C2.5 What are the properties of the transition metals? (separate science only) C2.5.1 recall the general properties of transition metals (melting point, density, reactivity, formation of coloured ions with different charges and uses as catalysts) and exemplify these by reference to copper, iron, chromium, silver and gold C2 The Periodic Table 32 Chapter C3 Chemicals of the natural environment C3.1 How are atoms held together in a metal? C3.1.1 describe the nature and arrangement of chemical bonds in metals C3 Structure and bonding 52 C3.1.2 explain how the bulk properties of metals are related to the type of bonds they contain C3 Structure and bonding 54 C3.2 How are metals with different reactivities extracted? C3.2.1 deduce an order of reactivity of metals based on experimental results including reactions with water, dilute acid and displacement reactions with other metals C5 Chemical Changes 84-87 C3.2.2 explain how the reactivity of metals with water or dilute acids is related to the tendency of the metal to form its positive ion to include potassium, sodium, calcium, aluminium, magnesium, zinc, iron, lead, [hydrogen], copper, silver C5 Chemical Changes 87 C3.2.3 use the names and symbols of common elements and compounds and the principle of conservation of mass to write formulae and balanced chemical equations and ionic equations C1 Atomic structure 6, 87 Ionic equations also mentioned C5 Chemical Changes: C4 Chemical Calculations Chapter also covers all this to Higher level C3.2.4 explain, using the position of carbon in the reactivity series, the principles of industrial processes used to extract metals, including the extraction of zinc C5 Chemical Changes 88 C3.2.5 explain why electrolysis is used to extract some metals from their ores C6 Electrolysis 106 C3.2.6 evaluate alternative biological methods of metal extraction (bacterial and phytoextraction) C14 The Earth's resources 212
C5.1.4 recall that chromatography involves a stationary and a mobile phase and that separation depends on the distribution between the phases C12 Chemical Analysis 182 C5.1.5 interpret chromatograms, including calculating Rf values C12 Chemical Analysis 183 C5.1.6 suggest chromatographic methods for distinguishing pure from impure substances PAG4 Including the use of: a) paper chromatography b) aqueous and non-aqueous solvents c) locating agents C12 Chemical Analysis 183 No mention of aqueous and non-aqueous solvents or locating agents C5.1.7 describe, explain and exemplify the processes of filtration, crystallisation, simple distillation, and fractional distillation PAG3, PAG7 C1 Atomic structure 8 C5.1.8 suggest suitable purification techniques given information about the substances involved PAG3, PAG7 C1 Atomic structure 8 C5.2 How do chemists find the composition of unknown samples? (separate science only) C5.2.1 describe the purpose of representative sampling in qualitative analysis Not explicit in book C5.2.2 interpret flame tests to identify metal ions, including the ions of lithium, sodium, potassium, calcium and copper C12 Chemical Analysis 186 C5.2.3 describe the technique of using flame tests to identify metal ions PAG5 C12 Chemical Analysis 186 C5.2.4 describe tests to identify aqueous cations and aqueous anions and identify species from test results including: PAG5 a) tests and expected results for metal ions in solution by precipitation reactions using dilute sodium hydroxide (calcium, copper, iron(II), iron(III), zinc) b) tests and expected results for carbonate ions (using dilute acid), chloride, bromide and iodide ions (using acidified dilute silver nitrate) and sulfate ions (using acidified dilute barium chloride or acidified barium nitrate) C12 Chemical Analysis C5.2.5 interpret an instrumental result for emission spectroscopy given appropriate data in chart or tabular form, when accompanied by a reference set in the same form C12 Chemical Analysis 190 0
