S/N CHEMISTRY 5073 SCIENCE (CHEMISTRY) 5076 / 5078

Transcription

1 1 EXPERIMENTAL DESIGN EXPERIMENTAL DESIGN Apparatus to measure time, temperature, mass and volume Apparatus to measure time, temperature, mass and volume Suggest suitable apparatus for simple experiments, like o Collection of gases o Measurement of rates of reaction 2 METHODS OF PURIFICATION AND ANALYSIS Suggest suitable apparatus for simple experiments, like o Collection of gases o Measurement of rates of reaction METHODS OF PURIFICATION AND ANALYSIS Methods of separation and purification: o Use of a suitable solvent o Filtration o Crystallisation o Evaporation o Sublimation o Distillation o Fractional distillation o Use of separating funnel o Paper chromatography Methods of separate mixtures: o Solid-solid o Solid-liquid o Liquid-liquid (miscible and immiscible) Methods of separation and purification: o Use of a suitable solvent o Filtration o Crystallisation o Evaporation o Distillation o Fractional distillation o Paper chromatography Methods of separate mixtures: o Solid-solid o Solid-liquid o Liquid-liquid (miscible) Interpret paper chromatograms Interpret paper chromatograms (include R f values) Analyse purity of substance by melting and boiling point Use of locating agent in chromatograms Analyse purity of substance by melting and boiling point Importance of purity (e.g. foodstuff, drugs) 1

2 3 QUALITATIVE ANALYSIS QUALITATIVE ANALYSIS Identify aqueous cations using aqueous sodium hydroxide and aqueous ammonia: o Aluminium o Ammonium o Calcium o Copper(II) o Iron(II) o Iron(III) o Lead(II) o Zinc Identify anions: o Carbonate (add dilute acid and subsequent use of limewater) o Chloride (react nitric acid and aqueous silver nitrate) o Iodide (react nitric acid and aqueous silver nitrate) o Nitrate (reduction with aluminium in sodium hydroxide to ammonia and subsequent use of litmus paper) o Sulfate (react nitric acid and aqueous barium nitrate) Identify gases: o Ammonia (use damp red litmus paper) o Carbon dioxide (use limewater) o Chlorine (use damp litmus paper) o Hydrogen (use burning splint) o Oxygen (use a glowing splint) o Sulfur dioxide (use acidified potassium manganate(vii)) Identify aqueous cations using aqueous sodium hydroxide and aqueous ammonia: o Ammonium o Calcium o Copper(II) o Iron(II) o Iron(III) o Lead(II) o Zinc Identify anions: o Carbonate (add dilute acid and subsequent use of limewater) o Chloride (react nitric acid and aqueous silver nitrate) o Nitrate (reduction with aluminium in sodium hydroxide to ammonia and subsequent use of litmus paper) o Sulfate (react nitric acid and aqueous barium nitrate) Identify gases: o Ammonia (use damp red litmus paper) o Carbon dioxide (use limewater) o Chlorine (use damp litmus paper) o Hydrogen (use burning splint) o Oxygen (use a glowing splint) o Sulfur dioxide (use acidified potassium manganate(vii)) 2

3 4 KINETIC PARTICLE THEORY KINETIC PARTICLE THEORY Describe solid, liquid and gaseous states of matter Describe solid, liquid and gaseous states of matter Explain inter-conversion in terms of kinetic particle theory and energy changes involved Explain inter-conversion in terms of kinetic particle theory and energy changes involved Explain diffusion in terms of particles Rate of diffusion is affected by o Molecular mass o Temperature 5 ATOMIC STRUCTURE ATOMIC STRUCTURE Relative charges & approximate relative masses of proton, neutron and electron Relative charges & approximate relative masses of proton, neutron and electron Structure of atom o Protons and neutrons (nucleons) in nucleus o Electrons arranged in shells (energy level) Structure of atom o Protons and neutrons (nucleons) in nucleus o Electrons arranged in shells (energy level) Define proton (atomic) number and nucleon (mass) number Define proton (atomic) number and nucleon (mass) number 12 Interpret and use symbols like 6 C 12 Interpret and use symbols like 6 C Define isotopes Define isotopes Deduce number of protons, neutrons and electrons in atoms and ions given proton and nucleon numbers Deduce number of protons, neutrons and electrons in atoms and ions given proton and nucleon numbers 3

