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Hydrogen bonding is found in molecules with an h atom bonded to an n atom, an o atom, or an f atom Therefore more energy is required to go from liquid to gas. The hydrogen bond is the strongest intermolecular force
Water (h 2 o), hydrogen chloride (hcl), ammonia (nh 3), methanol (ch 3 oh), ethanol (c 2 h 5 oh), and hydrogen bromide (hbr) Liquid to gas requires all the imfs to be overcome, whereas solid to liquid on requires some of the imfs to be overcome Hydrogen bonding is the strongest imf in h2
It is a type of intermolecular force that occurs when a hydrogen atom is bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine
It can only occur when the molecules in question have a highly electronegative atom directly bonded to a hydrogen atom, leading to an unusually extreme dipole For most purposes, these highly electronegative atoms are limited to only nitrogen, oxygen and fluorine. Van der waals forces are the weakest intermolecular forces. The strongest imf is hydrogen bonding, occurring between molecules with n, o, or f atoms bonded to hydrogen, significantly raising boiling points
The answer lies in the highly polar nature of the bonds between hydrogen and very electronegative elements such as o, n, and f The large difference in electronegativity results in a large partial positive charge on hydrogen and a correspondingly large partial negative charge on the o, n, or f atom. How is the strength of imfs related to the number of electrons in the atom (size of the atom) The bigger the molecules the stronger the imf's
With more electrons (larger atom) the electrons can create a larger partial charge and therefore stronger attractions between the molecules.
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