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I occasionally use peanut oil at home for cooking. However, it will often sit in the cupboard for months between uses. Using your knowledge from the presentation and what you found were the main components of peanut oil, propose the structures of the products that are the hallmarks of peanut oil rancidity.

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Wear safety glasses or goggles and suitable protective gloves while performing the experiments. Do not allow any of the chemicals used in this experiment t income in contact with your skin. If they do, immediately wash the affected areas with soap and water. Diethyl either is extremely volatile and flammable. Be certain there are no lames in your vicinity when using it for extraction and when removing it from the "Neutral Compound." Use caution in handingling wet glassware, because it can easily slip out of your grasp. When extracting a solution, vent the separatory funnel or vial often to avoid a buildup of pressure. Extract the clove oil from the distillate (saved on day 1) with two 20-mL portions of dichloromethane and combine the extracts. To do this...place the contents of the graduated cylinder and 20mL of dichloromethane in a closed separatory funnel. Cap the top with a glass stopper. Shake the contents to mix the layers then vent. Repeat the shaking/venting process 4-5 times. Allow the layers to separate. Drain the lower organic layer into a beaker. Add 20 mL of fresh dichloromethane to the separatory funnel then repeat the process. The two lower layers can be combined. In this extraction, the lower layer is the organic layer. The position of the layers depends on the densities of the two liquids involved. Because dichloromethane is halogenated, it has a density greater than 1, which makes it sink when combined with an aqueous solution having a density of about 1. You will need to be aware of the densities of liquids involved in later extractions to be able to track the layers. Extract the major component of clove oil from the dichloromethane solution obtained from the above extraction with two 15-mL portions of 1M sodium hydroxide (watch layers and think about what needs to be combined to get two layers in the separatory funnel). While monitoring with blue litmus paper, acidify the aqueous solution with 10 mL or more of 3M hydrochloric acid. Extract this aqueous solution with two 15-mL portions of dichloromethane and combine the organic extracts. Dry the dichloromethane solution from the previous paragraph with magnesium sulfate. Add small portions of magnesium sulfate to the dichloromethane solution. Magnesium sulfate clumps together as it picks up water from the solution. You have added enough when some of the magnesium sulfate is still freely moving in the dichloromethane solution. Adding too much will trap your product in the magnesium sulfate. Adding too little will leave large water impurities which we do not want for the IR at the end of lab. Carefully evaporate the dichloromethane using a pre-weighed flask on the rotavap (or by using a vacuum apparatus consisting of a pre-weighed, stoppered 50-mL filter flask heated on the lowest setting and a water trap cooled in an ice bath). When the boiling stops and the volume remains constant, weigh the product. Do not evaporate too much. Remember the product is volatile! Take your product and a clean and dry pipet to 346 to carry out the IR analysis, you may want to bring your graded pre-lab as well. You will be assisted in taking your IR, however, you will be expected to have a working knowledge next time. Pay attention! Mark the peaks that are given in your pre-lab list. Interpret your IR spectrum to prove the identity of the major component. You should be able to label enough peaks to prove beyond a shadow of a doubt what the main component is in your isolated clove oil. Draw a flowchart, similar lo the one on p. 163, to illustrate the extraction process (Day 2) for distillate to isolated major component. The start of the flowchart is given below. Based on the structures given on page 1, prepare a list of peaks to look for in the IR. Include the bond type and wavenumber. List two uses of an extraction in organic chemistry.

This experiment uses absolute ethanol and 95% ethanol. Describe the difference between the two and how each is used in this experiment.

slow fa st + H-Y H aromaticity destroyed H aromaticity restore A variety of electrophiles (Ey will react with benzene, and derivatives of benzene, to yield substitution products. Halogenation of benzene rings is an important reaction Br Pentab PBDE Br have important uses, e.g, pentabromodiphenyl ether CH PBDE; flame retardant) and Vancomycin (naturally because H, occurring antibiotic). However, halogens are not very CH, reactive toward benzene rings. and for this reason, they typically must be activated in some way to make them more electrophilic. For Cl, and Br this is accomplished through coordination to a Lewis acid, Fea, or FeBr, which polarizes the halogen and makes it more reactive. lodine (I) usually requires oxidation to I', or a species that acts like before it will react with a benzene ring. In this experiment, you will use EAS to iodinate salicylamide, a component of some analgesics. When salicylamide is monoiodinated, four different products may be formed. You will be asked to predict the major product of this reaction and explain how your prediction was made. You will then use IR spectroscopy to determine whether or not your prediction was correct NH2 NH2 Nal, NaOci NH2 EtOH NH2 possible products of monolodination of salicylamide possible products of monoiodination of sa UNDERSTANDING THE EXPERIMENT The "I" clectrophile that is required to iodinate a benzene ring is often generated by the of I, with various oxidizing agents (eg, hydrogen peroxide or a copper salt like CuClL.). In this experiment, " (possibly ICI or IOCH,CH) is generated by the oxidation of Nal with sodium hypochlorite, NaOCI, aka, common household bleach. Use of Nal is preferred to use of I, which is o iodinate a benzene ring is often generated by the oxidation Uise of Nal is preferred to uwe of I, which is Â·Fionne is an exception. It is too reactive and usually does not allow for isolation of monofluorinated products. Floorine i an exception I s too reactive and usuly does nor allou for isolation of 39

I need to fill out the table and show the reaction mechanism with all details please. Thank you

In a true science research lab, laboratory procedures do not present themselves in the "cookbook chemistry" fashion that most students have grown to expect. Chances are the chemist will use his/her previous knowledge and experience to develop their own procedure from scratch. If this procedure fails, the hardened chemist will not throw in the towel, but rather will make small adjustments and tweak the procedure until success is achieved. However, the smart chemist will always consult the chemistry literature to see if the procedure, or a similar procedure, has been previously performed and published. Chemists often follow procedures from primary literature sources such as Journal of the American Chemical Society or Journal of Organic Chemistry. These procedures are written with the understanding that the reader has a basic knowledge of laboratory techniques. Many of the specific details, such as the size and type of glassware utilized, along with common-knowledge, step-by-step procedures are omitted. In this experiment you are given a procedure to a Diels-Alder reaction as it may appear in a journal, and you need to be able to apply your chemistry laboratory experience to determine what glassware/equipment you will use. You will work individually on this experiment. Formation of the Diels-Alder Adduct To a solution of 0.3 g anthracene in 3 mL xylene was added an equimolar portion of maleic anhydride. This reaction mixture was refluxed for 30 minutes. The reaction was allowed to cool to room temperature and then chilled in an ice bath for 10 minutes. The observed crystals were collected, washed with cold xylene and dried. The mass, percentage yield, MP, and IR of these crystals was determined. Clearly draw the structure of your product in the space provided and then give the data for each pertinent peak in your IR spectrum. Attach your IR spectrum immediately after this page. Draw a complete reaction mechanism showing the formation of your major product from the starting materials. Make sure to show the flow of electrons by using curved arrows, as well as all charges and lone pairs where appropriate. Show all steps. Do not take shortcuts.

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