C5.2.6 describe the advantages of instrumental methods of analysis (sensitivity, accuracy and speed) C12 Chemical Analysis 190 C5.2.7 interpret charts, particularly in spectroscopy C12 Chemical Analysis 193 Flame emission spectrum comparison question C5.3 How are the amounts of substances in reactions calculated? C5.3.1 recall and use the law of conservation of mass C1 Atomic structure 6 C5.3.2 explain any observed changes in mass in non-enclosed systems during a chemical reaction and explain them using the particle model C1 Atomic structure 6 C5.3.3 calculate relative formula masses of species separately and in a balanced chemical equation C4 Chemical Calculations 62 C5.3.4 recall and use the definitions of the Avogadro constant (in standard form) and of the mole C4 Chemical Calculations 62 C5.3.5 explain how the mass of a given substance is related to the amount of that substance in moles and vice versa and use the relationship: number of moles = mass of substance (g) relative formula mass (g) C4 Chemical Calculations 62 C5.3.6 deduce the stoichiometry of an equation from the masses of reactants and products and explain the effect of a limiting quantity of a reactant C4 Chemical Calculations 67 C5.3.7 use a balanced equation to calculate masses of reactants or products C4 Chemical Calculations 64 C5.3.8 use arithmetic computation, ratio, percentage and multistep calculations throughout quantitative chemistry C4 Chemical Calculations 66 C5.3.9 carry out calculations with numbers written in standard form when using the Avogadro constant C4 Chemical Calculations 63 C5.3.10 change the subject of a mathematical equation C4 Chemical Calculations Throughout chapter C5.3.11 calculate the theoretical amount of a product from a given amount of reactant (separate science only) C4 Chemical Calculations 68 C5.3.12 calculate the percentage yield of a reaction product from the actual yield of a reaction (separate science only) C4 Chemical Calculations 69
C1.1.4 use data to predict states of substances under given conditions C2 Structure, bonding and the properties of matter 68 C1.1.5 interpret evidence for how it is thought the atmosphere was originally formed C9 The atmosphere 296 C1.1.6 describe how it is thought an oxygen-rich atmosphere developed over time C9 The atmosphere 298 C1.1.7 describe the major sources of carbon monoxide and particulates (incomplete combustion), sulfur dioxide (combustion of sulfur impurities in fuels), oxides of nitrogen (oxidation of nitrogen at high temperatures and further oxidation in the air) C9 The atmosphere 312 C1.1.8 explain the problems caused by increased amounts of these substances and describe approaches to decreasing the emissions of these substances into the atmosphere including the use of catalytic converters, low sulfur petrol and gas scrubbers to decrease emissions C9 The atmosphere 314 C1.1.9 use chemical symbols to write the formulae of elements and simple covalent compounds C1 Atomic structure and the periodic table 14 C1.1.10 use the names and symbols of common elements and compounds and the principle of conservation of mass to write formulae and balanced chemical equations C3 Chemical quantities and calculations 98 C1.1.11 use arithmetic computations and ratios when balancing equations C9 The atmosphere 316 C1.1.12 describe tests to identify oxygen, hydrogen and carbon dioxide C8 Chemical Analysis 272 C1.1.13 explain oxidation in terms of gain of oxygen C4 Chemical Changes 132 C1.2 Why are there temperature changes in chemical reactions? C1.2.1 distinguish between endothermic and exothermic reactions on the basis of the temperature change of the surroundings C5 Energy Changes 178 C1.2.2 draw and label a reaction profile for an exothermic and an endothermic reaction, identifying activation energy C5 Energy Changes 178 C1.2.3 explain activation energy as the energy needed for a reaction to occur C5 Energy Changes 178
C2.2.3 describe how discovery of new elements and the ordering elements by atomic number supports Mendeleev’s decisions to leave gaps and reorder some elements C1 Atomic structure and the periodic table 32 C2.2.4 describe metals and non-metals and explain the differences between them on the basis of their characteristic physical and chemical properties, including melting point, boiling point, state and appearance, density, formulae of compounds, relative reactivity and electrical conductivity C1 Atomic structure and the periodic table 34 C2.2.5 recall the simple properties of Group 1 elements including their reaction with moist air, water, and chlorine C1 Atomic structure and the periodic table 42 C2.2.6 recall the simple properties of Group 7 elements including their states and colours at room temperature and pressure, their colours as gases, their reactions with Group 1 elements and their displacement reactions with other metal halides C1 Atomic structure and the periodic table 44 C2.2.7 predict possible reactions and probable reactivity of elements from their positions in the Periodic Table C1 Atomic structure and the periodic table 46 C2.2.8 describe experiments to identify the reactivity pattern of Group 7 elements including