4 6 STRUCTURES AND PROPERTIES OF MATERIALS STRUCTURES AND PROPERTIES OF MATERIALS Compare elements, compounds and mixtures Compare elements, compounds and mixtures Compare structure of simple molecular substance (e.g. methane) with those of giant molecular structure (e.g. diamond) to deduce their properties Compare bonding and structure of diamond and graphite to deduce their properties (e.g. electrical conductivity, lubricating or cutting action) Deduce physical and chemical properties of substances from structures and bonding and vice versa 7 IONIC BONDING IONIC BONDING Describe formation of ions by electron loss/gain to obtain electronic configuration of noble gas Describe formation of ions by electron loss/gain to obtain electronic configuration of noble gas Describe formation of ionic bonds between metals and nonmetals Describe formation of ionic bonds between metals and nonmetals State that ionic materials contain giant lattice (ions held by electrostatic attraction) Relate physical properties (include electrical property) of ionic compounds to lattice structure. Deduce formulae of ionic compounds (binary compounds only) from diagrams of lattice structure Relate physical properties (include electrical property) of ionic compounds to lattice structure. 4

5 8 COVALENT BONDING COVALENT BONDING Describe formation of covalent bond by sharing electrons to gain electronic configuration of noble gas Describe formation of covalent bond by sharing electrons to gain electronic configuration of noble gas Describe formation of covalent bonds between non-metallic elements (use dot and cross diagrams) Describe formation of covalent bonds between non-metallic elements (use dot and cross diagrams) Deduce arrangement of electrons in other covalent molecules Deduce arrangement of electrons in other covalent molecules Relate physical properties (include electrical property) of covalent compounds to structure and bonding. 9 METALLIC BONDING - Relate physical properties (include electrical property) of covalent compounds to structure and bonding. Describe metal as lattice of positive ions in sea of electrons Relate electrical conductivity of metals to mobility of electrons in structure 5

6 10 FORMULAE, STOICHIOMETRY AND THE MOLE CONCEPT FORMULAE, STOICHIOMETRY AND THE MOLE CONCEPT State symbols of elements and formulae of compounds in syllabus State symbols of elements and formulae of compounds in syllabus Deduce formulae of simple compounds from relative numbers of atoms present and vice versa Deduce formulae of simple compounds from relative numbers of atoms present and vice versa Deduce formulae of ionic compounds from charges on ions present and vice versa Deduce formulae of ionic compounds from charges on ions present and vice versa Interpret chemical equations with state symbols Interpret chemical equations with state symbols Construct chemical equations, with state symbols, including ionic equations Construct chemical equations, with state symbols, including ionic equations Define relative atomic mass A r and relative molecular mass (and relative formula mass) M r (include calculating M r ) Define relative atomic mass A r and relative molecular mass (and relative formula mass) M r (include calculating M r ) Calculate percentage mass of an element in a compound Calculate empirical and molecular formulae Calculate stoichiometric reacting masses and volumes of gases (1 mole of gas occupies 24 dm 3 at room condition) Calculation involving idea of limiting reactants Calculate stoichiometric reacting masses and volumes of gases (1 mole of gas occupies 24 dm 3 at room condition) Calculation involving idea of limiting reactants Apply concept of solution concentration (in mol/dm 3 or g/dm 3 ) for volumetric experiments and solve problems Apply concept of solution concentration (in mol/dm 3 or g/dm 3 ) for volumetric experiments and solve problems Calculate % yield and % purity 6

7 11 ELECTROLYSIS - Describe electrolysis as conduction of electricity by ionic compound when molten or dissolved in water (electrolyte), leading to decomposition of electrolyte Describe electrolysis as evidence for existence of ions held in lattice structure when solid but free to move when molten or in solution Describe electrolysis of molten sodium chloride, using inert electrodes, in terms of mobility of ions present and electrode products Predict likely products of electrolysis of molten binary compound Apply idea of selective discharged based on: (using inert electrodes) o Cations: linked to reactivity series o Anions: halides, hydroxides and sulfates o Concentration effect Predict likely products of electrolysis of aqueous electrolyte Construct ionic equations for reactions occurring at electrodes during electrolysis Describe electrolysis of aqueous copper(ii) sulfate with copper electrodes (copper purification) Describe electroplating and one use of electroplating Describe production of electrical energy from simple cell linked to reactivity series and redox reactions 7

