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Notes/GCSE/Chemistry (Combined Science)/Edexcel/Higher

Syllabus

Edexcel GCSE Combined Science (1SC0) — Chemistry — Higher

    • •Formulae of elements, compounds and ions0.1
    • •Word equations0.2
    • •Balanced chemical equations and state symbols0.3
    • •Balanced ionic equations0.4
    • •Hazard symbols and precautions0.5
    • •Evaluating practical risks and precautions0.6
      • •Development of the atomic model1.1
      • •Structure of the atom1.2
      • •Charge and mass of subatomic particles1.3
      • •Atomic charge neutrality1.4
      • •Size of the nucleus1.5
      • •Mass distribution in the atom1.6
      • •Mass number1.7
      • •Atomic number and elements1.8
      • •Isotopes1.9
      • •Calculating subatomic particles1.10
      • •Relative atomic mass and isotopes1.11
      • •Calculating relative atomic mass1.12
      • •Mendeleev’s arrangement of the periodic table1.13
      • •Mendeleev’s prediction of new elements1.14
      • •Isotopes and Mendeleev’s atomic mass ordering1.15
      • •Atomic number and periodic table position1.16
      • •Periods and groups in the periodic table1.17
      • •Metals and non-metals in the periodic table1.18
      • •Electronic configurations of the first 20 elements1.19
      • •Electronic configuration and periodic table position1.20
      • •Formation of ionic bonds1.21
      • •Ions1.22
      • •Calculating subatomic particles in ions1.23
      • •Ion formation in ionic compounds1.24
      • •Naming compounds with -ide and -ate1.25
      • •Formulae of ionic compounds1.26
      • •Ionic lattice structure1.27
      • •Formation of covalent bonds1.28
      • •Covalent bonding and molecules1.29
      • •Size of atoms and small molecules1.30
      • •Simple covalent molecules1.31
      • •Bonding types and physical properties1.32
      • •Properties of ionic compounds1.33
      • •Properties of simple molecular substances1.34
      • •Graphite and diamond as giant covalent structures1.35
      • •Structures of graphite and diamond1.36
      • •Uses of graphite and diamond1.37
      • •Properties of fullerenes and graphene1.38
      • •Structure of simple polymers1.39
      • •Properties of metals1.40
      • •Limitations of bonding models1.41
      • •Properties of metals and non-metals1.42
      • •Relative formula mass and percentage composition1.43
      • •Empirical formula from composition1.44
      • •Empirical and molecular formulae1.45
      • •Empirical formula practical1.46
      • •Conservation of mass in reactions1.47
      • •Mass calculations from balanced equations1.48
      • •Concentration calculations in g dm–31.49
      • •Definition of the mole1.50
      • •Mole and particle calculations1.51
      • •Limiting reactants and product mass1.52
      • •Stoichiometry from reacting masses1.53
      • •Particle model of states of matter2.1
      • •Changes of state2.2
      • •Particle changes during state changes2.3
      • •Predicting physical state from data2.4
      • •Pure substances and mixtures2.5
      • •Melting points of pure substances and mixtures2.6
      • •Separation techniques for mixtures2.7
      • •Selecting separation techniques2.8
      • •Paper chromatography2.9
      • •Interpreting chromatograms and Rf values2.10
      • •Ink composition practical2.11
      • •Making water potable and pure for analysis2.12
      • •Acids and alkalis as ion sources3.1
      • •pH scale and neutral solutions3.2
      • •Acid–alkali indicators3.3
      • •Ion concentration and pH3.4
      • •pH changes and powers of ten3.5
      • •Calcium oxide/hydroxide and hydrochloric acid practical3.6
      • •Dilute and concentrated solutions3.7
      • •Weak and strong acids3.8
      • •Bases and salt formation3.9
      • •Alkalis as soluble bases3.10
      • •General reactions of acids3.11
      • •Tests for hydrogen and carbon dioxide3.12
      • •Neutralisation reactions3.13
      • •Ionic equation for acid–alkali neutralisation3.14
      • •Making soluble salts from insoluble bases3.15
      • •Making soluble salts by titration3.16
      • •Preparation of hydrated copper sulfate crystals3.17
      • •Acid–alkali titration method3.18
      • •Solubility rules for common salts3.19
      • •Predicting precipitate formation3.20
