Alkyl Halides

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.

We had performed two different parts to the experiment within a two day process and created a second objective. Our second objective was to separate a mixture by specifically using the filtration method. Before starting the experiment it is important to wear the appropriate protective gear such as goggles, gloves, and a lab coat. This will prevent injury to self or others. For the first experiment, the following materials were necessary:

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

In this experiment, 0.31 g (2.87 mmol) of 2-methylphenol was suspended in a 10 mL Erlenmeyer flask along with 1 mL of water and a stir bar. The flask was clamped onto a hotplate/stirrer and turned on so that the stir bar would turn freely. Based on the amount of 2-methylphenol, 0.957 mL (0.00287 mmol) NaOH was calculated and collected in a syringe. The NaOH was then added to the 2-methylphenol solution and allowed to mix completely. In another 10 mL Erlenmeyer flask, 0.34 g (2.92 mmol) of sodium chloroacetate was calculated based on the amount of 2-methylphenol and placed into the flask along with 1 mL of water. The sodium chloroacetate solution was mixed until dissolved. The sodium chloroacetate solution was poured into the 2-methylphenol and NaOH solution after it was fully dissolved using a microscale funnel.

The pipette was used to transfer 8 mL of the 0.5 molarity solution into the graduated cylinder. Distilled water was added to raise the bottom of the meniscus to the 20.0 mL line and the solution was transferred into the beaker after it was rinsed with the solution. The pipette was used to take a small quantity of the solution and rinse and then fill a test tube with the solution. The amount of 0.2 molarity solution needed to create 20.0 mL of 0.1 molarity solution was calculated as 10.0 mL. The pipette was used to transfer 10.0 mL of 0.2 molarity solution into the graduated cylinder and distilled water added until the bottom of the meniscus reached the 20.0 mL line. The solution was transferred to the rinsed beaker and then a portion placed into a test tube that had been rinsed with the solution. The amount of 0.1 molarity solution required to create 20.0 mL of 0.05 molarity solution was calculated to be 10.0 mL. The pipette was used to transfer 10.0 mL of 0.2 molarity solution into the graduated cylinder and distilled water added until the bottom of the meniscus reached the 20.0 mL line. The solution was then placed into a beaker that had been rinsed with the solution and then into a rinsed test

Abstract: In this experiment the conversion of alcohols to alkyl halides are investigated through reflux and simple distillation. These are common procedures used to separate substances. After the reflux and distillation is complete 13C NMR and IR spectrum is used to identify the product or products for each reaction: 1a, 1b, and 2. Every individual in the group was assigned either 1a (1-propanol) or 1b (2-pentanol), and 2 (1,4-dimethyl-3-pentanol). The purpose of this experiment was to understand and become familiar with the reaction mechanisms and be able to observe and compare the product or products for each of the reactions using 13C NMR and IR.

The final product formed was characterized by using an infrared spectroscopy and chemical reaction. The IR spectrum was expected to show a carbon double bond (alkene) and many C-H sp³ hybridization bonds (alkyl) from the final product. This was compared to the authentic sample with its vibrational bonds. Once done identifying how close the sample is with the authentic sample, that would be the evidence to support the product’s

If the gasses are correctly synthesized then there will be a clear reaction with the introduction of the flame, O2, CO2, Air, limewater, and Bromthymol indicator.

Day one lab was centered on the conversion of the alcohol of 2-methyl-2-butanol to the alkyl halide of 2-chloro-2-methylbutane. Initially 70 milliliters (mL) of the concentrated hydrochloric acid was gathered in a 125 mL Erlenmeyer flask. The flask was then cooled for 10 minutes. A 50 mL Erlenmeyer flask was filled with 27 mL of 2-methyl-2-butanol. Both liquids were transferred into a separatory funnel and were swirled occasionally while being unstoppered for five minutes.

The samples were prepared in vials with one milliliter of methanol and one microliter of sample. Every sample is run under each condition three times with ten microliters being injected each time. The flow rate is set at one milliliter per minute and the temperature is maintained at 20oC. The log of retention times

The purpose of this experiment was to get an understanding as to how to properly prepare chemical buffers. Also part of this experiment was to gauge the effectiveness of the buffers by measuring their pH levels in various titration solutions, using a pH meter.

The IR spectrum can determine an O-H bond, C-H bond, and so forth. A compound on an IR spectrum can be determined by the frequency number of the peak and also the shape of it. Different compounds have different frequency ranges that can establish which compound it would be. The starting materials of the two reagents were quite different than the product IR spectrum. There was found to be an O-H bond in both reagents but not in the products.

Place one end of the rubber tube that’s connected to the gas tap which is placed under the neck of the bottle and fill the bottle up to the level you marked out with Methane from the gas tap. Then start to fill the bottle up with oxygen. The bottle should contain a 2:1 ratio mixture of oxygen and methane by the volume.

20cm3 of organic acid was measured in a measuring cylinder and transferred to the separating funnel. This was

In this experiment, Acid-Base titration will be used to determine the concentration of 10mL of an HCl solution by adding a known volume 0.1003 M NaOH solution using a buret. The chemical equation for this reaction is NaOH(aq)+HCl(aq) → NaCl(aq)+H2O(l). Because the moles of NaOH equals the moles of HCl, the number of moles of NaOH that are added to the solution in order to neutralize it will equal the moles of HCl in the solution. The number of moles of NaOH added to the solution will be used to determine the moles of HCl, which will then be used to determine the molarity of the HCl solution by dividing the number of moles of HCl by the volume of HCl, according to the formula: Moles/Volume=Molarity.