displacement reactions PAG1 C1 Atomic structure and the periodic table 45 C2.2.9 describe experiments to identify the reactivity pattern of Group 1 elements C1 Atomic structure and the periodic table 42 C2.3 How do metals and non-metals combine to form compounds? C2.3.1 recall the simple properties of Group 0 including their low melting and boiling points, their state at room temperature and pressure and their lack of chemical reactivity C1 Atomic structure and the periodic table 40 C2.3.2 explain how observed simple properties of Groups 1, 7 and 0 depend on the outer shell of electrons of the atoms and predict properties from given trends down the groups C1 Atomic structure and the periodic table 47 C2.3.3 explain how the reactions of elements are related to the arrangement of electrons in their atoms and hence to their atomic number C1 Atomic structure and the periodic table 28 C2.3.4 explain how the atomic structure of metals and non-metals relates to their position in the Periodic Table C1 Atomic structure and the periodic table 36
C3.4.6 deduce the empirical formula of a compound from the relative numbers of atoms present or from a model or diagram and vice versa C3 Chemical quantities and calculations 91 C3.4.7 use arithmetic computation and ratio when determining empirical formulae C3 Chemical quantities and calculations 110 Use of ratios but not for empirical formulae C3.4.8 describe the arrangement of chemical bonds in simple molecules C2 Structure, bonding and the properties of matter 58 C3.4.9 explain covalent bonding in terms of the sharing of electrons C2 Structure, bonding and the properties of matter 64 C3.4.10 construct dot and cross diagrams for simple covalent substances C2 Structure, bonding and the properties of matter 64 C3.4.11 represent three dimensional shapes in two dimensions and vice versa when looking at chemical structures for simple molecules C2 Structure, bonding and the properties of matter 90 C3.4.12 describe the limitations of dot and cross diagrams, ball and stick models and two and three dimensional representations when used to represent simple molecules C2 Structure, bonding and the properties of matter 62-65 C3.4.13 translate information between diagrammatic and numerical forms C2 Structure, bonding and the properties of matter 90 C3.4.14 explain how the bulk properties of simple molecules are related to the covalent bonds they contain and their bond strengths in relation to intermolecular forces C2 Structure, bonding and the properties of matter 64 Also C7 Page 254 C3.4.15 describe the production of materials that are more useful by cracking C7 Hydrocarbons 236 C3.4.16 recognise functional groups and identify members of the same homologous series (separate science only) C7 Hydrocarbons 238-245 Alkenes 240, Alcohols 242, Carboxylic Acids 244 C3.4.17 name and draw the structural formulae, using fully displayed formulae, of the first four members of the straight chain alkanes and alkenes, alcohols and carboxylic acids (separate science only) C7 Hydrocarbons 238-245 Alkenes 240, Alcohols 242, Carboxylic Acids 244
C4.3 How do bonding and structure affect the properties of materials? C4.3.1 explain how the bulk properties of materials (including strength, melting point, electrical and thermal conductivity, brittleness, flexibility, hardness and ease of reshaping) are related to the different types of bonds they contain, their bond strengths in relation to intermolecular forces and the ways in which their bonds are arranged, recognising that the atoms themselves do not have these properties C2 Structure, bonding and the properties of matter 58 Also C7 Page 254 C4.3.2 recall that carbon can form four covalent bonds C2 Structure, bonding and the properties of matter 76-84 C4.3.3 explain that the vast array of natural and synthetic organic compounds occurs due to the ability of carbon to form families of similar compounds, chains and rings C2 Structure, bonding and the properties of matter 76-84 C4.3.4 describe the nature and arrangement of chemical bonds in polymers with reference to their properties including strength, flexibility or stiffness, hardness and melting point of the solid C2 Structure, bonding and the properties of matter 74 C4.3.5 describe the nature and arrangement of chemical bonds in giant covalent structures C2 Structure, bonding and the properties of matter 76 C4.3.6 explain the properties of diamond and graphite in terms of their structures and bonding, include melting point, hardness and (for graphite) conductivity and