1. C2 The Structure Of The Earth Construction Materials Metals and Alloys Acids and Bases Making Ammonia Making Cars Fertilisers And Crop Yields Chemicals From The Sea HOMEWORK – Finish Mind map and do first 6 mark Q

2. HOME The Structure The Earth is almost a sphere. These are its main layers, starting with the outermost: crust - relatively thin and rocky mantle - has the properties of a solid, but can flow very slowly outer core - made from liquid nickel and iron inner core - made from solid nickel and iron. It is difficult to study the structure of the Earth because: the crust is too thick to drill all the way through scientists need to study seismic waves made by earthquakes or man-made explosions. Plate Tectonics Volcanoes Magma is molten rock under the Earth’s surface. Lava is molten rock that escapes onto the Earth’s surface, for example from a volcanic eruption. Volcanic eruptions Some eruptions produce runny lava, while others produce thick lava that escapes violently. Geologists study volcanoes to try to predict future eruptions, and to gather information about the Earth’s structure. Volcanoes can be very destructive, but some people choose to live near them because volcanic soil is very fertile which makes it better for farming. Igneous rocks Igneous rocks are made when molten rock cools down and solidifies. The slower the molten rock cools, the larger the crystals become. Different types of igneous rocks form lava (molten rock on the Earth’s surface):  basalt is rich in iron - it formed from runny lava produced in a fairly safe volcanic eruption.  rhyolite is rich in silica - it formed from thick lava produced in an explosive eruption. The Structure of the Earth The Structure The Earth is almost a sphere. These are its main layers, starting with the outermost: crust - relatively thin and rocky mantle - has the properties of a solid, but can flow very slowly outer core - made from liquid nickel and iron inner core - made from solid nickel and iron. Plate Tectonics Volcanoes Energy transfer involving convection currents in the semi-rigid mantle cause the plates to move slowly. Oceanic crust is more dense than continental crust Collision – leads to subduction and partial melting Plates cooler at ocean margins so sink and pull plates down Theory of plate tectonics – Wegener’s continental drift theory (1914) was not accepted by scientists at the time. New evisence in 1960s – show ocean floor spreading. The theory was slowly accepted as subsequent research supported the theory Magma is molten rock under the Earth’s surface. Lava is molten rock that escapes onto the Earth’s surface, for example from a volcanic eruption. Volcanic eruptions Some eruptions produce runny lava, while others produce thick lava that escapes violently. Geologists study volcanoes to try to predict future eruptions, and to gather information about the Earth’s structure. Volcanoes can be very destructive, but some people choose to live near them because volcanic soil is very fertile which makes it better for farming. Igneous rocks Igneous rocks are made when molten rock cools down and solidifies. The slower the molten rock cools, the larger the crystals become. Different types of igneous rocks form lava (molten rock on the Earth’s surface):  basalt is rich in iron - it formed from runny lava produced in a fairly safe volcanic eruption.  rhyolite is rich in silica - it formed from thick lava produced in an explosive eruption. The Structure The Earth is almost a sphere. These are its main layers, starting with the outermost: crust - relatively thin and rocky mantle - has the properties of a solid, but can flow very slowly, cold and rigid outer core - made from liquid nickel and iron inner core - made from solid nickel and iron. Plate Tectonics Volcanoes

3. Rocks The materials used in the construction industry: MaterialHow it is made aluminium and ironmetals obtained from ores brickmade from clay glassmade from sand cement and concretemade using limestone granite, limestone and marble rocks mined or quarried from the ground Limestone and Marble Limestone and marble are both forms of calcium carbonate, CaCO 3. The UK’s limestone deposits are in areas of great natural beauty, and this creates environmental problems. Reactions of calcium carbonate Construction Materials Limestone and marble are mostly calcium carbonate. This breaks down when heated strongly. The reaction is called thermal decomposition. Here are the equations for the thermal decomposition of calcium carbonate: calcium carbonate calcium oxide + carbon dioxide CaCO 3 CaO + CO 2 Cement and concrete Cement and concrete are made from limestone, Cement is made by heating powdered limestone with clay. Concrete is made by mixing cement with sand, water and aggregate (crushed rock). Chemical reactions happen in the mixtures and eventually they set hard. Reinforced concrete Concrete is often reinforced with steel. A steel support is made by joining steel bars or cables together and this is then usually surrounded by a mould. Concrete is poured into the mould, where it fills the gaps in the steel support and sets hard. Reinforced concrete is an example of a composite material. Reinforced concrete is a composite material made from concrete and steel. It is a better construction material than concrete alone because:  concrete is hard and strong when squashed, but weak when stretched.  steel is flexible and strong when stretched. The composite material combines the best properties of both materials, so that it is hard and strong when squashed or stretched. This makes it useful for building bridges. HOME

