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Answered 2018-02-14 12:12:30

The intermolecular forces would be dispersion forces.

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These are polar forces, intermolecular forces of attraction between molecules.


The only intermolecular forces in this long hydrocarbon will be dispersion forces.


Dipole forces and London forces are present as intermolecular forces in these molecules.


The intermolecular forces operating in NO would be dipole interactions and dispersion forces.


The greater the intermolecular forces, the greater the solubility.


The oxygen molecule has a covalent bond; the intermolecular forces are London dispersion forces.


Intramolecular forces are not intermolecular forces !


In Br2 the intermolecular forces are London dispersion forces.



Pretty much the only intermolecular forces in gasoline would be London dispersion forces.


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surface tension increases with increasing intermolecular forces


London forces are the only intermolecular forces present in gaseous fluorine.



The intermolecular forces of propanol are hydrogen bonding, dipole-dipole forces and London dispersion forces.


The intermolecular forces are hydrogen bonding.


Glycerol have hydrogen bonds,but this intermolecular forces are slightly weaker than in water


The greater the intermolecular forces in a liquid, the higher is its boiling point.


The stronger the intermolecular forces in a solution, the less volatile the solution is.


Low intermolecular forces, low boiling point.


Yes, these intermolecular forces are exist, as an example hydrogen bonds.


Because N2 molecules are nonpolar, the intermolecular forces between them are dispersion forces, also called London forces.


The stronger the intermolecular forces, the higher the melting point and boiling point. The weaker the intermolecular forces, the lower the melting and boiling points are.


Intramolecular forces: forces that act in the interior of a melecule, between atoms Intermolecular forces: forces that act between different molcules


The intermolecular forces are the forces between molecules. These are weaker than the bonding forces within molecules, the covalent bonds.