British (UK)

The National Curriculum of England (UK) is a very structured curriculum that is designed to meet the needs of all students, stretching brighter children and supporting those who need it through differentiated teaching and learning activities. The curriculum extends and excites all students, whatever their interests or ability. Through it, teachers are able to identify, celebrate and nurture the talents and intelligences of students.

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

Cambridge - Science - Combined (Chemistry) - 0653

  • Overview
  • Chapters

Cambridge IGCSE Combined Science offers students the opportunity to study biology, chemistry and physics in a single Cambridge IGCSE. Each subject is covered in a separate syllabus section.

Students learn the basic principles of each subject through a mix of theoretical and practical studies, while also developing an understanding of scientific skills.

The Cambridge IGCSE Combined Science syllabus is aimed at candidates across a very wide range of ability, and allows them to show success over the full range of grades from A* to G.

The syllabus has been designed to enable co-teaching with the Co-ordinated Sciences (Double Award) syllabus as well as with the separate Biology, Chemistry and Physics syllabuses.

  • 1: The particulate nature of matter
    1.1: The particulate nature of matter
    1.1.1: The distinguishing properties of solids, liquids and gases
    1.1.2: The structure of solids, liquids and gases
    1.1.3: The changes of state
    1.1.4: Changes of state in terms of particle theory and the energy changes involved
    1.1.5: The pressure and temperature of a gas
    1.1.6: Atom, molecule and ion
  • 2: Experimental techniques
    2.1: Measurement
    2.1.1: The measurement of time, temperature, mass and volume
    2.2: Criteria of purity
    2.2.1: Simple chromatograms
    2.2.2: Simple chromatograms, including the use of Rf values
    2.3: Methods of purification
    2.3.1: Methods of separation and purification
    2.3.2: Suitable separation and purification techniques
  • 3: Atoms, elements and compounds
    3.1: Physical and chemical changes
    3.1.1: Physical and chemical changes
    3.2: Elements, compounds and mixtures
    3.2.1: The differences between elements, mixtures and compounds
    3.2.2: Solvent, solute, solution and concentration
    3.3: Atomic structure and the Periodic Table
    3.3.1: The structure of an atom
    3.3.2: The build-up of electrons in ‘shells’
    3.3.3: The charges and approximate relative masses of protons, neutrons and electrons
    3.3.4: Proton number (atomic number)
    3.3.5: Nucleon number (mass number)
    3.3.6: The basis of the Periodic Table
    3.4: Ions and ionic bonds
    3.4.1: The formation of ions by electron loss or gain
    3.4.2: The formation of ionic bonds between Group I and Group VII
    3.4.3: The formation of ionic bonds between metallic and non-metallic elements
    3.4.4: The lattice structure of ionic compounds
    3.5: Molecules and covalent bonds
    3.5.1: Non-metallic elements form simple molecules with covalent bonds between atoms
    3.5.2: The formation of single covalent bonds
    3.5.3: The bonding in the more complex covalent molecules
    3.5.4: The differences between ionic and covalent compounds
    3.5.5: The differences in melting point and boiling point
  • 4: Stoichiometry
    4.1: Stoichiometry
    4.1.1: The formulae of simple compounds
    4.1.2: The formula of an ionic compound
    4.1.3: The formula of a simple compound
    4.1.4: The formula of a simple compound from a model
    4.1.5: Word equations
    4.1.6: Simple symbol equations
    4.1.7: Symbol equations, with state symbols, including ionic equations
  • 5: Electricity and chemistry
    5.1: Electricity and chemistry
    5.1.1: Electrolysis
    5.1.2: Electrode, electrolyte, anode and cathode
    5.1.3: Gain of electrons by cations and loss of electrons by anions to form atoms
    5.1.4: The electrode products
    5.1.5: The products of the electrolysis of a specified molten binary compound
  • 6: Energy changes in chemical reactions
    6.1: Energy changes in chemical reactions
    6.1.1: Exothermic and endothermic reactions
    6.1.2: Bond breaking and forming
    6.1.3: Energy level diagrams
    6.1.4: Exothermic and endothermic reactions and the activation energy of a reaction
