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CHAPTER 4 REACTIVITY OF METALS.pptx

This document discusses reactivity of metals and minerals. It begins by describing the different types of minerals found in rocks and ores, including natural elements like gold and compounds like limestone. It then explains how the reactivity of metals can be determined by observing their reactions with oxygen and other substances. Experiments are described to determine the position of carbon and hydrogen in the reactivity series by observing whether they can displace metals from metal oxides when heated. The document concludes that understanding the reactivity series is important for extracting metals from their ores.

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Chapter 4 REACTIVITY OF METALS
 MINERALS IN THE EARTH CRUST  Each type of ore is different in terms of colour, structure, shape and texture because the ores contain different minerals.  NATURAL ELEMENTS  NON REACTIVE ELEMENTS  DOESN’T COMBINE WITH OTHER ELEMENTS  EXAMPLES : GOLD (AURUM) AND SILVER ( ARGENTUM)  NATURAL COMPOUNDS  COMBINATION OF TWO OR MORE ELEMENTS  COMBINATION BETWEEN METAL ELEMENTS AND NON-METALS ELEMENTS 1. MINERALS
1.Sedimentary rock limestone, sand stone 2. Igneous rock Granite,basalt, 3. Metamorphic rock Marble, gneiss EXAMPLE OF ROCK
Earth’s crust  rock  mineral Natural elements (gold) Natural compound Bauxite ( Al, O )
Gold, diamond, silver Diamond contain 100% atom carbon Gold=100% atom gold Silver= 100% atom of silver ELEMENTS MINERALS (MINERAL BENTUK ELEMENTS)
Rock : lime stone Contained mineral  calcium carbonate [compound], calcite Elements contained in calcium carbonate are calcium,oxygen and carbon NATURAL COMPOUND
= NOT elements But Compound Elements in Quartz are Silicon and Oxygen QUARTZ
MINERAL IN GRANITE(ROCK)
CAN BE DETERMINED BY MINERAL Hardness Resistance against erosion and scratches Example - diamond has the highest hardness Solubility in water Whether mineral dissolves in water or not Effects of heat Whether minerals decomposed (breakdown into simpler substances/elements) upon heating CHARACTERISTICS OF MINERALS
Common name Scientific name Combination of elements Diamond Diamond carbon Gold Gold Gold Silver Silver Silver NATURAL ELEMENTS
Common name Scientific name Combination of elements Hematite (Iron ore) Ferum(III) oxide Ferum(iron),oxygen Pyrite Ferum (II) sulphide Ferum, sulphur Cassiterite (Tin Ore) Stanum (IV) oxide Stanum,oxygen EXAMPLES OF NATURAL COMPOUNDS
Bauxite  elements of aluminium and oxygen Quartz element of silicon and oxygen Galena element lead and sulphur EXAMPLES OF COMPOUNDS AND THEIR ELEMENTS
Common name Scientific name Combination of elements Lime stone Calcium carbonate Calcium, carbon ,oxygen Sand stone Silicon dioxide Silicon, oxygen ELEMENTS OF LIME STONE
 Limestone is a natural compound  Formed from the combination of calcium, carbon and oxygen.  Also known as CALCIUM CARBONATE  Properties of Limestone  Insoluble in water  Decomposed upon heating to form CALCIUM OXIDE and CARBON DIOXIDE IS RELEASED.  = HEATED  Reacts with dilute acid to form SALT, WATER AND CARBON DIOXIDE. LIMESTONE CALCIUM CARBONATE CALCIUM OXIDE + CARBON DIOXIDE CALCIUM CARBONATE +DILUTE ACID SALT + WATER + CARBON DIOXIDE
Limewater shown CLOUDY because Carbon dioxide (CO2) is released HEATING OF LIMESTONE ( CALCIUM CARBONATE) ■ Calcium oxide is produced upon heating
After mixed hydrochloric acid: lime water turns cloudy/chalky/milky Because carbon dioxide gas released REACTION BETWEEN LIMESTONE AND DILUTE ACID
OBSERVATION transparent transparent cloudy cloudy
WORD EQUATIONS REACTION BETWEEN CALCIUM CARBONATE WITH DILUTE ACID CALCIUM CARBONATE + DILUTE SULPHURIC ACID CALCIUM SULPHATE + WATER + CARBON DIOXIDE CALCIUM CARBONATE + DILUTE HYDROCHLORIC ACID CALCIUM CHLORIDE + WATER + CARBON DIOXIDE CALCIUM CARBONATE + DILUTE NITRIC ACID CALCIUM NITRATE + WATER + CARBON DIOXIDE
METALS AND NON-METALS NATURAL ELEMENTS
 Metal reacts with non metals to form a more stable compounds  The rate of reaction is different of each metals  This is because some metals are reactive and some are less reactive  A more reactive metal such as potassium is more reactive than ferum because potassium reacts readily with other metals compare to ferum.  A more reactive metal doesn’t need heat to react, some need to be heated to react with other elements  In fig 4.3, potassium has the highest reactivity compare to other elements, whereas, Aurum or gold is a non reactive metal. REACTIVITY SERIES OF METALS REACTIVE METALS NON REACTIVE
