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Notes/IGCSE/Chemistry (Combined Science)/Edexcel/Modular

Syllabus

Pearson Edexcel International GCSE Science (Double Award) — Chemistry (Modular) — 4XSD1

      • •Particle arrangement, movement and energy1.1
      • •Changes of state1.2
      • •Dilution and diffusion1.3
      • •Solvents, solutes and solutions1.4
      • •Elements, compounds and mixtures1.8
      • •Melting and boiling points of pure substances1.9
      • •Separation techniques1.10
      • •Interpreting chromatograms1.11
      • •Rf calculations1.12
      • •Practical: paper chromatography1.13
      • •Atoms and molecules1.14
      • •Subatomic particles1.15
      • •Atomic number, mass number and isotopes1.16
      • •Relative atomic mass from isotopic abundances1.17
      • •Arrangement of the Periodic Table1.18
      • •Electronic configurations of the first 20 elements1.19
      • •Properties of metals and non-metals1.20
      • •Positions of metals and non-metals1.21
      • •Electronic configuration and position in the Periodic Table1.22
      • •Chemical properties within a group1.23
      • •The unreactivity of noble gases1.24
      • •Chemical equations and state symbols1.25
      • •Relative formula mass1.26
      • •The mole1.27
      • •Amount of substance and mass calculations1.28
      • •Reacting mass calculations1.29
      • •Percentage yield1.30
      • •Experimental determination of chemical formulae1.31
      • •Empirical and molecular formulae1.32
      • •Calculating empirical and molecular formulae1.33
      • •Practical: determining a metal oxide formula1.36
      • •Metal reactions with water and acids2.1
      • •Metal displacement reactions2.2
      • •The reactivity series2.3
      • •Conditions for rusting2.4
      • •Preventing rusting2.5
      • •Oxidation, reduction and redox2.6
      • •Practical: metals reacting with acids2.7
      • •Acid-base indicators2.14
      • •The pH scale2.15
      • •Universal indicator2.16
      • •Hydrogen and hydroxide ions2.17
      • •Neutralisation of acids by alkalis2.18
      • •Solubility rules2.20
      • •Proton transfer in acid-base reactions2.21
      • •Proton donors and acceptors2.22
      • •Acid reactions producing salts2.23
      • •Bases and alkalis2.24
      • •Preparing a soluble salt from an insoluble reactant2.25
      • •Practical: preparing copper(II) sulfate crystals2.28
      • •Exothermic and endothermic reactions3.1
      • •Calorimetry experiments3.2
      • •Heat energy change calculations3.3
      • •Molar enthalpy change calculations3.4
      • •Practical: temperature changes in reactions3.8
      • •Hydrocarbons4.1
      • •Representing organic molecules4.2
      • •Homologous series, functional groups and isomerism4.3
      • •Naming organic compounds4.4
      • •Structural and displayed formulae from molecular formulae4.5
      • •Substitution, addition and combustion reactions4.6
      • •Crude oil as a mixture4.7
      • •Fractional distillation of crude oil4.8
      • •Names and uses of crude oil fractions4.9
      • •Trends in crude oil fraction properties4.10
      • •Fuels and heat energy4.11
      • •Complete and incomplete combustion4.12
      • •Carbon monoxide poisoning4.13
      • •Nitrogen oxides from car engines4.14
      • •Sulfur dioxide from fuels4.15
      • •Acid rain4.16
      • •Catalytic cracking4.17
      • •Supply and demand for oil fractions4.18
      • •The general formula of alkanes4.19
      • •Saturated hydrocarbons4.20
      • •Alkane structures and names4.21
      • •Substitution reactions of alkanes4.22
      • •The alkene functional group4.23
      • •The general formula of alkenes4.24
      • •Unsaturated hydrocarbons4.25
      • •Alkene structures and names4.26
      • •Addition of bromine to alkenes4.27
      • •The bromine water test4.28
      • •Formation of ions5.1
      • •Charges of common ions5.2
      • •Formulae of ionic compounds5.3
      • •Dot-and-cross diagrams for ionic bonding5.4
      • •Electrostatic attraction in ionic bonding5.5
      • •Melting and boiling points of ionic lattices5.6
      • •Electrical conductivity of ionic compounds5.7
      • •Shared electron pairs in covalent bonds5.8
      • •Electrostatic attraction in covalent bonding5.9
      • •Dot-and-cross diagrams for covalent bonding5.10
      • •Simple molecular structures and intermolecular forces5.11
      • •Molecular mass and melting and boiling points5.12
      • •Giant covalent structures5.13
      • •Diamond, graphite and fullerene5.14
      • •Electrical conductivity of covalent compounds5.15
      • •Group 1 reactions with water6.1
      • •Reactivity trends in Group 16.2
      • •Predicting alkali metal properties6.3
      • •Physical properties of the halogens6.5
      • •Predicting halogen properties6.6
      • •Halogen displacement reactions6.7
      • •Composition of dry air6.9
      • •Determining the oxygen content of air6.10
      • •Combustion of elements in oxygen6.11
      • •Thermal decomposition of metal carbonates6.12
      • •Carbon dioxide and climate change6.13
      • •Practical: oxygen percentage in air6.14
      • •Tests for gases6.15
      • •Carrying out a flame test6.16
      • •Flame test colours6.17
      • •Tests for cations6.18
      • •Tests for anions6.19
      • •Chemical test for water6.20
      • •Testing the purity of water6.21
      • •Investigating factors affecting reaction rate7.1
      • •Effects of conditions on reaction rate7.2
      • •Collision theory7.3
      • •Catalysts7.4
      • •Catalysts and activation energy7.5
      • •Practical: marble chips and hydrochloric acid7.7
      • •Practical: catalytic decomposition of hydrogen peroxide7.8
      • •Reversible reactions7.9
      • •Examples of reversible reactions7.10
      • •Addition polymerisation8.16
      • •Repeat units of addition polymers8.17
      • •Deducing monomers and repeat units8.18
      • •Disposal of addition polymers8.19

Syllabus

Pearson Edexcel International GCSE Science (Double Award) — Chemistry (Modular) — 4XSD1

      • •Particle arrangement, movement and energy1.1
      • •Changes of state1.2
      • •Dilution and diffusion1.3
      • •Solvents, solutes and solutions1.4
      • •Elements, compounds and mixtures1.8
      • •Melting and boiling points of pure substances1.9
      • •Separation techniques1.10
      • •Interpreting chromatograms1.11
      • •Rf calculations1.12
      • •Practical: paper chromatography1.13
      • •Atoms and molecules1.14
      • •Subatomic particles1.15
      • •Atomic number, mass number and isotopes1.16
      • •Relative atomic mass from isotopic abundances1.17
      • •Arrangement of the Periodic Table1.18
      • •Electronic configurations of the first 20 elements1.19
      • •Properties of metals and non-metals1.20
      • •Positions of metals and non-metals1.21
      • •Electronic configuration and position in the Periodic Table1.22
      • •Chemical properties within a group1.23
      • •The unreactivity of noble gases1.24
      • •Chemical equations and state symbols1.25
      • •Relative formula mass1.26
      • •The mole1.27
      • •Amount of substance and mass calculations1.28
      • •Reacting mass calculations1.29
      • •Percentage yield1.30
      • •Experimental determination of chemical formulae1.31
      • •Empirical and molecular formulae1.32
      • •Calculating empirical and molecular formulae1.33
      • •Practical: determining a metal oxide formula1.36
      • •Metal reactions with water and acids2.1
      • •Metal displacement reactions2.2
      • •The reactivity series2.3
      • •Conditions for rusting2.4
      • •Preventing rusting2.5
      • •Oxidation, reduction and redox2.6
      • •Practical: metals reacting with acids2.7
      • •Acid-base indicators2.14
      • •The pH scale2.15
      • •Universal indicator2.16
      • •Hydrogen and hydroxide ions2.17
      • •Neutralisation of acids by alkalis2.18
      • •Solubility rules2.20
      • •Proton transfer in acid-base reactions2.21
      • •Proton donors and acceptors2.22
      • •Acid reactions producing salts2.23
      • •Bases and alkalis2.24
      • •Preparing a soluble salt from an insoluble reactant2.25
      • •Practical: preparing copper(II) sulfate crystals2.28
      • •Exothermic and endothermic reactions3.1
      • •Calorimetry experiments3.2
      • •Heat energy change calculations3.3
      • •Molar enthalpy change calculations3.4
      • •Practical: temperature changes in reactions3.8
      • •Hydrocarbons4.1
      • •Representing organic molecules4.2
      • •Homologous series, functional groups and isomerism4.3
      • •Naming organic compounds4.4
      • •Structural and displayed formulae from molecular formulae4.5
      • •Substitution, addition and combustion reactions4.6
      • •Crude oil as a mixture4.7
      • •Fractional distillation of crude oil4.8
      • •Names and uses of crude oil fractions4.9
      • •Trends in crude oil fraction properties4.10
      • •Fuels and heat energy4.11
