Syllabus - Chemistry Boutique

Cambridge IGCSE Chemistry 0620 syllabus for 2019.3 Subject contentAll candidates should be taught the Core subject content. Candidates who are only taught the Coresubject content can achieve a maximum of grade C. Candidates aiming for grades A* to C should betaught the Extended subject content. The Extended subject content includes both the Core and theSupplement.Scientific subjects are, by their nature, experimental. Learners should pursue a fully integrated coursewhich allows them to develop their practical skills by carrying out practical work and investigationswithin all of the topics listed.1The particulate nature of matter1.1The particulate nature of matterSupplementCore State the distinguishing properties of solids,liquids and gases Describe the structure of solids, liquidsand gases in terms of particle separation,arrangement and types of motion Describe changes of state in terms ofmelting, boiling, evaporation, freezing,condensation and sublimation Describe qualitatively the pressure andtemperature of a gas in terms of the motionof its particles Explain changes of state in terms of thekinetic theoryShow an understanding of the random motionof particles in a suspension (sometimesknown as Brownian motion) as evidence forthe kinetic particle (atoms, molecules or ions)model of matter Describe and explain Brownian motion interms of random molecular bombardment State evidence for Brownian motion Describe and explain diffusion Describe and explain dependence of rate ofdiffusion on molecular mass2Experimental techniques2.1MeasurementCore Name appropriate apparatus for themeasurement of time, temperature, massand volume, including burettes, pipettes andmeasuring cylindersBack to contents pagewww.cie.org.uk/igcse7

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content2.2Purity2.2.1 Criteria of purityCoreSupplement Demonstrate knowledge and understandingof paper chromatography Interpret simple chromatograms, includingthe use of Rf values Interpret simple chromatograms Identify substances and assess theirpurity from melting point and boiling pointinformation Understand the importance of purity insubstances in everyday life, e.g. foodstuffsand drugsOutline how chromatography techniquescan be applied to colourless substances byexposing chromatograms to substancescalled locating agents. (Knowledge of specificlocating agents is not required.)2.2.2 Methods of purificationCore Describe and explain methods of purificationby the use of a suitable solvent, filtration,crystallisation and distillation (includinguse of a fractionating column). (Refer tothe fractional distillation of petroleum insection 14.2 and products of fermentation insection 14.6.) Suggest suitable purification techniques,given information about the substancesinvolved3Atoms, elements and compounds3.1Atomic structure and the Periodic TableCore8 State the relative charges and approximaterelative masses of protons, neutrons andelectrons Define proton number (atomic number) as thenumber of protons in the nucleus of an atom Define nucleon number (mass number) as thetotal number of protons and neutrons in thenucleus of an atom Use proton number and the simple structureof atoms to explain the basis of the PeriodicTable (see section 9), with special referenceto the elements of proton number 1 to 20 Define isotopes as atoms of the sameelement which have the same proton numberbut a different nucleon number State the two types of isotopes as beingradioactive and non-radioactivewww.cie.org.uk/igcseSupplement Understand that isotopes have the sameproperties because they have the samenumber of electrons in their outer shellcontinuedBack to contents page

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content3.1Atomic structure and the Periodic Table continuedCore State one medical and one industrial use ofradioactive isotopes Describe the build-up of electrons in ‘shells’and understand the significance of the noblegas electronic structures and of the outershell electrons. (The ideas of the distributionof electrons in s and p orbitals and in d blockelements are not required.)Note: a copy of the Periodic Table, as shown inthe Appendix, will be available in Papers 1, 2, 3and 4.3.2Structure and bonding3.2.1 Bonding: the structure of matterCore Describe the differences between elements,mixtures and compounds, and betweenmetals and non-metals Describe an alloy, such as brass, as a mixtureof a metal with other elements3.2.2 Ions and ionic bondsCoreSupplement Describe the formation of ions by electronloss or gain Describe the formation of ionic bondsbetween metallic and non-metallic elements Describe the formation of ionic bondsbetween elements from Groups I and VII Describe the lattice structure of ioniccompounds as a regular arrangement ofalternating positive and negative ions3.2.3 Molecules and covalent bondsCoreSupplement Describe the formation of single covalentbonds in H2, Cl2, H2O, CH4, NH3 and HCl asthe sharing of pairs of electrons leading to thenoble gas configuration Describe the electron arrangement in morecomplex covalent molecules such as N2,C2H4, CH3OH and CO2 Describe the differences in volatility, solubilityand electrical conductivity between ionic andcovalent compoundsExplain the differences in melting point andboiling point of ionic and covalent compoundsin terms of attractive forcesBack to contents pagewww.cie.org.uk/igcse9

