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This can be a very complex question that you might be able to use some high end computational chemistry codes. But simply put you have van der waals forces, hydrogen bonding, and ionic bonding. You can think of it like coulumbic repulsion and attraction. hydrogen bonding has a slight negative charge on the oxygen and a slight positive charge on the hydrogen due to the covalent bond and the electron spending more time on the oxygen than the hydrogen, and the oxygens lone pair of electrons (this is inside a water molecule). Outside of the water molecule you dissolve salt nacl = na+, cl- . Since water has a slight negative charge on the oxygen, the oxygens in water molecules surround the Na+ atom pulling it into solution, and the hydrogen slight positive charge surrounds the chlorine anion. generally speaking polar groups like alcohols, ketones, amines,carboxylic acids are water soluble due to hydrogen bonding as long as there is not a large nonpolar R group. Van der waals forces control solubility on oily substances, those with large R groups like oil. since oil is a long chain of carbon it is very covalent with only very small positive and negative charges compared to water. That is why it is impossible to dissolve oil and water. Soap on the other hand has an oily R group bonded to a polar head. so one part of the molecule is polar (hydrogen bonding), and the other is non-polar and oily. A soap molecule can homogenize a solution of water and oil by being the bridge between the water molecule and the oil molecule. Hope this helps.
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What are the three factors to determine if solvation will occur?
The three factors that determine if solvation will occur are the polarity of the solute and solvent, the intermolecular forces between solute and solvent molecules, and the temperature at which the solvation process takes place.
How does the strength of intermolecular forces affect the vapor pressure of a substance?
The strength of intermolecular forces directly affects the vapor pressure of a substance. Stronger intermolecular forces result in lower vapor pressure, as it is harder for molecules to escape into the gas phase. Weaker intermolecular forces lead to higher vapor pressure, as molecules can more easily break free and enter the gas phase.
What is the relationship between intermolecular forces and vaporization points?
The greater the potential of a liquid's molecules to interact with each other through intermolecular forces, the lower the vapour pressure is going to be above the liquid (because molecules will preferentially stay liquid and interact with other molecules rather than fly away as a gas), and the lower the boiling point of the liquid. Therefore the relationship is an inverse one.
What can you say about the relative strength of the intermolecular forces in the two compounds?
The relative strength of intermolecular forces depends on the types of molecules involved. Compounds with hydrogen bonding, such as water, tend to have stronger intermolecular forces compared to those with only London dispersion forces, like diethyl ether. This results in higher boiling points for compounds with stronger intermolecular forces.
What intermolecular forces are present in cl2?
London forces are present in chlorine molecules.
What are the three factors to determine if solvation will occur?
The three factors that determine if solvation will occur are the polarity of the solute and solvent, the intermolecular forces between solute and solvent molecules, and the temperature at which the solvation process takes place.
What intermolecular force affects melting point the least?
Van der Waals forces
How does bonding effect the intermolecular forces?
Bonding affects intermolecular forces by influencing the strength of attractions between molecules. Covalent bonds within molecules contribute to intramolecular forces, while intermolecular forces, such as hydrogen bonding or van der Waals forces, occur between molecules. The type and strength of bonding within a molecule can impact the overall intermolecular forces affecting its physical properties.
How does the strength of intermolecular forces affect the vapor pressure of a substance?
The strength of intermolecular forces directly affects the vapor pressure of a substance. Stronger intermolecular forces result in lower vapor pressure, as it is harder for molecules to escape into the gas phase. Weaker intermolecular forces lead to higher vapor pressure, as molecules can more easily break free and enter the gas phase.
What is molecular solvation?
A molecular solid is a crystalline solid held together by intermolecular forces and composed of discrete molecules held together by van der Waals interactions. This type of solid can be contrasted with metallic solids and covalent solids, which are held together by stronger bonds.As one would expect based on the aforementioned information, molecular solids tend to be melted or sublimated at lower temperatures than other types of solids, because of their weak intermolecular bonding.
What is an intermolecular force that affects all polar molecules?
Dipole-dipole interactions are intermolecular forces that affect all polar molecules. These forces result from the attraction between the positive end of one polar molecule and the negative end of another polar molecule.
What interaction is not a type of intermolecular force?
Intramolecular forces are not intermolecular forces !
The process of an ion forming intermolecular attractions with solvent particles is called?
This process is called solvation. Basically, it is a chemical process in which there is intermolecular attraction or combining of solvent molecules with the molecules or ions of a solute.
What is the relationship between intermolecular forces and vaporization points?
The greater the potential of a liquid's molecules to interact with each other through intermolecular forces, the lower the vapour pressure is going to be above the liquid (because molecules will preferentially stay liquid and interact with other molecules rather than fly away as a gas), and the lower the boiling point of the liquid. Therefore the relationship is an inverse one.
What is the intermolecular ammonia and ammonia?
The intermolecular forces are hydrogen bonding.
How do thermal and intermolecular forces behave with each other?
When there is more thermal energy, then there are less intermolecular forces.
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.
