propanol is one of those inorganic molecules that can have both a polar and non-polar end. The polar end (OH-) gives it the ability to have dipole-dipole bonding with other polar molecules while the CH3 end gives it the ability to bond with non-polar molecules using London dispersion forces.
van der Waals force, dipole induced-dipole attraction.
HDPE - High-density polyethylene: has little branching and thus stronger intermolecular forces and tensile strength.
LDPE - Low density polyethylene: has more branching than HDPE, so its intermolecular forces are weaker.
Because propane is non-polar, the intermolecular force would be: London Dispersion Forces
The intermolecular forces of propanol are hydrogen bonding, dipole-dipole forces and London dispersion forces.
Propane is C3H8. This molecule is hydrophobic and nonpolar, so the intermolecular forces between the molecules of propane would be van der Waals forces.
Hydrogen fluoride, with the chemical formula HF, is a colorless gas that is the principal source of fluorine. The type of intermolecular forces that exist in HF are London forces, dipole-dipole.
ionic
London Dispersion Forces
Intermolecular forces are of the type(1) hydrogen bonds (2) dipole-dipole attractions (3) dispersion forces (van der Waals, etc.)
weak intermolecular forces because dry ice with sublime
In almost all hydrocarbons, the only type of intermolecular forces that exists is the London forces (Van der Waals forces).
intermolecular forces
Intramolecular forces are not intermolecular forces !
Hydrogen fluoride, with the chemical formula HF, is a colorless gas that is the principal source of fluorine. The type of intermolecular forces that exist in HF are London forces, dipole-dipole.
You think probable to intermolecular forces.
Dipole
ionic
yes it is - gentle warming will change it to vapor though.
London Dispersion Forces
The intermolecular forces are ionic for CoCl2 cobalt chloride. For COCl2 Phosgene they are polar covalent.
These are intermolecular forces.
London Dispersion