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Free-Radical Chain Reaction Lab Report

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In free-radical chain reactions, a diatomic halogen molecule is reacted with the most reactive hydrogen atom on a carbon chain to form a halide and a haloalkane. In the case of bromination, diatomic bromine is reacted with a carbon chain to form hydrobromic acid and an alkyl halide. The first step in the reaction is initiation, or the formation of bromine radicals. These radicals can then react with hydrogens along the carbon chain through propagation to form hydrobromic acid and a carbon radical. Additionally, the carbon radicals can react with other bromine radicals to form carbon-bromine bonds. The reaction is stopped through the termination step where two radicals react with each other to diminish the concentrations of free reacting radicals. Bromine was used because it is much more selective in reaction than other halogens. For example, diatomic chlorine …show more content…

The rates of reaction are determined by the types of hydrogens present in each molecule. Aromatic hydrogens are hydrogen atoms on a benzene or ring structure. Aliphatic hydrogens are hydrogen atoms attached to a sp3 hybridized carbon that are attached to another sp3 hybridized carbon. Benzylic hydrogens are hydrogen atoms attached to a sp3 hybridized carbon that are attached to an aromatic ring structure. Compounds with benzylic hydrogens react faster that compounds with aliphatic or aromatic hydrogens. Structures with aliphatic hydrogens react slightly faster than those with only aromatic hydrogens. Additionally, secondary benzylic structures react faster than primary benzylic structures. For aliphatic hydrogen structures, tertiary hydrogens are the most reactive while primary hydrogens are the least reactive. Secondary aliphatic hydrogens react faster than primary aliphatic hydrogens, but slower than tertiary aliphatic

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The relative reactivity was found by setting the reactivity per hydrogen of 1,4-dichlorobutane to 1.0. As shown in Figure 4, 1,3 dichlorobutane had the highest yield of 48% and the highest relative reactivity of 3. This is because it replaced the C-H bond that was furthest from the chloro substituent and formed a stable secondary intermediate. Next, 1,4-dichlorobutane had the second highest yield of 24%, but the third lowest reactivity of 1.0. Even though it was the furthest C-H bond from the chloro substituent, it formed a less stable primary radical intermediate.

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As the size of the radii atomic increased the further away the electron got from the nucleus. This also reduces the electrostatics attraction between the electron and the nucleus which means the electrons becomes more reactive. Therefore the reactions while going doing the list of group 1 elements increase.

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During the Bromine test, the bromine transformed from brown to clear indicating the presence of an alkene. Also during the permanganate test, the compound changed from purple to brown. This also indicates the presence of an alkene, which indicates the E2 reaction did occur. These two positive test allowed for a GC spectrum to be obtained, if the IR confirmed there was no water in the final compound. The IR spectrum obtained, did contain a peak at 3388 cm-1, indicating an alcohol group present, but the degree of the peak was so small that a GC spectrum could be obtained.

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The reaction was allowed to proceed for 30 minutes and was subsequently quenched using hydrochloric acid. The addition of hydrochloric acid permitted the protonation of the reduced ketone (O-) to form the two diastereomer

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Introduction SN2 stands for substitution, nucleophilic, bimolecular and occurs in one step where the nucleophile and electrophile react: the nucleophile attacks the electrophile 180° from the leaving group.3 The leaving group is nothing more than a group that leaves the electrophile attacked by the nucleophile. In this experiment the nucleophile is bromide, the electrophile is 1-butanol, and the leaving group is hydroxide. However, bromide must first be obtained from hydrobromic acid which gets bromide from a reaction between sodium bromide and sulfuric acid. The hydrogen and bromide in hydrobromic acid reacts with the oxygen in 1-butanol and the carbon attached to oxygen respectively to form 1-bromobutane. The overall reaction of this procedure

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The Mel-Temp was then used which determined the melting temperature of the precipitate and it also confirmed the isomerization of dimethyl maleate into dimethyl fumarate which are diastereomers. At the end of the isomerization reaction, cyclohexane was used to get rid of the residual bromine before disposing of the

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This means that all of the elements in the same group have a main aspect in common, except for a few exceptions. These elements react with the same specific compounds. This was used to identify the order of the groups from left to right and to determine which elements go under which group. Some research was conducted to identify all the names of the groups ranging from element number one to element number 20. Once all group names were recorded, it was researched which groups react with which compounds that are given on the element cards.

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In this process, the chemical structure that must be preserved for CO2 to be converted to methanol is the C =O bond of Carbon dioxide. During the selective hydrogenation process, the C=O bond of Carbon dioxide is broken, and a hydrogen atom is added to produce the methanol molecule. Therefore, preserving the C

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Based on resonance, donating groups tend to shift o-hydrogens upfield, while withdrawing groups do the opposite. Curphy-Morrison additivity constants were used to predict aryl hydrogen shifts of A and B, and the prediction for A matched the spectrum far more than B, supporting A as the major product. As a qualitative example, it is predicted that A would have Hf shifted downfield due to the o-hydroxyl group, while the same hydrogen in B would not be shifted far from that of a phenyl hydrogen due the o-hydroxyl and o-iodine effects cancelling; the shift for Hf at 6.95 ppm supports

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Catalytic hydrogenation is a heterogeneous reaction due to the different phases such as solid, liquid, and gas phases.

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Lithium- gives off hydrogen gas Sodium- sound is louder hydrogen gas is produced Potassium-lit on fire Rubidium -blew up Cesium- blew up and glass broke Francium- Will explode Stated and explained why reactivity increases or decreases down a group in terms of shielding because it’s easier to give off because of the higher atomic number. Explained why alkali metals are more reactive than the alkaline earth metals because there easier to give away (give and take). Experiment: several chemical reactions were examined. From the observations a list of 6 elements in their order of activity beginning with the most active element down to the least active element were constructed.

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2) Free Radicals: an injury by free radicals such as the reactive oxygen species, also known as oxidative stress (Huether & McCance, 2012, p. 66). This is an uncharged atom that makes the molecule unstable. In order to become stabilized, it needs to either get an electron or give up its electron. By doing this, it forms chemical bonds with protein,

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A free radical is an atom or molecule with at least one unpaired electron, making it especially reactive to other atoms or groups of atoms. A : B A · + B · If free radicals react with certain chemicals in the body, they may interfere with the ability of cells to function normally. One of the most important radicals is molecular oxygen.

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The reaction adds two electrons to the contaminating molecule, thus reducing the contaminant. In order for the reductive dehalogenation to proceed, a substance other than the halogenated contaminant must be present to serve as an electron donor. Possible electron donors are hydrogen and organic compounds of low molecular weight (lactate, acetate, methanol or

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