Why are Buckminsterfullerene (C60) solutions pink/purple?

A solution of [Buckminsterfullerene](https://en.wikipedia.org/wiki/Buckminsterfullerene) $\ce{(C60)}$ is shown below:


![C60 solution](https://upload.wikimedia.org/wikipedia/commons/thumb/d/d7/C60_Fullerene_solution.jpg/220px-C60_Fullerene_solution.jpg)


According to the April 8th [Wikipedia page](https://en.wikipedia.org/w/index.php?title=Buckminsterfullerene&oldid=945110359#Solution) on Buckminsterfullerene $\ce{(C60)}$:



> 
> Solutions of pure C60 have a deep purple color which leaves a brown residue upon evaporation. The 
>  reason for this color change is the relatively narrow energy width of the band of molecular levels 
>  responsible for green light absorption by individual C60 molecules. Thus individual molecules 
>  transmit some blue and red light resulting in a purple color. Upon drying, intermolecular 
>  interaction results in the overlap and broadening of the energy bands, thereby eliminating the blue 
>  light transmittance and causing the purple to brown color change.[[36]](https://en.wikipedia.org/w/index.php?title=Buckminsterfullerene&oldid=945110359#cite_note-36)
> 
> 
> 


Now, I'm not too bright in the field of quantum chemistry/electrochemistry, so this doesn't click with me very well. Does anyone have a good way to explain in layman's terms why the $\ce{C60}$ solutions appear pink/purple? I'm very curious why they experience such a definite color absorption when they are made solely of carbon atoms, while most organic dyes have a host of other heteroatoms and functional groups. Also, why do they exhibit a very specific absorption *only* when in solution? Any and all contributions are greatly appreciated.


