10 posts • Page 1 of 1
the stronger the intermolecular force, the higher the boiling point. for example, the boiling point of water is 100 C, while the boiling point of methane (CH4) is like -260 C. water molecules are polar, which means there will be dipole-dipole forces as well as LDF (LDF are present in all molecules i believe). water also has hydrogen-bonding, the strongest of intermolecular forces. methane is nonpolar, which means it only has LDF, which are the weakest of intermolecular forces
ValerieChavarin3E wrote:I'm confused between the melting point and the boiling point of a compound? Is this referring to the same thing?
There is a difference in which the boiling point is the temperature where a material goes from liquid to a gas and melting point is the temperature where a material changes from a solid to a liquid. When it comes to the stronger IMF, both the boiling point and melting point are higher than a compound with a weaker IMF.
705087773 wrote:What intermolecular forces cause higher boiling points? Lower boiling points? And what are some examples?
Something will have a higher boiling point when the IMFs are stronger, or there are more of them that makes them stronger. If something has two hydrogen bonds it will have a higher boiling point than if it had one. Also the type of IMF will have an effect on the boiling point. I think the order is something like this -- (strongest to weakest, according to textbook by Ep/(kJmol^-1): Ion-ion, hydrogen-bonds, ion-dipole, dipole-dipole, dipole induced dipole, induced dipole induced dipole.
Who is online
Users browsing this forum: Jaden Kwon 3I and 1 guest