  • 7: Chemical reactions
    7.1: Rate (speed) of reaction
    7.1.1: The rate of a reaction
    7.1.2: Experiments concerned with rate of reaction
    7.1.3: Collection of gases and measurement of rates of reaction
    7.1.4: The effect of concentration, particle size, catalysts and temperature
    7.1.5: The effect of changing concentration
    7.1.6: The effect of changing temperature
    7.2: Redox
    7.2.1: Oxidation and reduction in chemical reactions
    7.2.2: Oxidising agent
  • 8: Acids, bases and salts
    8.1: The characteristic properties of acids and bases
    8.1.1: Neutrality and relative acidity and alkalinity
    8.1.2: The characteristic properties of acids
    8.1.3: The importance of controlling acidity in soil
    8.2: Preparation of salts
    8.2.1: Preparation, separation and purification of salt
    8.2.2: Making a given salt from suitable starting material
    8.3: Identification of ions and gases
    8.3.1: Aqueous cations, cations, anions, and gases
  • 9: The Periodic Table
    9.1: The Periodic Table
    9.1.1: The Periodic Table
    9.2: Periodic trends
    9.2.1: The change from metallic to nonmetallic character across a period
    9.2.2: Metallic/non-metallic character
    9.3: Group properties
    9.3.1: Lithium, sodium and potassium in Group I
    9.3.2: The properties of other elements in Group I
    9.3.3: The halogens, chlorine, bromine and iodine in Group VII
    9.3.4: The reaction of chlorine, bromine and iodine with other halide ions
    9.3.5: The properties of other elements in Group VII
    9.3.6: Trends in other groups
    9.4: Transition elements
    9.4.1: The transition elements
    9.5: Noble gases
    9.5.1: The noble gases in Group VIII or 0
    9.5.2: The uses of the noble gases in providing an inert atmosphere
  • 10: Metals
    10.1: Properties of metals
    10.1.1: The general physical properties of metals
    10.1.2: Alloys
    10.1.3: Alloys are used instead of pure metals
    10.1.4: Representations of alloys from diagrams of structure
    10.2: Reactivity series
    10.2.1: Order of reactivity
    10.2.2: The reactivity series
    10.2.3: Order of reactivity from experimental results
    10.3: Extraction of metals from their ores
    10.3.1: The use of carbon in the extraction of copper from copper oxide
    10.3.2: The essential reactions in the extraction of iron from hematite
    10.3.3: Aluminium is extracted from the ore bauxite by electrolysis
    10.3.4: Method of extraction of a metal related to its position in the reactivity series
    10.3.5: Metal ores as a finite resource
  • 11: Air and water
    11.1: Water
    11.1.1: A chemical test for water
    11.1.2: The treatment of the water supply
    11.2: Air
    11.2.1: The composition of clean air
    11.2.2: The common pollutants in air
    11.2.3: The adverse effect of common air pollutants
    11.2.4: The conditions required for the rusting of iron
    11.2.5: Barrier methods of rust prevention
    11.3: Carbon dioxide and methane
    11.3.1: The formation of carbon dioxide
    11.3.2: Carbon dioxide and methane are greenhouse gases
    11.3.3: Increased concentrations of greenhouse gases cause an enhanced greenhouse effect
  • 12: Organic chemistry
    12.1: Fuels
    12.1.1: Coal, natural gas and petroleum are fossil fuels
    12.1.2: Methane as the main constituent of natural gas
    12.1.3: Petroleum as a mixture of hydrocarbons
    12.1.4: The properties of molecules within a fraction
    12.1.5: The uses of the fractions
    12.2: Homologous series
    12.2.1: The homologous series of alkanes and alkenes
    12.3: Alkanes
    12.3.1: Alkanes as saturated hydrocarbons
    12.3.2: The properties of alkanes
    12.3.3: The complete combustion of hydrocarbons to give carbon dioxide and water
    12.4: Alkenes
    12.4.1: Alkenes as unsaturated hydrocarbons
    12.4.2: Cracking is a reaction that produces alkenes
    12.4.3: The formation of smaller alkanes, alkenes and hydrogen
    12.4.4: Saturated and unsaturated hydrocarbons
    12.4.5: The formation of poly(ethene)
    12.4: Storage devices and media
    12.4.1: Identify storage devices, their associated media and their uses
    12.4.2: Describe the advantages and disadvantages of the storage devices

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