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content3.2.4 MacromoleculesCoreSupplement Describe the giant covalent structures ofgraphite and diamond Describe the macromolecular structure ofsilicon(IV) oxide (silicon dioxide) Relate their structures to their uses, e.g.graphite as a lubricant and a conductor, anddiamond in cutting tools Describe the similarity in properties betweendiamond and silicon(IV) oxide, related to theirstructures3.2.5 Metallic bondingSupplement 4Stoichiometry4.1StoichiometryDescribe metallic bonding as a lattice ofpositive ions in a ‘sea of electrons’ and usethis to describe the electrical conductivity andmalleability of metalsCoreSupplement Use the symbols of the elements and writethe formulae of simple compounds Determine the formula of an ionic compoundfrom the charges on the ions present Deduce the formula of a simple compoundfrom the relative numbers of atoms present Construct equations with state symbols,including ionic equations Deduce the formula of a simple compoundfrom a model or a diagrammaticrepresentation Deduce the balanced equation for a chemicalreaction, given relevant information Construct word equations and simplebalanced chemical equations Define relative atomic mass, Ar, as theaverage mass of naturally occurring atomsof an element on a scale where the 12C atomhas a mass of exactly 12 units Define relative molecular mass, Mr, as thesum of the relative atomic masses. (Relativeformula mass or Mr will be used for ioniccompounds.)(Calculations involving reacting masses insimple proportions may be set. Calculationswill not involve the mole concept.)10www.cie.org.uk/igcseBack to contents page

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content4.2The mole conceptSupplement5Electricity and chemistry5.1Electricity and chemistry Define the mole and the Avogadro constant Use the molar gas volume, taken as 24 dm3 atroom temperature and pressure Calculate stoichiometric reacting masses,volumes of gases and solutions, andconcentrations of solutions expressed ing / dm3 and mol / dm3. (Calculations involvingthe idea of limiting reactants may beset. Questions on the gas laws and theconversion of gaseous volumes to differenttemperatures and pressures will not be set.) Calculate empirical formulae and molecularformulae Calculate percentage yield and percentagepurityCoreSupplement Define electrolysis as the breakdown ofan ionic compound, molten or in aqueoussolution, by the passage of electricity Describe the electrode products and theobservations made during the electrolysis of:Relate the products of electrolysis to theelectrolyte and electrodes used, exemplifiedby the specific examples in the Core togetherwith aqueous copper(II) sulfate using carbonelectrodes and using copper electrodes (asused in the refining of copper) Describe electrolysis in terms of the ionspresent and reactions at the electrodes in theexamples given–– molten lead(II) bromide–– concentrated hydrochloric acid–– concentrated aqueous sodium chloride–– dilute sulfuric acidbetween inert electrodes (platinum or carbon) State the general principle that metalsor hydrogen are formed at the negativeelectrode (cathode), and that non-metals(other than hydrogen) are formed at thepositive electrode (anode) Predict the products of the electrolysis ofa specified binary compound in the moltenstate Predict the products of electrolysis of aspecified halide in dilute or concentratedaqueous solution Describe the electroplating of metals Outline the uses of electroplatingConstruct ionic half-equations for reactions atthe cathodecontinuedBack to contents pagewww.cie.org.uk/igcse11

