Eugenol Synthesis Lab Report

Abstract: The purpose of this experiment is to use the apparatus shown in figure 7-1 of experiment 6 found in the lab manual, to synthesize [1,3,5-C6H3(CH3)3]Mo(CO)3.(2016 Oleg) With this, characterization of the molecule can be accomplished using the infrared spectrum and NMR spectrum of the synthesized compound. It was found in the IR spectra of the product, that suitable stretches were found associated with the C-O bonds of mestylene and molybdenum. With One strong spectra was found at 1855.3973 cm-1 , one medium strength spectra was found at 1942.6002 cm-1 , and one weak spectra of C-O stretch was found at 1298.8638cm-1 . The 1H NMR spectrum of the product showed peaks at δ 2.28 and 5.25, while the H NMR spectrum of mesitylene gave peaks at δ

Diels-Alder Reaction Objective: The objective of this experiment is to demonstrate a typical Diels-Alder reaction by reacting anthracene (diene) with maleic anhydride (dienophile) to produce 9,10-dihydroanthracene-9,10-α,β-succinc acid anhydride, the product. Scheme 1. Cycloaddition through the Diels-Alder Reaction1 Experimental: Anthracene (1.00 g, 5.61 x 10-3 mol), maleic anhydride, (0.75 g, 7.65 x 10-3 mol), and xylene (5.0 mL) were combined in a 10 mL long-necked, round-bottomed flask. A stir bar was added and an empty distillation column was attached to the flask to function as an air condenser. The mixture was refluxed for 40 minutes over a sand bath, ensuring the temperature was monitored to prevent the reflux ring from surpassing the

The purpose of this lab was to utilize roasting, smelting, spectroscopy, and the carbonate test in order to determine the identity of an unknown copper mineral. I determined that the most useful of these tests in determining the mineral was roasting because it provides a fairly accurate percent composition of copper in the unknown mineral.

This week in lab a Diels-Alder reaction produced 4-cyclohexene-1, 2-dicarboxylic anhydride by combining 1,3 butadiene and maleic anhydride. They reaction basically combined 4 pi electrons from a diene and 2 pi elections from a double bond to produce an alkene ring. The diene must be in s-cis conformation for the reaction to even happen. All of the p-orbitals, both from the diene and the double bond must line up so it can attack from top or bottom, which creates a chair structure. Because of this, the trans conformation is favored due to the lesser steric interactions.

The purpose of this study was to conduct a Diels-Alder reaction with the reactants, anthracene-9-methanol and N-methylmaleimide, in conjunction with the principles and metrics of green chemistry: increasing atom economy, utilizing safer solvents, and preventing pollution.1 Upon completion of the calculation, the atom economy and percent yield were found to be 100% and 4.88% respectively. Subsequently, melting point range analysis yielded a melting range of 218-220℃. These findings could be useful for individuals looking to maximize the percent yield for other Diels-Alder reaction while utilizing benign green reagents and solvents.

Within this experiment a type of cycloaddition reaction was performed, called Diels-Alder reaction. This type of reaction involves both a 1,3-diene and an alkene, called the dienophile in this reaction. Within this reaction two new sigma bonds were formed at the 1 and 4 carbon atoms of the diene. Two other pi bonds are also formed simultaneously with the sigma bonds. Due to this concerted nature of the reaction the diene must be able to adopt a s-cis configuration, making the reaction stereospecific.

In this paper, the four Diels-Alder reactions observed in lab will be analyzed in terms of their mechanisms and experimental procedures. Through the Diels-Alder reaction, four different products were formed: dimethyl tetraphenyl phthalate, hexaphenylbenzene, tetraphenylnaphthalene, and triptycene. The general Diels-Alder rules and patterns were followed for each reaction, however, certain things such as solvents and experimental methods were changed in accordance to compounds in order to allow the Diels-Alder reactions to fully and wholly occur.

