Page 1 of 9 Minerals - Solid elements or compounds found naturally in the Earth s crust and forms it - Each mineral has its own chemical content and can be found in elements or compounds Natural Mineral Elements Natural Mineral Compounds - Minerals that exist naturally in form of elements are not active so it - Most elements are active and combine with others to form compounds can exist freely without combining with other elements - Tin Ore, Clay and Limestone - Gold, Platinum, Mercury - Most Minerals exists as compounds : Oxide, Carbonate, Sulphide & Silicate - Non-Metallic : Carbon & Silver Natural Mineral Type of Ore Mineral Content Elements Contained Bauxite (White) Aluminium Ore Aluminium Oxide Aluminium & Oxygen Cassiterite (Black) Tin Ore Tin Oxide Tin & Oxygen Hematite (Brown) Iron Ore Iron Oxide Iron & Oxygen Magnetite Magnesium Ore Magnesium Carbonate Magnesium, Carbon & Oxygen Malachite (Green) Copper Ore Copper Carbonate Copper, Carbon & Oxygen Iron Pyrite (Black) Iron Ore Iron Sulphide Iron & Sulphur Galena (Grey) Lead Ore Lead Sulphide Lead & Sulphur Chalcocite Copper Ore Copper Sulphide Copper & Sulphur Limestone (White) / - Calcium Carbonate Calcium, Carbon & Oxygen Marble/ Calcite Clay - Aluminium Silicate Aluminium, Silicon & Oxygen Mica - Potassium Aluminium Silicate Potassium, Aluminium, Silicon & Oxygen
Page 2 of 9 Properties of Minerals Hard, insoluble in water and characteristics depend on the arrangement of atoms which are divided into two types Physical Characteristics Chemical Characteristics - Minerals have different colour - Most minerals do not dissolve in water - Hardness (resistance against erosion and scratches) - Metal Oxide and Silicate normally do not decompose when - Hard minerals can scratch a softer mineral heated - All metal oxides, sulphides and carbonates are hard minerals - Metal Carbonates and Sulphides can easily be decomposed by heating - Most minerals exist in crystals with the same shape Effect of Heat Metal Carbonate Metal Oxide + Carbon Dioxide Metal Sulphide + Oxygen Metal Oxide + Sulphur Dioxide Test : Lime water will turn cloudy Test : Acidic Potassium Manganate (VII) will be bleached from purple Acidic Potassium Dichromate (VI) changes from orange to green Magnesium Carbonate Magnesium Oxide + CO 2 Formula : MgCO 3 MgO + CO 2 Calcium Carbonate Calcium Carbonate + CO 2 Formula : CaCO 3 CaO + CO 2 Copper Carbonate Copper Oxide + CO 2 Formula : CuCO 3 CuO + CO 2 Magnesium Sulphide + Oxygen Magnesium Oxide + SO 2 Formula : MgS + O 2 MgO + SO 2 Lead Sulphide + Oxygen Lead Oxide + SO 2 Formula : PbS + O 2 PbO + SO 2 Zinc Sulphide + Oxygen Zinc Oxide + SO 2 Formula : ZnS + O 2 ZnO + SO 2
Page 3 of 9 Reaction between Metals and Non-Metals Metals - Element with a shiny surface, ductile and malleable like cooking pots, frying pans, spoons, knives - Sodium, Iron, Zinc, Magnesium, Iron, Copper, Lead, Gold and Silver Reaction of metals with Oxygen Metal + Oxygen Metal Oxide Non-Metals - Element with a dull surface and brittle like Graphite (carbon), Sulphur, Oxygen and Chlorine Reaction of metals with Sulphur Metal + Sulphur Metal Sulphide Magnesium + Oxygen Magnesium Oxide Formula : Mg + O 2 MgO Zinc + Oxygen Zinc Oxide Formula : Zn + O 2 ZnO Copper + Oxygen Copper Oxide Formula :Cu + O 2 CuO Lead + Oxygen Lead Oxide Formula : Pb + O 2 PbO Calcium + Oxygen Calcium Oxide Formula : Ca + O 2 CaO Iron + Oxygen Iron Oxide Formula : Fe + O 2 FeO Lead + Sulphur Lead Sulphide Formula : Pb + S 2 PbS Calcium + Sulphur Calcium Sulphide Formula : Ca + S 2 CaS Iron + Sulphur Iron Sulphide Formula : Fe + S 2 FeS Copper + Sulphur Copper Sulphide Formula : Cu + S 2 CuS Magnesium + Sulphur Magnesium Sulphide Formula : Mg + S 2 MgS Zinc + Sulphur Zinc Sulphide Formula : Zn + S 2 ZnS
