Potassium Ocreate To Oxidize An Unknown Secondary Alcohol

The objective of this lab was to create a ketone through an oxidation reaction using a using a secondary alcohol and oxidizing agent in order to use that ketone in a reduction reaction with a specific reducing agent to determine the affect of that reducing agent on the diastereoselectivity of the product. In the first part of this experiment, 4-tert-butylcyclohexanol was reacted with NaOCl, an oxidizing agent, and acetic acid to form 4-tert-butylcyclohexanone. In the second part of this experiment, 4-tert-butylcyclohexanone was reacted with a reducing agent, either NaBH4 in EtOH or Al(OiPr)3 in iPrOH, to form the product 4-tert-butylcyclohexanol. 1H NMR spectroscopy was used to determine the cis:trans ratio of the OH relative to the tert-butyl group in the product formed from the reduction reaction with each reducing agent. Thin-layer chromatography was used in both the oxidation and reduction steps to ensure that each reaction ran to completion.

6. Summarize in a few sentences the halogenation and controlled oxidation reactions of 1°, 2°, and 3° alcohols.

The primary goal of this laboratory is to correctly identify an unknown substance. To achieve this task, one may use various tests that reveal both chemical and physical properties of a substance. By comparing the results of a known substance and the unknown substance, one may eliminate alternative possibilities and more accurately predict the undisclosed compound. Furthermore, by performing these tests, data can be collected and verified regarding chemical and physical properties of the unknown. Understanding the chemical properties of a known substance aids one’s understanding of the unknown based on comparative analysis of the results of the tests.

Catechol oxidase is an enzyme that speeds up the oxidation reaction when catechol is exposed to oxygen. When the reaction occurs, benzoquinone is produced turning the oxidized substance brown. It was hypothesized that the higher the concentration of catechol oxidase, the browner the substance will turn, and the faster it will achieve the color. In the present lab, different concentrations of catechol oxidase were mixed with pure catechol and the rate at which each solution browned was measured using a colorimeter. The

Abstract: Using hypochlorous acid to convert secondary alcohol called cyclododecanol to the corresponding ketone which is cyclododecanone by oxidation.

In this experiment, 0.31 g (2.87 mmol) of 2-methylphenol was suspended in a 10 mL Erlenmeyer flask along with 1 mL of water and a stir bar. The flask was clamped onto a hotplate/stirrer and turned on so that the stir bar would turn freely. Based on the amount of 2-methylphenol, 0.957 mL (0.00287 mmol) NaOH was calculated and collected in a syringe. The NaOH was then added to the 2-methylphenol solution and allowed to mix completely. In another 10 mL Erlenmeyer flask, 0.34 g (2.92 mmol) of sodium chloroacetate was calculated based on the amount of 2-methylphenol and placed into the flask along with 1 mL of water. The sodium chloroacetate solution was mixed until dissolved. The sodium chloroacetate solution was poured into the 2-methylphenol and NaOH solution after it was fully dissolved using a microscale funnel.

For the first part of this experiment, six dry test tubes were obtained and labeled accordingly to test the following halides: 2-chlorobutane, 2-bromobutane, 1-chlorobutane, 1-bromobutane, 2-chloro-2-methylpropane, and bromobenzene. To each of the six test tubes 2ml of 15% sodium iodide in acetone was added. 4 drops of the appropriate halide was added to the test tube labeled for that specific halide. After adding the halide, the test tube was then shaken to mix thoroughly. If a precipitate formed the time it took was recorded. Since none of the solutions formed a precipitate at room temperature after five minutes, the test tubes were placed inside of a hot bath at about 50°C. After one minute, the test tubes were taken out of the hot bath and allowed to cool. If any test tubes formed a precipitate, the time it took was recorded on a table.

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 step, a reflux will be done and then a microscale reflux for the reduction step. The products will be confirmed using Infrared spectroscopy, the chromic acid test, 2,4-DNP test and 13C NMR spectroscopy. The results of this

10ml of 2-chloro-2-methylbutane was added to 25ml of concentrated (12M) Hydrochloric Acid in a separatory funnel. The contents were swirled gently without the stopper and venting was done frequently to release excess pressure. Shake the funnel until the layers separate and able to recognize which one is the aqueous layer and which is the organic layer. The organic layer was washed with 10ml portions of saturated aqueous sodium chloride and cold saturated aqueous sodium bicarbonate. The organic layer was washed again with 10ml of water and saturated aqueous sodium chloride.

The overall aim for conducting this lab experiment is to learn how to separate substances from each other using the methods of decantation, extraction, and sublimation. In this lab experiment we used the procedure of decantation after adding water to dissolve the salt so we can then separate the salt water from the sand. We also used the procedure extraction by heating the mixture of ammonium chloride (NH4Cl) and then extracting the sodium chloride (NaCl) with the water. The process of sublimation was used in this experiment by letting the mixture heat under the flume hood to observe the white fumes passes out of the mixture.

The purpose of the experiment is to oxidize a secondary alcohol (2-octanol) by using sodium hypochlorite (bleach) to produce 2-octanone. The starting material consisted of a sample of 2-octanol that was placed into a three-neck flask along with acetic acid and acetone creating an acidic solution. While monitoring temperature fluctuations to ensure a temperature of 400 Celsius was not reached, sodium hypochlorite slowly dripped from a separatory funnel into the acidic solution. Once this reaction reached its entirety, the solution was combined with sodium bisulfate to remove any of the remaining oxidizing agent. This solution was then tested and brought to a neutral pH using a sodium hydroxide solution. The reaction material was extracted using ether and was then washed with a saturated sodium chloride solution. The organic solution was then dried using magnesium sulfate and was then decanted and placed onto the rotovap. The produced weighed .599g and based on the infrared spectrum analysis (see Figure 1) preformed on the product it was determined to be 86.1% 2-octanol, which means .516g of 2-octanol was obtained in the final product.

Alcohol is an organic compound, containing Oxygen, carbon and hydrogen , which is formed when any hydroxyl functional group is attached to a carbon atom (Alcohol, 2000). A hydroxyl fuctional group consists of one oxygen atom and one hydrogen atom (Alcohols, 2007). The behaviour of an alcohol molecule is usually determined by the number of functional groups it contains ( Masterton, 1989). Ethanol has a formula of C2H5OH(l), demonstrated in figure 1 below, has a melting Point of: -114°C and a boiling Point of 78.5°C. Ethanol has a heat of combustion of 1368 kJ mol-1 and its combustion equation is C2H5OH(l) + 3O2(g)

Experiment 15: Oxidation of Alcohol The purpose of the experiment was to use a computer and the application Excel to record data for the reaction of the oxidation of ethanol to ethanal using potassium dichromate. The reaction was studied. Additionally, a spectrophotometer synced to the computer was used to measure the rate of the reaction.

When chlorine is passed into boiling alcohol, both chlorination of the methyl group and oxidation of the primary alcohol group to an aldehyde occur, giving trichloro-acetaldehyde or chloral: When chloral is treated with caustic alkali, fission of the C-C linkage occurs, giving chloroform and a formate. Acetaldehyde and also many ketones, such as acetone, containing the CH3CO- group behave similarly when treated with calcium or sodium hypochlorite, chlorination of the CH3CO- group being immediately followed by fission of the molecule by the alkali present in the hypochlorite solution. The

The mass of the alcohol burnt from each interval and trial for all alcohols, was recorded. Using this data, the following formula was used to measure the heat enthalpy4: