Methylcyclohexane Lab Report

The objective of this laboratory experiment is to study both SN1 and SN2 reactions. The first part of the lab focuses on synthesizing 1-bromobutane from 1-butanol by using an SN2 mechanism. The obtained product will then be analyzed using infrared spectroscopy and refractive index. The second part of the lab concentrates on how different factors influence the rate of SN1 reactions. The factors that will be examined are the leaving group, Br – versus Cl-; the structure of the alkyl group, 3◦ versus 2◦; and the polarity of the solvent, 40 percent 2-propanol versus 60 percent 2-propanol.

The purpose of this experiment was to practice the functional group transformation procedure. The process of the experiment included the dehydration of 2-methylcyclohexanol in the presence of phosphoric acid and heat. The products that were formed from the reaction were 1-methylcyclohexene and 3-methylcyclohexene. The mass of the final product solution was 0.502g with a percent yield of 18.7% and a boiling point range of 84.5-98.5oC.

In radical halogenations lab 1-chlorobutane and 5% sodium hypochlorite solution was mixed in a vial and put through tests to give a product that can then be analyzed using gas chromatography. This experiment was performed to show how a radical hydrogenation reaction works with alkanes. Four isomers were attained and then relative reactivity rate was calculated. 1,1-dichlorobutane had 2.5% per Hydrogen; 1,2-dichlorobutane had 10%; 1,3-dichlorobutane had 23%; and 1,4-dichlorobutane had 9.34% per Hydrogen.

The purpose of this experiment was to determine the relative reactivities of different types of hydrogen atoms toward bromine atoms. Although the tested compounds were all arenes, their reactivities differ as they contain different types of hydrogens. The hydrogens could be of three different types and could also differ in being bonded to carbons that are attached to a different number of other carbons. The three different types of hydrogens that could be found were aromatic, aliphatic, and benzylic. The first category is aromatic hydrogens, which are attached to sp2 carbons or are those directly bonded to an aromatic ring. Aromatic hydrogens are the least reactive of the hydrogens in this experiment. The second type of hydrogen being investigated is aliphatic hydrogens, which are found bonded to an SP3 hybridized carbon which are bonded to another SP3 hybridized carbon. Aliphatic hydrogens can also be broken down into further categories according to their number of substituents into primary (less reactive), secondary (more reactive), and tertiary (most reactive). The third type of hydrogens are benzylic hydrogens, which are bonded to a SP3 hybridized carbon that is bonded to a benzene ring. Benzylic hydrogens are also broken into primary and secondary categories according to their substituents, and are all more reactive than aliphatic and aromatic hydrogens.

Since the purpose of our experiment was to synthesize Tetraphenylcyclopentadienone from benzyl,dibenzyl ketone,absolute ethanol ,and potassium hydroxyde, we finally got our product at the end which mean we were able to accomplish our purpose. that product is very dangerous for human and very toxics for aquatic organisms.

Chlorination is not very selective since the different hydrogens are so close in their relative rate1. Chlorination will form a mixture of every possible product, whereas bromination will typically form one product. In this experiment, the goal was to determine the effect of chloro substitution on the reactivity and selectivity of hydrogen. To determine this, the radical chlorination of 1-chlorobutane was carried out. Chlorine has poor selectivity, so it can react with any hydrogen attached to the carbon in butane.

As for the reaction itself, the formation of the radical follows the 3 step process of Initiation, Propagation, and Termination. The short run down of this is that the initiation step makes the radical via hydrogen abstraction, the propagation step forms products, and the termination ends the reaction and gives stable products. The rate determining step in this reaction is in the hydrogen abstraction. During hydrogen

In order to complete a certain experiment 20g of cyclohexanol was needed to proceed. However, the stock of cyclohexanol in the storeroom was depleted and the compound was on backorder. In order to proceed with the research as quickly as possible, it was decided that the needed cyclohexanol was to be synthesized in the lab.

