1 / 39

KS4 Chemistry

KS4 Chemistry. Useful Rocks. Contents. Useful Rocks. The rock cycle. Extraction and electrolysis of salt. Uses of the products of salt. Uses of limestone. Summary activities. The rock cycle. Contents. Useful Rocks. The rock cycle. Extraction and electrolysis of salt.

maxime
Download Presentation

KS4 Chemistry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. KS4 Chemistry Useful Rocks

  2. Contents Useful Rocks The rock cycle Extraction and electrolysis of salt Uses of the products of salt Uses of limestone Summary activities

  3. The rock cycle

  4. Contents Useful Rocks The rock cycle Extraction and electrolysis of salt Uses of the products of salt Uses of limestone Summary activities

  5. Three-quarters of the salt we use comes from rock salt. As the earth’s surface changed stretches of sea-water became landlocked. Evaporation of this water along with further geological changes led to deposits of rock salt in many countries including the UK. Rock salt

  6. Negative ions Salt consists of sodium ions (Na+) and chloride ions (Cl-). Chloride ions go to the anode where they lose an electron The neutral chlorine atoms produced join up into pairs Electrolysis of salt (1) Chlorine gas is formed 2Cl- - + 2e- Cl2

  7. Positive ions Na+ are not the only + ions present. There are also H+ ions because some water molecules split up into H+ and OH- ions. H+ accepts electrons more easily than Na+ does. This has important consequences at the cathode. Na+ Cl- H H H O O- Electrolysis of salt (2) H+

  8. Electrolysis of salt (3) • Na+ ions move to the cathode but do not accept electrons. • It is the hydrogen ions that gain electrons • As a result hydrogen gas is formed at the cathode. 2H+ + 2e-  H2

  9. No change “Spectator ion” Na+ Cl- Changed into chlorine gas at anode H Changed into hydrogen gas at cathode O- H+ No change “Spectator ion” Electrolysis of salt (4) • What happens to the various ions?

  10. Na+ Cl Cl Na+ Cl- H H H H O- O- H+ Solution Electrodes Electrolysis of salt (5) • Sodium hydroxide is what is left in the solution at the end of electrolysis

  11. Questions about salt Some salt is dug out of underground deposits of rock salt but most salt is obtained by pumping river water into the salt deposits which may be about 2000m below ground. The salt dissolves to form a solution called brine which travels up a second pipe to the surface. It is then stored in a brine reservoir prior to being used for various purposes. • Name one important winter use of solid rock-salt. • Draw a diagram illustrating the production of brine and its subsequent electrolysis. • Draw a diagram showing how you could remove the gritty impurities in rock-salt in the laboratory.

  12. Brine 2000m - + Dissolved salt. up to surface Rock Salt dissolves Hydrogengas Chlorine gas Sodium Hydroxide Electrolysis Cell Answers about salt (1) • An important winter use of solid rock-salt is to treat icy roads. • Diagram of brine production to electrolysis. pump River

  13. Residue: Gritty impurities Filter paper Filter funnel Filtrate: brine Conical flask Answers about salt (2) • Removal of gritty impurities from Rock Salt

  14. Contents Useful Rocks The rock cycle Extraction and electrolysis of salt Uses of the products of salt Uses of limestone Summary activities

  15. Sterilisation of water e.g. swimming pools and drinking water Bleaching agent, e.g. paper industry Uses of chlorine (1) electrolysis Sodium chloride ‘rock salt’ solution Chlorine gas

  16. Manufacture of HCl continued Uses of chlorine (2) Sterilisation of water e.g. swimming pools and drinking water electrolysis Sodium chloride ‘rock salt’ solution Bleaching agent, e.g. paper industry Chlorine gas Manufacture of Cl-containing organic chemicals

  17. Uses of chlorine (3) Manufacture of PVC and other plastics Manufacture of HCl

  18. Uses of chlorine (4) Manufacture of PVC and other plastics Manufacture of HCl Pesticides Manufacture of Cl-containing organic chemicals Solvents, e.g. solvent for tippex, & ‘dry cleaning’ dyes

  19. Uses of sodium hydroxide (1) Extraction of aluminium Manufacture of soap Sodium chloride ‘rock salt’ solution electrolysis Sodium hydroxide Manufacture of Paper

  20. Uses of sodium hydroxide (2) Extraction of aluminium Manufacture of soap Sodium chloride ‘rock salt’ solution Sodium hydroxide solution electrolysis Manufacture of Paper Textiles (wool, cotton)

  21. Uses of sodium hydroxide (3) Extraction of aluminium Manufacture of soap Sodium chloride ‘rock salt’ solution Sodium hydroxide solution electrolysis Manufacture of paper Textiles (wool, cotton) Neutralization of acid effluents

  22. bleach Sodium hydroxide soap Aluminium extraction Acid neutralization salt chlorine Hydrochloric acid hydrogen Organic chlorides pvc dyes Uses of products from salt Join the appropriate substances with arrows.

