2.5. Characterization Methods 1H–NMR and 13C–NMR spectra of HPPP‚ BOMP and HVPA were taken in CDCl3 on Bruker DPX–300 MHz spectrometer using tetramethylsilane (TMS) as an internal standard. FT–IR spectra of the synthesized compounds‚ HPPP‚ BOMP‚ HVPA and photocrosslinked polymers were recorded on Perkin-Elmer system 2000 (4000–400 cm–1) spectrometer‚ using KBr pellets. Medium pressure mercury vapour lamp to the power output of 125W/cm2 was used for the photocrosslinking study. The viscosity of the
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ChemActivity 10: Exercises 1. Draw a complete mechanism including the intermediate and most likely product for the reaction of each alkene below with H-X. H + H Cl + Cl Cl + + Br H Br H I Br + H I H + I H 2. Draw a complete mechanism of each pair of reactant including any favorable rearrangements and all important resonance structures of all intermediates. Reactant Pair 1 Cl H Br 1 + Cl No shift stable benzylic carbocation H: shift H H Br
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soluble if heated. Also tested was the reactivity of cyclohexane and cyclohexene in sulfuric acid which tested to prove reactivity between cyclohexene but not cyclohexane. Finally tested was the reaction between bromine and alkenes‚ which showed reaction between the more polar alkenes than non polar. Introduction
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single bonds) or unsaturated (wherein there are one or more carbon-to-carbon multiple bonds). Saturated aliphatic hydrocarbons are alkanes while unsaturated aliphatic hydrocarbons are alkenes and alkynes. The general formula of alkanes‚ alkenes and alkynes are CnH2n+2‚ CnH2n‚ and CnH2n-2‚ respectively. Alkanes‚ alkenes and alkynes can be open-chain (acyclic)‚ cyclic‚ unbranched or branched. Aromatic hydrocarbons are represented by a
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4th form Chemistry questionnaire 1. All of the following structures show the same molecule‚ except one. Which structure is different? H H H H A) H -- C -- C -- C --- C -- H B) CH3 CH2 CH2 CH3 H H H H H H -- C -- H CH3 C) H H D)
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ETHERS Classification of Ethers: Symmetrical ethers – two groups attached to O are identical Ex. CH3CH2OCH2CH3 – diethyl ether Unsymmetrical ethers – two groups attached to O are not identical Ex. CH3CH2OCH3 – ethyl methyl ether Physical Properties of Ethers: Ethers have much lower boiling points compared to alcohols of comparable MWs. BPs of ethers increases with increasing MW. BPs of isomeric ethers increase with increasing alkyl chain length. BPs of ethers are about the
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Hydrolysis of an alkyl nitrile on boiling with mineral acid or alkalis yield corresponding carboxylic acid . R–CN +H2O RCOOH +NH3 CH3–CN + 2H2O+HCL CH3COOH + NH4CL 4. BY OXIDATIVE CLEAVAGE OF ALKENES: Alkenes when heated with alkaline KMNO4 are cleaved at double bond to form carboxylic acids. R–CH=CH–R +4[O] 2RCOOH H3C–CH=CH–CH3 + [O] 2CH3COOH REACTIONS OF
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compared the boiling points of a group of straight chained alkanes to 2 branched alkanes‚ a ketone‚ an alcohol and an alkene. I plotted a graph of boiling points of straight chain alkanes against its molar mass. Here‚ it was noticed that as the molar mass increased‚ the boiling point increased as well. However‚ when I plotted the graph of the 2 branched alkanes‚ the ketone‚ alcohol and alkene‚ I noticed that they didn’t follow the same trend as the straight chain alkanes. The branched alkanes had a lower
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Experiment2: Preparation of Dibenzalacetone Aim: Using the cabon-cabon bond making ability in carbonyl chemistry‚ Dibenzalacetone is synthesized from 2 equivalent of benzaldehyde and 1 equivalent of acetone in a base catalyzed reaction. Physical Data1: *detailed risk and safety phrases are attached. substance Hazards‚ risks and safety practices MW (g/mol) Amt. Used Mol. mp (K) bp (K) density(g/cm^3) acetone R11‚ R36‚ R67‚ S9‚ S25‚ S26 58.08 0.24 g 0.004 178.2 329.4 0.79 benzaldehyde R22
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85°C which is very close to the theoretical melting point of Fluorenone which is about 83 °C. Since the melting point was off by about 1.5°C it is assumed that some sources of error was obtained in the experiment. Since there was very little of the alkene in the sample‚ and none of it eluded out‚ it may have been stuck in the stationary phase. Hence when the ketone passed through the stationary phase it may have gotten contaminated leading to the error. Also all of the MTBE may not have evaporated
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