This week’s lab was the third and final step in a multi-step synthesis reaction. The starting material of this week was benzil and 1,3- diphenylacetone was added along with a strong base, KOH, to form the product tetraphenylcyclopentadienone. The product was confirmed to be tetraphenylcyclopentadienone based of the color of the product, the IR spectrum, and the mechanism of the reaction. The product of the reaction was a dark purple/black color, which corresponds to literature colors of tetraphenylcyclopentadienone. The tetraphenylcyclopentadienone product was a deep purple/black because of its absorption of all light wavelengths. The conjugated aromatic rings in the product create a delocalized pi electron system and the electrons are excited
Friedel-Crafts Acylation is a chemical reaction, and it is a type of electrophilic aromatic substitution. Electrophilic Aromatic Substitution is a type of reaction that uses electrophile for aromatic ring from their substitution of one group of atoms. In other words, they can transfer acyl group to an aromatic ring. Friedel-Crafts has an acyl group that is attached to the structure that has aromatic ring. Acylation is used to give ketones. Carbonyl group makes electron to move back or move away in Friedel-Crafts Acylation, so it has not produced multiple acylations. Moreover, Lewis acid and acid anhydride are usually used in Friedel-Crafts Acylation. For example, the Friedel-Crafts Acylation of Benzene has a mechanism that the acyl halide reacts with the lewis acid, and
In this lab experiment, three milliliters of pure cyclohexane was placed within a test tube and lowered into an ice-water bath. The test tube had a temperature probe within it, which measured the cyclohexane lowering in temperature. Once the cyclohexane solution started to solidify, the cooling curve could be observed and the freezing temperature could be determined. The pure cyclohexane was then thawed, with 0.60 grams of biphenyl being added to the cyclohexane. The experiment was then run again. The result was a freezing point of around 8.6℃ for the pure cyclohexane and 7.0℃ for the cyclohexane-biphenyl solution. To confirm the results that the cyclohexane-biphenyl solution had a lower freezing point, the experiment was ran again. The results
The purpose of this experiment is to conduct an elimination reaction by dehydrating cyclohexanol to cyclohexane. The elimination reaction that is occurring in this experiment is an E1 reaction. An acid catalyst is used in the experiment because the alcohol functional group is a poor leaving group. The method used to achieve this reaction is to boil the azeotrope until it begins to distill into cyclohexene. Cyclohexene is removed from the mixture by keeping the distillation head below 90°C. After the purification of the product, the product will go under two addition reactions (bromine test and a permanganate test) and a IR spectrum. This will determine the identity and the characteristics of the product. The results of the bromine and permanganate
Through the experimentation of reactions between iron (III) nitrate and potassium thiocyanate, as well as cobalt (II) chloride hexahydrate in water, equilibrium systems disturbed by stress (changing the amount of reagents and temperature) will shift in order to minimize the stress. Therefore, if the concentration of reactant increases, the rate of the forward reaction will increase and equilibrium will reestablish when the concentration of products increase (vice versa). This can be observed through color changes of the solutions.
In this experiment, luminol was synthesized and investigated the chemiluminescence reaction. The starting material, 5-nitro-2,3-dihydrophtalazine, was added by reagents, refluxed and vacuum filtered to get luminol. Using stock solutions, we mixed our luminol product with sodium hydroxide, hydrogen peroxide and potassium ferricyanide in a dark room to observe a blue light. In the end there was a 121% yield of luminol and experienced a blue glow.
Our unknown solution, test tube 1024, contained mercury (I) and lead. Throughout the entire experiment, we performed the same reactions in a known solution that contained all three metal ions as a visual comparison to determine what qualities one should observe after each added compound. Because each ion was initially in a compound with nitrate (NO3) in an aqueous, solution we added hydrochloric acid (HCl) to both solutions, and both solutions formed a white precipitate. Because all three metal ions form a white precipitate when bonded with chlorine (Cl‐), it remained unclear which specific ions were present. We then decanted the supernatant and submerged each test tube with the remaining precipitate in a hot water bath. Lead (II) chloride,
General Protocol :Now repeat steps 17-28 for temperatures: 0°C, 10°C, 20°C, 30°C, 40°C, 50°C, and 60°C, testing three times each. Always put the catalase into the ice chest when not in use. Repeat with new hydrogen peroxide every time and make sure the temperature of the hydrogen peroxide is the temperature you are testing. Clean out jars immediately after testing and refill them with hydrogen peroxide, so multiple temperatures can be tested at once. There are 2 hours to test 20 runs (not including the 1st room temperature test) before the catalase starts denaturing (breaking down).