During the halogenation reactions of 1-butanol, 2-butanol, and 2-methyl-2-propanol, there is a formation of water from the OH atom of the alcohol, and the H atom from the HCl solution. The OH bond of the alcohol is then substituted with the Cl atom. Therefore all of the degrees of alcohol undergo halogenation reactions, and form alkyl halides as products. This is because the functional group of alkyl halides is a carbon-halogen bond. A common halogen is chlorine, as used in this experiment.

The experimental value of the maximum wavelength for 1-1’-diethyl-2-2’-cyanine iodide was 525nm and the calculated value when p=0nm is 141nm, which shows that 0nm is too small. To get a penetration distance for the dye Equation 4 was used and the value was 0.2439nm. This value of p is much larger than the original guess made for the penetration distance is the pre-lab. Using the calculated penetration distance from this dye, the wavelength of pinacyanol chloride is calculated to be 654nm. This value is about 50nm off the experimental value, which at this scale is significance. A penetration distance was found for pinacyanol chloride, using its experimental maximum wavelength, giving a value of 0.207nm. Using this value to solve for the

For this experiment, the major goal was to see the rate of Bromination of six different hydrocarbons in order to find the relative order of each reaction. An excess of each hydrocarbon is combined with molecular bromine and then the elapsed time of color disappearance is collected both in and out of light. The results are then compared for each hydrocarbon in an attempt to figure out the fastest and slowest reactions based on the hydrogen types.

In this experiment, an electrophilic aromatic substitution reaction was performed through the addition of a nitro group to bromobenzene. The experiment uses the nitronium ion, NO2+, which acts as an electrophile to replace a hydrogen atom in the aromatic system of bromobenzene. The bromine substituent on the benzene introduces the possibility of isomers from the reaction with the nitronium ion: NO2+ can be positioned in the ortho position (making 1-bromo-2-nitrobenzene), the meta position (making 1-bromo-3-nitrobenzene), or the para position (making 1-bromo-4-nitrobenzene). There is also a chance that poly-nitration can occur to produce dinitrobenzene. Since nitro groups are deactivators, it requires high temperatures to add another nitro group to the benzene ring.

If air is admitted to the sample, that spectrum is replaced by one consisting of a quintet of quintets, which we assign, on the basis of the further experiments described below, to the radical anion (1). Two reasonable routes by which the reaction might occur are illustrated in equation A, where the two rings become linked either by the condensation of cyclo- pentadienyl-lithium with cyclopentadienone resulting from the autoxidation of cyclopentadienyl-lithium, or by the coupling of two cyclopentadienyl radicals. The same spectrum is obtained by the autoxidation of the dilithium salt of dihydrofulvalene (2) prepared by Doering and Matzner's method (equation B) ; the pink colour of the suspension of the dianion (2) in tetrahydrofuran changes first to deep green then to violet when the e.s.r. spectrum of the radical anion becomes apparent. Further autoxidation gives the characteristic orange colour of fulvalene? and reaction of this with a sodium mirror and subsequent photolysis restores the colour and the e.s.r. spectrum of the radical anion. Similarly, electrolytic reduction of the fulvalene shows the same 25- line spectrum(equation

From the observations table, chloride is prominently the most reactive out of the three elements due to the facts a colour change occurred when the aqueous solution of chlorine was mixed with bromine and iodine, exhibiting a more reactive element displacing a less reactive element. In the aqueous solution of bromine, a colour change occurred only when mixed with iodine, justifying the fact that bromine is less reactive than chlorine though more reactive than iodine. Therefore, iodine is the least reactive due to the inability of displacing chlorine or bromine when mixed together, no colour change was evident in any of the

Background information: Four categories of contaminants have been identified by environmental scientists and have said to be existent in municipal water supplies. These pathogens can cause disease that can lead to cancer and acute poisoning. Public health officials have taken note of the issue and are now attempting to take action to counter the hazard.