Solubility of Iodine in Some Organic Solvents The solubilities of iodine in $\ce{CCl4,n-Hex,Et2O,PhCH3}$ were given respectively as 19 g/kg, 13 g/kg, 337 g/kg, and 182 g/kg. These results puzzle me for the following reasons:

1) Iodine, being a non-polar substance, should dissolve the most in nonpolar solvents. Yet diethyl ether the best solvent for iodine.

2) Toluene and n-Hexane, both being hydrocarbons, should have similar solubilities of iodine. Yet the solubility of Iodine in Toluene almost 20 times that of n-Hexane.

How do we qualitatively predict these results?

Note: This question's source is from HBCSE INCHO 2012, a chemistry test for high school students, without fancy tools such as the Abrahams' equation.
Iodine as a halogen has the strong electron affinity, what is the best met by the free electron pair of diethylether, then by $\pi$ electron density of toluene.

Note that iodine is also well soluble in ethanol, commercially used in medical treatment of skin injuries.