Synthesis of N,N-Diethyl-Meta-Toluamide

Purpose :
The purpose of this lab was to synthesize N,N-Diethyl-meta-toluamide (DEET) using the m-methylbenzyoic acid and diethylamine. DEET is the most active ingredient in insect repellents. It is used to protect the skin from insect bites.



Result:
The final weight obtained of the product, N,N-Diethyl-meta-toluamide, was 0.25grams.
The theoretical weight of N,N-Diethyl-meta-toluamide :
Moles of diethyl amine used = moles of N,N-Diethyl-meta-toluamide = 2.50mmol.
Theoretical weight = 2.50mmol x 191.27g/mol
= 0.478grams.
Percent yield of product = 0.25/0.478 x 100%=52.3%
Discussion :
The yield of product was 0.25grams, which was 52.3% of the theoretical yield expected. The discrepancy in the results might have risen from several sources in the experiment.
One possible source might have been a systemic error. All glass wares were required to be dried throughout the experiment and the solutions were expected to be kept cool in order to avoid evaporation of the intermediates. Therefore, the error might have resulted from the use of a wet glassware during the experiment, or if the solutions were left warm during the first part of the experiment.
Conclusion:
The synthesis of N,N-Diethyl-meta-toluamide was feasible with the methods and procedures used in this experiment. The obtained product, though the yield was low, had the physical and chemical properties of the product expected.
This experiment can be improved by using clean and dry glass wares in addition to keeping the initial solutions of diethyl amine cold during the experiment.

Preparation of Aldol Condensation Product

Purpose :
The purpose of this lab was to synthesize 2,6-Dibenzalcyclohexanone using an aldo condensation reaction between benzaldehyde and cyclohexanone. The product will be recrystallized using 95% ethanol, then characterized using melting point analysis.



Result:
The final weight of product obtained from the aldo condensation reaction was 0.42g of 2,6-Dibenzalcyclohexanone. The melting point obtained of the product was 108°C . The actual melting point of 2,6-Dibenzalcyclohexanone,however, is 120°C .
The theoretical weight of the product is
Grams of 2,6-Dibenzalcyclohexanone =
moles of 2,6-Dibenzalcyclohexanone x molecular weight of 2,6-Dibenzalcyclohexanone
moles of 2,6-Dibenzalcyclohexanone = moles of ketone used = 0.002mols
Theoretical weight = 274.36grams/mols x 0.002mols = 0.548grams.
Therefore, percent yield of product :
0.42/0.55 x 100%=76.5%

Discussion :
The yield of the product was 76.5% of 2,6-Dibenzalcyclohexanone, and the melting point was 108°C, which was about 12°C different from the actual melting point expected of the product. This discrepancy in result is due to some errors from the procedures. One source of the error may have been from the transfer of the product from one beaker to another after the reaction. During the process of transfer, some of the product may have been lost, which contributed to the lower yield of the product. Nonetheless, the product obtained was 2,6-Dibenzalcyclohexanone because it had similar properties.

Conclusion:
The purpose of theis experiment, which was to synthesize 2,6-Dibenzalcyclohexanone was accomplished with the method and procedure used in the experiment even though the yield was lower than expected. This experment, however, could be improved if the experiment is designed in such a way that tranferring product from one

Preparation of Para Red and Related Azo dyes

Purpose :
The purpose of this lab was to prepare two azo dyes, para red using a reaction of p-nitroaniline and 2-naphthol, and a related azo dye. Para dye is a chemical dye used in printing. It dyes cellulose fabrics to red.


[reaction diagram for the other azo dye is missing]

Result:
The reaction yielded the desired product, para red, a red colored dye with the use of p-nitroaniline and 2-naphthol.
The second reaction with p-anisidine and 1-naphthol yielded a darker red colored azo dye solution.

Discussion :
The first synthesis using the ketone, 2-napthol, and aldehyde,nitroaniline, produced a red colored para red solution while the other reaction with p-anisidine and 1-naphthol produced a darker red colored solution. The difference in colors of both azo dye was because of the difference in the attachment of the hydroxyl group to the compound. 1-naphthal contains a hydroxyl group on the first carbon, ortho to the attached benzo group while 1-naphthol contains a hydroxyl group on it’s second carbon, meta to the attached benzo group. The difference in color change can also been as a result of the aldehydes used in the solutions.

