Intermolecular forces and melting/boiling points

[harperlacroix1a]

How does hydrogen bonding, LDF forces, and dipole dipole interactions affect the melting and boiling points of molecules? does it have to do with the electronegativity or strong/weakness of the force?

[Jonathan Pai 2I]

Dipole Dipole is molecules having a concentration of charge in a certain area due to polarity, which allows for greater attraction with another molecule that has its charges concentrated in certain areas. Hydrogen bonding is just super strong Dipole Dipole because of the Hydrogen with very electronegative elements, F O N. Same with London's cause attraction with nearby molecules but much weaker because London's are random. That level of attraction causes higher melting and boiling points to break the attractions.

[harperlacroix1a]

Dipole Dipole is molecules having a concentration of charge in a certain area due to polarity, which allows for greater attraction with another molecule that has its charges concentrated in certain areas. Hydrogen bonding is just super strong Dipole Dipole because of the Hydrogen with very electronegative elements, F O N. Same with London's cause attraction with nearby molecules but much weaker because London's are random. That level of attraction causes higher melting and boiling points to break the attractions.

so higher levels of attraction (hydrogen and dip dip) equal a higher melting and BP?

[Max Hayama 4K]

Yes, the higher attractions between molecules due to intermolecular forces, the higher the melting and boiling points will be!

[Kelsey Warren 1I]

Another easy way to think about this is that increasing the strength of intermolecular attractions is like a bunch of molecules holding on tighter and tighter to each other. If they're holding on really tightly, it becomes very difficult for one to escape the others, therefore it takes more energy to break one molecule off from the others/ the boiling and melting points are raised.