Complete Chemistry for Cambridge IGCSE (2)

C a m b r i d g e i g cs e e x a m q u e s t i o n s 8 Iron is a transition element. 10 Zinc is extracted from zinc blende, ZnS. a W hich three of the following six statements a Zinc blende is heated in air to give zinc oxide about transition elements are correct? and sulfur dioxide. i The metals are highly coloured e.g. yellow, Most of the sulfur dioxide is used to make sulfur green, blue. trioxide. This is used to manufacture sulfuric ii The metals have low melting points. acid. Some of the acid is used in the plant, but iii Their compounds are highly coloured. most of it is used to make fertilisers. iv Their compounds are colourless. i Give another use of sulfur dioxide. [1] v The elements and their compounds are ii Describe how sulfur dioxide is converted often used as catalysts. into sulfur trioxide. [3] vi They have more than one oxidation state. [3] iii Name a fertiliser made from sulfuric acid.[1] b i In which Period in the Periodic Table b Some of the zinc oxide was mixed with an is iron? [1] excess of carbon and heated to 1000 °C. ii Use the Periodic Table to work out the Zinc distils out of the furnace. number of protons and the number of 2ZnO 1 C    2Zn 1 CO2   C 1 CO2    2CO neutrons in one atom of iron. [1] i Name the two changes of state involved in c Iron is extracted in a blast furnace. The list below gives some of the substances used or the process of distillation. [2] formed in the extraction. ii Why is it necessary to use an excess of carbon monoxide coke iron ore limestone slag carbon? [2] i Which substance is a mineral containing c The remaining zinc oxide reacts with largely calcium carbonate? [1] sulfuric acid to give aqueous zinc sulfate. ii Which substance is formed when impurities This is electrolysed with inert electrodes in the ore react with calcium oxide? [1] (the electrolysis is the same as that of iii Which substance is also called hematite? [1] copper(II) sulfate with inert electrodes). d State two functions of the coke used in the Ions present: Zn21(aq)  SO422 (aq)  H1(aq) OH2(aq). blast furnace. [2] e M ost of the iron is converted into mild steel i Z inc forms at the negative electrode or stainless steel. Give one use for each. [2] (cathode). Write the equation for this  Cambridge IGCSE Chemistry 0620 Paper 3 Q1 June 2006 reaction. [1] 9 The first three elements in Group IV are ii Write the equation for the reaction at carbon, silicon, germanium. the positive electrode (anode). [2] a The element germanium has a diamond-type iii Complete this sentence: structure. Describe the structure of germanium. The electrolyte changes from aqueous zinc A diagram is acceptable. [2] sulfate to ................. [1] b Unlike diamond, graphite is soft and is d Give two uses of zinc. [2] a good conductor of electricity.  Cambridge IGCSE Chemistry 0620 Paper 3 Q4 November 2007 i Explain why graphite has these properties. [3] 11 Aluminium is extracted by the electrolysis of ii Give a use of graphite that depends on a molten mixture that contains alumina, which one of these properties. [1] is aluminium oxide, Al2O3. a The ore of aluminium is bauxite. This contains c Carbon dioxide and silicon(IV) oxide have similar formulae but different types of structure. alumina, which is amphoteric, and iron(III) i Give the formulae of these oxides. [1] oxide, which is basic. The ore is heated with ii How are their structures different? [2] aqueous sodium hydroxide. d All these elements form compounds with Complete the following sentences. hydrogen called hydrides. The saturated The i….…... dissolves to give a solution of hydrides of carbon are the alkanes. Predict the formula of the hydride of germanium which ii.……... The iii……….does not dissolve and can be contains two germanium atoms. removed by iv……….. [4]  Cambridge IGCSE Chemistry 0620 Paper 3 Q4 June 2006 300

Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m b Complete the labelling of the diagram. c When nitric acid is added to water the following reaction occurs. waste gases carbon anode (+) HNO3  1  H2O    NO32  1  H3O1 i .................. mixture of aluminium Give the name and the formula of the particle .................. (–) oxide and ii .................. transferred from nitric acid to water. [2] iii .................. d This question is about the following oxides. temperature is iv .................. aluminium oxide Al2O3 c The ions involved in the electrolysis are calcium oxide CaO Al31 and O22. carbon dioxide CO2 i Write an equation for the reaction at the carbon monoxide CO cathode. [2] magnesium oxide MgO ii Explain how carbon dioxide is formed at sulfur dioxide SO2 the anode.  [2] i Which will react with hydrochloric acid but d Give an explanation for each of the following. not with aqueous sodium hydroxide? [1] i Aluminium is used extensively in the ii Which will react with aqueous sodium manufacture of aircraft. [1] hydroxide but not with hydrochloric acid?[1] ii Aluminium is used for food containers. [2] iii Which will react both with hydrochloric acid iii Aluminium electricity cables have a steel and aqueous sodium hydroxide? [1] core. [1] iv Which will react neither with hydrochloric  Cambridge IGCSE Chemistry 0620 Paper 3 Q6 June 2007 acid nor with aqueous sodium hydroxide?[1] 12 a Four bottles were known to contain aqueous  Cambridge IGCSE Chemistry 0620 Paper 3 Q3 June 2006 ammonia, dilute hydrochloric acid, sodium 13 H ydrogen reacts with the halogens to form hydrogen halides. hydroxide solution and vinegar, which is dilute a Bond energy is the amount of energy, in kJ, ethanoic acid. The bottles had lost their labels. that must be supplied (endothermic) to break one mole of a bond. The pH values of the four solutions were 1, 4, 10 and 13. Complete the table. [2] solution pH bond bond energy in kJ / mol aqueous ammonia dilute hydrochloric acid H2H 1436 F2F 1158 sodium hydroxide solution H2F 1562 vinegar Use the above data to show that the following b The following apparatus was set up to investigate reaction is exothermic. the electrical conductivity of dilute acids. H H 1 F F   2H F [3] bulb/lamp b They react with water to form acidic solutions. +–  HCl 1 H2O   H3O1 1 Cl2  HF 1 H2O   H3O1 1 F2 carbon carbon i Explain why water behaves as a base in anode cathode both of these reactions. [2] dilute sulfuric acid ii At equilibrium, only 1% of the hydrogen bubbles of chloride exists as molecules, the rest has hydrogen gas bubbles of formed ions. In the other equilibrium, 97% oxygen gas of the hydrogen fluoride exists as molecules, Dilute sulfuric acid is a strong acid. If it was only 3% has formed ions. What does this tell replaced by a weak acid, what two differences in you about the strength of each acid? [2] the observations would you expect to make? [2] iii How would the pH of these two solutions differ?[1]  Cambridge IGCSE Chemistry 0620 Paper 32 Q7 June 2009 301

C a m b r i d g e i g cs e e x a m q u e s t i o n s iii Complete the equations for the decomposition of their nitrates. 14 The reactivity series lists metals in order of reactivity. To find out which is more reactive, 2KNO3    .................  1  ............... zinc or tin, this experiment could be carried out. 2Ca(NO3)2    ..........  1  .............. 1 ............. piece of zinc  [4] shiny surface  Cambridge IGCSE Chemistry 0620 Paper 31 Q6 November 2008 tin(II) nitrate(aq) zinc surface still 15 The fractional distillation of crude oil usually shiny means produces large quantities of the heavier fractions. NO REACTION (NR) The market demand is for the lighter fractions and for the more reactive alkenes. The heavier fractions zinc surface covered are cracked to form smaller alkanes and alkenes as with a grey deposit means in the following example. REACTION (R) a The experiment could be carried out with other metals and the results recorded in a table. C8H18    C4H10 1 C4H8 octane butane butenes Then the order of reactivity can be deduced. i The order was found to be: a i Write a different equation for the cracking of octane. manganese most reactive zinc C8H18     ............. 1 .................. [1] tin ii The cracking of octane can produce isomers silver least reactive with the molecular formula C4H8. Draw the structural formulae of two of these isomers. Copy and complete this table of results from which the order was determined. [3] [2] aqueous tin Sn manganese silver zinc b i Give the essential condition for the reaction solution Mn Ag Zn between chlorine and butane. [1] tin(II) nitrate R NR R ii What type of reaction is this? [1] manganese(II) nitrate iii This reaction produces a mixture of products. silver(I) nitrate Give the names of two products that contain zinc nitrate four carbon atoms per molecule. [2] ii W rite the ionic equation for the reaction c Alkenes are more reactive than alkanes and between tin atoms and silver(I) ions. [2] are used to make a range of organic chemicals. iii The following is a redox reaction. Propene, CH3–CH5CH2, is made by cracking. Give the structural formula of the addition Mn 1 Sn21     Mn21 1 Sn product when propene reacts with these. Indicate on the equation the change which is i  water   ii  bromine [2] oxidation. Give a reason for your choice. [2] d Propene reacts with hydrogen iodide to form iv Explain why experiments of this type cannot 2-iodopropane. be used to find the position of aluminium CH32CH5CH2 1 HI CH32CHI2CH3 in the reactivity series. [2] 1.4 g of propene produced 4.0 g of 2-iodopropane. Calculate the percentage yield. b Potassium and calcium are very reactive metals at the top of the series. Because their i moles of CH32CH5CH2 reacted  5 ii maximum moles of CH3-CHI-CH3 that could ions have different charges, K1 and Ca21, their be formed  5 compounds behave differently when heated. mass of one mole of CH3-CHI-CH3 is 170 g iii maximum mass of 2-iodopropane that i Explain why the ions have different could be formed  5 iv percentage yield  5[4] charges. [2]  Cambridge IGCSE Chemistry 0620 Paper 3 Q7 June 2006 ii Their hydroxides are heated. If the compound decomposes, complete the word equation. If it does not decompose, write ‘no reaction’. Potassium hydroxide ............... Calcium hydroxide ............... [2] 302

Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m 16 The alcohols form a homologous series. d For each of the following predict the name of The first four members are methanol, ethanol, propan-1-ol and butan-1-ol. the organic product. a One characteristic of a homologous series is that i reaction between methanol and ethanoic the physical properties vary in a predictable way. The table below gives the heats of combustion of acid [1] the first three alcohols. ii oxidation of propan-1-ol by potassium dichromate(VI) [1] alcohol formula heat of iii removal of H2O from ethanol [1] combustion (dehydration) in kJ / mole  Cambridge IGCSE Chemistry 0620 Paper 3 Q6 November 2007 2730 methanol CH3OH 17 Copy and complete the following table. ethanol CH3-CH2-OH 21370 propan-1-ol CH3-CH2-CH2-OH gas test for gas butan-1-ol CH3-CH2-CH2-CH2-OH –­ 2020 ammonia bleaches damp litmus paper i The minus sign indicates there is less chemical hydrogen relights a glowing splint energy in the products than in the reactants. turns limewater milky In what form is the energy given out? [1] ii Is the reaction exothermic or endothermic? [1]  [5] iii Complete the equation for the complete  Cambridge IGCSE Chemistry 0620 Paper 3 Q1 November 2008 combustion of ethanol. C2H5OH  1  ....O2    ............... 1 .............. –700 number of carbon atoms per molecule 4  [2] –800 123 –900 iv D etermine the heat of combustion of butan- –1000 1-ol by plotting the heats of combustion of –1100 the first three alcohols against the number –1200 of carbon atoms per molecule. –1300 Label your graph as on the right. –1400 –1500 What is the heat of combustion of [3] –1600 butan-1-ol in kJ / mol? [2] heat of –1700 [2] combustion / v Describe two other characteristics of kJ / mol –1800 homologous series. –1900 –2000 b Give the name and structural formula of –2100 an isomer of propan-1-ol. –2200 –2300 c Methanol is made from carbon monoxide. –2400 –2500 CO (g) 1 2H2 (g)    CH3OH (g) –2600 –2700 The forward reaction is exothermic. –2800 i Describe how hydrogen is obtained from alkanes. [2] ii Suggest a method of making carbon monoxide from methane. [2] iii W hich condition, high or low pressure, would give the maximum yield of methanol? Give a reason for your choice. [2] 303

from paper 6C A M B R I D G E I G C S E E X A M Q U E S T I O N S 1 The colours present in some blackcurrant sweets 3 A student investigated the addition of four can be separated by chromatography. The colours different solids, A, B, C and D, to water. are water-soluble dyes. The diagrams show how Five experiments were carried out. the colours can be extracted from the sweets. Experiment 1 B By using a measuring cylinder, 30 cm3 of distilled water was poured into a polystyrene cup and the C initial temperature of the water was measured. A 4 g of solid A was added to the cup and the mixture stirred with a thermometer. The temperature of the solution was measured after 2 minutes. 30 30 25 25 a Name the pieces of apparatus labelled A to C.[3] 20 20 initial temperature final temperature The apparatus below was used to carry out the chromatography. glass cover Experiment 2 Experiment 1 was repeated using 4 g of solid B. chromatography beaker paper 30 30 solvent 25 25 20 20 initial temperature final temperature b i Name the solvent used.[1] ii Label, with an arrow, the origin on the Experiment 3 Experiment 1 was repeated using 4 g of solid C. diagram. [1] c On a larger copy of this 30 20 rectangle, sketch the 25 15 chromatogram you would expect if two different colours 20 10 were present in the sweets.[1] initial temperature final temperature  Cambridge IGCSE Chemistry 0620 Paper 6 Q1 November 2008 Experiment 4 Experiment 1 was repeated using 4 g of solid D. 2 Describe a chemical test to distinguish between each of the following pairs of substances. 30 30 Example: hydrogen and carbon dioxide 25 25 test: lighted splint result: with hydrogen gives a pop 20 20 result: with carbon dioxide splint is extinguished initial temperature final temperature a  zinc carbonate and zinc chloride[2] b ammonia and chlorine[3] c aqueous iron(II) sulfate and aqueous iron(III) sulfate[3]  Cambridge IGCSE Chemistry 0620 Paper 6 Q3 June 2009 304

Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m Experiment 5 4 Hydrogen peroxide 0 10 20 30 40 50 A little of the solution from Experiment 4 was added breaks down to form to a little of the solution from Experiment 2 in oxygen. The volume gas syringe a test-tube. The observations were recorded. of oxygen given off can be measured observations using this apparatus. a fast reaction vigorous effervescence and bubbles produced Solids W and X both catalyse the breakdown of hydrogen peroxide. The syringe diagrams show a Copy out the table and use the thermometer the volume of oxygen formed every 20 seconds diagrams for Experiments 1–4 to record the using these catalysts at 25 °C. initial and final temperatures. Calculate and record the temperature difference in the table. time/ s using catalyst W using catalyst X expt initial final difference 0 0 10 20 30 40 0 10 20 30 40 1 temperature / °C temperature / °C  / °C 2 3 20 0 10 20 30 40 0 10 20 30 40 4 40 0 10 20 30 40 0 10 20 30 40 [4] 60 0 10 20 30 40 0 10 20 30 40 b Draw a labelled bar chart of the results to [4] 80 0 10 20 30 40 0 10 20 30 40 Experiments 1, 2, 3 and 4 on graph paper. Label your bar chart as shown below. +10 100 0 10 20 30 40 0 10 20 30 40 +5 temperature 0 a Copy the table. Use the gas syringe diagrams difference / ºC to complete it. –5 time / s volume of oxygen / cm3 –10 catalyst W catalyst X 0 Use the results and observations from Experiments 20 40 1 – 5 to answer the following questions. 60 80 c i Which solid dissolves in water to produce 100 an exothermic reaction?[1] ii Give a reason why you chose this solid.[1] d W hich Experiment produced the largest  [3] temperature change?[1] b Plot a graph to show each set of results. e Predict the temperature change that would Clearly label the curves. [6] happen if c Which solid is the better catalyst in this i 8 g of solid B was used in Experiment 2, [1] reaction? Give a reason for your choice.[2] ii 60 cm3 of water was used in Experiment 4. d Why is the final volume of oxygen the same [1] in each experiment? [1] iii Explain your answer to e ii.[2] e Sketch a line on the grid to show the shape f Suggest an explanation for the observations of the graph you would expect if the reaction in Experiment 5. [2] with catalyst X was repeated at 40 °C.[2]  Cambridge IGCSE Chemistry 0620 Paper 6 Q4 November 2008  Cambridge IGCSE Chemistry 0620 Paper 6 Q6 June 2007 305

C a m b r i d g e i g cs e e x a m q u e s t i o n s 5 An experiment was carried out to determine 7 The diagram shows an experiment to pass the solubility of potassium chlorate at different electricity through lead bromide. Electricity has temperatures. The solubility is the mass of no effect on solid lead bromide. potassium chlorate that dissolves in 100 g of water. d.c.power supply The results obtained are shown in the table below. bulb temperature / °C 0 10 20 30 40 50 60 14 17 20 24 29 34 40 LEAD solubility in BROMIDE g  / 100 g of water TOXIC a Draw a smooth line graph to show the solubility of potassium chlorate at different temperatures. Label your graph as shown below. 50 40 heat a i Copy the diagram and clearly label the 30 electrodes.[1] solubility in g/100 g water ii Suggest a suitable material to make the 20 electrodes.[1] b Give two observations expected when the 10 lead bromide is heated to melting point. [2] c State two different safety precautions when 0 carrying out this experiment. [2] 0 10 20 30 40 50 60 70 temperature / ºC  Cambridge IGCSE Chemistry 0620 Paper 6 Q2 June 2008 [4] 8 Concentrated hydrochloric acid can be electrolysed b Use your graph to determine the solubility of using the apparatus shown. potassium chlorate at 70 °C. Show clearly on the graph how you obtained your answer. [2] c W hat would be the effect of cooling a saturated solution of potassium chlorate from 60 °C to 20 °C?[2]  Cambridge IGCSE Chemistry 0620 Paper 6 Q6 November 2008 6 The diagram shows the formation of a solution of magnesium hydroxide from magnesium. Universal A indicator solution solution of water magnesium magnesium magnesium hydroxide burning to form a Copy the diagram and label the position of magnesium oxide indicator C oxide turns heat blue the electrodes. [1] B b Give two observations when the circuit is a Name the pieces of apparatus labelled A – C. [3] switched on.[2] c i Name the product at the positive electrode. [1] b W hat type of chemical reaction is the burning of magnesium? [1] ii State a test for this product, and the result. [2] c Suggest a pH for the solution of magnesium  Cambridge IGCSE Chemistry 0620 Paper 6 Q2 June 2007 hydroxide.[1]  Cambridge IGCSE Chemistry 0620 Paper 6 Q1 November 2006 306

Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m 9 A student investigated the reaction between d About 1 cm3 of aqueous sodium hydroxide was potassium manganate(VII) and a metallic salt added to a little of the solution in the flask and solution. Two experiments were carried out. the observation noted. Experiment 1 observation  red-brown precipitate a About 1 cm3 of aqueous sodium hydroxide e i In which experiment was the greatest volume was added to a little of the salt solution A and the observation noted. of potassium manganate(VII) solution used?[1] observation  green precipitate formed ii Compare the volumes of potassium b Aburette was filled with potassium manganate(VII) solution up to the 0.0 cm3 mark. manganate(VII) solution used in By using a measuring cylinder, 25 cm3 of Experiments 1 and 2.[2] solution A of the salt was placed into a conical flask. The flask was shaken to mix the contents. iii Suggest an explanation for the difference The potassium manganate(VII) solution was in the volumes. [2] added to the flask, and shaken to mix thoroughly. Addition of potassium manganate(VII) solution f Predict the volume of potassium manganate(VII) was continued until there was a pale pink colour in the contents of the flask. solution which would be needed to react Copy the table of results below. completely with 50 cm3 of solution B.[2] Burette readings / cm3 g Explain one change that could be made to the Experiment 1 Experiment 2 experimental method to obtain more accurate final reading results. [2] initial reading h W hat conclusion can you draw about the salt difference solution from: i  experiment 1a,[1] ii  experiment 2d?[1]  Cambridge IGCSE Chemistry 0620 Paper 6 Q4 June 2008 10 This label is from a container of ‘Bite Relief’ solution. Use this burette diagram 25 BITE RELIEF to record the volume and 26 FOR FAST RELIEF FROM INSECT complete the column for Experiment 1 in BITES AND STINGS the table. Active ingredient: ammonia Also contains water and alcohol 27 DIRECTIONS FOR USE: Use cotton wool to dab the solution on the affected area of the skin. final reading a Give a chemical test to show the presence of Experiment 2 c Experiment 1b was repeated using a different ammonia in Bite Relief solution. solution B of the salt, instead of solution A. Give the result of the test. [2] Use the burette diagrams to record the volumes b What practical method could be used to in the table and complete the table. 15 28 separate the mixture of alcohol (b.p. 78 °C) and water (b.p. 100 °C)?[2] c Give a chemical test to show the presence 16 29 of water. Give the result of the test.[2] d What would be the effect of touching the 17 30 alcohol with a lighted splint?[1] final reading initial reading  Cambridge IGCSE Chemistry 0620 Paper 6 Q7 June 2008  [4] 307

C a m b r i d g e i g cs e e x a m q u e s t i o n s 11 Two solids, S and V, were analysed. S was copper(II) oxide. The tests on the solids, and some of the observations, are in the following table. Write down the observations that are missing from the table. test observation tests on solid S black solid slow effervescence a Appearance of solid S splint relit blue solution formed b Hydrogen peroxide was added to solid S in a test-tube. A glowing splint was inserted into the tube ………………………………………….…………[1] ……………………………………………….……[2] c Dilute sulfuric acid was added to solid S in a test-tube. ………………………………………..…………...[2] The mixture was heated to boiling point. …………………………………………………….[2] The solution was divided into three equal portions into test-tubes. i To the first portion of the solution excess sodium hydroxide was added. ii To the second portion of the solution, about 1 cm3 of aqueous ammonia solution was added. Excess ammonia solution was then added. iii To the third portion of the solution, dilute hydrochloric acid was added followed by barium chloride solution. tests on solid V black solid d Appearance of solid V rapid effervescence e Hydrogen peroxide was added to solid V in a test-tube. splint relit A glowing splint was inserted into the tube. f i Compare the reactivity of solid S and solid V with hydrogen peroxide. [1] ii Identify the gas given off in test e.[1] g What conclusions can you draw about solid V?[2]  Cambridge IGCSE Chemistry 0620 Paper 6 Q5 June 2009 308

Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m 12 A sample of solid C was analysed. C is a mixture of two salts, D and E. Solid D is insoluble lead carbonate and solid E is water-soluble. The tests on C, and some of the observations are in the following tables. Complete the observations that would go in the tables. tests observations a Describe the appearance of C. pale green solid b Using a spatula, place a little of C in a hard glass test-tube. paper turns blue Inside the top of the tube suspend a piece of damp indicator pH 8 to 11 paper. Heat C gently until gas comes out of the tube. c .............................................[3] c Using a spatula, place a little of C in a test-tube. Add about 2 cm3 of dilute nitric acid and test the gas. Solid C was added to a boiling tube containing distilled observations [2] water. The tube was shaken to mix the contents. d ............................................. The contents of the boiling tube were filtered. tests on the residue in the filter paper d Place the funnel in a test-tube. Pour dilute nitric acid onto the residue contained in the funnel. Add 2 cm3 of potassium iodide to the solution collected in the tube. tests on the filtrate observations e Divide the filtrate into three test tubes. white precipitate green precipitate i To the first portion add dilute hydrochloric acid and paper turns blue about 1 cm3 of aqueous barium nitrate. pH 8 to 11 ii To the second portion of solution add excess aqueous ammonia. iii To the third portion of solution, add an equal volume of aqueous sodium hydroxide. Warm the mixture gently. Test the gas with indicator paper. f Name the gas given off in c.[1] g Name the gas given off in e iii.[1] h What conclusions can you draw about salt E?[4]  Cambridge IGCSE Chemistry 0620 Paper 6 Q5 June 2007 309

Reference Glossary A B cathode  the negative electrode of an electrolysis cell acetylene  a gas (formula C2H2) used as a back reaction  the reaction in which the fuel, for example in the oxy-acetylene torch product breaks down again, in a reversible cation  another name for a positive ion reaction acid rain  rain that is acidic because gases cell (biological)  the building blocks for such as sulfur dioxide are dissolved in it bacteria  tiny organisms, some of which can animals and plants (from burning fossil fuels) cause disease; others break down dead plant and animal material cell (electrical)  a device that converts acidic solution  has a pH less than 7; an chemical energy to electrical energy acidic solution contains H 1 ions balanced equation  a chemical equation in which the number of each type of atom is cement  a substance used in building, made acid fermentation  the process in which the same on both sides of the arrow from limestone and clay bacteria convert ethanol to ethanoic acid base  a metal oxide or hydroxide; a base will ceramic  a hard, ureactive material that can addition reaction  where a molecule adds neutralise an acid, to form a salt and water withstand high temperatures, made by onto an alkene, and the C 5 C double bond baking clay in a kiln; ceramics are non- of the alkene changes to a single bond battery  a portable electrical cell; for conductors example a torch battery addition polymerisation  where small chalk  a rock made of calcium carbonate molecules join to form a very large molecule, biodegradable  will decay naturally in the by adding on at double bonds soil, with the help of bacteria change of state  a change in the physical state of a substance – for example from solid alcohols  a family of organic compounds, biopolymer  a polymer made by bacteria to liquid, or liquid to gas similar to the alkanes but with the OH functional group; ethanol is an example blast furnace  the chemical plant in which chemical change  a change in which a new iron is extracted from its ore, iron(III) oxide chemical substance forms alkali  a soluble base; for example sodium hydroxide boiling  the change from a liquid to a gas, chemical equation  uses chemical symbols which takes place at the boiling point to describe a chemical reaction in a short alkali metals  the Group I elements of the way Periodic Table boiling point  the temperature at which a substance boils chemical reaction  a process in which alkaline earth metals  the Group II chemical change takes place elements of the Periodic Table bond energy  the energy needed to break a bond, or released when the bond is formed; chromatogram  the paper showing the alkaline solution  has a pH above 7; it is given in kilojoules (kJ) per mole separated coloured substances, after paper alkaline solutions contain OH 2 ions chromatography has been carried out bonding  how the atoms are held together alkanes  a family of saturated hydrocarbons in an element or compound; there are three climate change  how climates around the with the general formula CnH2n 1 2; types of bonds: ionic, covalent, and metallic Earth are changing, because of the rise in ‘saturated’ means they have only single C–C average air temperatures bonds brittle  breaks up easily when struck coagulant  a substance that will make small alkenes  a family of unsaturated hydro- brine  the industrial name for a particles stick together; coagulants are used carbons with the general formula CnH2n ; concentrated solution of sodium chloride in in cleaning up water, ready for piping to their molecules contain a carbon 5 carbon water; it can be made by dissolving rock salt homes double bond burette  a piece of laboratory equipment for coke  a form of carbon made by heating allotropes  different forms of an element; delivering a measured volume of liquid coal diamond and graphite are allotropes of carbon burning  an exothermic chemical reaction combination  where two or more in which the reactant combines with oxygen substances react to form a single substance alloy  a mixture where at least one other to form an oxide; also called combustion substance is added to a metal, to improve its combustible  can catch fire and burn very properties; the other substance is often a C easily metal too (but not always) carbon cycle  the way carbon moves non- combustion  another name for burning amphoteric  can be both acidic and basic in stop between the atmosphere, living things, its reactions; for example aluminium oxide the land, and the ocean; it moves in the form compound fertiliser  it provides is an amphoteric oxide of carbon dioxide nitrogen, potassium, and phosphorus for plants anion  another name for a negative ion carboxylic acids  a family of organic acids, which have the COOH functional compound ion  an ion containing more anode  the positive electrode of a cell group;  ethanoic acid is an example than one element; for example the nitrate ion NO3– aquifer  underground rocks holding a large cast iron  iron from the blast furnace that is compound  a substance in which two or volume of water; it can be pumped out to run into molds to harden; it contains a high more elements are chemically combined give a water supply % of carbon, which makes it brittle concentration  tells you how much of one atmosphere  the layer of gases around the catalyst  a substance that speeds up a substance is dissolved in another; usually Earth; here at the Earth’s surface, we call it chemical reaction, without itself being used given as grams or moles per dm3 air up in the process condensation  the physical change in which atoms  elements are made up of atoms, catalytic converter  a device in a car a gas turns into a liquid on cooling which contain protons, neutrons, and exhaust, in which catalysts are used to electrons convert harmful gases to harmless ones condensation polymerisation  where molecules join to make very large molecules, Avogadro constant  the number of particles catalytic cracking  where large molecules by eliminating small molecules (such as in one mole of an element or compound; it of hydrocarbons are split up into smaller water molecules) is 6.02 3 1023 ones, with the help of a catalyst 310