Conclusion:
The synthesis of para red , and a similar azo dye were achieved through the experimental procedures undertaken, and the products were similar to the predicted azo dyes. The use of similar molecules with different hydroxyl positions reflected on the end result of the solution. However, this experiment may still be improved by careful division of the solutions prior to mixing both solutions because the experiment is skewed if too much of one carbonyl compound is added to the other.

Wittg Synthesis Of 1,4-Diphenyl-1,3-Butadiene

Purpose of Experiment
The purpose of this experiment was synthesize 1,4-Diphenyl-1,3-butadiene from benzyl triphenylphosphonium chloride and pure trans-cinnamaldehyde using Wittig reaction process to convert the carbonyl group in trans-cinnamaldehyde into a carbon carbon double bond.


Results
The weight of the product from the experiment was 0.156g, and the melting point obtained was 145°C. Therefore, the product was 1,4-Diphenyl-1,3-butadiene, which has a melting point in the range of 151-153°C, because it has a melting point which is closer to that of the unknown.
Below is the percent yield of the product obtained :
Mole of product is 1mmol because of 1:1 mole ratio of 1,4-Diphenyl-1,3-butadiene with trans-cinnamaldehyde
(1mmol )/(206.29g/mol) = 0.206grams of 1,4-Diphenyl-1,3-butadiene
Percentage yield = (0.156g )/0.206g x 100%=75.6%

Discussion
The yield obtained from the experiment was 75.6% of the actual yield. The discrepancy might have been from the design of the experiment. Before and after the aqueous sodium hydroxide was added to the reaction, the reaction was supposed to be mixed thoroughly in order to facilitate the reaction between the compounds added.The discrepancy might have resulted from incomplete reaction between the reaction constituents.
The lower yield of product might have been from the separation of the aqueous and the organic layer after washing the crude product. Pipetting away the product along with the aqueous layer might have resulted from a reduced product of 1,4-Diphenyl-1,3-butadiene.
The melting point obtained from the solution was 145°C , and differed from the actual melting point by 6-8°C. The discrepancy in the result might have been from the equipment used. The solution was inserted into the machine while it was warm (about 60°C). This might have led to the lower boiling point.
The obtained product was 1,4-Diphenyl-1,3-butadiene because the melting point was very similiar to that of the predicted product. The physical features such as color, which was white, melting point, melting point, texture and so on was also similar to that of the predicted product.

Conclusion
The method of characterization used in this experiment supports purity of the product obtained. The product was much like the hypothesized.
The purpose of the experiment was to synthesize 1,4-Diphenyl-1,3-butadiene using the Wittig reaction. The objective and purpose of the experiment was obatined with the method that was implemented to synthesize and purify the product. One way this experiment could be improved is the strictly follow the procedures, and avoid taking the melting point with a system that is not at room temperature.

Nitration of Naphthalene

Purpose of experiment:
The purpose of this experiment was to nitrate naphthalene with nitronium ion, which is formed at low concentration from a reaction of nitric acid and sulfuric acid. Naphthalene is a house product used... The major product from the reaction is the kinetic product, the one that forms the more stable cabocation intermediate.

Method and procedure:
Into a 5-ml conical vial, 1.0ml of mixed 1:1 sulfuric acid and nitric acid was added. 0.50g of finely divided naphthalene was added in small portions to the solution while stirring after each addition, and cooling to keep the temperature around 45-50°C. The reaction mixture was then stirred in a 60°C water bath for 20minutes after the addition of naphthalene.
When the reaction cooled to room temperature, the solution was transferred to a beaker containing 25ml of ice-cold was with stirring. Yellow crystals are allowed to form, and then the liquid content is removed with filter-tip pipet. The solid was then boiled with 10ml of fresh water for 10minutes.
The mixture was cooled in ice and the product was collected by vacuum filteration. 0.1 of the crude product was then recrystallized for 5minutes with 5ml of hexane under reflux. The hot solution was filtered using a preheated filtering paper. Crystallization occurred, and then the product was collect by vacuum filteration. Th product was dried and the melting and mass were measured of the product, nitronaphthalene.
Result:
The total mass of the product obtained was 0.57g, and the melting point of the product was between 45-50°C.
The theoretical yield of the product is as follows:
Moles of naphthalene = mass of naphthalene / molecular weight of naphthalene
Moles of naphthalene = 0.50g x 1mol/128.17g = 0.00390mole of naphthalene
Because nitronaphthalene and naphthalene are in 1:1 mole ration,
Moles of nitronaphthalene = 0.00390mole
Theoretical weight of nitronaphthalene = 0.00390mole x 173.17g/mol (molecular weight of nitronaphthalene) = 0.676grams
Perencent yield = 0.57/0.676 x 100% = 84.3%

