# Why is the buckminsterfullerene the purest form of carbon?

Other websites say that $\ce{C60}$ doesn't have surface bonds that are attracted by other atoms as in graphite and diamond.

I understand that graphite may be attracted by other atoms because of its dangling electron. But why diamond? Each carbon in diamond is covalently bonded to $4$ other carbon atoms in a tetrahedral fashion.

• Just to confuse you: I've read (albeit it has been a long while) that diamonds are somewhat resistant to impurities because it's difficult to get in its crystal lattice. Also if diamonds were pure, they would've been transparent. Diamonds are not transparent. I like bluish diamonds. Yellowish diamonds are also common. – Berry Holmes May 26 '17 at 6:54
• @BerryHolmes I almost got confused. But maybe $\ce{C60}$ is relatively more pure than diamond but I don't know why. Maybe because you told that diamond contains impurities, and $\ce{C60}$ is artificial. But yeah, thanks for the info. – Reeshabh Ranjan May 26 '17 at 7:54
• What happens at the edge of a diamond lattice... – bon May 26 '17 at 8:06
• @ReeshabhRanjan Buckminsterfullerene is not artificial - it is found in soot and has been detected in deep space. – Andrew Morton May 26 '17 at 9:34
• @AndrewMorton I didn't know about deep space, but l it isn't like any soot. The soot is made by, as Wikipedia writes, in an 'arc-process between two graphite electrodes in a helium atmosphere where the electrode material evaporates and condenses forming soot in the quenching atmosphere.' – Reeshabh Ranjan May 26 '17 at 9:51

• Thank you. Now I understand it well. The structure of $\ce{C60}$ clearly defines it's boundaries. – Reeshabh Ranjan May 26 '17 at 8:33