dispersion forces
the intermolecular forces are hydrogen bonds
C6H14 - dispersion forces H2O - hydrogen bonding, dipole, dispersion HCHO - dipole, dispersion C6H5OH - hydrogen bonding, dipole, dispersion
Hydrogen bonding and London Dispersion forces (the latter of which are in all molecules).
user-generated content: report abuseDipole-Dipole forces, Dispersion forces, and hydrogen bonding
dispersion, dipole-dipole, and hydrogen bonding forces
the intermolecular forces are hydrogen bonds
Dipole forces and London forces are present between these molecules.
hydrogen, London dispersion, and dipole - dipole
C6H14 - dispersion forces H2O - hydrogen bonding, dipole, dispersion HCHO - dipole, dispersion C6H5OH - hydrogen bonding, dipole, dispersion
NH3 exhibits hydrogen bonding in addition to dispersion forces. This significantly increases the intermolecular force, and raises the boiling point. PH3 does not exhibit hydrogen bonding and the dominant intermolecular force holding these molecules together is dispersion forces. (Dispersion forces also known as Van Der Waal Force)
Hydrogen bonding and London Dispersion forces (the latter of which are in all molecules).
The main intermolecular force holding water molecules together in hydrogen bonding. Also, there are diplole-dipole interactions and London dispersion forces. But hydrogen bonds are the major force keeping water in the liquid state.
user-generated content: report abuseDipole-Dipole forces, Dispersion forces, and hydrogen bonding
dispersion, dipole-dipole, and hydrogen bonding forces
The hydrogen bonding present between the two molecules is known as intermolecular hydrogen bonding, the molecules may be similar or may be dissimilar. The molecules having intermolecular hydrogen bonding have high melting and boiling points and low volatility. They are more soluble in water as compared to the molecules having intramolecular hydrogen bonding.
Ethane is a non-polar hydrocarbon, therefore its molecules will only experience London dispersion forces between them, which are the weakest of all the intermolecular attractions. This explains ethane's low boiling point.
It has dispersion forces, dipole dipole forces ,and hydrogen bonding. Source: I'm a chemistry professor