Is the smallest carbon molecule smaller than C20?

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Discussion Overview

The discussion centers around the existence of carbon molecules smaller than C20, specifically exploring the stability and bonding of smaller carbon molecules such as C2 and C4. Participants examine theoretical possibilities, natural occurrences, and stability issues related to these molecules.

Discussion Character

  • Exploratory
  • Debate/contested
  • Technical explanation

Main Points Raised

  • Some participants propose that C2 is a molecule smaller than C20, though its natural occurrence is uncertain.
  • Others express skepticism about the bonding capabilities of C2, suggesting it may not be stable or may not occur naturally.
  • One participant mentions that C2 exists but is very unstable, indicating it cannot be stored due to its reactivity with more stable carbon forms.
  • There are discussions about the geometric configurations of C4, with some participants speculating on its potential structures and stability, including the possibility of resonance stabilization.
  • One participant references theoretical studies on radical ions of C4, expressing doubt about its synthesis and stability.
  • Another participant brings up tetrahedral N4 as a high-energy compound, noting its proposed use as a rocket fuel, although it has not been synthesized either.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the existence and stability of smaller carbon molecules, with multiple competing views and uncertainties remaining about their bonding and natural occurrence.

Contextual Notes

Limitations include the unclear stability of proposed molecules, the dependence on theoretical models for bonding configurations, and the unresolved nature of experimental synthesis.

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Does there/or could there exist a molecule made only of carbon, that is smaller than C20?
 
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Yes. C2 is a molecule Smaller than C2O. Whether it's a naturally occurring one, I'm not sure.
 
Xtensity said:
Yes. C2 is a molecule Smaller than C2O. Whether it's a naturally occurring one, I'm not sure.

As far as I knew the bonding for C2 is not possible, that's why I asked. Maybe I was misinformed. Perhaps its just that it does not occur in nature. How would the bonding work?
 
I think C-C will wander until it picks up some -H for example, to make ethane.
 
Well if that is allowed, geometrically I can imagine C4, formally a square with two acetylenic bonds, or a tetrahedron with two double bonds. Both have very strained bond angles but would they get some resonance stabilisation? Could it be made difficult for them to decay into anything if e.g. in dilute gas*? :confused:

*for the reason below.
 
Last edited:
C2 is certainly very stable to dissociation and has been characterized completely in the gas phase. However it cannot be filled in bottles as there are other carbon modifications which are even more stable and to which C2 quickly reacts.
 
epenguin said:
Well if that is allowed, geometrically I can imagine C4, formally a square with two acetylenic bonds, or a tetrahedron with two double bonds.

Neither, C4 (if it exists) is planar and rhombic (since the double-bonds are shorter). I'm doubtful it's been synthesized, and I'm doubtful of its stability. There are some recent theoretical studies of its radical ions, though.

There's tetrahedral N4, which I'm a big fan of. Never synthesized either, but I know that one's supposed to be somewhat stable (energetic barrier to decomposition of around 10 kcal/mol or something). It's a very high-energy compound (something like 50 MJ/kg IIRC). It's been proposed as an environmentally-friendly rocket fuel. If someone could come up with some way of making it.
 

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