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How does molecule size affect melting point?
Intermolecular forces increase as molecular size increases, thus the bigger the molecular size, the bigger the molecular mass, the stronger the intermolecular forces, the more energy required to break the bonds between the molecule, thus a higher melting/boling point.
Why sih4 has lower boiling point than h2s?
SiH4 has a lower boiling point than H2S because SiH4 is a smaller molecule with weaker Van der Waals forces between its molecules compared to the larger H2S molecules, which have stronger Van der Waals forces. The strength of these intermolecular forces influences the boiling points of the substances, with stronger forces requiring more energy to overcome and boil.
Why ethane is a gas where as hexane is liquid at stp?
Ethane has very weak London dispersion forces because it doesn't have very many electrons. Hexane, however, has far more electrons, and therefore stronger dispersion forces, allowing more attraction between hexane molecules.
Do you expect the viscosity of glycerol to be larger or smaller than that of 1-propanol?
Glycerol is expected to have a larger viscosity than 1-propanol because glycerol is a larger molecule with more hydrogen bonding sites, leading to stronger intermolecular forces. These stronger interactions result in greater resistance to flow and higher viscosity compared to 1-propanol.
Which intermolecular force would affect the boiling point the least?
Van der Waals forces
Would you expect larger or smaller molecules to be components of a more viscous liquid?
Larger molecules tend to contribute to higher viscosity in liquids because they have more surface area to interact with neighboring molecules, resulting in stronger intermolecular forces that impede flow. Smaller molecules typically have lower viscosity as they facilitate easier movement between molecules.
Explain how the size of hydrocarobon molecules affects the strength of intermolecular forces?
The larger the hydrocarbon molecule, the greater the surface area available for van der Waals forces to act upon, leading to stronger intermolecular forces. Larger molecules have more electrons that can participate in these forces, increasing the overall strength of attraction between molecules. Smaller hydrocarbon molecules have less surface area and fewer electrons available for interaction, resulting in weaker intermolecular forces.
Do small molecules have high surface tension?
Generally larger molecules with stronger intermolecular forces have higher surface tension. This tendency can be seen if you look at the surface tensions of the alkanes. Water is a clear exeption to this pattern due to the very strong hydrogen bonds.
Why alcohol exist in a liquid state while smaller hydrocarbon tend to be gases?
Precisely because of the size of the molecules. Larger molecules have a greater tendency to stick together, because there are more places where they can interact, and thus, a greater total force.
How does molecule size affect melting point?
Intermolecular forces increase as molecular size increases, thus the bigger the molecular size, the bigger the molecular mass, the stronger the intermolecular forces, the more energy required to break the bonds between the molecule, thus a higher melting/boling point.
Does a hydrocarbon with large molecules have a higher boiling point that one with small molecules?
Yes, generally speaking, hydrocarbons with larger molecules have higher boiling points compared to those with smaller molecules. This is because larger molecules have stronger intermolecular forces, such as London dispersion forces, which require more energy to overcome in order to change from a liquid to a gas state.
Why sih4 has lower boiling point than h2s?
SiH4 has a lower boiling point than H2S because SiH4 is a smaller molecule with weaker Van der Waals forces between its molecules compared to the larger H2S molecules, which have stronger Van der Waals forces. The strength of these intermolecular forces influences the boiling points of the substances, with stronger forces requiring more energy to overcome and boil.
Do small hydrocarbons have with only a few carbon atoms have low or high boiling points?
Small hydrocarbons with only a few carbon atoms have low boiling points. This is because smaller molecules have weaker intermolecular forces, such as van der Waals forces, which require less energy to overcome compared to larger molecules with stronger intermolecular forces.
Would a large body of water molecules have a stronger attraction to fewer molecules?
A large body of water molecules would typically not have a stronger attraction to fewer molecules. It would however attempt to pull smaller molecules toward it.
Why do larger surface area evaporate faster?
Larger surface areas have more molecules exposed to the surrounding environment, increasing the chances of molecules with sufficient energy to overcome the intermolecular forces and evaporate. This leads to a higher rate of evaporation compared to objects with smaller surface areas, where fewer molecules are available to evaporate.
Why does methanol have a lower boiling point than ethanol?
Methanol and ethanol differ only by one carbon and 2 hydrogens. Both have the hydroxyl group and, thus, have hydrogen bonding and dipole-dipole interactions. What makes them different are their London forces (London forces are directly proportional to the number of electrons in a molecule and molecular size). Since methanol is smaller than ethanol, there is a smaller intermolecular London force. Less force holing the molecules together means they're easier to be pulled apart, which implies a lower boiling point.
Compared to the ingested food molecules the end product molecules of digestion are usually?
Smaller and simpler molecules that can be absorbed by the body, such as glucose, amino acids, and fatty acids.