4. Copper Copper can be extracted from its ore by heating it with carbon. Impure copper is purified by electrolysis in which the anode is impure copper, the cathode is pure copper and the electrolyte is copper sulphate solution. An alloy is a mixture of two elements, one of which is a metal. Alloys often have more useful properties than the metals they contain. Extraction and purification of copper Copper is less reactive than carbon, so it can be extracted from its ores by heating it with carbon. For example: copper(II) oxide + carbon → copper + carbon dioxide or 2CuO + C → 2Cu + CO 2 Removing oxygen from a substance is called reduction. The copper oxide is reduced to copper in the reaction above. Electrolysis Copper is purified by electrolysis. Electricity is passed through solutions containing copper compounds, such as copper(II) sulphate. Pure copper forms on the negative electrode. Alloys An alloy is a mixture of two elements, one of which is a metal. Alloys often have properties that are different to the metals they contain. This makes them more useful than the pure metals alone. For example, alloys are often harder than the metal they contain. Alloys contain atoms of different sizes, which distorts the regular arrangements of atoms. This makes it more difficult for the layers to slide over each other, so alloys are harder than the pure metal they contain. A summary of three common alloys, the metals they contain, and their typical uses: Copper and Alloys- Higher tier Metals and Alloys Electrolysis During electrolysis, the anode loses mass as copper dissolves, and the cathode gains mass as copper is deposited. Oxidisation Oxidation happens at the anode because electrons are lost. Reduction happens at the cathode because electrons are gained. Remember OIL RIG: Oxidation Is Loss of electrons, Reduction Is Gain of electrons. Smart Alloys Smart alloys have unusual properties. Nitinol is an alloy of nickel and titanium, and is known as a shape memory alloy. If nitinol is bent out of shape, it returns to its original shape when it is either heated or an electric current is passed through it. Copper Copper can be extracted from its ore by heating it with carbon. Impure copper is purified by electrolysis in which the anode is impure copper, the cathode is pure copper and the electrolyte is copper sulphate solution. An alloy is a mixture of two elements, one of which is a metal. Alloys often have more useful properties than the metals they contain. Extraction and purification of copper Copper is less reactive than carbon, so it can be extracted from its ores by heating it with carbon. For example: copper(II) oxide + carbon → copper + carbon dioxide or 2CuO + C → 2Cu + CO 2 Removing oxygen from a substance is called reduction. The copper oxide is reduced to copper in the reaction above. Electrolysis Copper is purified by electrolysis. Electricity is passed through solutions containing copper compounds, such as copper(II) sulphate. Pure copper forms on the negative electrode. Alloys

5. Making Cars Aluminium The main materials used in the manufacture of cars: Rusting Iron and steel rust when they come into contact with water and oxygen. Both water and oxygen are needed for rusting to occur. In the experiment below, the nail does not rust when air or water is not present. Remember that 21 per cent of the air is oxygen. Rusting is an oxidation reaction. The iron reacts with water and oxygen to form hydrated iron(III) oxide, which we see as rust. This is the word equation for the reaction: iron + water + oxygen → hydrated iron(III) oxide Salt dissolved in water does not cause rusting, but it does speed it up, as does acid rain. Unlike iron and steel, aluminium does not rust or corrode in moist conditions. Its surface is protected by a natural layer of aluminium oxide. This prevents the metal below from coming into contact with air and oxygen. Car Bodies Most iron is converted into steel (an alloy) before being used. Compared to iron, steel is:  harder and stronger  less likely to rust. Iron versus aluminium Iron and aluminium are used to build cars. They are both malleable - they can be bent or pressed into shape. The table summarises some differences in their properties.: Aluminium :  Lighter – so better fuel economy  Does not corrode – lasts longer BUT  It is more expensive to use. Making cars and recycling them Recycling European Union law requires that at least 85 per cent of a car’s materials can be recycled, rising to 95 per cent by 2015. Recycling reduces the amount of waste, and the use of natural resources. HOME