      • •Preparing insoluble salts3.21
      • •Electrolytes3.22
      • •Electrolysis process3.23
      • •Ion movement during electrolysis3.24
      • •Products of electrolysis with inert electrodes3.25
      • •Products of electrolysis of molten ionic compounds3.26
      • •Half equations in electrolysis3.27
      • •Oxidation and reduction and electrons3.28
      • •Redox at anode and cathode in electrolysis3.29
      • •Electrolysis of copper sulfate with copper electrodes3.30
      • •Copper sulfate electrolysis practical3.31
      • •Metal reactivity from reactions4.1
      • •Displacement as redox4.2
      • •Reactivity series and metal cations4.3
      • •Metal ores and uncombined metals4.4
      • •Oxidation and reduction with oxygen4.5
      • •Metal extraction as reduction of ores4.6
      • •Extraction methods and reactivity series4.7
      • •Biological metal extraction methods4.8
      • •Oxidation resistance and reactivity series4.9
      • •Advantages of recycling metals4.10
      • •Life-cycle assessment of products4.11
      • •Evaluating life-cycle assessment data4.12
      • •Reversible reactions and equilibrium symbol4.13
      • •Dynamic equilibrium4.14
      • •Ammonia formation and equilibrium4.15
      • •Conditions for the Haber process4.16
      • •Effect of conditions on equilibrium position4.17
      • •Classifying alkali metals, halogens and noble gases6.1
      • •Physical properties of alkali metals6.2
      • •Reactions of lithium, sodium and potassium with water6.3
      • •Reactivity pattern of alkali metals with water6.4
      • •Explaining alkali metal reactivity using electronic structure6.5
      • •Colours and states of chlorine, bromine and iodine6.6
      • •Physical properties and trends in the halogens6.7
      • •Chemical test for chlorine gas6.8
      • •Reactions of halogens with metals to form halides6.9
      • •Hydrogen halides and acidic solutions6.10
      • •Reactivity of halogens from displacement reactions6.11
      • •Displacement reactions of halogens as redox6.12
      • •Explaining halogen reactivity using electronic structure6.13
      • •Inertness of noble gases and electronic configuration6.14
      • •Uses of noble gases6.15
      • •Physical property trends in the noble gases6.16
      • •Rates of reaction practicals: gas production and colour change7.1
      • •Practical methods for measuring rate of reaction7.2
      • •Collision theory and rate of reaction7.3
      • •Factors affecting rate of reaction7.4
      • •Interpreting rate of reaction graphs7.5
      • •Definition of a catalyst7.6
      • •Catalysts and activation energy7.7
      • •Enzymes as biological catalysts7.8
      • •Temperature changes in solution reactions7.9
      • •Exothermic reactions7.10
      • •Endothermic reactions7.11
      • •Bond breaking and making and energy changes7.12
      • •Overall energy change in reactions7.13
      • •Bond energy calculations7.14
      • •Activation energy7.15
      • •Reaction profiles for endothermic and exothermic reactions7.16
      • •Hydrocarbons8.1
      • •Crude oil and its importance8.2
      • •Fractional distillation of crude oil8.3
      • •Fractions of crude oil and their uses8.4
      • •Differences between crude oil fractions8.5
      • •Homologous series8.6
      • •Complete combustion of hydrocarbons8.7
      • •Incomplete combustion of hydrocarbons8.8
      • •Toxicity of carbon monoxide8.9
      • •Problems from incomplete combustion8.10
      • •Sulfur dioxide from fuel impurities8.11
      • •Acid rain and its effects8.12
      • •Formation of oxides of nitrogen in engines8.13
      • •Hydrogen versus petrol as car fuels8.14
      • •Fossil fuels as non-renewable resources8.15
      • •Cracking of hydrocarbons8.16
      • •Need for cracking8.17
      • •Volcanic origins of the early atmosphere8.18
      • •Composition of the Earth’s early atmosphere8.19
      • •Formation of oceans by condensation8.20
      • •Decrease of atmospheric CO₂ in early oceans8.21
      • •Photosynthesis and rise of atmospheric oxygen8.22
      • •Chemical test for oxygen8.23
      • •Greenhouse effect and atmospheric gases8.24
      • •Evidence and uncertainties for human-caused climate change8.25
      • •Today’s atmosphere and effects of increased greenhouse gases8.26

