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Sn2 Synthesis Lab Report

886 Words4 Pages

In a two-day experiment, an SN2 reaction was conducted and benzyl bromide, sodium hydroxide, and an unknown were used. In a nucleophilic substitution reaction, the nucleophile and the alkyl carbon determine if the reaction is an SN2 or SN1 reaction. In an SN2 reaction, the process occurs in one step and works best with a primary carbon along with a strong nucleophile. During the experiment, recrystallization was used to purified the product; meanwhile, the melting point range and thin layer chromatography (TLC) data were used to identify the product of the reaction. After the completion, the unknown chemical was determined as 4-chlorobenzyl phenyl ether. To give an overview of the overall process, recrystallization is used to make a pure product, …show more content…

The melting point ranges supported that the purified product could either be sample D (4-chlorobenzyl phenyl ether) or sample E (4-Tert-butylbenzyl phenyl ether) because both share a similar melting point range. However, the tiny layer chromatography data supported only sample D (4-chlorobenzyl phenyl ether). Although the experiment was conducted to avoid mistakes, the yield does not really make sense because it is higher than 100%. The yield could be high because the sodium hydroxide (NaOH) did not completely dissolve or because the product did not fully dry. A way to test these proposed hypotheses is to repeat the experiment and reflux or dry for a longer time. Nevertheless, the recovery of the product does make sense because it is lower than 100% which means impurities were removed. The lost amount of product was about a third of the original mass. The increase melting point range of 52-60 to 59-64 for the product shows that impurities were removed because a pure product has a higher melting point range. The melting point of the product is slightly higher but still, falls around the melting point ranges of two possibilities. Therefore, using solely the melting point is not enough and therefore it is cannot be the only source to rely on. Another source of support to rely on is the thin layer chromatography to reinforce our hypothesis of the unknown. The data states that two compounds,

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The melting point of the product was observed to be 139.5 °C. The theoretical yield of the product is 152 °C (University of South Carolina Department of Chemistry and Biochemistry). The melting point percent difference was calculated by subtracting the theoretical melting point from the actual melting point, dividing the result by the theoretical melting point, and multiplying the result by 100%. The melting point difference was 8.22%. Example calculations are shown

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The following lab period the solid was weighed (0.0483 g) and percent yield was calculated (65.5%) with the limiting reagent being tetraphenylcyclopentadienone. The melting point was determined. The first melting point was 204-204.9 °C and the second melting point was 215.6-215.9°C. Finally, an infrared spectroscopy was obtained for the

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This resulted in a 7.2% yield of pure TPM and a percent recovery of 16%. Evidently, TPM was lost throughout the experiment and/or it was not completely synthesized. The first crude yield of 69% suggests that loss of product may have occurred during the synthesis of TPM and/or the washing/extraction process. Some of the magnesium may not have reacted with the bromobenzene to yield the Grignard reagent.

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Vacuum filtration was performed on the crude product, then it was recrystallized for purification. Melting point analysis was conducted on the recrystallized product to determine its identity. 3. The three possible mechanisms in this experiment were syn-addition

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The substitution reaction was successful but not fully effective. 19. If the data was inconclusive, then comparing various compounds and the unknown based on physical characteristics would be the first step, titrations would also be a good method. 20. To get a better yield, redoing the experiment would require careful attention in the recrystallization steps: amount of solvent used, how hot solvent is, if the mixture cools to room temperature before placing it in an ice

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Firstly, because the NaHCO3 compound was not stored in a sealed container, therefore dust particles could have changed the results, and making the product impure. Also, there are uncertainties associated with the instruments used in this experiment. This, if the products were measured slightly more than should be, this could have affected the concentrations of the solutions, and therefore causing a larger

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The final product weight for percent yield was only the solid E product, which missed one half of the final product produce. If both products were weight, the percent yield would have been larger that it was. Instead of 22.33%, it could have been 44.66%. To prove that both products were obtained, but only one of the two products was analyze, a TLC plate of the DCM layer, that contains both products, and of the final product, was obtain.

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The actual data is the result on our experiment vs theoretical, which is based on the calculations above. I have also learned to pay more attention to draining out all of the product completely before continuing to test the experiment, as any small drop of contaminant can veer our results into a different

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Multiple experiments were conducted to test the rate at which O2 production was influenced by the availability of inorganic carbon. In all experiments, a varying concentration of (either 0.1%, 0.4%, 0.6%, 0.8%, or 1.0%) sodium bicarbonate was assigned to each lab bench, to use as the solution in which the aquatic plants were submerged. In the experiment my partner and I conducted, ~225 mL of distilled water was poured into two 250 mL Erlenmeyer flasks. These would later be used as photosynthetic systems— an experimental control to regulate temperature changes.

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Recrystallization is a method used for purification and relies on varying solubulites at different temperatures. At low temperatures the solute does not dissolves the chosen solvent, but does in the boiling solvent, and this allows the supersaturation to occur. When the solution is cooled, recrystallization forms for the pure substance, and the impurities remain in the solution. This is caused because the impurities will not fit or bond with the structure of the pure crystallized substance. Then vacuum filtration is used to separate the pure component from its impurities.

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The melting point range for the crude product was 113-115.3℃. the melting point range for the purified product was also 113-116℃. This melting point range was almost perfect to that of the theoretical melting point which is 113-115℃ proving that the product was in fact created. When looking at the percent yield of the crude acetanilide, there was an 81% yield which was a very good yield because the average percent yield is between 80-90%. The percent recovery of the acetanilide was 88% which is also very good because much of the product was recovered meaning that the product was in fact

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A melting point of 130 to 135 degrees shows is over 200 degrees lower than the melting point of triphenylmethanol (360-380 degrees C). This could be due to a few reasons. One, the product was not pure. Any contamination, would it be DCM or the petroleum ether, could result in a lower temperature. What supports this possibility was the fact the product was unable to be 100% dried.

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In Experiment One we will be recrystallizing Benzoic Acid from water. In Experiment Two we will be recrystallizing Benzoic Acid using a solvent pair made up of Methanol and Water. The Seven step process of recrystallization consists of adding a solid organic substance into a solvent, then dissolving the chosen solute, decolorizing the solution, filtering solids, then recrystallize the solute by slowly cooling

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