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For most experiments there is a link to the instructions for the experiment. For some experiments there is a page number of where the experiment is described in your Edexcel IGCSE Chemistry student book. For others there is a link to a __video__ clip or a brief description.
 * **__ Section __** 1a ||  **__ Experiments __**  The experiments below are experiments suggested by Edexcel. There is the expectation that you understand these experiments. We will carry out most of these experiments but will not be able to do __all__ of them.

You will notice that you need to be able to describe some of the experiments which means that you could be asked how you will carry out the experiment i.e. the main steps (no need to include amounts). For those experiments, the learning objective (in red) has been included in the box. || 1.7 Describe experimental techniques for the separation of mixtures, including simple distillation, fractional distillation, filtration, crystallization, and paper chromatography. This means writing down the details how to carry out the experiment and explaining how the components are separated and on which property this technique relies. 1.23 Understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water and salts containing water of cystalization (=hydrated salts) 1.53 Describe experiments to investigate electrolysis using inert electrodes (e.g carbon), of aqueous solutions such as sodium chloride, copper (II) sulphate and dilute sulfuric acid and predict the products.
 * 1b || 1.4 Describe and explain experiments to investigate the small size of particles and their movement including (i) dilution of coloured solutions and (ii) diffusion experiments
 * Dilution of a coloured solution: Using a 100 ml measuring cylinder you take 10 ml form a coloured solution and add 90 ml water to the 100 ml mark. This is a 10x dilution. Now take 10 mol from the diluted solution and add again 90 ml of water. This is again a 10 x dilution but a 100x dilution of the original solution. Continue this process until you cannot see any colour anymore.
 * Diffusion of NH3(g) and HCl(g): [[file:chemistryatdulwich/Diffusion in gases.pdf|Diffusion in gases.pdf]] - book p4.
 * [[file:Diffusion in liquids.pdf|Diffusion in liquids.pdf]]
 * [[file:Separating sand from salt.pdf|Separating sand from salt.pdf]] (includes filtration and crystallization)
 * Evaporate a solution to dryness to determine the mass of solute in a given mass of solution: measure the mass of an evaporating basin, add the solution, measure the mass of the basin and solution, evaporate the solution to dryness, measure mass again until constant (i.e. no more decrease), do the necessary subtractions i.e to find the mass of the solution and the mass of the solute.
 * [[file:Paper chromatography.pdf|Paper chromatography.pdf]] and page 91. There is also this experiment involving chlorophyll: [[file:Paper chromatography2.pdf|Paper chromatography2.pdf]]
 * Distillation and fractional distillation: page 89 and 90. ||
 * 1d || * [[file:Volume of 1 mole of hydrogen gas-1.pdf|Volume of 1 mole of hydrogen gas-1.pdf]] ||
 * 1e || * Investigate mass changes before and after the reaction of e.g. copper sulfate and sodium carbonate: [[file:Investigating mass changes in chemical reactions.doc|Investigating mass changes in chemical reactions.doc]]. This investigation uses lead nitrate and potassium iodide but the principles are the same as using copper sulphate and sodium carbonate.
 * Finding the empirical formula of magnesium oxide: [[file:chemistryatdulwich/MgO formula.doc|MgO formula.doc]]
 * Determine the formula of copper oxide by reduction of the oxide to copper: Use this worksheet to check your understanding of this investigation: [[file:Finding empirical formula of an oxide of copper.doc|Finding empirical formula of an oxide of copper.doc]]
 * Determine the formula of a hydrated salt such as barium chloride or copper sulfate by heating to drive off water of crystallisation: [[file:finding the formula of a hydrated salt.doc|finding the formula of a hydrated salt.doc]]
 * Prepare a substance and calculate the % yield, given the theoretical yield: remember % yield = actual yield (mass of the substance prepared/theoretical yield x 100): [[file:Calculating percentage yield.doc|Calculating percentage yield.doc]]
 * Determine the molar volume by measuring the volume and mass of a gas using a heavier gas (e.g. carbon dioxide): the mass of a heavy gas can be measured by measuring the mass of an empty gas syringe, add the gas and measure the mass again and subtract the mass of the empty cylinder; use the gas syringe to also measure the volume of the gas. Convert the mass of the gas into number of moles. Divide the volume by the number of moles to obtain the molar volume.
 * Acid and alkali titrations - titrations can also be used to find the unknown concentration of an acid or alkali: [[file:chemistryatdulwich/acid-base titration.pdf|acid-base titration.pdf]] ||
 * 1f, g and h || * Classify different types of elements and compounds by investigating their melting points and boiling points, solubility in water and electrical conductivity (as solids and in solution) including sodium chloride, magnesium sulfate, hexane, liquid paraffin, silicon(IV) oxide, copper sulfate, and sucrose (sugar)
 * Investigate the properties of typical ionic compounds: [[file:Investigating properties of ionic solids.doc|Investigating properties of ionic solids.doc]]
 * Investigate the typical properties of simple and giant covalent compounds. ||
 * 1i || 1.51 Describe experiments to distinguish between electrolytes and non-electrolytes.
 * Check the test on electrical conductivity in [[file:Investigating properties of ionic solids.doc]]
 * valent compounds.
 * Electrolysis of lead bromide: [[file:chemistryatdulwich/electrolysis of lead bromide.pdf|electrolysis of lead bromide.pdf]]
 * Electrolysis of copper sulphate solution, dilute sulphuric acid (=acidified water), sodium chloride solution (brine/seawater): [[file:chemistryatdulwich/Identifying the products of electrolysis.doc|Identifying the products of electrolysis.doc]] - page 118 and 198.
 * Investigate the mass changes at the electrodes during the electrolysis of copper sulfate solution using copper electrodes: [[file:Electrolysis of copper sulphate using carbon and copper electrodes.doc|Electrolysis of copper sulphate using carbon and copper electrodes.doc]]
 * Investigate the migration of ions in for instance potassium manganate (VII) solution: [[file:MIgration of ions.doc|MIgration of ions.doc]]
 * Electroplate a metal object: [[file:Electroplating.pdf|Electroplating.pdf]] ||
 * 2a || * Investigate properties of metals: simple experiments to investigate electrical and thermal conductivity
 * the reactions of calcium compounds: the decomposition of calcium carbonate and the reaction of calcium oxide with water; the reaction of calcium carbonate with acid: decomposition of calcium carbonate is carried out in "Thermal stability of carbonates" in 2f and reaction of calcium carbonate with acid in "Reactions of acids" in 4a.
 * Investigate the properties of a group of elements, e.g. Group 2: [[file:Reactions of magensium and calcium in water.pdf|Reactions of magensium and calcium in water.pdf]]
 * Carry out an activity to show that transition metal salts have a variety of colours: well, take some transition metal compounds and look at them. ||
 * 2b || 2.6 Describe the reactions of the alkali metals with water and understand that the reactions provide a basis for their recognition as a family of elements.
 * Reactions of alkali metals and water:[[file:alkali metals and water.pdf|alkali metals and water.pdf]] ||
 * 2c || 2.14 Describe experiments to demonstrate that a more reactive halogen will displace a less reactive halogen from a solution of one of its salts.
 * Displacement reactions of halogens: [[file:chemistryatdulwich/Halogens experiment.doc|Halogens experiment.doc]]
 * Dissolving hydrogen chloride in water and methyl benzene: Blue litmus goes red in hydrogen chloride dissolved in water as the hydrogen chloride has dissociated and hydrogen ions have been formed making hydrochloric acid. The blue litmus remains blue when hydrogen chloride dissolves in methyl benzene as it does not dissociate and therefore not form any hydrogen ions.
 * Halogens reacting with iron wool: the more reactive the halogen the more vigorous the reaction. Watch this __video__ clips:[|halogens and iron wool] ||
 * 2d || 2.17 Explain how experiments involving the reactions of elements such as copper, iron and phosphorus with air can be used to determine the percentage by volume of oxygen in air.
 * Investigate the proportion of oxygen in the atmosphere: using copper: [[file:Proportion of oxygen in air using copper oxide.pdf|Proportion of oxygen in air using copper oxide.pdf]]
 * Using iron to measure oxygen in the air: page 55
 * Investigate the volume of air used up and products formed when candles are burned : [|watch this clip]

2.18 Describe the laboratory preparation of oxygen from hydrogen peroxide using manganese (II) oxide as catalyst
 * Laboratory preparation of oxygen: catalytic decomposition of hydrogen peroxide. - page 47 and 55.