Discussion:
The result obtained from the experiment was 84.3% yield of the product, and the melting point ranged from 45-50°C. The melting point of the possible results are 61°C for 1-nitronaphthalene, and 79°C for 2-nitronaphthalene.
Even though there is discrepancy in the result obtained from the experiment, the product is more likely to be 1-nitonaphthalene because its melting point is closer to that of the product obtained. They also exhibit the same physical and chemical properties.
The discrepancy in the result obtained may have been from various sources during the experiment. During vacuum filtering, if not properly performed, some of the product might have been lost, therefore decreasing the amount of the product obtained. Another source might have been from the addition of naphthalene to the m1:1 mixture of nitric acid and sulfuric acid. The reaction probably did not fully react if the naphthalene was added at once without stirring. Again, this might have caused the discrepancy in result.
Conclusion:
The purpose of the experiment, which was to synthesize nitronaphthalene, was accomplished through the method implemente in this experiment because of the similarity between the obtained product and the predicted outcome.
This experiment can be improved by circumspectly following the procedure, carefully adding the finely divided naphthalene in little amounts in order to facilitate a good reaction between the nitronium ion and naphthalene.

Synthesis of Triphenylmethanol

Purpose of this experiment:
The purpose of this experiment was to synthesize triphenylmethanol. Triphenylmethanol is a white crystalline aromatic compound, which produces an intensely yellow color in a strong acidic solution due to formation of carbocation. Grignard reaction technique was used in this synthesis.



Method and procedures:
Into a 3-ml conical vial, 3.80mmol of benzophenone was dissolved in 2.0ml of anhydrous ethyl ether . When the reaction cooled, after the ether stops boiling, the septum cap was removed, and a dry stir bar was dropped into the reaction flask and the cap was replaced afterwards. The stirrer was started. A syringe was used to add about three drops of benzophenone solution at a rate sufficient to keep the reaction mixture boiling gently without external heating.
When the addition was complete, 0.5ml anhydrius ether was used to rinse the vial that contained benzophenone solution. A warm water bath was used to heat the reaction mixture for another ten minutes, while stirring with stir bar still in the solution.
The reaction was then allowed to cool to room temperature. A syringe was used to add 1.0ml of water drop by drop to the reaction flask, and the reaction is allowed to subside. While stirring, 2.0ml of 5% (1.4M) hydrochloric acid was added to the reaction. When all the reaction subsides, and all the white solid dissolved, stirring was stopped.
The reaction was transferred to a centrifuge tube using a small amount of solvent-grade ether, leaving the stirr bar and any undissolved magnesium behind. The solution was shaked gently to mix the layers thoroughly. Emulsion might formed in the solution, but a wooden applicator stick was used to break it up.
The aqueous layer was removed and discarded from the solution circumspectly. The remaining solution was washed with 3ml of 5% aqueous soldium bicarbonate, and then with 3ml of saturated aqueous soldium chloride. The ether solution was then dried with anhydrous magnesium sulfate. Then the ether was evaporated and a solid residue was left behind.
To the solid residue, 2.0ml of hexane was added. A flat-bladed microspatula was used to rub and grind the solid in the solvent for 2-3minutes. The product was collected by vacuum filteration. The product, crude phenylmethanol, was then recrystallized from a 2/1 mixture of hexane with absolute ethanol. Triphenylmethanol crystals was allowed to form (slowly) for about 30minutes.It was dried, weighed and it’s melting point was recorded.
Result:
The final weight of product obtained from the reaction was 0.51grams, and the melting point ranged from 132-140°C. The actual melting point of triphenylmethanol is 164°C.
The percent yield of the product obtained is as follows :
(0.00380mol benzophenone)/1 x (1mol triphenylmethanol)/(1mol benzophenone) = 0.00380mol triphenylmethanol
Theroetical yield : moles of triphenylmethanol x molecular weight of triphenylmethanol
0.00380mol x 260.33g/mol = 0.989grams.
Percent yield = (actual yield)/(theoretical yield) x (100 %)/1
Percent yield = (0.51mol triphenylmethanol)/(0.989mol triphenylmethanol) x (100 %)/1 = 51.57%