Reference condenser  a piece of laboratory equipment electrolyte  the liquid through which the fractional distillation  a method used to used to cool a gas rapidly, and turn it into a current is passed, in electrolysis; the current separate two or more liquids that have liquid is carried by ions in the electrolyte different boiling points conductor  a substance that allows heat or electron distribution  how the electrons in fractions  the different groups of electricity to pass through it easily an atom are arranged in shells (2 1 8 1 …) compounds that a mixture is separated into, by fractional distillation; fractions are Contact process  the industrial process for electron shells  the different energy levels collected one by one making sulfuric acid which electrons occupy, around the nucleus freezing  the change from liquid to solid, corrosion  where a substance is attacked by electronic configuration  another term for  that occurs at the freezing point (5 melting air or water, from the surface inwards; the electron distribution point) corrosion of iron is called rusting electrons  the particles with a charge of 1– fuel  a substance we use to provide energy; covalent bond  the chemical bond formed and almost no mass, in an atom most fuels are burned to release their energy when two atoms share electrons (but nuclear fuels are not) electroplating  coating one metal with covalent compound  a compound made of another, using electrolysis fuel cell  a cell in which a chemical reaction atoms joined by covalent bonds provides electricity (to light homes and so element  a substance that cannot be split on) cracking  reactions in which long-chain into anything simpler, in a chemical reaction hydrocarbon molecules are broken down to functional group  the part of the molecule shorter, more useful molecules empirical  found by experiment of an organic compound, that largely dictates how it reacts; for example the OH cross-linking  the chemical bonds between empirical formula  shows the simplest group in molecules of the alcohol family the long-chain molecules in some polymers, ratio in which the atoms in a compound that hold the chains together are combined G crude oil  the fossil fuel formed over millions endothermic  takes in energy from the galvanising  coating iron with zinc, to of years from the remains of tiny sea plants surroundings prevent the iron from rusting and animals; it is also called petroleum enzymes  proteins made by living cells, that giant structure  where a very large number crystallisation  the process in which act as biological catalysts of atoms or ions are held in a lattice by crystals form, as a saturated solution cools strong bonds; metals, diamond and ionic equation  it uses symbols to describe a solids such as sodium chloride are all giant D chemical reaction (but a word equation uses structures just words) decomposition reaction  where a substance global warming  the rise in average breaks down to give two or more products equilibrium  the state where the forward temperatures taking place around the world; and back reactions are taking place at the many scientists believe that carbon dioxide denature  to destroy the structure of an same rate, in a reversible reaction; so there (from burning fossil fuels) is the main cause enzyme by heat, or a change in pH is no overall change greenhouse gas  a gas in the atmosphere degradeable  will break down naturally ester  a compound formed when an alcohol that traps heat, preventing its escape into (for example through the action of reacts with a carboxylic acid; esters often space; carbon dioxide and methane are bacteria) smell of fruit or flowers examples density  tells you how ‘heavy’ something is; evaporation  the physical change where a group  a column of the Periodic Table; the density of a substance is its mass per liquid turns to a gas at a temperature below elements in a group have similar properties unit volume; for water it is 1 g / cm3 its boiling point H diatomic  a substance is called diatomic if exothermic  gives out energy its molecules contain two atoms joined by a Haber process  the process for making covalent bond extract  to remove a metal from its ore ammonia from nitrogen and hydrogen, in industry diffusion  the process in which particles F mix by colliding randomly with each other, half-equation  an equation that shows the and bouncing off in all directions fermentation  the process in which the reaction taking place at an electrode enzymes in yeast break down sugars, to displacement reaction  a reaction in form ethanol and carbon dioxide halogens  the Group VII elements of the which a more reactive element takes the Periodic Table place of a less reactive one, in a compound fertilisers  substances added to soil to help crops grow well heating curve  a graph showing how the dissolving  the process in which a soluble temperature of a substance changes on substance forms a solution filtering  separating solids from liquids by heating, while it goes from solid to liquid to pouring the mixture through filter paper gas distillation  separating a liquid from a mixture by boiling it off, then condensing it filtrate  the liquid obtained from filtration homologous series  a family of organic (after the solid has been removed) compounds, that share the same general double bond  a covalent bond in which two formula and have similar properties atoms share two pairs of electrons flammable  burns easily hydrated  has water molecules built into its ductile  can be drawn out into a wire; for flue gas desulfurisation  the removal of crystal structure; for example copper(II) example copper is ductile sulfur dioxide from the waste gases at power sulfate: CuSO4.5H2O stations, to stop it getting into the hydrocarbon  a compound containing only dynamic equilibrium  where forward and atmosphere carbon and hydrogen back reactions take place at the same rate, so there is no overall change formula  uses symbols and numbers to tell hydrogenation  adding hydrogen you what elements are in a compound, and E the ratio in which they are combined hydrogen fuel cell  it uses the reaction between hydrogen (from a tank), and electrodes  the conductors used to carry forward reaction  the reaction in which oxygen (from the air), to give an electric current into and out of an electrolyte; they the product is made, in a reversible reaction current could be graphite rods, for example fossil fuels  petroleum (crude oil), natural electrolysis  the process of breaking down gas, and coal; they are called the fossil fuels a compound by passing a current through it because they were formed from the remains of living things, millions of years ago 311

Reference hydrolysis  the breaking down of metallic bond  the bond that holds the O a compound by reaction with water atoms together in a metal ore  rock containing a metal, or metal hypothesis  a statement you can test by metalloid  an element that has properties of compounds, from which the metal is doing an experiment and taking both a metal and a non-metal extracted measurements microbe  a microscopic (very tiny) living organic chemistry  the study of organic I organism, such as a bacterium or virus compounds (there are millions of them!) incomplete combustion  the burning of minerals  compounds that occur naturally in organic compound  a compound containing fuels in a limited supply of oxygen; it gives the Earth; rocks contain different minerals carbon, and usually hydrogen; petroleum is a carbon monoxide instead of carbon dioxide mixture of many organic compounds mixture  contains two or more substances indicator  a chemical that shows by its that are not chemically combined oxidation  a chemical reaction in which a colour whether a substance is acidic or substance gains oxygen, or loses electrons alkaline molar solution  contains one mole of a substance in 1 dm3 (1 litre) of water oxidation state  every atom in a formula inert  does not react (except under extreme can be given a number that describes its conditions) mole  the amount of a substance that oxidation state; for example in NaCl, the contains the same number of elementary oxidation states are +I for sodium, and – I inert electrode  is not changed during units as the number of carbon atoms in 12g for chlorine electrolysis; all it does is conduct the current of carbon-12; you obtain it by weighing out the Ar or Mr of the substance, in grams oxide  a compound formed between oxygen in excess  more than is needed for a molecular  made up of molecules and an other element reaction; some will be left at the end molecule  a unit of two or more atoms held oxidising agent  a substance that brings insoluble  does not dissolve in a solvent together by covalent bonds about the oxidation of another substance insulator  a poor conductor of heat or monatomic  made up of single atoms; for ozone  a gas with the formula O3 electricity example neon is a monatomic element ozone layer  the layer of ozone up in the atmosphere, which protects us from harmful intermolecular forces  forces between monomers  small molecules that join UV radiation from the sun molecules together to form polymers P ion  a charged atom or group of atoms N formed by the gain or loss of electrons paper chromatography  a way to separate native  describes a metal that is found in the the substances in a mixture, using a solvent ionic bond  the bond formed between ions Earth as the element and special paper; the substances separate of opposite charge because they travel over the paper at negative electrode  another name for the different speeds ionic compound  a compound made up of cathode, in an electrolysis cell ions, joined by ionic bonds percentage composition  it tells you which negative ion  an ion with a negative charge elements are in a compound, and what % of ionic equation  shows only the ions that each is present by mass actually take part in a reaction, and ignores neutral (electrical)  has no charge any other ions present; the other ions are period  a horizontal row of the Periodic called spectator ions neutral (oxide)  is neither acidic nor basic; Table; its number tells you how many carbon monoxide is a neutral oxide electron shells there are isomers  compounds that have the same formula, but a different arrangement of neutral (solutions)  neither acidic nor periodicity  the pattern of repeating atoms alkaline; neutral solutions have a pH of 7 properties that shows up when elements are arranged in order of proton number; you isotopes  atoms of the same element, that neutralisation  the chemical reaction can see it in the groups in the Periodic Table have a different numbers of neutrons between an acid and a base or a carbonate, giving a salt and water Periodic Table  the table showing the L elements in order of increasing proton neutron  a particle with no charge and a mass number; similar elements are arranged in lattice  a regular arrangement of particles of 1 unit, found in the nucleus of an atom columns called groups lime  the common name for calcium oxide nitrogenous fertiliser  it provides nitrogen petroleum  a fossil fuel formed over millions for plants, in the form of nitrate ions or of years from the remains of tiny sea plants limewater  a solution of the slightly soluble ammonium ions and animals; it is also called crude oil compound calcium hydroxide, which is used to test for carbon dioxide noble gases  the Group 0 elements of the pH scale  a scale that tells you how acidic or Periodic Table; they are called ‘noble’ alkaline a solution is; it is numbered 0 to 14 locating agent  used to show up colourless because they are so unreactive substances, in chromatography; it reacts photochemical reaction  a reaction that with them to give coloured substances non-metal  an element that does not show depends on light energy; photosynthesis is metallic properties: the non-metals lie to the an example M right of the zig-zag line in the Periodic Table, (except for hydrogen, which sits alone) photodegradeable  can be broken down by macromolecule  a very large molecule; for light example a molecule in a polymer non-renewable resource  a resource such as petroleum that we are using up, and photosynthesis  the process in which plants malleable  can be bent or hammered into which will run out one day convert carbon dioxide and water to glucose shape and oxygen non-toxic  not harmful health mass spectrometer  an instrument used to physical change  a change in which no new find the masses of atoms and molecules nucleon number  the number of protons chemical substance forms; melting and plus neutrons in an atom of an element boiling are physical changes melting point  the temperature at which a solid substance melts nuclear fuel  contains radioisotopes such physical properties  properties such as as uranium-235; these are forced to break density and melting point (that are not melting  the physical change from a solid to down, giving out energy about chemical behaviour) a liquid nucleus  the centre part of the atom, made metal  an element that shows metallic up of protons and neutrons properties (for example conducts electricity, and forms positive ions) 312