  23. Contents Useful Rocks The rock cycle Extraction and electrolysis of salt Uses of the products of salt Uses of limestone Summary activities

  24. Limestone is a sedimentary rock. It comes from the shells of sea creatures or from solids formed in the oceans long ago. It is mostly made of calcium carbonate - CaCO3. It is an important raw material for both the chemical and the construction industries. Limestone

  25. It is capable of neutralising acids but because it is insoluble in water it does so without ever making the solution strongly alkaline. Carbonates fizz (effervesce) when they react with acids. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Neutralizes acid - without the need for strong alkali Limestone as a base Limestone is a base with the formula CaCO3.

  26. During indigestion the stomach may produce too much (excess) acid. Indigestion tablets neutralise some of this acid. These tablets often contain purified calcium carbonate. Limestone for stomachs! Limestone is a base with the formula CaCO3. H2O + CaCl2 + CO2 2HCl + CaCO3 

  27. Acidity can build up in soils. This can inhibit the growth of many crops. Consequently farmers need to adjust the pH back towards neutral. Limestone provides a cheap way of neutralising soil acidity. Limestone for soil Limestone is used in agriculture. pH 5 6 7

  28. Limestone is one of three major raw materials used to extract iron from its ores. It reacts with acidic impurities changing them into a slag that separates from the iron. CaCO3 + SiO2 Limestone – extraction of iron In the blast furnace limestone removes acidic earthy impurities that would ruin the quality of iron. CaSiO3 +CO2

  29. Limestone is heated in huge ovens known as lime kilns. The calcium carbonate decomposes into calcium oxide (quicklime) and carbon dioxide. Quicklime is a vital ingredient of cement, concrete and of most types of glass. Quicklime – the limekiln CaCO3 CaO +CO2

  30. Limekiln Calcium oxide is made industrially in a limekiln. calcium carbonate (limestone) waste air and carbon dioxide 1,500°C hot air hot air calcium oxide (lime)

  31. If water is added to quicklime the calcium oxide changes into calcium hydroxide (slaked lime). Slaked lime is a vital ingredient of various building materials. Slaked lime CaO + H2O  Ca(OH)2 • A solution of calcium hydroxide (limewater) is also used to test for carbon dioxide gas (it goes cloudy).

  32. The main raw materials for cement are limestone and clay. A small amount of gypsum is also added to help the cement set at the right speed. Limestone or chalk Clay or shale Gypsum (calcium sulphate) Manufacture of cement heat Cement

  33. To make concrete cement is mixed with small stones or gravel. Mortar consists of cement mixed with calcium hydroxide. This makes a smooth slow setting mixture suitable for bricklaying Cement, concrete and mortar Cement, concrete and mortar all set when interlocking crystals grow between cement particles joining them together.

  34. Limestone, sand and sodium carbonate are the raw materials used to make most glass. Sodium carbonate Glass heat water Manufacture of glass Limestone Lime (calcium hydroxide) heat Sand (silicon dioxide)

  35. Join matching pairs with arrows. Limestone for indigestion Iron Manufacture CaO + H2O  Ca(OH)2 CaCO3 CaO + CO2 CaCO3 + 2HCl CaCl2 + H2O +CO2 CaCO3 + SiO2 CaSiO3 + CO2 Slaking of lime Manufacture of quicklime Uses of limestone

  36. Contents Useful Rocks The rock cycle Extraction and electrolysis of salt Uses of the products of salt Uses of limestone Summary activities

  37. Glossary • brine – A strong solution of salt, especially sodium chloride. • electrolysis – The process in which an electric current is passed through sodium chloride solution to produce chlorine, hydrogen and sodium hydroxide. • limestone – A sedimentary rock containing mainly calcium carbonate. • quicklime – Calcium oxide. Produced by heating limestone in a limekiln. • rock cycle – A series of processes that cause rocks to change from one type to another. • rock salt – Naturally-occurring crystalized sodium chloride.

  38. Anagrams

  39. Multiple-choice quiz

More Related