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content5.1Electricity and chemistry continuedCoreSupplement Describe the reasons for the use of copperand (steel-cored) aluminium in cables, andwhy plastics and ceramics are used asinsulatorsDescribe the transfer of charge duringelectrolysis to include:–– the movement of electrons in the metallicconductor–– the removal or addition of electrons fromthe external circuit at the electrodes–– the movement of ions in the electrolyte Describe the production of electrical energyfrom simple cells, i.e. two electrodes in anelectrolyte. (This should be linked with thereactivity series in section 10.2 and redox insection 7.4.) Describe, in outline, the manufacture of:–– aluminium from pure aluminium oxide inmolten cryolite (refer to section 10.3)–– chlorine, hydrogen and sodium hydroxidefrom concentrated aqueoussodium chloride(Starting materials and essential conditionsshould be given but not technical details ordiagrams.)6Chemical energetics6.1Energetics of a reactionCoreSupplement Describe the meaning of exothermic andendothermic reactions Interpret energy level diagrams showingexothermic and endothermic reactionsDescribe bond breaking as an endothermicprocess and bond forming as an exothermicprocess Draw and label energy level diagrams forexothermic and endothermic reactions usingdata provided Calculate the energy of a reaction using bondenergies6.212Energy transferCoreSupplement Describe the release of heat energy byburning fuels State the use of hydrogen as a fuel Describe radioactive isotopes, such as 235U,as a source of energywww.cie.org.uk/igcseDescribe the use of hydrogen as a fuelreacting with oxygen to generate electricityin a fuel cell. (Details of the construction andoperation of a fuel cell are not required.)Back to contents page

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content7Chemical reactions7.1Physical and chemical changesCore Identify physical and chemical changes, andunderstand the differences between them7.2Rate (speed) of reactionCoreSupplement Describe and explain the effect ofconcentration, particle size, catalysts(including enzymes) and temperature on therate of reactions Devise and evaluate a suitable method forinvestigating the effect of a given variable onthe rate of a reaction Describe the application of the above factorsto the danger of explosive combustion withfine powders (e.g. flour mills) and gases (e.g.methane in mines) Demonstrate knowledge and understandingof a practical method for investigating therate of a reaction involving gas evolution Interpret data obtained from experimentsconcerned with rate of reactionDescribe and explain the effects oftemperature and concentration in terms ofcollisions between reacting particles. (Anincrease in temperature causes an increasein collision rate and more of the collidingmolecules have sufficient energy (activationenergy) to react whereas an increase inconcentration only causes an increase incollision rate.) Describe and explain the role of light inphotochemical reactions and the effect oflight on the rate of these reactions. (Thisshould be linked to section 14.4.) Describe the use of silver salts inphotography as a process of reduction ofsilver ions to silver; and photosynthesis as thereaction between carbon dioxide and waterin the presence of chlorophyll and sunlight(energy) to produce glucose and oxygenNote: Candidates should be encouraged to usethe term rate rather than speed.7.3Reversible reactionsCoreSupplement Predict the effect of changing the conditions(concentration, temperature and pressure) onother reversible reactions Demonstrate knowledge and understandingof the concept of equilibriumUnderstand that some chemical reactionscan be reversed by changing the reactionconditions. (Limited to the effects of heatand water on hydrated and anhydrouscopper(II) sulfate and cobalt(II) chloride.)(Concept of equilibrium is not required.)Back to contents pagewww.cie.org.uk/igcse13

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content7.4RedoxCoreSupplement Define redox in terms of electron transfer Identify redox reactions by changesin oxidation state and by the colourchanges involved when using acidifiedpotassium manganate(VII), andpotassium iodide. (Recall of equationsinvolving KMnO4 is not required.) Define oxidising agent as a substancewhich oxidises another substance during aredox reaction. Define reducing agent as asubstance which reduces another substanceduring a redox reaction. Identify oxidising agents and reducing agentsfrom simple equationsDefine oxidation and reduction in terms ofoxygen loss/gain. (Oxidation state limited toits use to name ions, e.g. iron(II), iron(III),copper(II), manganate(VII).)8Acids, bases and salts8.1The characteristic properties of acids and basesCoreSupplement Describe the characteristic properties of acidsas reactions with metals, bases, carbonatesand effect on litmus and methyl orange Define acids and bases in terms of protontransfer, limited to aqueous solutions Describe the characteristic properties ofbases as reactions with acids and withammonium salts and effect on litmus andmethyl orange Describe the meaning of weak and strongacids and bases Describe neutrality and relative acidity andalkalinity in terms of pH measured usingUniversal Indicator paper (whole numbersonly) Describe and explain the importance ofcontrolling acidity in soil8.2 Types of oxides14CoreSupplement Classify oxides as either acidic or basic,related to metallic and non-metallic characterwww.cie.org.uk/igcseFurther classify other oxides as neutral oramphotericBack to contents page