Page 4 of 9 Note! - Avoid mixing metal fillings with Potassium Manganate (VII) crystals because it may cause an explosion when heated together - Do not look directly into the glittering flame of a burning magnesium strip because it may damage your eyes Metal Magnesium Aluminum Observation of reaction between Metal and Oxygen Burns with a bright white glittering flame Burns with a clear flame that spreads quickly Note! Observation of reaction between Metal and Sulphur Zinc Bright flame that spreads slowly Mixture produces very bright - Carry out this activity in a fume chamber - Both experiments show the reactivity of metals in decreasing order : Magnesium Aluminum Zinc Iron Lead Copper Reactivity Equation of reaction Mixture burns very brightly Very reactive Magnesium + Oxygen Magnesium Oxide Mixture burns brightly Very reactive Aluminum + Oxygen Aluminum Oxide embers Reactive Zinc + Oxygen Zinc Oxide Iron Embers that spread slowly Mixture produces bright embers Reactive Iron + Oxygen Iron Oxide Lead Red hot embers Mixture produces dim embers Less reactive Lead + Oxygen Lead Oxide Copper Dim embers Mixture produces very dim embers Less reactive Copper + Oxygen Copper Oxide
Page 5 of 9 Silicon Compounds Silicon Silica Silicate - Second most abundant non-metal element - Also known as silicon dioxide - A compound that contains silicon, metal and - Not found as a free element - sand, quartz, flint oxygen - usually combines with metal and oxygen to form a - Silicon + Oxygen Silicon Dioxide - clay, mica, asbestos, jade, ruby, topaz compound like silica and silicate (Silica) - Silicon + Metal + Oxygen Silicate Properties of Silicon Compounds Do not dissolve in water, react with acid, decompose when heated Uses of Silicon Compounds in Daily Life Silica Silicate - Sand is used to make bricks, mortar, cement, concrete and glassware - Asbestos is used as a heat insulator in the form of sheets like firefighters outfits - Flint is used to light lighters and gas stoves - Topaz, ruby, sapphire, emerald and jade are used as ornamental stones - Quartz is mixed with cement to make concrete - Mica is used as an electric insulator in electrical equipment - Clay (aluminum silicate) is used to make ceramic goods (flower pots, pottery) - Water glass (sodium silicate) is used to preserve eggs, make furniture and floor polish and silica gel (absorbs water vapour) Additional Information - Pure silicon is used to make electronic chips (silicon chips) which contains many complicated electronic components used in electronic equipment (computers) - Fibers made from silicon compounds are called optic fibers and are used to o Replace copper wire to send information like sound data, video at the speed of light o Observe internal organs without having to operate on the patient
Page 6 of 9 Calcium Compounds Calcium Carbonate (CaCO 3) - Formed upon the combination of calcium, carbon and oxygen compounds like corals, egg shells, snail shells, cockle shells, human bones and teeth - Exists in various types of natural rock like marble, calcite and limestone Properties of Calcium Carbonate (CaCO 3) Reaction with acid Calcium Carbonate + dilute acid Calcium Salt + Carbon Dioxide + Water Characteristics A white and hard solid matter that does not dissolve in water Calcium Carbonate + dilute sulphuric acid Calcium Sulphate +CO 2 + H 2 0 Formula : CaCO 3 + H 2 SO 4 CaSO 4 + CO 2 + H 2 0 Calcium Carbonate + hydrochloric acid Calcium Chloride +CO 2 + H 2 0 Formula : CaCO 3 + HCl CaCl 2 + CO 2 + H 2 0 Calcium Carbonate + nitric acid Calcium Nitrate +CO 2 + H 2 0 Formula : CaCO 3 + HNO 3 Ca(NO 3 ) 2 + CO 2 + H 2 0 Effect of heat - Calcium Carbonate (limestone) Calcium Oxide (quicklime) + Carbon Dioxide Formula : CaCO 3 CaO + CO 2 - Carbon Dioxide makes limewater cloudy Note! Remove test tube containing lime water before the one with marble from the flame to prevent the lime water from being sucked into the hot test tube and cracking it
