90696 906960 For Supervisor’s use only 3 Level 3 Chemistry‚ 2008 90696 Describe oxidation-reduction processes Credits: Three 9.30 am Friday 28 November 2008 Check that the National Student Number (NSN) on your admission slip is the same as the number at the top of this page. You should answer ALL the questions in this booklet. A periodic table is provided on the Resource Sheet L3–CHEMR. If you need more space for any answer‚ use the page(s) provided at the back of this booklet and clearly
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Equation form for silver halides: Ag + + e - Ag Species produced include: Ag2+‚ Ag2o‚ Ag3+‚ Ag3o‚ Ag4+‚ Ag4o In 1556‚ the alchemist Fabricius was the first to discover that light can photochemically react with these crystals to change the silver ions (Ag+) to elemental silver (AgO). As the reaction proceeds‚ the silver atoms grow into clusters‚ which are large enough to scatter light and produce colors in a pattern identical to that of the original light source. Photography utilizes this chemical
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become soluble in water‚ potassium iodide is added‚ forming triiodide (MEL Science‚ 2015). When reacted with starch attach to structures within a starch molecule‚ leading to a blue-black colour (Ophardt‚ 2003). Starch is a carbohydrate‚ which contains two types of polysaccharides that are connected in two different ways‚ linear amylose and branched amylopectin (Goedecke‚ 2016). When iodine reacts with amylose‚ the iodine ‘gets stuck’ in the starch coils‚ forcing the ion/iodine to become linear as well
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1 : 2 C. 2 : 1 D. 1 : 3 E. 3 : 1 24. A solution contains the ions Ag+‚ Pb2+‚ and Ni2+. Dilute solutions of NaCl‚ Na2SO4‚ and Na2S are available to separate the positive ions from each other. In order to effect separation‚ the solutions should be added in which order? A. Na2SO4‚ NaCl‚ Na2S B. Na2SO4‚ Na2S‚ NaCl C. Na2S‚ NaCl‚ Na2SO4
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In acidic solution‚ iodide ions should be oxidized by the hypochlorite ions to iodine and therefore gave a purple black color. The result of this experiment was not very satisfactory‚ although the reaction was carefully controlled so that the temperature was kept more or less at 40oC. First of all
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away/donate/release its (outermost) electron more | | | | | |easily/readily. | |1 | | | |or‚ Rb can form ion/cation/positive ion more easily/readily. | |(1) | | | |or‚ The strength of metallic bond between Rb atoms is weaker than that between K atoms/Rb can atomize more | | | |
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Exercise 14: Qualitative Anion Tests PURPOSE: The purpose of this experiment is to identify some commonly occurring anions & to study some of the reactions used for their identification. PROCEDURE: You must first determine to which of the three groups the various anions belong. Since no two people observe the same event in exactly the same way it is important to also conduct specific confirmation tests on the known samples of each anion. This information will help identify the anion
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and the effect that the solvent has on the rates of SN1 and SN2 reactions. The SN1 mechanism is a two-step nucleophilic substitution‚ or unimolecular displacement. In the first step of the mechanism‚ the carbon-halogen bond breaks and the halide ion leaving group leaves in a slow‚ rate-determining step to form a carbocation intermediate. The carbocation intermediate is then immediately detained by the weak nucleophile in a fast‚ second step to give the product. A solution of ethanol with some silver
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orange peel as heavy metals absorberInternational Journal of Advanced Engineering Technology E-ISSN 0976-3945 Research Article STATE OF ART OF BIOSORPTION TECHNIQUE FOR TREATMENT OF HEAVY METALS BEARING WASTES Dr. Nitin W. Ingole‚ Sachin V. Dharpal Address for Correspondence Professor‚ Assistant Professor‚ Civil Engineering Department‚ Prof Ram Meghe Institute of Technology and Research‚ Badnera (Amravati) Maharastra – 444701 ABSTRACT Adsorption is one of the Physico-chemical treatment
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Definition: Substances that release hydrogen ions (H+) when dissolved in water. Strong Acids | Weak Acids | Chemical Name | Chemical Formula | Organic acids such as citric acid‚ ethanoic acid. | Hydrochloric acid | HCl | | Sulphuric acid | H2SO4 | | Nitric acid | HNO3 | | Note: The strength of an acid depends on the extent of its ionization in water; strong acids fully ionize in water to produce H+ ions. Characteristics of Acids * sour taste
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