The surface tension -- the attraction between like molecules -- is a function of the collective strength of the intermolecular forces.
Water and isopropanol both exhibit hydrogen bonding along with all three of the van der Waals forces. Cooking oil has strong London dispersion forces, and acetone exhibits the three van der Waals forces. Acetone and isopropanol have similar structures. Acetone has a greater dipole moment, but a lower boiling point compared to isopropanol. They will probably have similar surface tensions. The outlier in terms of structure and intermolecular attraction is the cooking oil. It will have a much greater boiling point than even water due to the strength of the London dispersion forces. Therefore, it may very well have a greater surface tension than either acetone or isopropanol. One still has to think that water will have the greatest surface tension of the group of four liquids.
........................ Surface Tension
Weakest ............. ................ ............. Strongest
acetone .... isopropanol .... cooking oil .... water
(The following is from a handout which I wrote for my students.)
More on intermolecular forces
Note: There are three van der Waals forces (Keesom forces, Debye forces and London dispersion forces). Some textbooks and some teachers' dusty old notes erroneously equate van der Waals forces only with London dispersion forces.
1. London dispersion forces .... forces between all molecules. In the past London dispersion forces were characterized as the attraction between temporary dipoles. There may be more to it than that. Dispersion forces are a quantum interaction. All molecules exhibit London dispersion forces, LDF's. The strength of LDF's is proportional to the polarizability of the molecule, which in turn, depends on the number of electrons and the surface area of the molecule. Contrary to what some teachers and even some authors say, in many cases London dispersion forces can be stronger than Keesom or Debye forces and are second only to hydrogen bonding.
2. Keesom forces (dipole-dipole attraction) ... the attraction of one polar molecule for another. Oppositely charged ends of the molecules undergo electrostatic attraction.
3. Debye forces (induced attraction) .... the attraction between a polar molecule and one which is nonpolar, where the polar molecule induces a charge separation in the nonpolar molecule. Debye forces can also exist between two polar molecules, even the same kind of molecule.
4. Hydrogen bonding .... The weakly covalent bonds found between the hydrogen atom of one molecule where it is bonded to N, O or F, and the N, O, or F of an adjacent molecule. The hydrogen atom functions as a bridge, forming a bond between two molecules. Hydrogen bonding is more than an electrostatic attraction between molecules, instead there is evidence of orbital overlap and covalent bond formation.