Formation of Quicklime (Calcium oxide) and Slaked Lime (calcium hydroxide) Chapter 6 - Land and its Resources Page 7 of 9 Calcium Carbonate heated Calcium Oxide Add a little water Solid Calcium Hydroxide Dissolve in water Calcium Hydroxide Solution (limestone/marble) (Quicklime) (Slaked Lime) (Lime water) A white powder A lot of heat is released Add a little water to Product formed is lime forms on the when a few drops of dissolve and form lime water because : surface of limestone water is added. A sizzling water It has alkaline which is quicklime sound is heard and the characteristics (ph>7) solid formed is slaked It is used to determine the lime presence of Carbon Dioxide Uses of Calcium Compounds Calcium Carbonate Calcium Oxide Calcium Hydroxide Lime stone is used to : - Make quicklime and glass - Make cement when mixed with clay and water - Eliminate impurities during extraction of metal ore - Marble is used to make some parts of a building (floor) Quicklime is used to : - Dry ammonia gas and alcohol - Make slaked lime - Make lime water Slaked lime is used to : - Neutralise acidity of soil and water (reservoir) - Make white wash (paint walls), plaster, and clay more porous Lime water is used to test the presence of CO 2 by turning cloudy Equation : CO 2 +CaOH 2 CaCO 3 + H 2 0
Page 8 of 9 Petroleum Formation Characteristics - Black and viscous liquid - Formed from decayed dead animals and plants that settled on the sea bed millions of years ago - These sediments were subjected to high temperature and pressure for a long time - Normally trapped between two layers of impermeable rocks and obtained - Do not dissolve in water and consists of a mixture of various hydrocarbon compounds which can be separated through fractional distillation - Normally done in a fractional distillation tower with different sections for different boiling points because each type of hydrocarbon has different boiling points - The higher the boiling point of a petroleum fraction : together with natural gas o o o o The darker its colour The higher its viscosity More difficult to burn More soot produced by its flames Petroleum Fraction Petroleum Gas Petrol Naphta Kerosene Diesel Lubricating Oil - Crude oil is heated until 400 o C to produce a mixture of liquid and vapour - The mixture is then channeled into the tower and the liquid will condense but the vapour that is still hot rises to the top Cooking fuel Use Fuel for cars, motorcycles, aeroplane Resource of chemical substances / make plastic / As a solvent Fuel for jet aeroplanes, cooking and for lamps Fuel for heavy vehicles (lorries, buses, trains, ships, tractors, machines) Vehicle engine & machine lubricant Fuel Oil Fuel for ships & electric generators Bitumen - Road surfacing material (tar) - Waterproof Material
Page 9 of 9 Natural Gas - Hydrocarbon compound usually obtained together with petroleum - Used : o As fuel in industries and in homes o Make ammonia and nitrogen-based fertilizers (urea) - Contributions : o Fuel about 75 % of total energy used in industries o Expansion of various industries like petrochemistry o Providing job opportunities o Country s revenue (income) Coal and Wood - Formed from dead swamp plants (millions of years ago) that has been compressed by layers of Earth - High temperature and pressure changed them into coal and their main content is carbon - Uses of firewood : o Fuel in the form of firewood and charcoal (originates from mangrove tree) o Planks to make furniture, houses, bridges o Turned into pulp to make paper - Uses of coal : o Generate electric energy in thermoelectric generating stations o Extracting metal from ore using coke in a blast furnace o Making chemical substances like dye and naphthalene (moth balls) o Warming the house during winter - However, firewood and charcoal are used less often because they cause air pollution (smoke, soot) Design and use fuel-saving devices Emphasize on use of renewable energy Efficient ways of saving Fuel Resources Develop technology to improve effectiveness in processing and using these resources Recycle substances like plastic, Reusing chemical substances from used goods. Reducing the use of raw chemical substances like petroleum