Syllabus

Edexcel GCSE Combined Science (1SC0) — Chemistry — Higher

    • •Formulae of elements, compounds and ions0.1
    • •Word equations0.2
    • •Balanced chemical equations and state symbols0.3
    • •Balanced ionic equations0.4
    • •Hazard symbols and precautions0.5
    • •Evaluating practical risks and precautions0.6
      • •Development of the atomic model1.1
      • •Structure of the atom1.2
      • •Charge and mass of subatomic particles1.3
      • •Atomic charge neutrality1.4
      • •Size of the nucleus1.5
      • •Mass distribution in the atom1.6
      • •Mass number1.7
      • •Atomic number and elements1.8
      • •Isotopes1.9
      • •Calculating subatomic particles1.10
      • •Relative atomic mass and isotopes1.11
      • •Calculating relative atomic mass1.12
      • •Mendeleev’s arrangement of the periodic table1.13
      • •Mendeleev’s prediction of new elements1.14
      • •Isotopes and Mendeleev’s atomic mass ordering1.15
      • •Atomic number and periodic table position1.16
      • •Periods and groups in the periodic table1.17
      • •Metals and non-metals in the periodic table1.18
      • •Electronic configurations of the first 20 elements1.19
      • •Electronic configuration and periodic table position1.20
      • •Formation of ionic bonds1.21
      • •Ions1.22
      • •Calculating subatomic particles in ions1.23
      • •Ion formation in ionic compounds1.24
      • •Naming compounds with -ide and -ate1.25
      • •Formulae of ionic compounds1.26
      • •Ionic lattice structure1.27
      • •Formation of covalent bonds1.28
      • •Covalent bonding and molecules1.29
      • •Size of atoms and small molecules1.30
      • •Simple covalent molecules1.31
      • •Bonding types and physical properties1.32
      • •Properties of ionic compounds1.33
      • •Properties of simple molecular substances1.34
      • •Graphite and diamond as giant covalent structures1.35
      • •Structures of graphite and diamond1.36
      • •Uses of graphite and diamond1.37
      • •Properties of fullerenes and graphene1.38
      • •Structure of simple polymers1.39
      • •Properties of metals1.40
      • •Limitations of bonding models1.41
      • •Properties of metals and non-metals1.42
      • •Relative formula mass and percentage composition1.43
      • •Empirical formula from composition1.44
      • •Empirical and molecular formulae1.45
      • •Empirical formula practical1.46
      • •Conservation of mass in reactions1.47
      • •Mass calculations from balanced equations1.48
      • •Concentration calculations in g dm–31.49
      • •Definition of the mole1.50
      • •Mole and particle calculations1.51
      • •Limiting reactants and product mass1.52
      • •Stoichiometry from reacting masses1.53
      • •Particle model of states of matter2.1
      • •Changes of state2.2
      • •Particle changes during state changes2.3
      • •Predicting physical state from data2.4
      • •Pure substances and mixtures2.5
      • •Melting points of pure substances and mixtures2.6
      • •Separation techniques for mixtures2.7
      • •Selecting separation techniques2.8
      • •Paper chromatography2.9
      • •Interpreting chromatograms and Rf values2.10
      • •Ink composition practical2.11
      • •Making water potable and pure for analysis2.12
      • •Acids and alkalis as ion sources3.1
      • •pH scale and neutral solutions3.2
      • •Acid–alkali indicators3.3
      • •Ion concentration and pH3.4
      • •pH changes and powers of ten3.5
      • •Calcium oxide/hydroxide and hydrochloric acid practical3.6
      • •Dilute and concentrated solutions3.7
      • •Weak and strong acids3.8
      • •Bases and salt formation3.9
      • •Alkalis as soluble bases3.10
      • •General reactions of acids3.11
      • •Tests for hydrogen and carbon dioxide3.12
      • •Neutralisation reactions3.13
      • •Ionic equation for acid–alkali neutralisation3.14
      • •Making soluble salts from insoluble bases3.15
      • •Making soluble salts by titration3.16
      • •Preparation of hydrated copper sulfate crystals3.17
      • •Acid–alkali titration method3.18
      • •Solubility rules for common salts3.19
      • •Predicting precipitate formation3.20
      • •Preparing insoluble salts3.21
      • •Electrolytes3.22
      • •Electrolysis process3.23
      • •Ion movement during electrolysis3.24
