Complete lesson and workbook Content Understand why covalent compounds do not conduct electricity Understand why ionic compounds conduct electricity only when molten or in solution Know that anion and cation are terms used to refer to negative and positive ions respectively Describe experiments to investigate electrolysis, using inert electrodes, of molten compounds (including lead(II) bromide) and aqueous solutions (including sodium chloride, dilute sulfuric acid and copper(II) sulphate) and to predict the products electricity Write ionic half-equations representing the reactions at the electrodes during electrolysis and understand why these reactions are classified as oxidation or reduction Know that most metals are extracted from ores found in the Earth’s crust and that unreactive metals are often found as the uncombined element carbon Explain how the method of extraction of a metal is related to its position in the reactivity series, illustrated by carbon extraction for iron and electrolysis for aluminium Be able to comment on a metal extraction process, given appropriate information detailed knowledge of the processes used in the extraction of a specific metal is not required

Complete Lessons and workbook Content Know that alcohols contain the functional group OH Understand how to draw structural and displayed formulae for methanol, ethanol, propanol (propan-1-ol only) and butanol (butan-1-ol only), and name each compound (the names propanol and butanol are acceptable) Know that ethanol can be manufactured by: reacting ethene with steam in the presence of a phosphoric acid catalyst at a temperature of about 300 oC and a pressure of about 60–70 atm 2.the fermentation of glucose, in the absence of air, at an optimum temperature of about 30 oC and using the enzymes in yeast oxide Know that ethanol can be oxidised by: burning in air or oxygen (complete combustion) reaction with oxygen in the air to form ethanoic acid (microbial oxidation) heating with potassium dichromate(VI) in dilute sulfuric acid to form ethanoic acid Know that carboxylic acids contain the functional group COOH Understand how to draw structural and displayed formulae for unbranched chain carboxylic acids with up to four carbon atoms in the molecule, and name each compound Describe the reactions of aqueous solutions of carboxylic acids with metals and metal carbonates Know that vinegar is an aqueous solution containing ethanoic acid Know that esters contain the functional group COOR Know that ethyl ethanoate is the ester produced when ethanol and ethanoic acid react in the presence of an acid catalyst

Complete lessons and workbook Content Know that chemical reactions in which heat energy is given out are described as exothermic and those in which heat energy is taken in are endothermic Describe simple calorimetry experiments for reactions such as combustion, displacement, dissolving and neutralisation Calculate the heat energy from a measured temperature change using the expression Q = mcΔT Calculate molar enthalpy change (ΔH ) from heat energy change Q Draw and explain energy level diagrams to represent exothermic and endothermic reactions Know that bond-breaking is an endothermic process and that bond-making is exothermic Use bond energies to calculate the enthalpy change during a chemical reaction

Complete lessons and workbook Content Describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic & alkaline solutions Understand how to use the pH scale, from 0–14, to classify solutions as strongly acidic (0-3), weakly acidic (4-6), neutral (7), weakly alkaline (8-10) and strongly alkaline (11-14) Describe the use of Universal Indicator to measure the approximate pH value of an aqueous solution Know that acids in aqueous solution are a source of hydrogen ions and alkalis in an aqueous solution are sources of hydroxide ions Know that metal oxides, metal hydroxides and ammonia can be classified as bases and that alkalis are bases that are soluble in water Know that bases can neutralise acids Understand acids and bases in terms of proton transfer and that an acid is a proton donor and a base is a proton acceptor Understand how to use acid-base character of oxides to classify elements as metals or non-metals Describe the combustion of elements in oxygen, including magnesium, hydrogen and sulfur Describe the reactions of hydrochloric, sulfuric and nitric acids with: metals (but not with nitric acid) bases metal carbonates Describe an experiment to prepare a pure, dry sample of a soluble salt starting from an insoluble reactant Describe an experiment to prepare a pure, dry sample of a soluble salt starting from an acid and an alkali Describe an experiment to prepare a pure, dry sample of an insoluble salt starting from two soluble reactants

Complete lessons and workbook Content Understand how the formulae of simple compounds can be btained experimentally, including metal oxides, water and alts containing water of crystallisation Know what is meant by the terms empirical and molecular ormula Calculate empirical and molecular formulae from xperimental data Calculate reacting masses using experimental data and hemical equations Calculate percentage yield Describe the formation of carbon dioxide from the thermal ecomposition of metal carbonates, including copper (II) arbonate Understand how to carry out calculations involving gas olumes and the molar volume of a gas (24 dm3 and 24,000 m3 at room temperature and pressure (rtp))

