KnowledgeSetKnowledgeSet
Pricing
Log InGet Started

The learning loop

See all features →
01

Build understanding

Clear explanations. Connected ideas. Help when you need it.

02

Put it into practice

Try it, get feedback, and learn from every attempt.

03

Know what to work on next

See your progress and find a clearer next step.

Key Stage 3
Coming soon
GCSE
  • Biology
  • Chemistry
  • Physics
  • Biology (Combined)
  • Chemistry (Combined)
  • Physics (Combined)
  • Maths
  • Geography
IGCSE
  • Biology
  • Chemistry
  • Physics
A-Level
  • Biology
  • Chemistry
  • Physics
11+
Coming soon
Product
See all features →

Build understanding

Clear explanations. Connected ideas. Help when you need it.

Put it into practice

Try it, get feedback, and learn from every attempt.

Know what to work on next

See your progress and find a clearer next step.

Subjects
Pricing
Log InGet Started
HomeCalendarSubjectsAnalyticsSageAILessonsNotesFlashcardsQuestionsFeedback
Notes/GCSE/Chemistry (Combined Science)/Edexcel/Foundation

Syllabus

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

    • •Formulae of elements, compounds and ions0.1
    • •Word equations0.2
    • •Balanced chemical equations and state symbols0.3
    • •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
      • •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
      • •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
      • •Calcium oxide/hydroxide and hydrochloric acid practical3.6
      • •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
      • •Electrolysis of copper sulfate with copper electrodes3.30
      • •Copper sulfate electrolysis practical3.31
      • •Metal reactivity from reactions4.1
      • •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
      • •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
      • •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
      • •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
      • •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 — Foundation

    • •Formulae of elements, compounds and ions0.1
    • •Word equations0.2
    • •Balanced chemical equations and state symbols0.3
    • •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
      • •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
      • •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
      • •Calcium oxide/hydroxide and hydrochloric acid practical3.6
      • •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
      • •Electrolysis of copper sulfate with copper electrodes3.30
      • •Copper sulfate electrolysis practical3.31
      • •Metal reactivity from reactions4.1
      • •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
      • •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
      • •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
      • •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
      • •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

Properties of simple molecular substances

Edexcel·Chemistry (Combined Science)·1.34·Foundation

Notes Coming Soon

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