      • •Products of electrolysis with inert electrodes3.25
      • •Products of electrolysis of molten ionic compounds3.26
      • •Half equations in electrolysis3.27
      • •Oxidation and reduction and electrons3.28
      • •Redox at anode and cathode in electrolysis3.29
      • •Electrolysis of copper sulfate with copper electrodes3.30
      • •Copper sulfate electrolysis practical3.31
      • •Metal reactivity from reactions4.1
      • •Displacement as redox4.2
      • •Reactivity series and metal cations4.3
      • •Metal ores and uncombined metals4.4
      • •Oxidation and reduction with oxygen4.5
      • •Metal extraction as reduction of ores4.6
      • •Extraction methods and reactivity series4.7
      • •Biological metal extraction methods4.8
      • •Oxidation resistance and reactivity series4.9
      • •Advantages of recycling metals4.10
      • •Life-cycle assessment of products4.11
      • •Evaluating life-cycle assessment data4.12
      • •Reversible reactions and equilibrium symbol4.13
      • •Dynamic equilibrium4.14
      • •Ammonia formation and equilibrium4.15
      • •Conditions for the Haber process4.16
      • •Effect of conditions on equilibrium position4.17
      • •Classifying alkali metals, halogens and noble gases6.1
      • •Physical properties of alkali metals6.2
      • •Reactions of lithium, sodium and potassium with water6.3
      • •Reactivity pattern of alkali metals with water6.4
      • •Explaining alkali metal reactivity using electronic structure6.5
      • •Colours and states of chlorine, bromine and iodine6.6
      • •Physical properties and trends in the halogens6.7
      • •Chemical test for chlorine gas6.8
      • •Reactions of halogens with metals to form halides6.9
      • •Hydrogen halides and acidic solutions6.10
      • •Reactivity of halogens from displacement reactions6.11
      • •Displacement reactions of halogens as redox6.12
      • •Explaining halogen reactivity using electronic structure6.13
      • •Inertness of noble gases and electronic configuration6.14
      • •Uses of noble gases6.15
      • •Physical property trends in the noble gases6.16
      • •Rates of reaction practicals: gas production and colour change7.1
      • •Practical methods for measuring rate of reaction7.2
      • •Collision theory and rate of reaction7.3
      • •Factors affecting rate of reaction7.4
      • •Interpreting rate of reaction graphs7.5
      • •Definition of a catalyst7.6
      • •Catalysts and activation energy7.7
      • •Enzymes as biological catalysts7.8
      • •Temperature changes in solution reactions7.9
      • •Exothermic reactions7.10
      • •Endothermic reactions7.11
      • •Bond breaking and making and energy changes7.12
      • •Overall energy change in reactions7.13
      • •Bond energy calculations7.14
      • •Activation energy7.15
      • •Reaction profiles for endothermic and exothermic reactions7.16
      • •Hydrocarbons8.1
      • •Crude oil and its importance8.2
      • •Fractional distillation of crude oil8.3
      • •Fractions of crude oil and their uses8.4
      • •Differences between crude oil fractions8.5
      • •Homologous series8.6
      • •Complete combustion of hydrocarbons8.7
      • •Incomplete combustion of hydrocarbons8.8
      • •Toxicity of carbon monoxide8.9
      • •Problems from incomplete combustion8.10
      • •Sulfur dioxide from fuel impurities8.11
      • •Acid rain and its effects8.12
      • •Formation of oxides of nitrogen in engines8.13
      • •Hydrogen versus petrol as car fuels8.14
      • •Fossil fuels as non-renewable resources8.15
      • •Cracking of hydrocarbons8.16
      • •Need for cracking8.17
      • •Volcanic origins of the early atmosphere8.18
      • •Composition of the Earth’s early atmosphere8.19
      • •Formation of oceans by condensation8.20
      • •Decrease of atmospheric CO₂ in early oceans8.21
      • •Photosynthesis and rise of atmospheric oxygen8.22
      • •Chemical test for oxygen8.23
      • •Greenhouse effect and atmospheric gases8.24
      • •Evidence and uncertainties for human-caused climate change8.25
      • •Today’s atmosphere and effects of increased greenhouse gases8.26

Bond breaking and making and energy changes

Edexcel·Chemistry (Combined Science)·7.12·Higher

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