Objectives After studying this Unit‚ you will be able to • name haloalkanes and haloarenes according to the IUPAC system of nomenclature from their given structures; • describe the reactions involved in the preparation of haloalkanes and haloarenes and understand various reactions that they undergo; • correlate the structures of haloalkanes and haloarenes with various types of reactions; • use stereochemistry as a tool for understanding the reaction mechanism; • appreciate the applications of organo-metallic
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thiosulphate Notes: 1. Yellow precipitate (sulphur) is formed. 2. The reaction is slow. Potassium Dichromate (VI) with Ethanedioic Acid Cr2O72- + 14H+ + 3C2O42- ⎯→ 6CO2 + 7H2O + 2Cr3+ Notes: 1. In the reaction‚ the orange colour of the solution turns into green. Cr2O72-: dichromate(VI) ion (Orange) C2O42-: ethanedioate ion (Colourless) Cr3+ : Chromium(III) ion (green) Potassium Manganate(VII) with Ethanedioic Acid 2MnO4- + 16H+ + 5C2O42- ⎯→ 10CO2 + 8H2O + 2Mn2+ Notes: 1
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SCIENCE RATIONALE This syllabus is prepared with a view to address new trends in integrated science teaching and science teacher education. Science has gained world-wide acceptance as a course of study for various reasons such as the concern for social relevance and environmental issues. The teacher is seen‚ as the key to the success of the Educational Reform in Zambia and the effective implementation of the science curriculum will thus depend on the commitment‚ competence and resourcefulness
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atoms/molecules/ions as there are atoms in a 12g sample of carbon -12 12g of carbon-12 contains a constant number of atoms. This number is known as the Avogadro constant (L) and is equal to 6.02 x 1023. 1 mole of carbon-12 contains 6.02 x 1023 atoms. Therefore‚ 1 mole of any substance contains 6.02 x 1023 atoms/molecules/ions. For example‚ 1 mole of aluminium contains 6.02 x 1023 Al atoms 1 mole of ammonia contains 6.02 x 1023 NH3 molecules 1 mole of iron ions contains 6.02 x
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Determination of Chlorine and Iodine in Water I. Introduction The purpose of this laboratory was to determine the amount of chlorine and iodine in a sample of water by titration using a starch indicator and to standardize a sodium thiosulfate solution. Chlorine is added to municipal water supplies to purify it enough to become safe to drink. Iodine is also added to water when people camp or go hiking in the back country where they cannot bring purified water along. Chlorine and iodine are
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The reaction rate can be studied by measuring the time taken for sufficient quantity of yellow sulfur to be formed. Over time‚ a ‘’cross’’ marked on a piece of paper under the conical flask gradually disappears when viewed from above. 1 time taken for the ‘’cross’’ to disappear because the amount of sulfur formed is considered fixed. To study the order of reaction‚ the experiment is repeated by varying the concentration of each of the reactants (Na2S2O3
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will be the most important tool to have on hand for this exercise and for every quiz‚ exam and most homework problems you do. Write on it‚ use color for regions‚ and individualize it for yourself. You have been learning how to combine metal ions with nonmetal ions to write ionic compounds in lecture. In this exercise you will be learning how to name the formulas for many of these compounds‚ along with many of those you have been using in the previous experiments‚ and examples. Communication skills
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Subject Content Most of the objectives specified in this section relate to Knowledge with Understanding‚ although some indication has been given as to where the skills of Handling Information and Solving Problems may be developed. Teachers are reminded that‚ in the written papers‚ 40% of the marks are allocated to these higher ’thinking’ skills. In almost every section‚ students should therefore be given practice at dealing with unfamiliar situations so that these higher thinking skills can be developed
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unstable and inconvenient to work with‚ you will titrate vitamin C samples in this lab with potassium iodate‚ KIO3‚ in the presence of an acidic iodide solution. The iodate ion oxidizes iodide to iodine. IO3Ϫ ϩ 5IϪ ϩ 6Hϩ 1 3I2 ϩ 3H2O Notice that an equilibrium is established. To ensure that the reaction goes to completion‚ it is necessary to use excess iodide and to make the solution acidic. The iodine formed in this reaction immediately
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I2. The brown iodine solution can be reduced by vitamin C (ascorbic acid) to form colourless iodide ions. However‚ I2 solution is not normally prepared directly by dissolving iodine in water because iodine is too volatile so it is almost impossible to avoid loss while the solution is being prepared. Therefore iodine is prepared in situ by mixing pure potassium iodate (KIO3 ) and potassium iodide (KI) in acidified medium. IO3- + 5I- + 6H+ → 3I2 + 3H2O The excess iodine
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