6. Ammonia Ammonia NH3 is a raw material used in the manufacture of fertilisers, explosives and cleaning fluids. It is produced using a reaction between nitrogen and hydrogen called the Haber process. Production costs are based on different factors:  the price of energy  The price of labour  The price of raw materials  The price of equipment  The rate of reaction. The raw materials for this process are:  hydrogen  Nitrogen Hydrogen is obtained by reacting natural gas with steam, or from cracking oil fractions nitrogen is obtained from the air. In the Haber process, nitrogen and hydrogen react together under these conditions:  a high temperature - about 450ºC  a high pressure  an iron catalyst. The Haber Process Manufacturing costs -Higher Factors that increase cost include:  high pressures (they increase the cost of the equipment)  high temperatures (they increase the energy costs). Factors that decrease  catalysts (they increase the rate of reaction).  recycling unreacted starting materials.  automating equipment (because fewer people need to be employed, cutting the wage bill). Economic considerations When a chemical is manufactured, the optimum conditions used are the ones that give the lowest cost. These conditions are not necessarily the ones that give the fastest reaction or highest percentage yield. For example:  the rate of reaction must be high enough to make enough product each day  the percentage yield must be high enough to make enough product each day. The Haber Process Making Ammonia HOME Ammonia Ammonia NH3 is a raw material used in the manufacture of fertilisers, explosives and cleaning fluids. It is produced using a reaction between nitrogen and hydrogen called the Haber process. Production costs are based on different factors:  the price of energy  The price of labour  The price of raw materials  The price of equipment  The rate of reaction. The raw materials for this process are:  hydrogen  Nitrogen Hydrogen is obtained by reacting natural gas with steam, or from cracking oil fractions nitrogen is obtained from the air. In the Haber process, nitrogen and hydrogen react together under these conditions:  a high temperature - about 450ºC  a high pressure  an iron catalyst. The Haber Process

7. Acids and Bases Acids and alkalis The pH scale The chemical properties of many solutions enable them to be divided into three categories - acids, alkalis and neutral solutions. The strength of the acidity or alkalinity is expressed by the pH scale.  solutions with a pH less than 7 are acidic  solutions with a pH of 7 are neutral  solutions with a pH greater than 7 are alkaline. If universal indicator is added to a solution it changes to a colour that shows the pH of the solution. Bases and Acids Bases are substances that can react with acids and neutralise them. Bases such as metal oxides and metal hydroxides react with acids to form neutral products. Examples of bases include:  copper(II) oxide  zinc hydroxide. Neutralisation When an alkali is added to an acid the pH of the mixture rises. This is because the alkali reacts with the acid to form neutral products. The reverse situation also happens too: when an acid is added to an alkali the pH of the mixture falls. This is because the acid reacts with the alkali to form neutral products. A reaction in which acidity or alkalinity is removed is called neutralisation. A neutralisation involving an acid and a base (or alkali) always produces salt and water. Naming salts The name of the salt produced in a neutralisation reaction can be predicted. The first part of the name is ‘ammonium’ if the base used is ammonia. Otherwise, it is the name of the metal in the base. The second part of the name comes from the acid used:  chloride, if hydrochloric acid is used  nitrate, if nitric acid is used  sulphate, if sulphuric acid is used  phosphate, if phosphoric acid is used Carbonates and acids Carbonates also neutralise acids. As well as a salt and water, carbon dioxide is also produced. For example: hydrochloric acid + potassium carbonate → potassium chloride + water + carbon dioxide Neutralisation equations- Higher Ions in solution  Acids in solution contain hydrogen ions, H +.  Alkalis in solution contain hydroxide ions, OH -. Neutralisation can be written as an ionic equation: H + + OH - H 2 O Neutralisation equations You need to be able to write balanced symbol equations for neutralisation reactions between acids and bases, and between acids and carbonates. The equations will involve these acids:  hydrochloric acid, HCl  nitric acid, HNO 3  sulfuric acid, H 2 SO 4. The equations will involve these bases:  ammonia, NH 3 - in solution, this is NH 4 OH  potassium hydroxide, KOH  sodium hydroxide, NaOH  copper(II) oxide, CuO. They will involve these carbonates:  sodium carbonate, Na 2 CO 3  calcium carbonate, CaCO 3. HOME

