Does polychloroethylene have only van der Waals/London forces between its molecules? Surely, if all the chlorine atoms are on one side, due to the fact that chlorine is more electronegative than carbon, shouldn’t it have permanent dipole-dipole forces?
$\begingroup$
$\endgroup$
7
-
2$\begingroup$ Everything has London forces. $\endgroup$– Ivan NeretinCommented May 24, 2018 at 17:12
-
$\begingroup$ There are permanent dipoles there,so no idea why you'd think otherwise. $\endgroup$– MithoronCommented May 24, 2018 at 17:24
-
$\begingroup$ PVC tends to have a relatively high stereoregularity, for sth. made by radical polymerisation, but a local dipole moment perpendicular to the backbone would be there any way. Not a very large one, compare methylene chloride, chloroform, etc. $\endgroup$– KarlCommented May 24, 2018 at 18:29
-
$\begingroup$ @Karl dipole moment can be completely cancel out by C-C rotations...it follows of your reasoning... $\endgroup$– user43021Commented Sep 23, 2018 at 2:07
-
$\begingroup$ @santimirandarp hm, C-C rotations are not so easy in a polymer backbone, especially if it's substituted with a bulky chlorine atom $\endgroup$– KarlCommented Sep 23, 2018 at 10:02
|
Show 2 more comments
1 Answer
$\begingroup$
$\endgroup$
1
No, but for polymers of any reasonable size, the dispersion (and excluded volume) forces completely overwhelm any dipole-dipole forces, since they grow with the size of the molecule and dipole-dipole forces do not. Also, bear in mind that the chlorines aren't all on one side of the molecule first because the way it's manufactured tends to put Cls randomly on each side of the chain, and second because the molecule has considerable conformational flexibility. That's true even in the solid state, which for polymers is usually substantially glassy with interspersed domains of crystal.
answered May 25, 2018 at 2:38
-
$\begingroup$ PVC has a rather high stereoregularity, not random atactic, and ist partially crystalline, ordinary polystyrene is just an amorphous glas, PE is partially crystalline and it's glass transition temperature is below -60°C. ?!? $\endgroup$– KarlCommented May 27, 2018 at 16:19