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 8<sup>th</sup> [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.[<sup>[36]</sup>](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. Any and all contributions are greatly appreciated.