated hydrocarbons called alkane
    10.2.2: Alkane molecules
    10.2.3: Some properties of hydrocarbons depend on the size of their molecules
    10.2.4: Most fuels contain carbon and/or hydrogen and may also contain some sulfur
    10.2.5: The combustion of hydrocarbon fuels releases energy
    10.2.6: Ethanol can be made by reacting ethene with steam
    10.2.7: Biofuels, including biodiesel and ethanol, are produced from plant material
    10.3: Obtaining useful substances from crude oil
    10.3.1: Hydrocarbons can be broken down (cracked) to produce smaller molecules
    10.3.2: The products of cracking include alkanes and alkenes
    10.3.3: Unsaturated hydrocarbon molecules
    10.3.4: Alkenes react with bromine water, turning it from orange to colourless
    10.3.5: Some of the products of cracking are useful as fuels
    10.4: SYNTHETIC AND NATURALLY OCCURRING POLYMERS
    10.4.1: Alkenes can be used to make polymers such as poly(ethene) and poly(propene)
    10.4.2: The properties of polymers
    10.4.3: Thermosoftening polymers consist of individual, tangled polymer chains
    10.4.4: Polymers have many useful applications and new uses are being developed
    10.4.5: Many polymers are not biodegradable, ie they are not broken down by microbes
    10.4.6: Plastic bags are being made from polymers and cornstarch
    10.5: ORGANIC COMPOUNDS – THEIR STRUCTURE AND REACTIONS :Alcohols
    10.5.1: Alcohols contain the functional group –OH
    10.5.2: Methanol, ethanol and propanol
    10.5.3: Ethanol can be oxidised to ethanoic acid
    10.6: Carboxylic acids
    10.6.1: Ethanoic acid is a member of the homologous series of carboxylic acids
    10.6.2: Carboxylic acids
    10.7: Esters
    10.7.1: Esters have the functional group –COO–
    10.7.2: Esters are volatile compounds with distinctive smells

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