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Вы можете ознакомиться и скачать презентацию на тему Uses of chlorine and its compounds. Доклад-сообщение содержит 8 слайдов. Презентации для любого класса можно скачать бесплатно. Если материал и наш сайт презентаций Mypresentation Вам понравились – поделитесь им с друзьями с помощью социальных кнопок и добавьте в закладки в своем браузере.

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Uses of chlorine and its compounds 11.4B - Group 17 (The Halogens)

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Learning objectives 11.2.1.12 know how chlorine water is formed and the reactions of chlorine with aqueous sodium hydroxide 11.2.1.13 understand the use of chlorine as a water treatment and understand the balance of risks and benefits in this process

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Success criteria - justifies the use of chlorine for water purification (drinking water, pool water) - considers the formation of substances with chlorinated water and their effect on humans - considers the advantages and disadvantages of chlorination of water - considers the harmful effects of unchlorinated water

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Disproportionation The element chlorine (Cl2, oxidation number=0) undergoes a type of redox reaction called disproportionation when it reacts with alkali. Disproportionation can be thought of as a ‘self reduction/oxidation’ reaction. When chlorine reacts with dilute alkali some chlorine atoms are reduced and some are oxidised in the same reaction. The actual reaction that takes place depends on the temperature.

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Chlorine in cold alkali (15 °C) Chlorine in cold alkali (15 °C) Cl2(aq) + 2NaOH(aq) → NaCl(aq) + NaClO(aq) + H2O(l) sodium chlorate(I) The ionic equation for the reaction is: Cl2(aq) + 2OH−(aq) → Cl−(aq) + ClO−(aq) + H2O(l) 0 −1 +1 oxidation number of Cl The ionic equation for this redox reaction can be split into two half-equations, showing the reduction and oxidation. The reduction reaction (in which chlorine’s oxidation number is reduced is): ½Cl2 + e− → Cl− 0 −1 The oxidation reaction is: ½Cl2 + 2OH− → ClO− + H2O + e− 0 +1

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Chlorine in hot alkali (70 °C) When we add chlorine and hot concentrated aqueous sodium hydroxide a different disproportionation reaction takes place:

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Uses of the halogens and their compounds Chlorination of water Adding a small amount of chlorine to a water supply will kill bacteria and make the water safer to drink. The chlorine undergoes disproportionation in water: Cl2(aq) + H2O(l) → HCl(aq) + HClO(aq) 0 −1 +1 HClO is called chloric(I) acid, and it decomposes slowly in solution. One theory suggests that it produces reactive oxygen atoms that can kill bacteria in water: HClO → HCl + [O]

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Bleach Bleach Bleach is an equal mixture of sodium chloride (NaCl) and sodium chlorate(I) (NaClO), made from chlorine and cold alkali. It ‘bleaches’ colours and stains because oxygen atoms from the chlorate(I) ions oxidise dye and other coloured molecules. They also kill bacteria when toilets are cleaned with bleach.