Reference pipette  a piece of laboratory equipment refining (metals)  the process of purifying structural formula  the formula of a used to deliver a known volume of liquid, a  metal; copper is refined using electrolysis compound displayed to show the bonds accurately between the atoms as lines; we often show relative atomic mass (Ar)  the average organic compounds this way plastics  a term used for synthetic polymers mass of the atoms of an element, relative to (made in factories, rather than in nature) the mass of an atom of carbon-12 T pollutant  a substance that causes harm if it relative formula mass (Mr)  the mass of thermal decomposition  the breaking gets into the air or water one formula unit of an ionic compound; you down of a compound by heating it find it by adding together the relative atomic pollution  when harmful substances are masses of the atoms in the formula thermite process  the redox reaction released into the environment between iron oxide and aluminium, which relative molecular mass  the mass of a produces molten iron polymer  a compound containing very large molecule; you find it by adding the relative molecules, formed by polymerisation atomic masses of the atoms in it titration  a laboratory technique for finding the exact volume of an acid solution that will polymerisation  a chemical reaction in renewable resource  a resource that will react with a given volume of alkaline which many small molecules join to form not run out; for example water, air, sunlight solution, or vice versa very large molecules; the product is called a polymer residue  the solid you obtain when you toxic  poisonous separate a solid from a liquid by filtering positive ion  an ion with a positive charge transition elements  the elements in the respiration  the reaction between glucose wide middle block of the Periodic Table; they precipitate  an insoluble chemical and oxygen that takes place in the cells of all are all metals and include iron, tin, copper, produced during a chemical reaction living things (including you) to provide and gold energy precipitation reaction  a reaction in which trend  a gradual change; the groups within a precipitate forms reversible reaction  a reaction that can go the Periodic Table show trends in their both ways: a product can form, then break properties; for example as you go down product  a chemical made in a chemical down again; the symbol is used to show a Group I, reactivity increases reaction reversible reaction triple bond  the bond formed when two protein  a polymer made up of many rusting  the name given to the corrosion of atoms share three pairs of electrons; a different amino acid units joined together iron; oxygen and water attack the iron, and nitrogen molecule has a triple bond rust forms proton number  the number of protons in U the atoms of an element; it is sometimes S called the atomic number universal indicator  a paper or liquid you sacrificial protection  allowing one metal can use to find the pH of a solution; it proton  a particle with a charge of 1+ and a to corrode, in order to protect another metal changes colour across the whole range of pH mass of 1 unit, found in the nucleus of an atom salt  an ionic compound formed when an unreactive  does not react easily acid reacts with a metal, a base, or a pure  there is only one substance in it carbonate unsaturated compound  an organic compound with at least one double bond Q saturated compound  an organic between carbon atoms compound in which all the bonds between quicklime  another name for calcium oxide carbon atoms are single covalent bonds V R saturated solution  no more of the solute valency  a number that tells you how many will dissolve in it, at that temperature electrons an atom gains, loses or shares, in radioactive isotopes (radioisotopes)  forming a compound unstable atoms that break down, giving out single bond  the bond formed when two radiation atoms share just one pair of electrons valency electrons  the electrons in the outer shell of an atom random motion  the zig-zag path a particle slaked lime  another name for calcium follows as it collides with other particles and hydroxide variable valency  an element shows bounces away again variable valency if its atoms can lose solubility  the amount of solute that will different numbers of electrons, in forming rate of reaction  how fast a reaction is dissolve in 100 grams of a solvent, at a given compounds; for example copper forms Cu+ temperature and Cu2 1 ions reactant  a starting chemical for a chemical reaction soluble  will dissolve in a solvent viscosity  a measure of how runny a liquid is; the more runny it is, the lower its viscosity reactive  tends to react easily solute  the substance you dissolve in the solvent, to make a solution viscous  thick and sticky reactivity  how readily a substance reacts solution  a mixture obtained when a solute volatile  evaporates easily, to form a vapour reactivity series  the metals listed in order is dissolved in a solvent of their reactivity W solvent  the liquid in which a solute is recycling  reusing resources such as scrap dissolved, to make a solution water of crystallisation  water molecules metal, glass, paper and plastics built into the crystal structure of a sonorous  makes a ringing noise when compound; for example in copper(II) sulfate, redox reaction  any reaction in which struck CuSO4.5H2O electrons are transferred; one substance is weak acids  acids in which only some of the oxidised (it loses electrons) and another is spectator ions  ions that are present in a molecules are dissociated, to form H 1 ions; reduced (it gains electrons) reaction mixture, but do not actually take ethanoic acid is a weak acid part in the reaction reducing agent  a substance which brings Y about the reduction of another substance stable  unreactive yield  the actual amount of a product reduction  when a substance loses oxygen, state symbols  these are added to an obtained in a reaction; it is often given as a or gains electrons equation to show the physical states of the % of the theoretical yield (which you can reactants and products (g 5 gas, l 5 liquid, work out from the equation) refining (petroleum)  the process of s 5 solid, aq 5 aqueous) separating petroleum (crude oil) into groups of compounds with molecules fairly close in size; it is carried out by fractional distillation 313

Reference I II The Periodic Table of the Elements III IV V Group 1 H Hydrogen 1 7 9 45 48 51 52 55 56 59 59 64 65 11 12 14 Li Be Sc Ti V Cr Mn Fe Co Ni Cu Zn B C N Lithium Beryllium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Boron Carbon Nitrogen 3 4 23 24 25 26 27 28 29 30 5 6 7 21 22 23 24 93 101 103 106 108 112 27 28 31 89 91 96 Na Mg Nb Ru Rh Pd Ag Cd A Si P Y Zr Mo Tc Sodium Magnesium Niobium Ruthenium Rhodium Palladium Silver Cadmium Aluminium Silicon Phosphorus 11 12 Yttrium Zirconium 41 Molybdenum Technetium 44 45 46 47 48 13 14 15 39 40 42 43 39 40 181 190 192 195 197 201 70 73 75 139 178 184 186 K Ca Ta Os Ir Pt Au Hg Ga Ge As La Hf W Re Potassium Calcium Tantalum Osmium Iridium Platinum Gold Mercury Gallium Germanium Arsenic 19 20 Lanthanum Hafnium 73 Tungsten Rhenium 76 77 78 79 80 31 32 33 85 88 57 * 72 140 74 75 115 119 122 Rb Sr Ce In Sn Sb Rubidium Strontium Cerium Indium Tin Antimony 37 38 58 49 50 51 133 137 232 204 207 209 Cs Ba Th T Pb Bi Caesium Barium Thorium Thallium Lead Bismuth 55 56 90 81 82 83 Fr 226 227 Francium Ra Ac 87 Radium Actinium 88 89 † *58–71 Lanthanoid series 141 144 Pm 150 152 157 159 163 165 167 †90–103 Actinoid series Pr Nd Promethium Sm Eu Gd Tb Dy Ho Er 61 Praseodymium Neodymium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium 59 60 62 63 64 65 66 67 68 238 Np Pu Am Cm Bk Cf Es Fm Pa U Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium 93 94 95 96 97 98 99 100 Protactinium Uranium 91 92 The symbols and proton numbers of the elements Element Symbol Proton Element Symbol Proton Element Symbol Proton Element Symbol Proton number number number number actinium Ac calcium Ca francium Fr lawrencium Lw 103 aluminium Al 89 californium Cf 20 gadolinium Gd 87 americium Am 13 carbon C 98 gallium Ga 64 lead Pb 82 antimony Sb 95 cerium Ce germanium Ge 31 3 argon Ar 51 chlorine Cl 6 gold Au 32 lithium Li arsenic As 18 chromium Cr 58 hafnium Hf 79 71 astatine At 33 cobalt Co 17 helium He 72 lutetium Lu 12 barium Ba 85 copper Cu 24 holmium Ho 25 berkelium Bk 56 curium Cm 27 hydrogen H 2 magnesium Mg 101 beryllium Be 97 dysprosium Dy 29 indium In 67 80 bismuth Bi einsteinium Es 96 iodine I manganese Mn 42 boron B 4 erbium Er 66 iridium Ir 1 60 bromine Br 83 europium Eu 99 iron Fe 49 mendelevium Md 10 cadmium Cd fermium Fm 68 krypton Kr 53 93 caesium Cs 5 fluorine F 63 lanthanum La 77 mercury Hg 28 35 100 26 41 48 36 molybdenum Mo 7 55 9 57 neodymium Nd neon Ne neptunium Np nickel Ni niobium Nb nitrogen N 314