8 12 ENERGY FROM CHEMICALS ENERGY FROM CHEMICALS Describe enthalpy change in terms of exothermic (ΔH negative) and endothermic (ΔH positive) reactions Represent energy changes by energy profile diagrams, in including reaction enthalpy changes and activation energies Describe bond breaking as endothermic process and bond making as exothermic process Describe exothermic as process or chemical reaction which o Transfer energy, often as heat, to the surroundings o May be detected by an increase in temperature Describe exothermic as process or chemical reaction which o Transfer energy, often as heat, from the surroundings o May be detected by a decrease in temperature Explain overall enthalpy changes in terms of energy changes associated with breaking and making of covalent bonds Describe hydrogen, derived from water or hydrocarbons, as potential fuel, reacting with oxygen to generate electricity in a fuel cell 8

9 13 SPEED OF REACTION SPEED OF REACTION Explain, in terms of collision between reacting particles, speed of reaction can be affected by o Concentration o Pressure o Particle size o Temperature Explain, in terms of collision between reacting particles, speed of reaction can be affected by o Concentration o Pressure o Particle size o Temperature Define catalyst and describe its effect (include enzymes) on speeds of reactions Interpret data obtained from experiments concerned with speed of reaction Explain how pathways of lower activation energies account for increase in speed of reaction. State that some compounds act as catalysts in industrial processes and that enzymes are biological catalysts Suggest suitable method to investigate effect of given variable on speed of reaction Interpret data obtained from experiments concerned with speed of reaction 9

10 14 REDOX REDOX Define oxidation and reduction (redox) in terms of o Oxygen/hydrogen gain/loss o Electron transfer o Changes in oxidation state Define oxidation and reduction (redox) in terms of o Oxygen/hydrogen gain/loss o Electron transfer o Changes in oxidation state Identify redox reactions in terms of o Oxygen/hydrogen gain/loss o Electron gain/loss o Changes in oxidation state Describe use of aqueous potassium iodide and acidified potassium manganate(vii) to test for oxidising and reducing agents from resulting colour changes Describe use of aqueous potassium iodide and acidified potassium manganate(vii) to test for oxidising and reducing agents from resulting colour changes 10

11 15 ACIDS AND BASES ACIDS AND BASES Describe meanings of acids and alkalis in terms of ions produce in aqueous solution and effect on Universal Indicator Describe meanings of acids and alkalis in terms of ions produce in aqueous solution and effect on Universal Indicator Describe test for hydrogen ion concentration and hence relative acidity using Universal Indicator and ph scale Describe test for hydrogen ion concentration and hence relative acidity using Universal Indicator and ph scale Compare strong and weak acids based on extent of ionisation Describe characteristic properties of acids as in reactions with metals, bases and carbonates. Describe characteristic properties of acids as in reactions with metals, bases and carbonates. State the uses of sulfuric acid (manufacturing detergent and fertiliser; as battery acid) Describe H + + OH H 2 O as neutralisation Describe H + + OH H 2 O as neutralisation Describe importance of controlling ph in soil and treating excess acidity using calcium hydroxide Describe characteristic properties of bases in reactions with acids and with ammonium salts Describe importance of controlling ph in soil and treating excess acidity using calcium hydroxide Classify oxides, based on metallic/non-metallic character, as acidic, basic, amphoteric or neutral Describe characteristic properties of bases in reactions with acids and with ammonium salts Classify oxides, based on metallic/non-metallic character, as acidic, basic, amphoteric or neutral 11