 Metal reacts with oxygen to form METAL OXIDE  The rate of reaction is different of each metal (based on the reactivity series)  Heat energy and/maybe light energy will be produced  Non-reactive metals such as silver, gold and platinum do not react with oxygen  Reactive metals such as potassium and sodium will react with oxygen even without the presence of heat  Other metals react with oxygen need heating.  To supply oxygen to the reaction, POTASSIUM MANGANATE (VII) CRYSTAL is heated.  Precautions when carrying out this experiment  Do not mix the metal fillings with potassium manganate (VII) crystal – mixture will cause explosion  Don’t look directly at the flame of burning reactive metal (such as magnesium) – it can damage your eyes  Asbestos paper and glass are dangerous, handle them with extra caution. REACTION BETWEEN METAL AND OXYGEN METAL + OXYGEN METAL OXIDE
EXPERIMENT
METAL OBSERVATION RATE OF REACTION COLOUR OF FLAME COLOUR OF PRODUCTS/RESIDUE MAGNESIUM Metal burns very quickly and brightly Bright white flame Solid white Magnesium oxide ALUMINIUM Metal burns quickly and brightly Bright white flame Solid white Aluminium oxide ZINC Metal burns slowly Bright green blue flame Solid yellow-hot Solid white – cold Zinc oxide IRON Metal glows brightly Bright yellow Solid brown Iron oxide LEAD Metal glows dimly No flame (glow) Solid brown – hot Solid yellow – cold Lead oxide OBSERVATION
REACTION BETWEEN METAL AND OXYGEN CONCLUSION Burns very fast with oxygen
 Page 133 QUESTIONS AND ANSWERS Magnesium oxide
 Carbon is a non-metal  Carbon reacts with oxygen to form carbon dioxide  The position of carbon in the reactivity series can be determined by the reaction of carbon with other metals  When a mixture of carbon and metal oxide is heated strongly,  REACTION WILL OCCUR if carbon is MORE REACTIVE than metal (CARBON WILL REMOVE METAL FROM ITS METAL OXIDE)  NO REACTION will occur if Carbon is LESS REACTIVE than the metal POSITION OF CARBON IN THE REACTIVITY SERIES IN METALS CARBON + METAL OXIDE METAL + CARBON DIOXIDE
 1.mixture of carbon and zinc oxide  Repeated by:-  Carbon and aluminium oxide  Carbon and lead oxide DETERMINING THE POSITION OF CARBON IN THE REACTIVITY SERIES OF METALS
Aluminium Oxide + Carbon  NO REACTION CARBON + ALUMINIUM OXIDE
BEFORE HEATING Aluminium oxide carbon
AFTER HEATING … NO REACTION Aluminium oxide carbon CARBON CANNOT REMOVE ALUMINIUM FROM ALUMINIUM OXIDE BECAUSE ALUMINIUM IS MORE REACTIVE THAN CARBON ( CARBON IS LESS REACTIVE THAN ALUMINIUM)
ZINC OXIDE + CARBON  ZINC + CARBON DIOXIDE CARBON + ZINC OXIDE
LEAD OXIDE + CARBON  LEAD + CARBON DIOXIDE CARBON + LEAD OXIDE
BEFORE Lead oxide carbon
 LEAD CARBON DIOXIDE  CARBON CAN REMOVE OXIDE FROM LEAD OXIDE BECAUSE CARBON IS MORE REACTIVE THAN LEAD. AFTER
RESULTS MIXTURE OBSERVATION INFERENCE ZINC OXIDE + CARBON MIXTURE GLOWS BRIGHTLY CARBON IS MORE REACTIVE THAN ZINC ALUMINIUM OXIDE + CARBON NO REACTION CARBON IS LESS REACTIVE THAN ALUMINIUM LEAD (II) OXIDE + CARBON MIXTURE GLOWS CARBON IS MORE REACTIVE THAN LEAD Aluminium, carbon, zinc, copper
CARBON POSITION OF CARBON IN THE REACTIVITY OF METALS
 Hydrogen is a non-metal  The position of hydrogen in the reactivity series of metal is also determined by its ability to remove oxygen from metal oxide.  If HYDROGEN is MORE REACTIVE than the metal, HYDROGEN WILL REMOVE OXYGEN from the METAL OXIDE.  HYDROGEN POSITION OF HYDROGEN IN THE REACTIVITY SERIES
APPARATUS SET-UP TO DETERMINE THE POSITION OF HYDROGEN IN THE REACTIVITY SERIES OF METALS
RESULTS
Aluminium Oxide + Hydrogen NO REACTION Zinc Oxide + Hydrogen  NO REACTION Iron oxide + Hydrogen  IRON + WATER Copper oxide + Hydrogen COPPER + WATER WORD EQUATIONS
 Most metals in metal ores exist in the form of metal oxides, metal sulphides and metal carbonates  Extraction of metals involve in the reducing of metal ores to metal or obtaining metal from their ores  Position of metals in the reactivity series will determine the suitable method for the extraction of metals  Carbon is widely used to extract iron, tin, zinc and lead from their ores because carbon is more reactive than these metals.  CARBON IS KNOWN AS REDUCING AGENT EXTRACTION OF METALS FROM THEIR ORES
 THANK YOU AND GOOD LUCK  IF YOU HAVE DONE YOUR VERY BEST, YOUR BEST IS ENOUGH!  TCER P