lubricating action C2 Structure, bonding and the properties of matter 77 Diamond pg 80, Graphite pg 82, pg 84 C4.3.7 represent three dimensional shapes in two dimensions and vice versa when looking at chemical structures e.g. allotropes of carbon C2 Structure, bonding and the properties of matter 90 C4.3.8 describe and compare the nature and arrangement of chemical bonds in ionic compounds, simple molecules, giant covalent structures, polymers and metals C2 Structure, bonding and the properties of matter 56-64 C4.4 Why are nanoparticles so useful? C4.4.1 compare ‘nano’ dimensions to typical dimensions of atoms and molecules C2 Structure, bonding and the properties of matter 86 C4.4.2 describe the surface area to volume relationship for different-sized particles and describe how this affects properties C2 Structure, bonding and the properties of matter 87
C3.3.2 predict the products of electrolysis of binary ionic compounds in the molten state C4 Chemical Changes 117 C3.3.3 recall that metals (or hydrogen) are formed at the cathode and non-metals are formed at the anode in electrolysis using inert electrodes C4 Chemical Changes 117 C3.3.4 use the names and symbols of common elements and compounds and the principle of conservation of mass to write half equations C4 Chemical Changes 104 Also C11 page 289 C3.3.5 explain reduction and oxidation in terms of gain or loss of electrons, identifying which species are oxidised and which are reduced C4 Chemical Changes 103 C3.3.6 explain how electrolysis is used to extract some metals from their ores including the extraction of aluminium C4 Chemical Changes 119 C3.3.7 describe competing reactions in the electrolysis of aqueous solutions of ionic compounds in terms of the different species present, including the formation of oxygen, chlorine and the discharge of metals or hydrogen linked to their relative reactivity C4 Chemical Changes 120 C3.3.8 describe the technique of electrolysis of an aqueous solution of a salt PAG2 C4 Chemical Changes 121 C3.4 Why is crude oil important as a source of new materials? C3.4.1 recall that crude oil is a main source of hydrocarbons and is a feedstock for the petrochemical industry C7 Organic Chemistry 171 C3.4.2 explain how modern life is crucially dependent upon hydrocarbons and recognise that crude oil is a finite resource C7 Organic Chemistry 172 C3.4.3 describe and explain the separation of crude oil by fractional distillation PAG3 C7 Organic Chemistry 173 C3.4.4 describe the fractions of crude oil as largely a mixture of compounds of formula CnH2n+2 which are members of the alkane homologous series C7 Organic Chemistry 172 C3.4.5 use ideas about energy transfers and the relative strength of chemical bonds and intermolecular forces to explain the different temperatures at which changes of state occur C2 Bonding, Structure and the properties of matter 39
C3.4.18 predict the formulae and structures of products of reactions (combustion, addition across a double bond and oxidation of alcohols to carboxylic acids) of the first four and other given members of these homologous series (separate science only) C7 Organic Chemistry Alkanes 172, Alkenes 177, Alcohols 181, Carboxylic Acids 183 C3.4.19 recall that it is the generality of reactions of functional groups that determine the reactions of organic compounds (separate science only) C7 Organic Chemistry Alkanes 172, Alkenes 177, Alcohols 181, Carboxylic Acids 183
C4.3 How do bonding and structure affect the properties of materials? C4.3.1 explain how the bulk properties of materials (including strength, melting point, electrical and thermal conductivity, brittleness, flexibility, hardness and ease of reshaping) are related to the different types of bonds they contain, their bond strengths in relation to intermolecular forces and the ways in which their bonds are arranged, recognising that the atoms themselves do not have these properties C2 Bonding, Structure and the properties of matter 39 C4.3.2 recall that carbon can form four covalent bonds Not explicit C4.3.3 explain that the vast array of natural and synthetic organic compounds occurs due to the ability of carbon to form families of similar compounds, chains and rings C2 Bonding, Structure and the properties of matter 54 C4.3.4 describe the nature and arrangement of chemical bonds in polymers with reference to their properties including strength, flexibility or stiffness, hardness and melting point of the solid C2 Bonding, Structure and the properties of matter 43 C4.3.5 describe the nature