Oxidation Of 4-Nitrobenzyl Essay

Reaction 2 - 1.Used a Beral- type pipet, added about 2mL (40 Drops) of 1M hydrochloric acid solution to a small test tube.

Melting points are indicative of identifying an unknown product and the level of impurity the product contains. In this case, the possible identity of the product based on its melting points are determined by comparing the obtained melting points of the product to the melting points of the five possible products. Two mini capillaries, containing the product only, were used to determine the product’s melting point. For one mini capillary, the temperature range was 132.1-134.2℃, and the product’s melting point for the second minicapillary ranged from 135.1-137.5℃. In addition, melting points were obtained with the product mixed with meso-hydrobenzoin. The temperature range was 135.0-136.0℃ and 135.0-137.5℃. Although the recorded melting point values fall into the racemic range, but the results still indicate that the product is a meso-hydrobenzoin. The melting point values for the product mixed with the meso-hydrobenzoin standard explains that it is unlikely that the product is racemic. The melting point values were two degrees from each other due to the meso-hydrobenzoin standard making

Repeat steps 4–6 but this time test the solution without oxygen by making the following changes:

The first step that needed to be done in this experiment was adding hydrochloric acid (HCl)

Place the test tube containing cold water in a test tube clamp and hold the test tube above the burning alcohol. Observe the outside of the test tube for evidence of product formation.

Gather 0.61 grams of CaCO3 and 0.768 grams of HNO3, a 250 mL beaker, distilled water, and a heating pad. Put the compounds into the 250 mL beaker and add distilled water. Stir until the compounds are dissolved in the water. After the reaction is done, place the beaker onto a heating pad to evaporate the water. Scrape the remaining compound out of the beaker and mass it.

together with the same reactants used before. Thirdly, mix 0.1M Na2SO4 with those reactants. Then, mix 0.1M NaOH with the same reactants used before again.

in cold stock with the aromatics and bring to a boil. Reduce the heat to

The reaction is carried out in saturated aqueous ammonium chloride solution. Thus no special drying of solvents, reagents, or glassware is required. The reaction mechanism for this experiment can be seen below (Fig. 2)

The pipet was put into the top of the condenser and leaving no open spaces. The vacuum served to get rid of the nitrogen oxide gases that were formed during the oxidation reaction. The solution was heated for 30 minutes, beginning the time when the first sign of nitrogen oxide fumes were observed. After the 30 minutes, the solution was removed and cooled for a few minutes. The solution turned was a brownish-yellow color and all the crystal were dissolved, leaving a liquid. The solution was then transferred, using a Pasteur pipet, to 3 mL of water in a beaker. The reaction flask was rinsed to remove the remainder of the solution. The solution was stirred with a glass rod until room temperature of the solution was achieved. A yellow solid was to form, but instead the solution remained aqueous in the case of the specific experiment explained here. With additional scraping of the solution with a glass rod, no crystals formed at all. The next procedure, if the crystals had formed was to crush the solid with the glass rod and filter the solid until the crystals were dry. The mass would then be weighed and the crystals were to be recrystallized with 95% ethanol. The crystals were to be cooled in ice water to get full crystallization and then the crystals were to be filtered and air dried, then weighed.

The samples were measured for the optical rotations using a polarimeter. The polarimeter reading showed -1.5° rotation with just the achiral solvent, ethanol, which theoretically should be 0°. Thus, this value was used to calibrate the values measured for other samples, i.e. in Table 5, the calibrated optical rotation of camphor from camphor tree (_Cinnamomum camphora_) was 17.8°

The method used in this experiment is called an oxidation reaction. An oxidizing agent takes away electrons from other reactants during a redox reaction. The oxidizing agent typically takes these electrons for itself, thus gaining electrons and being reduced (Helmstein, Ph. D 2017). The organic oxidant used in this experiment is sodium hypochlorite, which is also known as “household bleach’. Sodium hypochlorite in acetic acid is an alternate oxidizing agent used for the development of ketones that was developed by Stevens, Chapman and Weller due to the many advantages it displays (J. Org. Chem, 1980, 45, 2030). This particular oxidation of sodium hypochlorite is an exothermic reaction meaning that it releases heat as an energy form. Due to the exothermic nature of this experiment, temperature ranges should be monitored throughout the experiment. The overall objective in this experiment is to yield a

Once again, after the reaction, we need to clean the products, to remove namely the other reagents used during the reaction. The protocol for this reaction is described in annex n°5

The conditions for this type of reaction vary depending on what degree of alcohol you are trying to oxidize. In our case, we oxidized a secondary alcohol at room temperature. It was

The procedure was performed as follows: For run 1, 20cm3 of acetone, 10cm3 of sulphuric acid and 145cm3 of water was added to a conical flask. 25cm3 of iodine was then added to this solution which started the reaction and immediately, 20cm3