Reference Key Relative atomic masses (Ar) for calculations a IV V VI VII 0 Element Symbol Ar X 27 19 4 aluminium Al 80 b bromine Br 40 F He calcium Ca 12 a = relative atomic mass carbon C 35.5 Fluorine Helium X = atomic symbol chlorine Cl 64 9 2 b = proton number copper Cu 19 fluorine F 4 12 14 16 35.5 20 helium He 1 hydrogen H 127 C N O C Ne iodine I 56 iron Fe 207 Carbon Nitrogen Oxygen Chlorine Neon lead Pb 6 7 8 17 10 lithium Li 7 magnesium Mg 24 28 31 32 80 40 manganese Mn 55 neon Ne 20 Si P S Br Ar nitrogen N 14 oxygen O 16 Silicon Phosphorus Sulfur Bromine Argon phosphorus P 31 14 15 16 35 18 potassium K 39 silver Ag 108 73 75 79 127 84 sodium Na 23 sulfur S 32 Ge As Se I Kr zinc Zn 65 Germanium Arsenic Selenium Iodine Krypton 32 33 34 53 36 119 122 128 At 131 Sn Sb Te Astatine Xe 85 Tin Antimony Tellurium Xenon 50 51 52 54 207 209 Po Rn Pb Bi Polonium Radon 84 86 Lead Bismuth 82 83 165 167 169 173 175 Ho Er Tm Yb Lu Holmium Erbium Thulium Ytterbium Lutetium 67 68 69 70 71 Es Fm Md No Lr Einsteinium Fermium Mendelevium Nobelium Lawrencium 99 100 101 102 103 Element Symbol Proton Element Symbol Proton Element Symbol Proton number number number nobelium thallium osmium No 102 rhodium Rh 45 thorium Tl 81 oxygen Os 76 rubidium Rb 37 thulium Th 90 palladium O 8 ruthenium Ru 44 tin Tm 69 phosphorus Pd 46 samarium Sm 62 titanium Sn 50 platinum P 15 scandium Sc 21 tungsten Ti 22 plutonium Pt 78 selenium Se 34 uranium W 74 polonium Pu 94 silicon Si 14 vanadium U 92 potassium Po 84 silver Ag 47 xenon V 23 praseodymium K 19 sodium Na 11 ytterbium Xe 54 promethium Pr 59 strontium Sr 38 yttrium Yb 70 protactinium Pm 61 sulfur S 16 zinc Y 39 radium Pa 91 tantalum Ta 73 zirconium Zn 30 radon Ra 88 technetium Tc 43 Zr 40 rhenium Rn 86 tellurium Te 52 Re 75 terbium Tb 65 315

Index Index Where several page numbers ammonium ion, test for  285 butane 252 changes of state  8–11 are given and one is bold, amphoteric oxides  157 butanoic acid  258 charcoal 234 look that one up first. anode 104 but-1-ene 254 charge (for blast aqueous solution  17 A Ar 70 C furnace) 198 acetone 17 argon  37, 48, 172–173 calamine lotion  153 charge (on sub-atomic acetylene 213 artificial elements  30, 167 calcium acidic oxides  157 artificial fertilisers  228 particles) 32 acidity 150 atmosphere 210 reaction with oxygen  93 chemical change  46, 47 atoms 30, 32 reactivity of  184, 188 chemical equations  68–69 and pH number  149 Avogadro constant  76 calcium compounds chemical properties  42 acid rain  214, 225 Avogadro’s Law  80 carbonate  236, 241 chemical reaction  47 acids 148–155 aquifer 218 hydroxide  16, 148, 241 chlorine oxide  93, 199, 205, and pH  149 B as a member of Group as proton donors  154, 155 back reaction  124 240, 241 VII  170–­ 171 carboxylic 258–259 bacteria  35, 141, 142, 218 calcium ions, test for  286 reactions of  152–153 baking soda  52, 153 calculations from bonding in  55 strong and weak 148, 150 balancing equations  68–69 from electrolysis of addition barium sulfate  160, 287 equations 78–79 polymerisation 264–265 bases 152–153 cancer treatment by brine 108 air 210–213 reaction with sodium  alanine 274 alkalis (soluble radioisotopes 35 alcoholic drinks  256 bases) 148–152 carbohydrates 272–273 48–50 alcohols 256–257 uses of  109 algae 229 and acids  152–153 complex 273 chlorine water  171 alkali metals  166, 168–169 as proton acceptors  155 carbon  chloromethane 253 alkaline earth metals  166, reactions of  152 chlorophyll 144 182 basic oxides  156 allotropes of  61 chromatogram 23 alkalis 148–152 batteries 122–123 as a reducing agent  196 chromatography (paper)  alkanes  250, 251, 252–253 bauxite (aluminium in steel  204, 205 23–25 alkenes 254–255 ore) 195, 200 isotopes of  34 chromium  175, 204 allotropes (of carbon)  61, biological catalysts  140 reactivity compared to use in plating  111 234 biological detergents  141 citric acid  148 alloys  203, 204  bio-polymers 271 metals 186, 188 climate change  239 alumina (aluminium bitumen 247 carbon-12  34, 70, 76 coal 214, 244 oxide)  200, 201 blast furnace  198–199 carbonates 236 cobalt chloride  124 aluminium bleaching carbon cycle  234–235 coke 198 alloys of  203 by chlorine  285 carbon dioxide  236 collision theory (for reaction apparent unreactivity  191 by hydrogen peroxide  87 rate) 138–139 corrosion in  191, 201 by sulfur dioxide  231 and global warming  combustion  93, 114 extraction of  200–201 boiling (change of state)  11 238–239 competition among in the Earth’s crust  194 boiling points  9 metals 186–187 in the reactivity series  188 and purity  19 and the carbon cycle  compound ions  53 ore  195, 197, 200 for ionic compounds  59 234­–235 compounds 46 properties of  201 for molecular and mixtures  46 uses of  200, 202 bonding in  57 covalent  56–57, 58–59 aluminium ions, test for  286 substances  54, 59 in photosynthesis  235 forming 48 aluminium oxide  195, bond breaking and properties of  236 ionic  50–51, 58–59 197, 201 carbonic acid  148, 236 names and formulae  amide linkage  266, 274 making 116 carbon monoxide  236 amino acids  24, 274, bond energies  116 as a reducing agent  196 66–67 276, 277 bonding carboxyl functional percentage composition ammonia 225–227 group 258   as an alkali  148, 151 between ions  50–51 carboxylic acids  258–259 of 73 bonding in  57 in giant covalent car exhausts  215 compression of gases  12 Haber process for  226 cast iron  199 concentration of a in making fertilisers  229 structures 60–61 catalysts 140–141 laboratory in metals  62 biological (enzymes)  140, solution 82–83 in molecules  54–57 finding by titration  preparation 225 brass 203 142–143 162–163 manufacture 126–127, breathalyser test  99 in car exhausts  215 brine 108 transition elements concrete 241 226–227 electrolysis of  108–109 condensation 11 test for  285 bromide ion, test for  287 as  141, 175 condensation ammonium compounds bronze 206 cathode 104 chloride 225 burning of fuels  114, cell (producing polymerisation 263, nitrate  225, 228 118–119 266–267 energy from  118, 119 electricity) 120 condenser 22 cellulose 263 conductivity of metals  42, cement 241 63, 103 chain length conductors 102–103 Contact process  232 and boiling point  251 and homologous series 251 in polythene  264 316

index copper 174 electroplating 111 effect of temperature indicators 149 bonding in  62 elements 30–31 on 12 indigestion 155 in reactivity series  188 empirical formula  84–85 insoluble salts  160–161 refining of  110 endothermic reactions  115 pressure in  12 insulators 102 uses of  202 energy changes during gasoline (petrol)  247 iodide ion, test for  287 giant covalent structures  iodine 170 copper ion, test for  286 reactions 114–115 copper(II) oxide  92 energy from fuels  118–119 60–61 displacement of  171 copper(II) sulfate  158 energy level diagram  114, 115 global warming  238–239 ionic bonds  50–51 enzymes  140, 141, 142–143 glucose 272, 273 ionic compounds  50, 51 electrolysis of equations 68–69 glycerol 275 solution 110 glycine 274 and electrolysis  104 calculations using  78–79 gold 195 formulae of  52 in testing for water  124 half-equations 94 graphite 61 names of  52–53 corrosion ionic equations  95, 154 greenhouse gases  238 properties of  59 equilibrium (in reversible groundwater 218 ions  49, 52, 53 of aluminium  191 reactions) 125 groups in Periodic Table  compound ions  53 of iron  216–217 ester linkage  259, 267, 275 mass of  71 covalent bond  54–55 esters 259 31, 166 iron  174, 175 covalent compounds  56–57 ethane 252 Group 0 (noble alloys of  204–205 covalent giant structures  ethanoates 259 gases) 172–173 corrosion (rusting) 60–61 ethanoic acid  258, 259 Group I (alkali cracking of ethanol  256, 257 metals) 168–169 of 216–217 hydrocarbons 248–249 ethene  254, 255 Group II (alkaline earth extraction of  198–199 crude oil (petroleum)  evaporation 11 metals) 166 in the Earth’s crust  194 244–245 exothermic reactions  114 Group VII (halogens)  in reactivity series  188 crystallisation 20 explosions 137 170–171 ore 198 cysteine 274 extraction of metals  196–197 properties of  174, 175, 204 gypsum 241 iron ions, test for  286 D F iron(III) oxide  156, 198 decay (radioactivity)  34 fats 275 H iron sulfide  46 denature (enzymes)  141 fatty acids  275 Haber process  226–227 isomers  253, 255 density 182 fermentation 142, 256 haemoglobin  236, 274 isotopes  34, 70 detergents (biological)  141 fertilisers 228–229 half-equations 94 diamond 60 filtering 20 halides 170 K diaphragm cell  108 filtrate 20 halogens 170–171 kerosene 247 diatomic 54 flue gas desulfurisation  241 heating curve  9 kilojoule (kJ)  114 dichloromethane 253 fluoride (in water helium  37, 172, 173 kinetic particle theory  11 diesel (fraction from hematite (iron ore)  198 krypton  172, 173 supply) 219 homologous series  251 petroleum) 247 formulae  46, 66 hydrocarbons  251, 252, 254 L diffusion  7, 13 hydrochloric acid  148, 150 lattice  50, 58 displacement reactions  171, empirical 84–85 lead molecular 86–87 electrolysis of dilute  105 185, 187 of compounds  66–67 electrolysis of and extraction dissolving 16 of ionic compounds  52–53 methods 196 distillation 22 formula mass  71 concentrated 105 distilled water  22 forward reaction  124 hydrogen 224 ‘lead’ in pencils  61 double bonds  55 fossil fuels  244 reactivity of  185, 186, 188 fountain experiment  225 as a fuel  119, 121 lead bromide, electrolysis in alkenes  254 fractional distillation  22 bonding in  54 of  104, 106 ductile (of metals)  63, 182 fractions in fractional displacement of  185 Le Chatelier’s principle  126 dynamic equilibrium  125 distillation 246 from electrolysis of light (and photochemical fractions from refining reactions) 144–145, 253 E petroleum 247 brine 108 lime  153, 240 Earth’s crust  194 freezing 8 in Periodic Table  167 limestone 153, 240–241 electricity 102 freezing point  8 reactivity relative to limewater  241, 285 electrode 104 fuel cell  121 liquids 8–11 electrolysis 102–111 fuel oil  247 metals 188 lithium 123, 168, 169 fuels 118–119 test for  285 litmus 148 in extraction of functional group  251, 254, uses of  109 locating agent  25 aluminium 201 256, 258 hydrogen chloride  116, 150 lubricating fraction  247 bonding in  56 in extraction of G hydrogen ions, in acids  M metals 196–197 galena (ore)  230 150, 154 macromolecules 262, galvanising  191, 217 hydrogen sulfide  67, 230 of brine  108 gas chromatography  26 hydrolysis 272–275 of copper(II) sulfate gases  8, 10, 12–13 in digestion  276 magnesium  51, 132, 185 in the lab  277 magnesium chloride  51, solution 110 and Avogadro’s Law  80 hydroxide ions (and of molten compounds  104 compression of  12 alkalinity) 151 132, 185 of solutions  105 diffusion in  13 hydroxides  152, 184, 189 magnesium oxide  51, 85, 186 electrolyte 103 magnesium sulfate (Epsom electron distribution  36–37 I electrons  32, 36 impurities 18–17 salts) 52 electron shells  36 incomplete combustion  252 electron transfer (in redox reactions) 94 317

Index N oxygen mask  213 changing properties names for compounds  52– oxygen tent  213 of 268 malleable (of metals)  63, 174 oxygen, test for  285 manganese (and variable 53, 66–67 uses of  269 naphtha  247, 249 P potassium (as Group I valency) 96 natural gas  118, 244 painting (against rust)  217 manganese(IV) oxide  natural polymers  263 palmitic acid  275 metal) 168–169 neon 48, 172–173 paper chromatography  23, reactivity  184, 185, 188 122, 140 neutralisation reactions  153, mass of atoms, molecules 24­–25 potassium compounds 154–155 paraffin (kerosene)  247 bromide, and and ions  70–71 neutral liquids (and pH)  149 particles in matter  6–7, displacement 171 melting  8, 9, 10 neutral oxides  157 bromide, and melting points  8, 9 neutrons  32, 33 10–11 electrolysis 105 nickel 174 evidence for 6, 7 bromide, and and purity  19 ninhydrin 25 photography 161 of ionic compounds  59 nitrate ion, test for  287 pentane 250 dichromate(VI), as of metals  62 nitrates  152, 160, 189 percentage composition of oxidising agent  99 of molecular covalent nitric acid  148 iodide, and nitrogen 224 compounds 73 displacement 171 compounds 59 percentage purity  73, 88–89 iodide, as reducing of giant covalent bonding in  55 percentage yield  88 agent 99 for plants  228 Periodic Table  166–167, hydroxide  148, 151, 184 structures 60 production in manganate(VII) and metallic bonds  62 178–179 diffusion 7 metalloids 176 industry 212 petrol (gasoline)  87, 247 manganate(VII), as metal oxides  156, 157 uses 213 petroleum (crude oil)  oxidising agent  98 metals  42, 43, 182–183 nitrogen oxides as pollutants 214 244–245 potassium for plants  228 bonding in  62–63 noble gases  172–173 and pollution  214 power stations  118, 119, compared with non- electron distribution in  48 refining of  246–247 in Periodic Table  166 sulfur extraction from  230 231, 241  metals 42–43 uses of  173 precipitation 160–161 extraction from ores  non-conductor 102 pH scale  149 pressure in gases  12 non-metals  42, 43 phenolphthalein 149 propane 250, 252 196–197 compared with metals  42 phosphorus propane-1,2,3-triol in Earth’s crust  194 in Periodic Table  31 in Periodic Table  182 reactions with oxygen  157 combustion in oxygen  157 (glycerol) 275 in reactivity series  188 non-renewable resource  245 impurity in steel- propanoic acid  258 ores 195 nuclear fuels  119 propanone 17 properties of  182–183 nucleon number  33 making 205 propene 254 reactions with nucleus of atoms  32 for plants  228 proteins 263, 272 nylon  266, 269 phosphorus pentoxide  157 oxygen 156 photographic film  145, 161 from polymerisation of reactivity of  184–188 O photosynthesis  144, 234 amino acids  274 stability of oil (petroleum)  244–245 physical change  47 physical properties  42 hydrolysis of  276, 277 compounds 189 and pollution  214 phytoplankton 235 proton donors and transition elements  refining of  246–247 plastics 262, 268–269 sulfur extraction from  230 and pollution  270–271 acceptors 155 174–175 ores  195, 196 made by proton number  32, 33 uses of 175, 202–203 organic chemistry  237 protons 32 metal salts  152, 158–161 organic compounds  237, 250 polymerisation 264–267 purity 18 methane 252 oxidation 92 platinum as fuel (natural gas) 244 and electron transfer  94–95 and melting and boiling as greenhouse gas  238 oxidation state  96–97 in catalytic converters  215 points 19 bonding in  56 oxides 156–157 in the Earth’s crust  194 methanoic acid  252, 258 oxidising agents  98–99 for inert electrodes  104 percentage  73, 88, 89 methyl orange indicator 149 oxy-acetylene torch  213 pollution PVC (polychloroethene)  mild steel  204 oxygen  in air  214–215 mining of metal ores  195 in air  210–211 by plastic  270–271 265, 269 mixtures 16 bonding in the polyamide 266 compared with poly(chloroethene) or Q molecule 55 PVC 265 quartz 60 compounds 46 bonding in ionic polyester 267 quicklime  240, 241 mobile phase (in polymerisation  255, 263, compounds 51 264–267 R chromatography) 26 reaction with metals and polymers  262–263, 264–267 radiation  34, 35 molar volume of a gas  80 poly(propene) 265 radioactivity 34–35 molar solution  82 non-metals 156–157 polysaccharide 273 radioisotopes 34 mole 76 separation from air  212 polystyrene 265 random motion of molecular formulae  uses 213 polythene, or poly(ethene) 262, 264 particles 6 46, 66 and chain lengths  264 rate of reaction  131, molecular substances  and pollution  270 130–145 54–57, 59 and catalysts  140–141 molecules 54 and concentration  134, 138 masses of  71 monomer  262, 264, 266 monosaccharides 273 Mr 71 318