2.20 Describe the laboratory preparation of carbon dioxide from calcium carbonate and dilute hydrochloric acid.
 * Making carbon dioxide: page 59.
 * Method collecting gases: page 92.

2.19 Describe the reactions with oxygen in air of magnesium, carbon and sulphur, and the acid- base character of the oxides produced.
 * Burning elements in oxygen: see handout section 2d: oxygen and oxides.

2.21 Describe the formation of carbon dioxide from the thermal decomposition of metal carbonates such as copper(II) carbonate.
 * The thermal decomposition of copper (II) carbonate: see "Thermal stability of carbonates" in 2f. ||
 * 2e || 2.25 Describe the reactions of dilute hydrochloric acid and dilute sulfuric acid with magnesium, aluminum, zinc and iron.
 * Making hydrogen using metals and acids: see "Reactions of acids" in section 4a; a reaction with an acid and a metal reactive enough produces a salt and hydrogen - page 73.

2.27 Describe the use of anhydrous copper (II) sulphate in the chemical test for water. 2.39 Describe tests for gases: temperature of about 30°C
 * Testing for water using anhydrous copper sulphate: [[file:Testing for water.pdf|Testing for water.pdf]] ||
 * 2f || 2.30 Describe how reactions with water and dilute acids can be used to deduce the following order of reactivity: potassium, sodium, lithium, calcium, magnesium, zinc, iron and copper.
 * Investigate properties of metals (also 2a).
 * Reactions of metals with acids: see "Reactions of acids" in 4a.
 * Reactions of metals with water: page 65.
 * Investigate the reactions of calcium compounds: the decomposition of calcium carbonate and the reaction of calcium oxide with water; the reaction of calcium carbonate with acid (also in 2a).
 * Displacement reactions of metals:[[file:Displacement of metals.pdf|Displacement of metals.pdf]] - some photos on page 63.
 * Competition for oxygen between metals (e.g thermite reaction)(redox reactions): [[file:Competition for oxygen.pdf|Competition for oxygen.pdf]]
 * ** Investigate the ease of thermal decomposition of carbonates, including calcium carbonate, zinc carbonate and copper carbonate: [[file:Thermal stability of metal carbonates.pdf|Thermal stability of metal carbonates.pdf]] **
 * Causes and prevention of rusting of iron: [[file:Rusting.pdf|Rusting.pdf]] ||
 * 2g || 2.37/2.38 Describe the tests for cations and anions
 * [[file:Test for ions.pdf|Test for ions.pdf]] - photos of precipitates.
 * Flame tests: page 94.
 * Tests for gases: page 92 ||
 * 3b || 3.5 Describe the substitution reaction of methane with bromine to form bromomethane in the presence of sunlight.
 * Reaction of methane in the presence of UV: see page 157
 * Investigate products of complete combustion of a hydrocarbon: [[file:Combustion products of alkanes.pdf|Combustion products of alkanes.pdf]] ||
 * 3c || 3.8 Describe the addition reaction of alkenes with bromine, including the decolourising of bromine water as a test for alkenes.
 * Testing for unsaturation using bromine water: [[file:testing for alkenes.doc|testing for alkenes.doc]]
 * Cracking alkanes: [[file:Cracking alkanes.pdf|Cracking alkanes.pdf]] ||
 * 3d || 3.10 Describe the manufacture of ethanol by the fermentation of sugars, for example glucose, at a
 * Fermentation: [[file:Fermentation.pdf|Fermentation.pdf]]

