The phrase "intermolecular attraction" is correct and usable in written English.
It can be used in scientific contexts, particularly in chemistry, to describe the forces that occur between molecules.
Example: "The properties of liquids can be explained by the strength of intermolecular attraction between the molecules."
Alternatives: "molecular forces" or "molecular attraction".
As the temperature increases, the intermolecular attraction between the nanoparticles and their base fluids weakens [53].
The thiol group also improves the adsorptive interaction with the surface, as the carboxylate groups provide extra intermolecular attraction.
This is attributed to the presence of strong intermolecular attraction such as dipole-dipole and dipole-induced dipole interaction (Ali et al. 1996; Ali and Nain 1996).
It is mainly used to study the intermolecular interactions involving the Van der Waals type dipole dipole forces, etc., because the larger the dipole moment as shown in Table 3, the stronger will be the intermolecular attraction [45].
This would mean that the alloying element slightly reduces the intermolecular attraction between species in the liquid, but it is difficult to attribute it to any particular element's intrinsic chemical properties such as its position in the periodic table.
The isotherms are congruent only with respect to potential on the negative side of the electrocapillary maximum and in this region a Frumkin isotherm is obeyed with an interaction parameter equal to α = 0.3 corresponding to intermolecular attraction.
The hard and soft regions are thus held together by mechanical interlocking and by strong intermolecular attractions, but they are not chemically interlinked into a permanent network as is the case with traditional vulcanized rubbers.
Because of the relatively weak intermolecular attractions (van der Waals forces) between the separate P4 molecules, the solid melts easily at 44.1° C and boils at about 280° C. Formation of tetrahedra requires bond angles of 60° instead of the preferred 90° 109° angles, so that white phosphorus is a relatively unstable, or metastable, form.
These intermolecular attractions in gases came to be known as van der Waals forces.
By accounting for the intermolecular attractions of different gases, van der Waals extended the idealized gas laws of Robert Boyle and others to the behavior of real gases.
Parameters derived from MOPAC AM1 energies scaled to yield higher barriers to torsional motion, as suggested by ab initio results, provide a large trans barrier and stronger intermolecular attractions, which will probably be important for dynamics investigations into the nature of the solid-state phase transitions and helical defects.