Discussion:
The yield obtained from the experiment was 0.51g, which was 51.57% of product expected. The melting point was 132-140°C, which differred from the actual melting point by about 30°C . However, the product obtained exhibited the same properties as the expected compound, triphenylmethanol.
There was a lot of discrepancy from the results of the experiment. Sources of the discrepancy was from a few mistakes in the procedures. While vacuum filterating, some of the product were spilled, and as a reult this decreased the final weight.
Since the method implemented in this experiment required the use of dried equipments in order to avoid contamination of reaction, an error might have resulted from improper use of clean dry equipments as expected.
Another source of error might have been from washing and drying the product. While performing this procedure, part of the organic part of the liquid might have been removed and discarded along with the aqueous layer.This also might have caused the inconsistency in results obtained
Conclusion:
Although a few sources of errors caused a reduced yield of product, the purpose of the experiment, which was to synthesize triphenylmethanol, was achieved through the method and procedure used in this experiment. One way this experiment could be improved is to ensure that the reaction is not been contaminated by water or spilled while heating, stirring or vacuum filterating.

Ring-Closing Metathesis using the Grubb's catalyst complex

Preparation of synthetic banana oil

Purpose of experiment
The purpose of the experiment was to synthesize banana oil known by several chemical names such as isopentyl acetate, isoamyl acetate, and ethanoate using isopentyl alcohol and acetic acid.


Method and procedure
A 20.0mmole of isopentyl alcohol was added to a 5-ml conical vial. About 40mmole of galactic acid was added to the solution, and carefully stirred as six drops of concentrated sulfuric acid was then added. Then the solution was heat under a gentle reflux with a water-cooled condenser for one hour. The solution is then monitored as it reflux and the heat applied to it was reduced from time to time as the reflux rose to about 2cm of the top of the condenser.
After heating, the reaction was cooled to nearly room temperature. Then it was transferred to a screw-cap centrifuge tube with the aid of 6ml of water. The reaction was washed with water, and then the aqueous layer was removed. The organic layer, which was left in the centrifuge tube, was then washed with two portion of about 3ml of 5% aqueous sodium bicarbonate in order to help eliminate the water content. Then the aqueous layer was removed after each washing.
The product, crude isopentyl acetate, was dried with a small amount of anhydrous sodium sulfate. The capped tube was shake vigorously, and let to stand for ten minutes. The sodium sulfates absorbed the water content and formed crystals at the bottom. The liquid was then transferred to a pre-weighed beaker, leaving the anhydrous sodium sulfate in the vial. The obtained product was then weighed and recorded.
Result
The final weight obtained of the product is 1.77g . Because the reactant, both have one to one mole ratio, the theoretical weight predicted from the reaction was
Therefore, the percentage yield of the product is as follows:


Discussion
The final the product obtained was , but the weight was about 68.0% of the theoretical yield which indicated that there might have been a few errors in the experiment. Because the procedure required circumspect handling while synthesizing , the sources of the errors that caused the discrepancy may have been from washing and drying the product. A few part of the organic layer might have been removed in the process of removing the aqueous layer, water or sodium bicarbonate. Another area would have been at the time of drying the product. Too much anhydrous sodium sulfate might have been added because the procedure was not specific as to what quantity should be added.

Conclusion
Isopentyl acetate, the product, was achieved through the method implemented in this experiment. With the use of isopentyl alcohol and acetic acid under the reaction method help to obtain the predicted product. One way this experiment could be developed is to specific precise amount of each compound need to be used in the reaction in order to obtain a better yield of the product.

