Methylcyclohexane Lab Report

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Arenes 5. Introduction In this experiment, the relative rates of free-radical chain bromination where determined. Five arenes were used for this comparison along with two controls for each set. One set was kept in the dark while the other was put under light. This allowed for better observation of the reactions, as the light set would proceed fast to show which arenes reacted slowest, while the dark set would proceed slowly to show relative differences between the faster reacting arenes. The time it took for the arenes to react was recorded to determine the relative rates of the reactions. 6. Data and Results The five arenes used for this experiment were toluene, ethylbenzene, tert-butylbenzene, cyclohexane, and methylcyclohexane. All solutions were a dark orange right after the addition of bromine. Toluene had 1º benzylic and 2º aromatic hydrogens. Ethylbenzene had 2º benzylic, 1º aliphatic, and 2º aromatic hydrogens. tert-butylbenzene had 1º aliphatic and 2º aromatic hydrogens. Cyclohexane had 2º aliphatic hydrogens and methylcyclohexane had 1º, 2º, and 3º aliphatic hydrogens. In the set that was exposed to light, Ethylbenzene was the first to react. It turned from a dark orange color to a colorless liquid. Next, toluene turned colorless. After that, none of the other solutions turned colorless. However, …show more content…

More specifically, secondary benzylic hydrogens are more reactive than primary benzylic hydrogens, which are more reactive than tertiary aliphatic hydrogens and so on. This is due to the fact that secondary benzylic hydrogens are more accessible than primary benzylic hydrogens due to less steric hindrance. With less steric hindrance, the transition states formed from secondary benzylic hydrogens are more stable than transition states formed from primary benzylic hydrogens and therefore the resulting products are more

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