Hi! For hydrogen fluoride: the predominant intermolecular force is hydrogen bonding. In hydrogen bonding, fluorine acts as a \"bridge\" (the middle atom) between two hydrogen molecules. The only other atoms that can participate in hydrogen bonding are nitrogen, oxygen and sulfur. The other intermolecular forces are present in hydrogen fluoride as well, but they are not as significant as hydrogen bonding. For carbon tetrafluoride: the predominant intermolecular force is dispersion (also called London dispersion or van der waals forces) due to the fact that this is a non-polar, symmetrical molecule and the difference in electronegativity between carbon and hydrogen is not great enough for the bond to be considered truly polar. For hydrogen chloride: the predominant intermolecular force is dipole-dipole. Chlorine cannot participate in hydrogen bonding, however, the chlorine atom has a considerable difference in electronegativity relative to hydrogen so the covalent bond is considered polar. There are also dispersion forces present, but they are not as significant as the dipole-dipole forces here. I hope this helps! Please don\'t forget to rate : ) Solution Hi! For hydrogen fluoride: the predominant intermolecular force is hydrogen bonding. In hydrogen bonding, fluorine acts as a \"bridge\" (the middle atom) between two hydrogen molecules. The only other atoms that can participate in hydrogen bonding are nitrogen, oxygen and sulfur. The other intermolecular forces are present in hydrogen fluoride as well, but they are not as significant as hydrogen bonding. For carbon tetrafluoride: the predominant intermolecular force is dispersion (also called London dispersion or van der waals forces) due to the fact that this is a non-polar, symmetrical molecule and the difference in electronegativity between carbon and hydrogen is not great enough for the bond to be considered truly polar. For hydrogen chloride: the predominant intermolecular force is dipole-dipole. Chlorine cannot participate in hydrogen bonding, however, the chlorine atom has a considerable difference in electronegativity relative to hydrogen so the covalent bond is considered polar. There are also dispersion forces present, but they are not as significant as the dipole-dipole forces here. I hope this helps! Please don\'t forget to rate : ).

1. Hi!
For hydrogen fluoride: the predominant intermolecular force is hydrogen bonding. In hydrogen
bonding, fluorine acts as a "bridge" (the middle atom) between two hydrogen molecules. The
only other atoms that can participate in hydrogen bonding are nitrogen, oxygen and sulfur. The
other intermolecular forces are present in hydrogen fluoride as well, but they are not as
significant as hydrogen bonding.
For carbon tetrafluoride: the predominant intermolecular force is dispersion (also called London
dispersion or van der waals forces) due to the fact that this is a non-polar, symmetrical molecule
and the difference in electronegativity between carbon and hydrogen is not great enough for the
bond to be considered truly polar.
For hydrogen chloride: the predominant intermolecular force is dipole-dipole. Chlorine cannot
participate in hydrogen bonding, however, the chlorine atom has a considerable difference in
electronegativity relative to hydrogen so the covalent bond is considered polar. There are also
dispersion forces present, but they are not as significant as the dipole-dipole forces here.
I hope this helps! Please don't forget to rate : )
Solution
Hi!
For hydrogen fluoride: the predominant intermolecular force is hydrogen bonding. In hydrogen
bonding, fluorine acts as a "bridge" (the middle atom) between two hydrogen molecules. The
only other atoms that can participate in hydrogen bonding are nitrogen, oxygen and sulfur. The
other intermolecular forces are present in hydrogen fluoride as well, but they are not as
significant as hydrogen bonding.
For carbon tetrafluoride: the predominant intermolecular force is dispersion (also called London
dispersion or van der waals forces) due to the fact that this is a non-polar, symmetrical molecule
and the difference in electronegativity between carbon and hydrogen is not great enough for the
bond to be considered truly polar.
For hydrogen chloride: the predominant intermolecular force is dipole-dipole. Chlorine cannot
participate in hydrogen bonding, however, the chlorine atom has a considerable difference in
electronegativity relative to hydrogen so the covalent bond is considered polar. There are also
dispersion forces present, but they are not as significant as the dipole-dipole forces here.
I hope this helps! Please don't forget to rate : )