Analysis:2. Among the alcohols tested, 1-butanol was found to contain the strongest intermolecular attractive forces (IMFs), while methanol contained the weakest. Through experimentation it was discovered that methanol induced the highest ?T of all the alcohols tested and that, conversely, 1-butanol induced the lowest ?T. The atomic structure of all four alcohols is very similar, as starting from 1-butanol you lose a CH2 group as you go from 1-butanol to 1-propanol to ethanol and then back to methanol. Each structure is quite linear and contains one H-bond to oxygen, so the real change is found in the loss of the CH2 group, this lowers the molecular mass of the liquid, thus decreasing the London forces as you move from 1-butanol to 1- Propanol and ethanol, to Methanol. Since the IMFs within 1-Butanol are stronger than the other three alcohols, it has a higher ?Hvap. During the experiment, all 4 alcohols tested (actually all 7 liquids tested) were exposed to room temperature air in the laboratory. Thus, gas particles floating in the laboratory air were able to impart kinetic energy to the sampled liquids, at a constant rate under fairly controlled and consistent conditions. This resulted in the absorption of the kinetic energy coming from the air surrounding the temperature probe into the liquid, causing a drop in the temperature of the air itself, which was appropriately reported by the probe and used to calculate the ?T of the liquid. In the case of 1-butanol the ?T was very small, indeed lower than that of any other liquid tested. Furthermore, it took a long time in comparison to reach the minimum, as opposed to a liquid with a high ?T like methanol, which was quite fast. We therefore find an inverse relationship between the ?T and the strength of the IMF...... middle of paper...... any liquid. With molecular weight, as the weight increased, so did the IMF strength, especially the London forces. Then, as IMF increased, the propensity of the liquid to evaporate decreased, leading to both a lower ?T and a slower time to reach ?T overall. Conclusion: In conclusion it was discovered that there is an inverse relationship between the strength of the intermolecular forces that hold the molecules together and the speed with which these molecules evaporate. As the bonds become stronger, more energy is required to separate them and allow the molecules to escape into the vapor phase. This was the goal of the laboratory and it was achieved. Significant improvements could only be made with a significant investment in time and cost and are not necessary since the outlined laboratory procedure was more than sufficient to derive the necessary relationship through comparison.