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content8.3Preparation of saltsCoreSupplement Demonstrate knowledge and understandingof the preparation of insoluble salts byprecipitation Suggest a method of making a given saltfrom a suitable starting material, givenappropriate informationDemonstrate knowledge and understandingof preparation, separation and purification ofsalts as examples of some of the techniquesspecified in section 2.2.2 and the reactionsspecified in section 8.18.4Identification of ions and gasesCore Describe the following tests to identify:aqueous cations:aluminium, ammonium, calcium,chromium(III), copper(II), iron(II), iron(III) andzinc (using aqueous sodium hydroxide andaqueous ammonia as appropriate). (Formulaeof complex ions are not required.)cations:use of the flame test to identify lithium,sodium, potassium and copper(II)anions:carbonate (by reaction with dilute acid andthen limewater), chloride, bromide and iodide(by reaction under acidic conditions withaqueous silver nitrate), nitrate (by reductionwith aluminium), sulfate (by reaction underacidic conditions with aqueous barium ions)and sulfite (by reaction with dilute acids andthen aqueous potassium manganate(VII))gases:ammonia (using damp red litmus paper),carbon dioxide (using limewater), chlorine(using damp litmus paper), hydrogen (usinglighted splint), oxygen (using a glowingsplint), and sulfur dioxide (using aqueouspotassium manganate(VII))Back to contents pagewww.cie.org.uk/igcse15

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content9The Periodic Table9.1The Periodic TableCore Describe the Periodic Table as a method ofclassifying elements and its use to predictproperties of elements9.2Periodic trendsCoreSupplement Describe the change from metallic to nonmetallic character across a period9.3Group propertiesCoreSupplement Describe lithium, sodium and potassiumin Group I as a collection of relatively softmetals showing a trend in melting point,density and reaction with water Predict the properties of other elements inGroup I, given data, where appropriate Describe the halogens, chlorine, bromine andiodine in Group VII, as a collection of diatomicnon-metals showing a trend in colour anddensity and state their reaction with otherhalide ions Predict the properties of other elements inGroup VII, given data where appropriate9.416Describe and explain the relationshipbetween Group number, number of outershell electrons and metallic/non-metalliccharacterIdentify trends in Groups, given informationabout the elements concernedTransition elementsCoreSupplement Describe the transition elements as acollection of metals having high densities,high melting points and forming colouredcompounds, and which, as elements andcompounds, often act as catalystswww.cie.org.uk/igcseKnow that transition elements have variableoxidation statesBack to contents page

Cambridge IGCSE Chemistry 0620 syllabus for 2019. Subject content9.5Noble gasesCore Describe the noble gases, in Group VIII or 0,as being unreactive, monoatomic gases andexplain this in terms of electronic structure State the uses of the noble gases in providingan inert atmosphere, i.e. argon in lamps,helium for filling balloons10Metals10.1 Properties of metalsCore List the general physical properties of metals Describe the general chemical properties ofmetals, e.g. reaction with dilute acids andreaction with oxygen Explain in terms of their properties why alloysare used instead of pure metals Identify representations of alloys fr

Changes to this syllabus for 2019 43 Changes to this syllabus The latest syllabus is version 3, published January 2019. There are no significant changes which affect teaching. Any textbooks endorsed to support the syllabus for examination from 2016 are still suitable for use with this syllabus.