3.12 Describe the dehydration of ethanol to ethene, using aluminium oxide.
 * [[file:chemistryatdulwich/dehydration of ethanol to form ethene.doc|dehydration of ethanol to form ethene.doc]] - page 161 ||
 * 4a || * The effect of acids and alkalis on a selection of indicators: if the indicator is a paper form then make it damp; know your colours!!
 * Reactions of acids with metals, metal carbonates and metal oxides: [[file:chemistryatdulwich/Reactions of acids.pdf|Reactions of acids.pdf]] - page 42

4.7 Describe experiments to prepare soluble salts from acids
 * Making crystals of a soluble salt using an insoluble metal oxide or metal carbonate: [[file:chemistryatdulwich/Excess base method of making salt.pdf|Excess base method of making salt.pdf]]

4.9 Describe experiments to carry out acid-alkali titrations
 * Making crystals of a soluble salt by titration: [[file:chemistryatdulwich/Titration making sodium chloride.pdf|Titration making sodium chloride.pdf]]

4.8 Describe experiments to prepare insoluble salts using precipitation reactions
 * Precipitation reactions: [[file:chemistryatdulwich/precipitating salts.pdf|precipitating salts.pdf]]
 * Making dry samples of insoluble salts: see "precipitating salts" above and in your handout section 4a.
 * Test predictions of whether a precipitate forms when soluble salts are combined: know your solubility rules! ||
 * 4b || 4.11 Describe simple calorimetry experiments for reactions, such as combustion, displacement, dissolving and neutralisation in which heat energy changes can be calculated from measured temperature changes.
 * Endothermic reactions – sodium carbonate decahydrate with citric acid crystals: [[file:chemistryatdulwich/Exothermic or endothermic.doc|Exothermic or endothermic.doc]]
 * Measurement of enthalpy change (displacement reactions; combustion)(c ompare the temperature rise produced when the same volume of water is heated by different fuels) : [[file:chemistryatdulwich/Heat of neutralization.pdf|Heat of neutralization.pdf]] and [[file:chemistryatdulwich/combustion of fuels.pdf|combustion of fuels.pdf]] ||
 * 4c || 4.17 Describe 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.
 * Effect of surface area on rate using marble chips and hydrochloric acid: [[file:chemistryatdulwich/Reaction and particle size.pdf|Reaction and particle size.pdf]]
 * Effect of concentration on rate (metals/marble chips with acid; sodium thiosulphate with acid; clock reactions): [[file:chemistryatdulwich/The effect of concentration on a reaction rate.doc|The effect of concentration on a reaction rate.doc]] and [[file:chemistryatdulwich/The effect of concentration on a reaction rate.doc|The effect of concentration on a reaction rate.doc]]
 * Effect of temperature on rate (metals/marble chips with acid; sodium thiosulphate with acid; clock reactions): [[file:chemistryatdulwich/The effect of temperature on a reaction rate.doc|The effect of temperature on a reaction rate.doc]]
 * Catalytic decomposition of hydrogen peroxide: [[file:chemistryatdulwich/catalyst.pdf|catalyst.pdf]] ||
 * 4d || 4.23 Describe reversible reactions such as the dehydration of hydrated copper (II) sulfate and the effect of heat on ammonium chloride.
 * Effect of heat on ammonium chloride; a reversible reaction: [[file:Heating ammonium chloride.doc|Heating ammonium chloride.doc]] - page 125.
 * Effect of heat on copper sulphate: [[file:Heating copper sulphate.doc|Heating copper sulphate.doc]] ||
 * 5a ||   ||
 * 5b || * Investigate the fractional distillation of ‘artificial crude oil’ and the ease of ignition and viscosity of its fractions.

5.14 Describe how long-chain alkanes are converted to alkenes and shorter-chain alkanes by catalytic cracking, using silica or alumina as the catalyst and a temperature in the range of 600–700°C.
 * Cracking of alkanes: [[file:chemistryatdulwich/cracking alkenes.pdf|cracking alkenes.pdf]] ||
 * 5c || * Making nylon: [[file:chemistryatdulwich/Nylon.pdf|Nylon.pdf]] ||