12 16 SALTS SALTS Describe techniques used to prepare, separate and purify salts Describe techniques used to prepare, separate and purify salts Describe general rules of solubility for common salts, include o Nitrates o Chlorides (including silver and lead) o Sulfates (including barium, calcium and lead) o Carbons o Hydroxides o Group I cations o Ammonium salts Suggest method to prepare salt from suitable starting materials, include o Precipitation o Titration o Reactions of acids with metals, insoluble bases and insoluble carbonates Suggest method to prepare salt from suitable starting materials, include o Precipitation o Titration o Reactions of acids with metals, insoluble bases and insoluble carbonates 17 AMMONIA - Describe use of nitrogen (from air) and hydrogen (from cracking of crude oil) to manufacture ammonia State that some chemical reactions are reversible, like manufacture of ammonia Describe essential conditions to manufacture ammonia by Haber process Describe displacement of ammonia from its salts 12

13 18 PERIODIC TRENDS PERIODIC TRENDS Describe Periodic Table as arrangement of elements in increasing proton (atomic) number Describe Periodic Table as arrangement of elements in increasing proton (atomic) number Describe how position of element in Periodic Table is related to proton number and electronic structure Describe how position of element in Periodic Table is related to proton number and electronic structure Describe relationship between group number and ionic charge of element Explain similarities between elements in same group of Periodic Table in terms of electronic structure Explain similarities between elements in same group of Periodic Table in terms of electronic structure Describe change from metallic to non-metallic character from left to right across a periodic of the Periodic Table Describe change from metallic to non-metallic character from left to right across a periodic of the Periodic Table Describe the relationship between group number, number of valency electrons and metallic/non-metallic character Describe the relationship between group number, number of valency electrons and metallic/non-metallic character Predict properties of elements in Group I and VII using Periodic Table Predict properties of elements in Group I and VII using Periodic Table 13

14 19 GROUP PROPERTIES GROUP PROPERTIES Describe lithium, sodium and potassium in Group I (alkali metals) as o Relatively soft o Low density o Showing trend in melting point and reaction with water Describe lithium, sodium and potassium in Group I (alkali metals) as o Relatively soft o Low density o Showing trend in melting point and reaction with water Describe chlorine, bromine and iodine in Group VII (halogens) as o Diatomic non-metals o Showing trend in colour state and displacement reactions with solutions of other halide ions Describe chlorine, bromine and iodine in Group VII (halogens) as o Diatomic non-metals o Showing trend in colour state and displacement reactions with solutions of other halide ions Describe Group 0 elements (noble gases) as monatomic elements that are chemical unreactive and hence important in providing an inert atmosphere (e.g. argon and neon in light bulbs, helium in balloons, argon in manufacture of steel) Describe lack of reactivity of noble gases in terms of electronic structures Describe lack of reactivity of noble gases in terms of electronic structures 20 TRANSITION ELEMENTS - Describe transition elements as metals with o High melting points o High density o Variable oxidation state o Forming coloured compounds State that elements and/or their compounds can often act as catalysts 14

15 21 PROPERTIES OF METALS PROPERTIES OF METALS Describe general physical properties of metals as solids having high melting and boiling points, malleable, good conductors of heat and electricity in terms of structure Describe general physical properties of metals as solids having high melting and boiling points, malleable, good conductors of heat and electricity in terms of structure Describe alloys (e.g. brass, stainless steel) as mixture of metal with another element Describe alloys (e.g. brass, stainless steel) as mixture of metal with another element Identify representation of metals and alloys from diagrams of structure Identify representation of metals and alloys from diagrams of structure Explain why alloys have different physical properties to their constituent elements 22 REACTIVITY SERIES REACTIVITY SERIES Place calcium, copper, (hydrogen), iron, lead, magnesium, potassium, silver, sodium, zinc in the reactivity series, referring to: o Reactions with water, steam, dilute hydrochloric acid o Reduction of oxides by carbon and/or by hydrogen Describe reactivity series as related to tendency of metal to form position ion, illustrated by reactions with o Aqueous ions of other listed metals o Oxides with other listed metals Place calcium, copper, (hydrogen), iron, lead, magnesium, potassium, silver, sodium, zinc in the reactivity series, referring to: o Reactions with water, steam, dilute hydrochloric acid Deduce order of reactivity from given set of experimental results Deduce order of reactivity from given set of experimental results Describe action of heat on carbons of listed metals and relate thermal stability to the reactivity series 15

