Epoxides Lab Report

In this lab, the oxidation of a secondary alcohol was performed and analyzed. An environmentally friendly reagent, sodium hypochlorite, was used to oxidize the alcohol, and an IR spectrum was obtained in order to identify the starting compound and final product. The starting compound could have been one of four alcohols, cyclopentanol, cyclohexanol, 3-heptanol, or 2-heptanol. Since these were the only four initial compounds, the ketone obtained at the end of the experiment could only be one of four products, cyclopentanone, cyclohexanone, 3-heptanone, or 2-heptanone. In order to retrieve one of these ketones, first 1.75g of unknown D was obtained.

[22]. Before solution application, the HPTLC plates were sprayed with 10% (w/v) disodium ethylene diaminetetraacetic acid (Na2EDTA) solution in which the pH had been adjusted to 4 using glacial acetic acid. This Na2EDTA solution helps to avoid binding of the tetracyclines with trace metals in the adsorbents used [23]. Since OTC and TC have similar chemical and physicochemical properties they form chelate complexes with metal ions and bind with proteins and silanol groups in the stationary phase. These undesirable properties have been controlled by the use of EDTA for plate treatment [23].

Tertiary alkyl halides tend to give a mixture with both inverted and retained configurations at reaction centers. This is because this reaction proceeds through a stable carbocation intermediate and the carbon at the reaction center goes to sp2 hybridized state (planar geometry). The incoming nucleophile can attack from both sides of the plane and can give two products with retained and inverted configuration. If there is a partial interaction with the leaving group (nucleofuge) with carbocation there will be more product with inverted configuration and if there is no interaction with leaving group racemic mixture can be obtained. The rate of the reaction depends on the formation of a carbocation (which is the slow step) and there is one molecule

1.3 Organosilane [66] Monomeric silicon chemicals are known as silanes and any chemical that contains at least one carbon-silicon bond is known as an organosilane. Generally, organosilanes contain three key elements beside silicon; X represents for an organic moiety that is non-hydrolysable which can be either reactive or non-reactive depending on its type. OR\ is a hydrolysable group such as alkoxy or an acetoxy is known to be unstable when present with hydroxyl groups. Finally, R is a space moiety, which can be aryl or alkyl chain.

Abstract In this laboratory, methanol is reacted with a tertiary alkyl chloride to make ether. The triphenylmethyl is isolated from the triphenylmethyl chloride. Methanol is then added and the class does the recrystallization . The methanol acts as a solvent for the reaction as a nucleophile.

Molecules tend to tie with different particles to get solidness. Much the same as in Ionic holding, Covalent holding shapes mixes which are brought into utilization once a day. This can be found as gasses, fluids, or solids and are surrounding us. Not at all like in ionic, they are not dissolvable in water. The iotas of materials with covalent bonds are bound firmly to each other in stable atoms, yet, they are for the most part not extremely pulled in to different particles in or around the material.

DESCRIPTION  A simple reaction, followed by isolation of the desired product from the solution, will illustrate a typical application of extraction.  Some organic acids are liquid and are soluble in water as indicated. The sodium salts of these acids are ionic compounds that are also very soluble in water. If an aqueous solution of one such salt is acidified with a strong mineral acid, the much weaker organic acid is produced. 

2.3.2.2 Chemical Interesterification Chemical interesterification is the process to redistribute the component of fatty acid and glycerol ions to form new gylcerolester with the presence of sodium methoxide as a catalyst. Chemical interesterification is also known as directed interesterification since this reaction is directed to produce a particular type of glyceride (O’Brien, 2009). This process is conducted at mild temperature with a range between 20°C to 100°C. O’Brien (2009) states that only catalyst that is active at low temperature is effective. Besides, he also states that the rate of random rearrangement is crucial since the trisaturated glycerides can precipitate as fast as they are produced in the liquid phase.

The prior state of charge is restored when the leaving group (LG) departs with an electron pair. The principal product in this case is R-Nuc. In such reactions, the nucleophile is usually electrically neutral or negatively charged, whereas the substrate is typically neutral or positively charged. An example of Nucleophilic substitution is the hydrolysis of an alkyl bromide, R-Br, under basic conditions, where the attacking nucleophile is the base OH− and the leaving group is Br−. R-Br + OH− → R-OH + Br− Nucleophilic substitution reactions are commonplace in organic chemistry, and they can be broadly categorized as taking place at a carbon of a saturated aliphatic compound carbon or (less often) at an aromatic or other

Salmonella typhimurium account 1,2-propanediol, de-oxy sugars. Identify an equimolar extent of 1, 2-propanediol when (methyl pentose), rhamnose or fucose was used as substrate. However, still 1, 2-propanediol is not further metabolized by anaerobic cultures, and will disappear gradually from the middle in s. typhimurium cultures maintained in similar surroundings. This meticulous inquiry discovered that when grown on rhamnose, s. typhimurium excreted 1.0 M 1, 2-propanediol/m of sugars in the middle. Now, after collapse of the sugar, the diol concentration has arrived to its maximum and step by step it departed when the culture was kept in the same conditions for more time.

They are only soluble in polar solvents, like water. This is due to the ions inside the lattice becoming surrounded by water molecules which easily bond to the ions. This means there is a decrease in the attraction that the ions have, resulting in the ionic structure breaking down. When in a solid state, they are unable to conduct electricity.