and photochemical sand 60 starch  263, 272 index reactions 140–141 saturated compounds from polymerisation of glucose 273 U and surface area  136–137, (alkanes) 252 hydrolysis of  276, 277 universal indicator  149 139 saturated solutions  17 unsaturated (organic scientific method  280 state symbols  68 compounds) 254 and temperature  135, 139 semi-conductors 177 steel 175 measuring  131, 132–137 separation methods  20–25 test for unsaturation  255 reactants 68 shells (electron)  36 electroplating of  111 unsaturated fats  275 reactions, equations for  silicon dioxide (silica)  60, galvanising of  191 68–69 manufacture of  204–205 V energy changes in  114–115 61, 66 recycling of  205 valency  66, 67, 176 reversible 124–125 silver (a transition styrene 265 valency electrons  166 reactivity substitution reaction  253 variables (in experiments)  280 of Group I metals  168–169 element) 174 sulfates 152 vinegar 258 of Group VII and electroplating  111 solubility of  160 vinyl chloride  265 in film photography  145 sulfur 30, 230 viscosity  247, 251 (halogens) 170–171 reactivity of  184, 185, 188 sulfur dioxide  157, 231 volatile liquids  17, 246 of Group 0 (noble and flue gas voltage (of cells)  190 silver bromide  145, 161 vulcanizing 230 gases) 172 single bond  54 desulfurisation 241 of metals  184–187 slag  199, 205 as pollutant  214, 231 W reactivity series of slaked lime  153, 241 sulfur trioxide  232 water 224 metals 188 smoke particles  6 sulfuric acid  233 recycling iron and steel  205 soap 277 manufacture of  232 as solvent  16, 17 redox reactions  92–97 sodium properties  233 bonding in  56 and electron transfer  sulfurous acid  231 changes of state for  8 as alkali metal  168–169 surface area of solid formula of  46 94–95 extraction of  196 heating curve for  9 and oxidation state  96–97 properties of  168–169 reactant reaction with metals  184 reducing agent  98, 99 sodium chloride  48 and rates of tests for  124 reduction 92–95 bonding in  48, 50 reaction  136–137, 139 uses of  218 in metal extraction  196 electrolysis of molten and risk of explosions  137 water supply  218–219 refining petroleum (oil)  22, symbols for elements  30 water vapour  8 246–247 compound 105 synthetic polymers  262 relative atomic mass, Ar 70 electrolysis of X relative formula mass, Mr 71 T xenon  172, 173 relative molecular mass, solutions  105, 106–108 Teflon  265, 269 Mr 71 structure and Terylene  267, 269 Y residue from filtration  20 tests in the laboratory yeast 142, 256 respiration 234, 235 properties  58, 59 yield 88 reversible reactions  124–125 sodium hydroxide  184 for anions and Rf value  25  cations 286–287 in making ammonia  126, rock salt  195 as alkali  148, 151 227 rotary kiln  240 from electrolysis of for gases  285 rubber (vulcanizing of)  230 for unsaturation  255 Z rusting and its prevention brine 108 for water  124 zinc  174, 182 216–217 uses of  109 tetrachloromethane 253 soil acidity  153, 240 thermal decomposition  189, extraction of  197 S solidifying 11 240, 248 reactivity of  184–186, 188 sacrificial protection  191, solids  8, 11 thermite process  190 uses of  202 solutions 16–17 tin (for plating steel)  111 zinc blende (ore)  197 217 concentration of  82–83 titanium 108, 206, 207, 264 zinc chloride  185 salt (sodium chloride)  50, 58 electrolysis of  105, titrations 159, 162–163 zinc oxide  157 salts 152 tracers 35 zinc sulfate  131 106–107 transition elements  167, making in laboratory  solvents  16, 17 174–175 158–161 sonorous 182 as catalysts  141, 175 stability of metal trichloromethane 253 solubility of some  160 compounds 189 stainless steel  204, 205 standard solution  162 319

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Winters/Science Photo Library; P96t: OUP; P96b: OUP; P97t: Shutterstock; P241t: Emmanuel R Lacoste/Shutterstock; P241b: Ruslan Gilmanshin/ OUP; P97b: OUP; P98: OUP; P99t: OUP; P99m: Jim Varney/Science Photo Library/ Istockphoto; P244tl: Paul Rapson/Science Photo Library; P244tm: Oleksandr Photolibrary; P99b: OUP; P102t: OUP; P102b: Muellek Josef/Shutterstock; P103l: OUP; Kalinichenko/Shutterstock; P244tl: Hywit Dimyadi/Istockphoto; P245tl: Lya Cattel/ P103m: OUP; P103r: OUP; P108t: Georg Gerster/Photo Researchers; P108b: OUP; P109l: Istockphoto: P245tm: OUP; P245tr: OUP; P245b: Eyeidea/Istockphoto; P247: Mike Clarke/ Andrzej Drozdza/Istockphoto; P109r: Mona Makela/Shutterstock; P111l: Ullstein Ecopix/ Istockphoto; P248t: Zybr/Shutterstock; P248b: Christian Lagerek/Shutterstock; P249t: Still Pictures; P111r: OUP; P114l: OUP; P114m: OUP; P114r: OUP; P115l: OUP; P115m: Tony Tremblay/Istockphoto; P249b: MirAgareb/Istockphoto; P250: Rtimages/Istockphoto; Sciencephotos/Alamy; P115r: OUP; P116: Charles D. Winters/Science Photo Library; P252: Sciencephotos/Alamy; P253: Mark Evans/Istockphoto; P245: NFSphoto/ P118l: Jiri Jura/Shutterstock; P118m: Sagasan/Shutterstock; P118r: Chris G. Parkhurst/ Shutterstock; P255: Andre Blais/Shutterstock; P256t: Originalpunkt/Shutterstock; P256b: Shutterstock; P119t: Carolina K. Smith, M.D./Shutterstock; P119b: Postnikova Kristina/ Tish1/Shutterstock; P257t: Celso Pupo/Shutterstock; P257bl: Carroteater/Istockphoto; Shutterstock; P121: American Honda Motor Co., Inc.; P122t: Jon Schutte/Istockphoto; P257br: Tomas Bercic/Istockphoto; P258: Gordana Sermek/Shutterstock; P259: OUP; P122b: Hywit Dimyadi/Shutterstock; P123: Stepanov/Shutterstock, Design/Shutterstock, P262tl: OUP; P262tm: OUP; P262tr: Gelpi/Shutterstock; P262b: RMG; P263tl: Highviews/ Agita Leimane/Shutterstock, Konstantin Chagin/Shutterstock; P124l: OUP; P124r: OUP; Shutterstock; P263tm:Istockphoto; P263tr: Gabi Moisa/Shutterstock; P263b: Chris P125: Peter Albrektsen/Shutterstock; P130tl: OUP; P130tm: Jorgen Schytte/Photolibrary; Hellyar/Istockphoto; P264t: Miguel Malo/Istockphoto; P264b: Andriscam/Shutterstock; P130tr: Charles Schug/Istockphoto; P130bl: Best Images/Shutterstock; P130bm: Valeria/ P265: Istockphoto; P266t: Charles D.Winters/Science Photo Library; P266b: Dreamstime; Shutterstock; P130br: Seraficus/Istockphoto; P131l: OUP; P131m: OUP; P131r: OUP; P132: P267t: OUP; P267b: Shutterstock; P268t: P268t: Tomas Bercic/iStockphoto; P268b: OUP; OUP; P134: OUP; 135t: Filipe Varela/Istockphoto; 135b: Christine Glade/Istockphoto; P269t: Alexey U/Shutterstock; P269bl: Christina Richards/Istockphoto; P269br: Uyen Le/ P136l: OUP; P136r: OUP; P137t: Tyler Stableford/Getty Images; P137b: STR New/Reuters; Istockphoto; P270t: Izabela Habur/Istockphoto; P270bl: Andreas Weiss/Istockphoto; P141t: James L. Amos/Corbis; P141b: Gabi Moisa/Shutterstock; P142t: Dmitry Knorre/ P270br: Andy Davies/Science Photo Library; P271t: Maxine Adcock/Photolibrary; P271b: Istockphoto; P142m: Grasko/Shutterstock; P142bl: Volker Steger/Science Photo Library; Peter Yates/Science Photo Library; P273t: Michał Krakowiak/Istockphoto; P273b: Tania A/ P142br: OUP; P143t: Shannon Matteson/Shutterstock; P143m: Tomas Bercic/Istockphoto; Shutterstock; P275: Heldur Netocny/Photolibrary; P276t: Anita Patterson Peppers/Big P143b: NOAA Photo Library; P144t: Power And Syred/Science Photo Library; P144b: Nigel Stock; P276m: Martin Turzak/Shutterstock; P276b: Shout/Rex Features; P277: Alandj/ Cattlin/FLPA; P148tl: OUP; P148tm: OUP; P148tr: OUP; P148m: OUP; P148b: OUP; P150t: Istockphoto. Dino O./Shutterstock; P150b: Rob Cruse/Istockphoto; P151: RMG; P152t: OUP; P152m: OUP; P152b: OUP; P153t: INSADCO Photography/Alamy; P153b: Ivanschenko Roman/ Shutterstock; P154: Andrew Lambert Photography/Science Photo Library; P155: RMG; P157t: OUP; P157b: Jodi Jacobson/Istockphoto; P158: Canis Maior/Shutterstock; P159: Laurence Gough/Istockphoto; P160: OUP; 161t: Brenda Carson/Shutterstock; 161bl: 320

Complete Authors RoseMarie Gallagher Chemistry Paul Ingram for Cambridge IGCSE® Second Edition Complete Chemistry for Cambridge IGCSE® provides clear and comprehensive RoseMarie Gallagher support for the Cambridge International Examinations syllabus for Chemistry. This and Paul Ingram are bestselling resource now includes a CD with past paper questions and revision a well-known author checklists to fully develop understanding. team with a wealth of teaching, examining Oxford and Cambridge are world leaders in international education. Our combined and authoring expertise and knowledge shape Oxford’s resource packages for Cambridge IGCSE. experience. You can rely on: ● Fully comprehensive, endorsed student textbooks, mapped to the Cambridge syllabus, equipping students to tackle complex theory ● Customisable digital Teacher Kits endorsed by Cambridge and loaded with digital material to support effective delivery ● Thorough revision support focused on building exam confidence and supporting achievement Step-by-step approach simplifies complex ideas Application boxes link learning to the real world Also available: 978 0 19 913881 4 978 0 19 915266 7 1 How to get in contact: web www.oxfordsecondary.co.uk/cambridge email [email protected] tel +44 (0)1536 452620 fax +44 (0)1865 313472