16 23 EXTRACTION OF METALS Describe ease of obtaining metals from their ores by relating elements to positions in reactivity series 24 RECYCLING OF METALS EXTRACTION OF METALS Describe ease of obtaining metals from their ores by relating elements to positions in reactivity series RECYCLING OF METALS Describe metal ores as finite resource and hence the need to recycle metals Describe metal ores as finite resource and hence the need to recycle metals 25 IRON Discuss social, economic and environmental issues of recycling metals IRON Discuss social, economic and environmental issues of recycling metals Describe and explain essential reactions in iron extraction using haematite, limestone and coke in blast furnace Describe and explain essential reactions in iron extraction using haematite, limestone and coke in blast furnace Describe steels as alloys of iron with carbon or other metals and controlled use of additive changes properties of iron State uses of mild steel (e.g. machinery) and stainless steel (e.g. surgical instruments) Describe essential conditions for corrosion (rusting) of iron Prevention of rusting o Placing a barrier (e.g. painting, greasing, plastic coating) Describe essential conditions for corrosion (rusting) of iron Prevention of rusting o Placing a barrier (e.g. painting, greasing, plastic coating) o Sacrificial protection by a more reactive metal which corrodes preferentially (e.g. underwater pipes have a piece of magnesium attached to them) 16

17 26 AIR AIR Describe volume composition of gases in dry air Describe volume composition of gases in dry air Name common atmospheric pollutants Name common atmospheric pollutants State sources of atmospheric pollutants: o Carbon monoxide o Nitrogen oxides o Sulfur dioxide State sources of atmospheric pollutants: o Carbon monoxide o Nitrogen oxides o Sulfur dioxide Describe reactions as solutions to problems caused by pollutants: o Catalytic converter o Flue gas desulfurisation Describe effects of pollutants on health and environment: o Poisonous nature of carbon monoxide o Role of nitrogen dioxide and sulfur dioxide in formation of acid rain and effect on respiration and building Describe effects of pollutants on health and environment: o Poisonous nature of carbon monoxide o Role of nitrogen dioxide and sulfur dioxide in formation of acid rain and effect on respiration and building Discuss importance of ozone layers and problems involved with depletion of ozone layer by reaction with chlorofluorocarbons (CFCs) Describe carbon cycle in simple terms, to include o Combustion, respiration, photosynthesis o Regulation of amount of carbon dioxide in atmosphere State that greenhouse gases (e.g. carbon dioxide and methane) may contribute to global warming, give the sources of these gases and discuss possible consequences of an increase in global warming 17

18 27 FUELS AND CRUDE OIL FUELS AND CRUDE OIL Name natural gases, mainly methane, and petroleum as sources of energy Name natural gases, mainly methane, and petroleum as sources of energy Describe petroleum as mixture of hydrocarbons and its separating into useful fraction by fractional distillation Describe petroleum as mixture of hydrocarbons and its separating into useful fraction by fractional distillation Name and state the uses of the fractions: o Petrol (gasoline) o Naphtha o Paraffin (kerosene) o Diesel o Lubricating oils o Bitumen Name and state the uses of the fractions: o Petrol (gasoline) o Naphtha o Paraffin (kerosene) o Diesel o Lubricating oils o Bitumen Describe issues relating to competing uses of oil as energy source and as a chemical feedstock 18

19 28 ALKANES ALKANES Describe a homologous series as group of compounds with a general formula, similar chemical properties, showing graduation in physical properties as a result of increase in size and mass of molecules, e.g. melting and boiling points, viscosity, flammability Describe a homologous series as group of compounds with a general formula, similar chemical properties, showing graduation in physical properties as a result of increase in size and mass of molecules, e.g. melting and boiling points, viscosity, flammability Describe alkanes as homologous series of saturated hydrocarbon with general formula C n H 2n+2. Describe alkanes as homologous series of saturated hydrocarbon with general formula C n H 2n+2. Draw structure of branched and unbranched alkanes, C 1 to C 4 and name unbranched alkanes Draw structure of branched and unbranched alkanes, C 1 to C 3 and name unbranched alkanes Define isomerism and identify isomers Describe properties of alkanes (exemplified by methane) as being generally unreactive except in terms of combustion and substitution by chlorine Describe properties of alkanes (exemplified by methane) as being generally unreactive except in terms of combustion and substitution by chlorine 19

