polar molecules
Hydrogen bonds can be considered as the strongest intermolecular attraction forces.
Hydrogen bonds are much stronger than other intermolecular forces.
Intermolecular forces are of the type(1) hydrogen bonds (2) dipole-dipole attractions (3) dispersion forces (van der Waals, etc.)
Intermolecular forces are strongest in the solid phase. This is because the atoms/molecules are at the closet possible distance without repulsion occurring; the van der Waals contact distance.
Water molecules can make hydrogen bonds with other water molecules. Hydrogen bonds are the strongest type of intermolecular forces. This explains the high surface tension of water.
hydrogen bonding
Hydrogen bonds can be considered as the strongest intermolecular attraction forces.
Hydrogen bonds can be considered as the strongest intermolecular attraction forces.
The only intermolecular "bond" would be hydrogen "bonds". More appropriately, perhaps, one might as about the intermolcular "forces" in octanol. Since this is a primary alcohol, it will have hydrogen bonds (the strongest) and it will have London dispersion forces also.
hydrogen bonds
Hydrogen bonds are much stronger than other intermolecular forces.
Glycerol have hydrogen bonds,but this intermolecular forces are slightly weaker than in water
They are electrically attract each other and form hydrogen bonds. One of the strongest intermolecular forces.
The intermolecular force that hold together adjacent water molecules are hydrogen bonds. Hydrogen bonds are the strongest type of intermolecular forces, but it is still relatively weak compared to ionic and covalent bonds. Hydrogen bonds occur because of the large difference between hydrogen atoms and the highly electronegative atoms such as F, N and O.
These are intermolecular forces.
weakest to strongest: they are in this order: London dispersion, dipole-dipole, hydrogen bonding, ionic
Both are intermolecular forces.