      • •Complete and incomplete combustion4.12
      • •Carbon monoxide poisoning4.13
      • •Nitrogen oxides from car engines4.14
      • •Sulfur dioxide from fuels4.15
      • •Acid rain4.16
      • •Catalytic cracking4.17
      • •Supply and demand for oil fractions4.18
      • •The general formula of alkanes4.19
      • •Saturated hydrocarbons4.20
      • •Alkane structures and names4.21
      • •Substitution reactions of alkanes4.22
      • •The alkene functional group4.23
      • •The general formula of alkenes4.24
      • •Unsaturated hydrocarbons4.25
      • •Alkene structures and names4.26
      • •Addition of bromine to alkenes4.27
      • •The bromine water test4.28
      • •Formation of ions5.1
      • •Charges of common ions5.2
      • •Formulae of ionic compounds5.3
      • •Dot-and-cross diagrams for ionic bonding5.4
      • •Electrostatic attraction in ionic bonding5.5
      • •Melting and boiling points of ionic lattices5.6
      • •Electrical conductivity of ionic compounds5.7
      • •Shared electron pairs in covalent bonds5.8
      • •Electrostatic attraction in covalent bonding5.9
      • •Dot-and-cross diagrams for covalent bonding5.10
      • •Simple molecular structures and intermolecular forces5.11
      • •Molecular mass and melting and boiling points5.12
      • •Giant covalent structures5.13
      • •Diamond, graphite and fullerene5.14
      • •Electrical conductivity of covalent compounds5.15
      • •Group 1 reactions with water6.1
      • •Reactivity trends in Group 16.2
      • •Predicting alkali metal properties6.3
      • •Physical properties of the halogens6.5
      • •Predicting halogen properties6.6
      • •Halogen displacement reactions6.7
      • •Composition of dry air6.9
      • •Determining the oxygen content of air6.10
      • •Combustion of elements in oxygen6.11
      • •Thermal decomposition of metal carbonates6.12
      • •Carbon dioxide and climate change6.13
      • •Practical: oxygen percentage in air6.14
      • •Tests for gases6.15
      • •Carrying out a flame test6.16
      • •Flame test colours6.17
      • •Tests for cations6.18
      • •Tests for anions6.19
      • •Chemical test for water6.20
      • •Testing the purity of water6.21
      • •Investigating factors affecting reaction rate7.1
      • •Effects of conditions on reaction rate7.2
      • •Collision theory7.3
      • •Catalysts7.4
      • •Catalysts and activation energy7.5
      • •Practical: marble chips and hydrochloric acid7.7
      • •Practical: catalytic decomposition of hydrogen peroxide7.8
      • •Reversible reactions7.9
      • •Examples of reversible reactions7.10
      • •Addition polymerisation8.16
      • •Repeat units of addition polymers8.17
      • •Deducing monomers and repeat units8.18
      • •Disposal of addition polymers8.19

Electronic configuration and position in the Periodic Table

Edexcel·Chemistry (Combined Science)·1.22·Modular

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The concept content for this specification point is being prepared. Check back soon.