20 29 ALKENES ALKENES Describe alkenes as homologous series of unsaturated hydrocarbon with general formula C n H 2n Describe alkenes as homologous series of unsaturated hydrocarbon with general formula C n H 2n Draw structures of branched and unbranched alkenes, C 2 to C 4, and name the unbranched alkenes Draw structures of branched and unbranched alkenes, C 2 to C 3, and name the unbranched alkenes Describe manufacture of alkenes and hydrogen by cracking hydrocarbons and recognise that cracking is essential to match demand for fractions containing smaller molecules from refinery process Describe manufacture of alkenes and hydrogen by cracking hydrocarbons and recognise that cracking is essential to match demand for fractions containing smaller molecules from refinery process Compare saturated and unsaturated hydrocarbons from molecular structures and by using aqueous bromine Compare saturated and unsaturated hydrocarbons from molecular structures and by using aqueous bromine Descry properties of alkenes (exemplified by ethene) in terms of combustion, polymerisation and addition reactions with bromine, steam and hydrogen Descry properties of alkenes (exemplified by ethene) in terms of combustion, polymerisation and addition reactions with bromine and hydrogen State the meaning of polyunsaturated when applied to food products State the meaning of polyunsaturated when applied to food products Describe manufacture of margarine by addition of hydrogen to unsaturated vegetable oils to form a solid product Describe manufacture of margarine by addition of hydrogen to unsaturated vegetable oils to form a solid product 20

21 30 ALCOHOLS ALCOHOLS Describe alcohols as homologous series containing OH group Describe alcohols as homologous series containing OH group Draw structures of alcohols, C 1 to C 4, and name unbranched alcohols Draw structures of alcohols, C 1 to C 3, and name unbranched alcohols Describe properties of alcohols in terms of combustion and oxidation to carboxylic acids Describe properties of alcohols in terms of combustion and oxidation to carboxylic acids Describe formation of ethanol by catalysed addition of steam to ethene and by fermentation of glucose Describe formation of ethanol by fermentation of glucose State some uses of ethanol (e.g. as a solvent, as a fuel, as a constituent of alcoholic beverages) 21

22 31 CARBOXYLIC ACIDS CARBOXYLIC ACIDS Describe carboxylic acids as an homologous series containing the CO 2 H group Describe carboxylic acids as an homologous series containing the CO 2 H group Draw structures of carboxylic acids, methanoic acid to butanoic acid and name unbranched acids Describe carboxylic acids as weak acids, reacting with carbonates, bases and some metals Describe formation of ethanoic acid by oxidation of ethanol by atmospheric oxygen or acidified potassium manganate(vii) Describe formation of ethanoic acid by oxidation of ethanol by atmospheric oxygen or acidified potassium manganate(vii) Describe reaction of carboxylic acid with alcohol to form ester, e.g. ethyl ethanoate State commercial uses of esters, e.g. flavourings, perfumes 22

23 32 MACROMOLECULES MACROMOLECULES (UNDER ALKENES) Describe macromolecules as large molecules built up from small units, different macromolecule having different units and/or different linkages Describe formation of poly(ethene) as example of addition polyermisation of ethene as monomer State uses of poly(ethene) as typical plastic (e.g. plastic bags) Deduce structure of polymer product from given monomer and vice versa Describe formation of poly(ethene) as example of addition polyermisation of ethene as monomer State uses of poly(ethene) as typical plastic (e.g. plastic bags) Deduce structure of addition polymer product from given monomer and vice versa Describe pollution problems causes by disposal of nonbiodegradable plastics Describe nylon, a polyamide and Terylene, a polyester, as condensation polymers, the partial structure of nylon being represented as and partial structure of Terylene as State some typical uses of man-made fibres like nylon and Terylene, e.g. clothing, fishing line, parachutes Describe pollution problems causes by disposal of nonbiodegradable plastics END 23