The acid compound, which contain a carboxylic group is altered chemically when an aqueous sodium hydroxide, a strong base, is added to the mixture to change its distribution between a pair of solvent, methylene chloride and water. This reaction produce a salt, which contain a Na+ in its chemical structure that is soluble in water but not in our organic solvent, methylene chloride. Also this reaction will yield water, which is immiscible with most organic solvent. The salt will be soluble in water and the neutral compound will be mixed with methylene
The pure product was also analyzed under infrared spectroscopy. Due to time, the infrared spectrum obtained was of another’s product. According to Figure 1, the IR shows two areas of interest. There is a one band at 3463.97 cm-1, which indicates the presence of an alcohol. It is a small band though; the presence of alcohol is small. The is also another peak at 3061.88 cm-1, signifying C-H bonds for an aromatic ring. Even though the infrared spectrum was accurate, it doesn’t aligned with the product synthesized. The synthesis of triphenylmethanol was successfully completed, but the result was not
Instead, the spectrum for station 2 was examined and compared to an IR spectrum of carvone. In the IR spectrum of carvone, the Peak located at ~1680 cm-1 indicates a carbon oxygen double bond, and the small peaks located just under 3000 cm-1 indicate carbon hydrogen bonds. In the spectrum for the product, the peak the broad Peak ranging from 3300 to 3400 cm-1 indicates an oxygen hydrogen alcohol bond. The peaks just below 3000 cm-1 also indicate hydrogen carbon bonds, and the peak just above 3000 cm-1 indicate vinyl carbon hydrogen bonds. Also the two peaks at around 1600 cm-1 and 1500 cm-1 with the small overtones located at the range of 1800 cm-1 to 2000 cm-1 indicate a benzene ring is present in the product. Based on these peaks, it indicates that the product is carvacrol, and station 2’s experiment was
Abstract: The safety of pool water is reliant on chemical sterilisation, to destroy dangerous pathogens. The most common steriliser is chlorine, in the form of hypochlorite ions (OCl-) and hypochlorous acid (HOCl). However sunlight causes drastic decomposition of these chemicals, thus methods to protect chlorine from sunlight have been created for pools. Some of these include pool covers, or chemical stabilisers which combine with the free hypochlorite ions to reduce decomposition. The most common stabiliser is isocyanuric acid ((CONH)3), added until a concentration of 50mg/L is reached. An experiment was devised to test whether the pool cover or the stabiliser would be more effective at retaining chlorine concentrations, however the results
The aim of this experiment is to carry out a reaction that results in the synthesis of Methyl Benzoate by Fischer Esterification. Methyl Benzoate is an organic compound, it is an Ester with the chemical formula C6H5COOCH3 and it is formed by the condensation of methanol and benzoic acid. Methyl Benzoate is strongly reminiscent of the fruit of the feijoa tree, and it is used in the making of perfumes. (6)
An organic molecule is a molecule that contains hydrogen and carbon. They are carbohydrates, proteins, lipids, and nucleic acids. The carbon bonds to other atoms through covalent bonding. They are often large, have many atoms, and are associated with living organisms.
Medical diagnosis and lab testing can becommercial uses for biochemical testing to diagnose diseases. Animals are also checked for diseases and to make sure they are acceptable for human ingestion.
For the reaction, thiamine was used in our reaction in the formation of the product. Thiamine attacks the carbonyl carbon of an aldehyde in the same way a cyanide ion does. By removing a relatively acidic proton on the five-membered thiazolium ring of thiamine by a base, carbanion that is nucleophilic is produce and can attack the carbonyl. Moreover, thiamine hydrochloride was chosen as the reagent over cyanide because of dangers involved in the use of cyanide, which is a lethal poison that can kill with little warning. Thiamine HCL has been shown to be an efficient and safer catalyst for the condensation of benzaldehyde, which could qualify this reaction as a green chemistry reaction. This reaction turned the aldehyde into a hydroxy ketone by adding a benzyl alcohol, forming a new C-C bond. The Cannizzaro reaction did not occur in this reaction, as benzoic acid or benzyl alcohol would have formed instead of