During the experiment, there were two tasks performed; the synthesization of luminol and the display of chemiluminescence. The starting material used was 5-nitro-2,3-dihydrophthalazine-1,4-dione, and after the addition of NaOH, sodium hydrosulfite, acetic acid and water, we were left with the product of crude luminol.1 Then, the crude luminol was dissolved into a stock solution that contained NaOH.1 That stock solution A was then diluted with water, which turned it into solution A.1 That solution was then combined with solution B, a mixture made from potassium ferricyanide and hydrogen peroxide then diluted with water, which allowed us to observe the blue light emission that was chemiluminescence.1

The purpose of my experiment was to see what liquids will speed up the corrosion process on a clean penny. If I soak a clean penny in bleach then the rate of corrosion on the penny will increase because the chemicals in the bleach will react with the copper and speed up the corrosion process. I tested my hypothesis by filling 9 cups with either bleach, water, or vinegar and letting the pennies sit in each cup for 3 days. My results for my experiment were surprising. The bleach corroded the penny the most. I rated those pennies 3, 4 and a 2. The water only corroded the pennies a little bit. Those pennies were rated 2, 3, and a 2. The vinegar surprisingly cleaned the pennies. I rated those pennies 0, 1, and a 1. To sum it up, I discovered that

In Part A of the experiment, isoborneol was oxidized. First, 0.5 grams of isoborneol was dissolved in 1.5 mL of glacial acetic acid inside a 25 mL Erlenmeyer flask. Next, 4.0 mL of household bleach was added to the solution with swirling. The solution was swirled for the next 15 minutes and then was tested against starch-iodine paper. If there was a blue color, then that indicated there was an excess of NaOCl. If the test was negative, a small amount of bleach (~0.5 mL) was added and tested again. The mixture was then diluted with 15 mL of water and transferred to a separatory funnel. 15 mL of diethyl ether and 0.5-1.0 mL NaHSO3 was added. The funnel was shaken and the layers were allowed to separate. The aqueous layer was removed. The ether layer was washed (separated) with 10 mL NaHCO3 solution. The aqueous layer was then tested against litmus paper to confirm that it was basic. The ether layer was dried by anhydrous Na2SO4.

Dispense .5 mL water into the already weighed conical vial, replace cap and face insert on its down side.

The information above shows the results observed from the experiment. The unknown substance was first observed to be a white, powder that had no smell. When it was mixed with the water, it produced a clear odorless solution. The pH was taken immediately from the solution once it was mixed properly. The pH came out to a 10 on a 14 level scale. This indicated that the solution was a strong alkaline base. With this information, the list of possible solutions are narrowed down to only basic solutions. After dividing the solution into five test tubes, the first test was conducted. The first test was conducted using silver nitrate. The results shows a milky white precipitate. According to Doc Brown, an online informational website, by adding the

There's a variety of different types of chemical reactions, but the ones I'm going to name down low are the main points of chemical reactions. The names of the different types of reactions is Decomposition, Combustion, Acid/base,Synthesis,Single-Replacement, Double- Replacement and Precipitation. Decomposition is one of the eight chemical reactions. Decomposition is when you get something complex and break it down into smaller molecules. Decomposition is the opposite of synthesis reaction.

In 1937, Robert Hill isolated chloroplasts and demonstrated that chloroplasts can give off oxygen in the absence of CO2. The presence of an electron acceptor, 2,6-dichlorophenolindophenol, otherwise known as DCPIP, will turn from a blue color to clear when electrons have been accepted. This artificial electron acceptor intercepts electrons before those electrons reach PS I. Based upon this chemical feat, this will allow for the measurement the absorbance of 600nm wavelength of cuvettes containing free chloroplast reactions at various conditions, such as the effects of uncouplers (Ammonia), herbicides {3-(3,4-dichlorophenyl)-1,1-dimethylurea} (DCMU), light color, and distance from light. Using the isolated chloroplast, sodium chloride buffer, and the artificial electron acceptor, these manipulations will be carried out and the rate of the reaction measured using a spectrophotometer. The results expressed both the uncoupler and herbicide decrease reaction rate, 30 cm away from a 60 watt light bulb is prime for fast reaction rate, and green light demonstrated the fastest reaction rate.

In this experiment, methyl benzoate was synthesized from benzoic acid and methanol with acid catalyze using Fisher Esterification. First benzoic acid and methanol were mixed in 100 mL round bottom flask. We cooled the mixture in ice and poured 3 mL of conc. H2SO4 and swirled to mix compounds. Then we refluxed the mixture for 1 hour. We let the solution cool and then decanted into a separatory funnel containing 50 mL of water and rinsed the round bottom flask with 35 mL of tert-butyl methyl ether and added that to a separatory funnel. We shook and vented thoroughly and drained the aqueous layer which contained a bulk of methanol and H2SO4. We washed the solution in the separatory funnel with 25 mL of water, followed by 25 mL of sat. sodium bicarbonate