larger amount of intermolecular force between each electron. This increase in intermolecular attraction means that the required heat energy to reach the boiling point increases. Fluorine has a significantly lower boiling point than the rest of the halides because it has a set of electrons that produces repulsion between them. This weakens the bond. Chlorine has a boiling point of -34.6°C because its covalent bond is stronger than fluorine’s and so on until Iodine which has a boiling point of 184.0°C
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stereoselectivity of the product. The level of electron density on the carbenoid is greatly influenced by the nature of the groups attached to the carbene (Figure 3): electron withdrawing acceptor groups act to decrease electron density‚ which increases reactivity‚ while electron donating donor groups serve to increase electron density which stabilises the structure and raises chemoselectivity. Figure
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chlorides and silver halides groups. AIMS The main objective of this experiment was to identify certain inorganic reaction types and the differences in solubility of silver halides. Thus‚ a series of inorganic reactions was carried out as an introduction to complex formation and precipitation. All the reaction in this experiment
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compulsory Cool-off time is 15 minutes 1] Defects modify the properties of crystals [4 marks] A] Give differences between Schottky and Frenkel defects [2.0] B] On heating zinc oxide becomes yellow in colour. Why? [1.0 ] C] Alkali metal halides on heating in presence of alkali metal produce characteristic colours.Give reason [1.0] 2] Colligative properties depend on the number of solute particles in solution [4 marks] A] Give the name of colligative property suitable for the measurement
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mixture of the major product a with the minor product b. A mixture of the major product b with the minor product a. 10. Consider the SN2 reaction of butyl bromide with OH- ion. Assuming no other changes‚ what effect on the rate would result from simultaneously doubling the concentrations of both butyl bromide and OH- ion? CH3CH2CH2CH2Br + OH- CH3CH2CH2CH2OH +
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noble gas. c) When atoms form chemical bonds by transferring electrons‚ they form ions. Atoms that lose electrons become positively charged ions. Atoms that gain electrons become negatively charged ions. Ions have the electronic structure of a noble gas (Group 0). d) The elements in Group 1 of the periodic table‚ the alkali metals‚ all react with non-metal elements to form ionic compounds in which the metal ion has a single positive charge. e) The elements in Group 7 of the periodic table‚
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on a surface coated with silver atoms. The reaction is possible due to the light-sensitive properties of silver halide crystals. 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
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Comparison of Three Isomers of Butanol Introduction An alcohol’s reactivity is determined based on the attachment of their hydroxyl functional group. The location of this hydroxyl functional group will impact the molecular structure of the alcohol‚ making it either primary (1° )‚ secondary (2° )‚ or tertiary (3° ). The purpose of this experiment is to observe and predict the reactions that take place between all three alcohols and an oxidizing agent‚ as well as to test our theories of how the
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Title: Competing Nucleophiles (Exp 24‚ pp 211-221‚ pp 808-823‚ pp 836-842) Purpose: The purpose of this experiment is to determine the nucleophilic strength of chloride and bromide ions as it reacts with 1-butanol (n-butyl) and 2-methyl-2-propanol (t-butyl alcohol) under SN1 and SN2 conditions. Method: 40 g of ice and approximately 30 ml of sulfuric acid is cautiously added to a 100 mL beaker respectively. Weigh 7.6 g of ammonium chloride and 14.0 g of ammonium bromide and place it in
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very light bluish color Conclusion: The purpose of this experiment is to work with aqueous solutions of ionic substances. Aqueous solutions are those solutions in which water is the solvent. When ionic substances are dissolved in water‚ the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates. The goal of this experiment is to study the nature of ionic reactions‚ write balanced equations‚ and to write net ionic equations for precipitation
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