These are intermolecular forces.
These are hydrogen bonds and dispersion forces.
weakest to strongest: they are in this order: London dispersion, dipole-dipole, hydrogen bonding, ionic
Hydrogen bonding and London Dispersion forces (the latter of which are in all molecules).
Hydrogen bonds are stronger than dipole-dipole and Van der Waals forces.
Hydrogen bonds, dipole - dipole bonds, and London dispersion forces.
These are hydrogen bonds and dispersion forces.
weakest to strongest: they are in this order: London dispersion, dipole-dipole, hydrogen bonding, ionic
HYDRO the whole question is to order the following inter molecular forces by increasing strength of bonds: covalent bonds ionic bonds- london dispersion forces dipolar forces hydrogen bonds metallic bonds
Hydrogen bonding and London Dispersion forces (the latter of which are in all molecules).
Hydrogen bonds are stronger than dipole-dipole and Van der Waals forces.
Hydrogen bonds, dipole - dipole bonds, and London dispersion forces.
Intermolecular forces are of the type(1) hydrogen bonds (2) dipole-dipole attractions (3) dispersion forces (van der Waals, etc.)
the intermolecular forces are hydrogen bonds
It has dispersion forces, dipole dipole forces ,and hydrogen bonding. Source: I'm a chemistry professor
Yes, hydrogen bonding may be the strongest force but dispersion forces (London dispersion) increases strength in bonds with size. The greater size the greater strength. Therefore, if you have a huge carbon molecule the forces might be stronger than the H-bond.
Hydrogen exists as H2. This means it's symmetrical. This means that it's non polar. This literally leaves dispersion forces as the only answer.
the intermolecular forces present in methanol are hydrogen bond between the oxygen and hydrogen part of the molecule and van der waals forces between the carbon and hydrogen part of the molecule.