Title: The Green Oxidation of Borneol to Camphor Date Conducted: February 8‚ 2012 April 27‚ 2012 Abstract: The goal of this experiment was to perform a Green Oxidation of Borneol to Camphor‚ without the use of Chromium synthesis since it is toxic to the environment. Reagent Table: |Chemical Name |Amount used |Molecular weight |Concentration |Density g/mL |BP °C |MP °C |Chemical Formula
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Oxidation of Borneol to Camphor Objectives: The purpose of this experiment was to use oxidation to convert (1S)-(-)-borneol into (1S)-(-)-camphor‚ which was done via the use of reagents such as glacial acetic acid and sodium hypochlorite and laboratory techniques learned in previous labs. Afterward‚ the final desired product was obtained‚ and to characterize and ensure the purity of the product‚ further lab techniques were implemented. Overall Reaction: 0 out of 10 Oxidation Reaction:. Mechanism:
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Introduction Reduction/Oxidation (Redox) reactions are ones that change the oxidation state of a compound. The oxidation state refers to the acquired charge (gained or lost electrons) of an element in relation to its original charge (i.e. S + 2e- S2+); in a compound‚ the overall oxidation state is calculated by adding all the charges of the elements present. The addition of electrons makes the element “reduced” and the loss of electrons is called “oxidized”. These reactions can be carried out
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Borneol; An Oxidation-Reduction Scheme Nicolas Gibson Lab Time: Tuesday 11:30 am Abstract: In this experiment‚ the main objective was to synthesize a ketone from borneol via an oxidation reaction and secondly‚ to produce a secondary alcohol from camphor via a reduction reaction. Therefore‚ the hypothesis of this lab is that camphor will be produced in the oxidation reaction and isoborneol will be the product of the reduction reaction because of steric hindrance. For the oxidation
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Introduction: Borneol (FIGURE-1)‚ first reported and published in the Tang Bencao in 659 A.D.‚ is often used in drug treatment‚ especially in Chinese drugs. It is helpful in opening obstruction of orifices‚ heat syndromes and pain releasing (Dharmananda). Nowadays artificially synthesized borneol‚ a mixture of borneol and isoborneol (FIGURE-2)‚ becomes more popular than pure natural borneol because of the lower cost in drug production. However‚ isoborneol is more toxic than borneol and thus is not
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Experiment 39 Oxidation – Reduction Titrations II : Analysis of Bleach A. Standardization of 0.05 M Na2S2O3 Solution KIO3 concentration 0.01 M Volume of KIO3 Trial #1 Trial #2 Final burette reading 15.01 mL 30.00 mL Initial burette reading 0.00 mL 15.01 mL Milliliters of KIO3 used 15.01 mL 14.99 mL Volume of Na2S2O3 Trial #1 Trial #2 Final burette reading 13.40 mL 25.78 mL Initial burette reading 0.03 mL 13.37 mL Milliliters of Na2S2O3 used
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YOUR NAME: Erin Alston‚ Kennedy Stuart‚ Amber Lamb and Stephonya Williams EXPERIMENT TITLE: Oxidation: Cyclohexanone from Cyclohexanol by Hypochlorite Oxidation and Adipic Acid from Cyclohexanone DATE: 4/18/2014 INTRODUCTION: In experiment 4‚ alcohol is oxidized to a ketone with household bleach. The product is then isolated by steam distillation and is extracted into the distillate with ether. After the removal of ether‚ it leaves the product cyclohexanone. In experiment 6‚ cyclohexanone is
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Name: Date of experiment: 04/02/12 Date of report: 04/03/12 Title: Oxidation – Reduction Activity Series Purpose: To determine relative oxidizing and reducing strengths of a series of metals and ions. Oxidation and reduction reaction occur simultaneously side by side. A reduction reaction occurs only if an oxidation reaction occurs and vise-versa. Electrons are given in oxidation while in reduction electrons are gained. Oxidizing agent is a chemical substance which has a large tendency to
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1. Mechanism of oxidation process In an oxidation process of silicon that usually takes place at very high temperature (thermal oxidation)‚ silicon (Si) reacts with either water vapor (H20) or oxygen (O2) to form silicon dioxide‚SiO2 on the silicon surface. The reaction is represented by following equations: Dry oxidation: Si + O2 → SiO2 Wet oxidation: Si + 2H2O → SiO2 + 2H2 The oxidation process can be implemented through diffusion
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potassium permanganate solution was titrated thrice to give clear Mn2+ with an analyte of acidified FeSO4 until all the Fe2+ in the solution was oxidized to Fe3+. The color of the MnO4-/Mn2+ was used as the indicator for the titration. A balanced oxidation-reduction‚ the molarity/normality of the standards potassium permanganate‚ and the volume of potassium permanganate used allowed the determination of the concentration of the FeSO4. Equipment and Chemicals: Chemicals: * Iron (II) ammonium sulfate
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