and arrangement of chemical bonds in giant covalent structures C2 Bonding, Structure and the properties of matter 44 C4.3.6 explain the properties of diamond and graphite in terms of their structures and bonding, include melting point, hardness and (for graphite) conductivity and lubricating action C2 Bonding, Structure and the properties of matter 54-55 C4.3.7 represent three dimensional shapes in two dimensions and vice versa when looking at chemical structures e.g. allotropes of carbon C2 Bonding, Structure and the properties of matter 54-55 C4.3.8 describe and compare the nature and arrangement of chemical bonds in ionic compounds, simple molecules, giant covalent structures, polymers and metals C2 Bonding, Structure and the properties of matter 33-46 Not direct comparison but all the information is given to allow comparison
C4.4 Why are nanoparticles so useful? C4.4.1 compare ‘nano’ dimensions to typical dimensions of atoms and molecules C2 Bonding, Structure and the properties of matter 51 C4.4.2 describe the surface area to volume relationship for different-sized particles and describe how this affects properties C2 Bonding, Structure and the properties of matter 52 C4.4.3 describe how the properties of nanoparticulate materials are related to their uses including properties which arise from their size, surface area and arrangement of atoms in tubes or rings C2 Bonding, Structure and the properties of matter 52 C4.4.4 explain the properties fullerenes and graphene in terms of their structures C2 Bonding, Structure and the properties of matter 55 C4.4.5 explain the possible risks associated with some nanoparticulate materials including: a) possible effects on health due to their size and surface area b) reasons that there is more data about uses of nanoparticles than about possible health effects c) the relative risks and benefits of using nanoparticles for different purposes C2 Bonding, Structure and the properties of matter 53 C4.4.6 estimate size and scale of atoms and nanoparticles including the ideas that: a) nanotechnology is the use and control of structures that are very small (1 to 100 nanometres in size) b) data expressed in nanometres is used to compare the sizes of nanoparticles, atoms and molecules C2 Bonding, Structure and the properties of matter 51 C4.4.7 interpret, order and calculate with numbers written in standard form when dealing with nanoparticles C2 Bonding, Structure and the properties of matter 51 C4.4.8 use ratios when considering relative sizes and surface area to volume comparisons C2 Bonding, Structure and the properties of matter 52 C4.4.9 calculate surface areas and volumes of cubes C2 Bonding, Structure and the properties of matter 52
C6.2.3 explain the effects on rates of reaction of changes in the size of the pieces of a reacting solid in terms of surface area to volume ratio C6 The rate and extent of chemical change 153 C6.2.4 describe the characteristics of catalysts and their effect on rates of reaction C6 The rate and extent of chemical change 153 C6.2.5 identify catalysts in reactions C6 The rate and extent of chemical change 153 C6.2.6 explain catalytic action in terms of activation energy C6 The rate and extent of chemical change 153 C6.2.7 suggest practical methods for determining the rate of a given reaction including: PAG8 for reactions that produce gases: i. gas syringes or collection over water can be used to measure the volume of gas produced ii. mass change can be followed using a balance measurement of physical factors: iii. colour change iv. formation of a precipitate C6 The rate and extent of chemical change 156 C6.2.8 interpret rate of reaction graphs C6 The rate and extent of chemical change 150 C6.2.9 interpret graphs of reaction conditions versus rate (separate science only) i an understanding of orders of reaction is not required C6 The rate and extent of chemical change 150 C6.2.10 use arithmetic computation and ratios when measuring rates of reaction C6 The rate and extent of chemical change 150 Questions C6.2.11 draw and interpret appropriate graphs from data to determine rate of reaction C6 The rate and extent of chemical change 150 Questions C6.2.12 determine gradients of graphs as a measure of rate of change to determine rate C6 The rate and extent of chemical change 150 C6.2.13 use proportionality when comparing factors affecting rate of reaction Not obvious C6.2.14 describe the use of enzymes as catalysts in biological systems and some industrial processes C6 The rate and extent of chemical change 154