In experiment one, acetone evaporated the most quickly because its molecules have the lowest force of attraction. Ethanol evaporated the slowest because it has the highest force of attraction. This shows that if molecules have a strong force of attraction, it takes longer for them to separate from each other into a gaseous form. Hexane didn’t evaporate most quickly due to the long length of its carbon chains, which holds the molecules together with london dispersion bonds more strongly than for hydrocarbons with shorter carbon chains.
Ethanol curved by far the most when a charged rod was moved near it in experiment two. When the cloth was rubbed on the glass rod, it transferred electrons onto the rod, creating static electricity. The substances …show more content…
Non polar chemicals, such as hexane, were the least viscous because their molecules aren't held strongly together by dipole-dipole bonds. Polar molecules such as water and ethanol are more viscous because they are held more strongly together by dipole-dipole--and in these molecules case--hydrogen bonds. Liquids that are hydrocarbons can also be more viscous because they have longer carbon chains. For example, hexane has much less carbons than mineral oil and is therefor much less viscous. It seems that intermolecular bonds in hydrocarbons become stronger as the number of carbons in the chain increases. Additionally, C-H series seem to have weaker bonds than C-OH series. This is because C-H series only have one intermolecular force: london dispersion, which is very weak. C-OH series are have london dispersion forces, also have the much stronger forces of dipole-dipole bonds and hydrogen bonds. Hydrogen bonds are the strongest intermolecular …show more content…
Mineral oil has eighteen carbons, making it very viscous. Hexane and pentane are both not very viscous because they only have four and five carbons. Paraffin wax is a solid, and has over twenty hydrocarbons, while methane and butane are gases and have less than five carbons. This shows that at room temperature, hydrocarbons with less than five carbons are gases, hydrocarbons with five to eighteen carbons are liquid, and hydrocarbons with over twenty are solid.
Error occurred in experiment one because my lab partner and I were both in charge of reading and recording the temperature of two thermometers at the same time. This means that we checked one before the other every single time we took measurements. The reading of our second thermometer was especially delayed if the first temperature was difficult to determine. This would have made the first temperatures we read, water and hexane delayed by a few seconds. In the second and third experiments, the data was collected solely upon observations. Often the results appeared so close that it was difficult to distinguish which bent the most and which was
Ethanol curved by far the most when a charged rod was moved near it in experiment two. When the cloth was rubbed on the glass rod, it transferred electrons onto the rod, creating static electricity. The substances …show more content…
Non polar chemicals, such as hexane, were the least viscous because their molecules aren't held strongly together by dipole-dipole bonds. Polar molecules such as water and ethanol are more viscous because they are held more strongly together by dipole-dipole--and in these molecules case--hydrogen bonds. Liquids that are hydrocarbons can also be more viscous because they have longer carbon chains. For example, hexane has much less carbons than mineral oil and is therefor much less viscous. It seems that intermolecular bonds in hydrocarbons become stronger as the number of carbons in the chain increases. Additionally, C-H series seem to have weaker bonds than C-OH series. This is because C-H series only have one intermolecular force: london dispersion, which is very weak. C-OH series are have london dispersion forces, also have the much stronger forces of dipole-dipole bonds and hydrogen bonds. Hydrogen bonds are the strongest intermolecular …show more content…
Mineral oil has eighteen carbons, making it very viscous. Hexane and pentane are both not very viscous because they only have four and five carbons. Paraffin wax is a solid, and has over twenty hydrocarbons, while methane and butane are gases and have less than five carbons. This shows that at room temperature, hydrocarbons with less than five carbons are gases, hydrocarbons with five to eighteen carbons are liquid, and hydrocarbons with over twenty are solid.
Error occurred in experiment one because my lab partner and I were both in charge of reading and recording the temperature of two thermometers at the same time. This means that we checked one before the other every single time we took measurements. The reading of our second thermometer was especially delayed if the first temperature was difficult to determine. This would have made the first temperatures we read, water and hexane delayed by a few seconds. In the second and third experiments, the data was collected solely upon observations. Often the results appeared so close that it was difficult to distinguish which bent the most and which was