8. Nitrates or phosphates from fertilisers can cause eutrophication in water Problems if too much fertiliser is used it can pollute water supplies. It may also lead to eutrophication, a situation where there is not enough oxygen dissolved in the water for aquatic organisms to survive. HOME Most fertilisers are made by the reaction of an acid and an alkali. The table shows some examples. Fertilisers- Higher tier Eutrophication Fertilisers Fertilisers:  make crops grow faster and bigger so that crop yields are increased.  They are water-soluble minerals.  They must be able to dissolve in water so that plants can absorb them through their roots.  Fertilisers provide plants with the essential chemical elements needed for growth particularly nitrogen, phosphorus and potassium. Examples of fertilisers, their formula and the essential elements: Making fertilisers Fertilisers and Crop Yield Making a fertiliser in the lab The preparation of a fertiliser in a lab involves the following equipment:  a measuring cylinder to measure a particular volume of an alkali solution  a burette to add acid a little at a time until the alkali has been neutralised  a filter funnel to remove solid crystals of fertiliser after evaporating some of the water from the neutral fertiliser solution. To make ammonium nitrate you should be able to predict that nitric acid and ammonia will be needed.

9. Chemicals from the Sea Useful substances can be obtained by the electrolysis of sodium chloride solution. Products from sodium chloride The products of the electrolysis of sodium chloride solution have important uses in the chemical industry. Hydrogen Hydrogen is used in the manufacture of ammonia and margarine (it is used to harden vegetable oils). Chlorine Chlorine is used to:  kill bacteria in drinking water and swimming pool water  make solvents  make plastics such as polyvinyl chloride (PVC)  make household bleach. Sodium hydroxide Sodium hydroxide is used to make soap and household bleach. Bleach Household bleach, sodium chlorate, is made when sodium hydroxide and chlorine react together: sodium hydroxide + chlorine → sodium chloride + water + sodium chlorate 2NaOH + Cl 2 → NaCl + H 2 O + NaClO Household bleach is used to clean and disinfect toilets, drains and kitchen surfaces. Obtaining sodium chloride Common salt is sodium chloride, NaCl. It can be made in a laboratory by the reaction of sodium with chlorine. However, it is found naturally in large amounts:  in sea water  in underground deposits Mining Salt can be mined as rock salt which is used to treat icy roads in the winter. It lowers the melting point of the ice on the roads so that it melts, even when the temperature is below 0ºC. Salt can also be mined by solution mining. This happens in Cheshire in the North West of England: 1.Water is pumped underground and into the salt deposit. 2.Salt dissolves in the water, forming a concentrated salt solution. 3. This is then pumped up to the surface ready for use by the chemical industry. Solution mining is safer than sending miners underground. Problems with mining:  can lead to subsidence. The weight of the ground above causes the ground to sink downwards and this subsidence can damage buildings and roads. Electrolysis During electrolysis:  chlorine gas forms at the anode (positive electrode)  hydrogen gas forms at the cathode (negative electrode)  a solution of sodium hydroxide forms. These products are reactive, so it is important to use inert (unreactive) materials for the electrodes. A half-equation shows you what happens at one of the electrodes during electrolysis. Electrons are shown as e –. These are the half- equations: anode: 2Cl – – 2e – → Cl2 (oxidation) cathode: 2H + + 2e – → H2 (reduction). HOME