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Why Do Liquids Evaporate Intermolecular Rates

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INTRODUCTION The objective in this experiment is to better understand why liquids evaporate at different rates. In doing so, investigation of the factors that determine the intensity of the intermolecular forces by the rate of evaporation must be obtained in the following seven liquids: methanol, ethanol, propanol, butanol, water, pentane, and acetone. Intermolecular forces are forces that exist between molecules whereas intramolecular forces are the forces that hold atoms together within a molecule. Each of the seven liquids consists of intermolecular force energy; hydrogen bonding, dipole-dipole bonding, or london dispersion bonding. The type of intermolecular forces in a molecule is a result of bond polarity, which is determined by the electronegativity differences, and molecular shape, that is determined by an electron-dot structure. A hydrogen bond is a bond that consists of an attraction force between a hydrogen and an electronegative atom of …show more content…

After performing the investigation, it was concluded that each of the seven liquids will have different evaporation rates based upon strength and type of their intermolecular force. This is supported by (Figure 1.), in which Distilled Water contained the slowest rate of evaporation at 0.00686 degrees Celsius per second, therefore having the strongest intermolecular force because of its hydrogen bond. Pentane had the fastest rate of evaporation, as shown in (Figure 1.), at 0.349 degrees Celsius per second because it consisted of the weakest intermolecular force, a london dispersion bond. This evidence was not only supported through the experiment in which my group performed, but it was also supported by claims made by other groups who performed the same experiment. Overall, the molecular shape and the intermolecular bond type affects the rate of evaporation in liquids, causing each liquid to evaporate at its own specific

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In the “Drops of Water on a Penny” lab, I used the pipette to place 30 drops of regular water on the penny. As I was placing the drops of water on the penny, the water began to form a bubble on the penny, sticking together tightly so that it had risen above the penny. This occurred because of the high surface tension water has due to its hydrogen bonding. On the other penny with the soapy water, I was only able to place 24. Soap is a surfactant to water by interfering the hydrogen bonding and decreasing the surface tension so that the water does not stick to each as well as would have.

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Our hypothesis was partially correct, the property changing substances did have the weakest coherency with the lowest drop counts of 23(carbonated), and 14(soap), and pure water did have the strongest bond. What we also found was the the salt also dampened the liquid’s ability to hold onto a penny in large volumes, as all the different salts had a drop average of 24(28x2 & 16), five less than Tap water’s drop count (30). This led us to conclude that pure water has the strongest bond and that all foreign materials weaken the coherency of water. This evidence has led me to believe that similar substances are attracted and are more coherent towards themselves, in this case the water pieces get separated and generally less connected on a really small level due to the obstruction of foreign objects, this is why the different salts perform better than the huge air bubbles or the slippery properties of soap since the latter is more obstructive and the former dissolves with the water and blocks less. When studying a few other groups’ conclusions and data we did indeed find differences: some groups had differing data where a solution had better coherence than water itself which led to differing conclusions.

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Firstly, intermolecular forces and strengths of different chemical substances could be identified using valence shell electron pair repulsion shapes and prior knowledge of various kinds of intermolecular forces: London Dispersion, Dipole-Dipole, and Hydrogen bonding. Knowing this, Acetone was seen to possess London Dispersion and Dipole-Dipole forces. Propanol was seen to possess London Dispersion, Dip0le-Dipole forces, and Hydrogen Bonding. Acetic Acid was seen to possess Hydrogen Bonding and Dipole-Dipole forces. Overall,

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Introduction The intent of this experiment is to understand how hot and cold water interact with each other by combining clear hot water and black ice cold water. I hope to learn more about how hot and cold water interact with each other. As of now, I know that cold water is denser than hot water. Knowing this I formed my hypothesis.

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(2005) states that all molecules have different boiling points, this is due to the intermolecular forces between the atoms. Therefore, the more intense the intermolecular force is the higher the boiling point, and the lower intensity, the lower the boiling point. This paper aims to discusses the order of the boiling points of 3-methyl-1-butanol and 3-methylbutanal, 1-Hexanol and 1-Pentanol, examining the differences between them. (De Marco et al. 2014). Results Table 1.

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These intermolecular forces are London Dispersion Forces, dipole forces, hydrogen bondings, and ion-dipole forces. The weakest of these forces are London Dispersion Forces which are present in everything, especially our hearts and there are the strongest and most annoying ones, ion-dipole forces. Then we have kinetic molecular theory. One of the easiest things you could’ve possibly learned all year. The theory states firstly that there are no interactions between gas particles.

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