Identification of a Conjugated Diene from Eucalyptus Oil

Purpose of Experiment
The purpose of this experiment was identify an unknown conjugated diene from Eucalyptus Oil. Diel-Alder adduct of the unknown conjugated is prepared in Eucalyptus oil , separated and identified using the melting point of the adduct. The reaction carried out in this experiment is as follows :


Methods and proceduce
Into a 5-ml conical vial, 1.00g of eucalptus oil was dissolved in 2.0ml of anhydrous ethyl ether. Then 0.360g of powdered maleic anhydride was added. The reaction was then heated using a cooled condenser for under a gentle reflux at about sixty degrees forty-five minutes.
After the reaction was over, the mixture was let to cool to room temperature. Crystals formed in the vial as the mixture cooled. When crystallization was almost complete, the vial was then cooled in an ice bath for a few minutes to allow more formation of cryatals.
The adduct was collected by vaccum filteration with 1.5ml of cold, low-boiling point ether used to wash the cystals off the vial. The adduct was then recystallized from dry methanol just immediately the methanol began to boil. The adduct was dried and measured. The melting point of the adduct was also recorded and used to deduce the identity of the eucalyptus oil diene.
Results
The weight of the product from the experiment was 0.47g, and the melting point obtained fell in the range of 107°C-112°C. Therefore, the conjugated diene was α-phellandrene, which has a melting point between 126°C-127°C, because it has a melting point which is closer to that of the unknown.
Below is the percent yield of the product obtained :
(1g oil 50% eucalyptus oil )/(136.2g/mol) = 0.00367mole of eucalyptus oil
Because euclyptus oil and the unknown compound are in 1:1 mole ratio, 0.00367mole of unknown compound (α-phellandrene) will be obtained.
Actual of α-phellandrene = 0.47grams
Theoretical of α-phellandrene = 0.00367moles x molecular weight of α-phellandrene = Mgrams
Percentage yield = (0.47g )/Mg x 100%=Y%
Discussion
The yield obtained from the experiment was 94.0% of the actual yield. Possible sources led to the error in the results. Some of the product might have been lost in the process of vacuum filteration. This lead to few crystals been obtained as product, and decreased the weight. The reaction took longer time to react because the stirring bar did not properly stirr the solution. It might have also lead to less yield of product.
The melting point obtained from the solution was between 107°C-112°C , and differed from the actual melting point by 15°C-19°C. The discrepancy in the result might have been from the equipment used. The solution was inserted into the melting point apparatus while it was warm (about 60°C). This might have led to the lower boiling point obtained as supposed to that of α-phellandrene, which is between 126°C-127°C.
The method of characterization used in this experiment supports purity of the product obtained. The product was much like the hypothesized diene. The physical features such as color, which was white, melting point, melting point, texture and so on are similar to that of α-phellandrene.
Conclusion
The purpose of the experiment was to identify an unknown diene using the Diels-Alder reaction. The objective and purpose of the experiment was obatined with the method that was implemented to purify the product. One way this experiment could be improved is to strictly follow the procedures of the experiment, and avoid taking the melting point with a melting point apparatus that is not at room temperature.

Learning to use the Fourier transform infrared spectroscopy (FT-IR)

Purpose of Experiment
The purpose of this experiment was identify an unknown compound using the Fourier transform infrared spectroscopy (FT-IR).
Methods and proceduce
Fourier transform infrared spectroscopy (FT-IR) was used to take the absorbance of the unknown solution. A graph of the results from the spectroscopy was plotted, and used to determine the organic substance. A correlation factor was also obtained from the FT-IR.
Results
The correlation factor obtained was 0.963274, which showed that the mostly likely compound is benzaldehyde from the FT-IR spectrometer and the graph obtained
structure of benzaldehyde
Discussion
The solution is benzaldehyde because the graph plotted showed a C=O strong spike at about 1700, and an indication of benzene ring at about 1600. On the graph, there was an O=H spike at about 3300. Also, the presence of two spikes between 2700 and 2900 indication the presence of an aldehyde as seen in the structure of benzaldehyde. These featured proved that the compound was truly benzaldehyde because the graph obtained showed a lot similarity to that of benzaldehyde.
Conclusion
The purpose of the experiment, which was to identify the unknown compound using the FT-IR spectroscopy, was achieved because the graph showed features which proved that the correlation molecule benzaldehyde was contained in the unknown.