Content Understanding the general rules for predicting the solubility of salts in water: all common sodium, potassium and ammonium salts are soluble all nitrates are soluble 3.common chlorides are soluble, except silver chloride common sulfates are soluble, except those of barium and calcium 5.common carbonates are insoluble, except those of sodium, potassium and ammonium Describing simple tests for the cations (positive ions): Cu2+, Fe2+ , Fe3+ and NH4+ using sodium hydroxide solution Describe simple tests for the anions (negative ions): Cl-, Br- and I-, using dilute nitric acid and silver nitrate solution SO42-, using dilute hydrochloric acid and barium chloride solution CO32-, using dilute hydrochloric acid and identifying the carbon dioxide evolved Writing word and symbol (full and ionic) equations for these tests

Content Describing experiments to investigate the effects of changes in surface area of a solid, concentration of solutions, temperature and the use of a catalyst on the rate of a reaction Describing the effects of changes in surface area of a solid, concentration of solutions, pressure of gases, temperature and the use of a catalyst on the rate of a reaction Explaining the effects of changes in surface area of a solid, concentration of solutions, pressure of gases and temperature on the rate of a reaction in terms of particle collision theory Knowing that a catalyst is a substance that increases the rate of a reaction, but is chemically unchanged at the end of the reaction Knowing that a catalyst works by providing an alternative pathway with lower activation energy Skills Drawing and explaining reaction profile diagrams showing ΔH and activation energy

Topics Understanding how to represent organic molecules using empirical, molecular, structural, displayed and general formulae Knowing what is meant by the terms homologous series, functional group and isomerism Understanding how to name compounds relevant to this specification for compounds containing up to six carbon atoms Knowing that alkanes have the general formula CnH2n+2 Explaining why alkanes are classified as saturated hydrocarbons Knowing that alkenes contain the functional group >C=C< Knowing the general formula for alkenes CnH2n Explaining why alkenes are classified as unsaturated hydrocarbons Understanding how to write possible structural and displayed formulae of an organic molecule given its molecular formula Understanding how to draw the structural and displayed formulae for alkanes with up to five carbon atoms in a molecule, and to name the unbranched isomers Describing the reactions of alkanes with halogens in the presence of UV light and classify them as substitution reactions (limited to mono-substitution) Understanding how to draw structural and displayed formulae for alkenes with up to four carbon atoms and name unbranched- chain isomers cis/trans or E/Z is not required Describing the reactions of alkenes with bromine to produce dibromoalkanes Describing how bromine water can be used to distinguish between an alkane and an alkene

Topics Understanding how to classify a substance as an element, a compound or a mixture Knowing what is meant by the terms atom and molecule and understand that not all substances exist as molecules Knowing the names and symbols of common elements Knowing that the Periodic Table is an arrangement of elements in groups and periods Understanding what is meant by a chemical formula, including use of brackets (not water of crystallisation at this stage) Naming simple binary compounds (including use of mono, di, tri etc (but not oxidation state at this stage) Understanding the use of word equations to describe chemical reactions Understanding what is meant by state symbols s, l, g and aq Describing a test for the presence of water using of anhydrous copper(II) sulfate Describing a physical test to show whether a sample of water is pure Knowing that elements can be classified as metals and non-metals according to their position in the Periodic Table and their electrical conductivity Appreciating that the name of some chemical compounds do not follow a system and know the name and formula of water, ammonia, methane, hydrochloric, sulphuric and nitric acids Recognising and name common atom groupings, restricted to hydroxide, ammonium, carbonate, sulphate and nitrate (no information about ions or charges at this stage) Understanding what is meant by a balanced chemical equation and be able to write balanced equations given sufficient information about the formulae of reactants and products Describing tests for these gases: • hydrogen • oxygen • carbon dioxide • ammonia • chlorine

Topics Understanding the following in terms of gain or loss of oxygen and loss or gain of electrons: • Oxidation • Reduction • Redox • Oxidising agent • Reducing agent Knowing the approximate percentages by volume of the four most abundant gases in dry air Knowing the conditions under which iron rusts Understanding how the rusting of iron may be prevented by barrier methods, galvanizing and sacrificial protection Understanding how to determine the percentage by volume of oxygen in air using experiments involving the reactions of metals (e.g. iron) and non-metals (e.g. phosphorus) Understanding how metals can be arranged in a reactivity series based on their reactions with: • Water • Dilute hydrochloric or sulfuric acid Understanding how metals can be arranged in a reactivity series based on their displacement reactions between: • Metals and metal oxides • Metals and aqueous solutions of metal salts Knowing the order of reactivity of these metals: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver, gold