{"id":27788,"date":"2024-10-01T15:35:37","date_gmt":"2024-10-01T14:35:37","guid":{"rendered":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=27788"},"modified":"2026-03-13T17:41:02","modified_gmt":"2026-03-13T17:41:02","slug":"a-carbon-carbon-one-electron-bond-or-a-weak-carbon-carbon-interaction","status":"publish","type":"post","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=27788","title":{"rendered":"A carbon-carbon one-electron bond! Or a weak carbon-carbon interaction?"},"content":{"rendered":"
\n

More than 100 years ago, before the quantum mechanical treatment of molecules had been formulated, G. N. Lewis proposed[1]<\/a><\/span> a simple model for chemical bonding that is still taught today. This is the idea of the three categories of bond we know as single, double and triple, comprising respectively two, four and six shared electrons each, at least for the very common carbon-carbon bond. A little more than a decade ago, this was extended upwards to the eight-electron quadruple bond.[2]<\/a><\/span>. Now, at the other extreme of downwards, a molecule has been characterised in the solid state with a one-electron C-C bond.[3]<\/a><\/span> In this sub-two-electron region, bonds such as hydrogen bonds have long been recognised and they form part of a class of “weak” bonding known instead as exhibiting “non-covalent-interactions” or NCI. But specifically a one-electron carbon-carbon bond stands apart from these weaker types and so it is certainly news when one such is reported and characterised in the crystalline state by x-ray diffraction. <\/p>\n

\"\"<\/p>\n

To start the investigation, a search of the crystal structure database was performed using the following more general query of the structure above. The central C-C bond (in green below) was not added, leaving the two carbons as 3-coordinate.<\/p>\n

\"\"<\/p>\n

This resulted in 10 hits, all revealed as dications, with the central C-C distance ranging from 2.8Å to 3.0Å. So the unique feature of this new report is that they were able to find a system where oxidation did not proceed directly to the dication, but stopped at the 1-electron level to give a radical cation instead. This new structure poses a bit of a quandry for the curators of the CSD. The index for this database is built on the basis of whether any two atoms in a molecule are connected by a “bond”, and the allowed values for bonds range from single to quadruple, with various intermediate descriptions (such as aromatic) and finally “any”. This latter basically means any of the previous, but what I am pretty certain of is that it does not mean “one-electron”, or “half”. The new compound has not yet been indexed in my current version of the CSD, so this presumption is not yet tested.‡<\/sup><\/p>\n

\"\"<\/p>\n

The authors[3]<\/a><\/span> did also make the dication and they report a length of 3.03Å for this species, broadly in accord with the range shown above and a reduced value of 2.92Å for the radical cation (Δr<\/sub> 0.11Å). This is quite a small contraction induced by the formation of the one-electron bond, which is already hinting that it might actually be a weak bond.<\/p>\n

Next, I proceeded by performing my own DFT calculations on these species, at the ωB97XD\/Def2-TZVPP level.(FAIR data DOI: [4]<\/a><\/span>) At this level the di- and monocationic C-C bond lengths came out as 3.075Å and 2.867Å (Δr<\/sub> 0.21Å), a slightly larger contraction than that reported, but still representing a weak bond.<\/p>\n

With wavefunctions now available for the species, I decided to inspect the electron densities. This was calculated at the geometry of the radical cation, and then at the same geometry, the dication was calculated and the two electron densities subtracted. The resulting density surface (contour level 0.002au) representing one electron is shown below. As expected, the most significant feature occurs in the C-C region, but quite a lot of this one electron is distributed around the aromatic rings (I must find out how to integrate regions!). So already we see that this “1-electron” bond is in fact only a fraction of one electron. Again an indication that it is a weak bond.<\/p>\n

\"\"<\/p>\n

A procedure often used to identify weak bonds is called NCI, or noncovalent-interactions.[5]<\/a><\/span> These are by definition interactions weaker than the single bonds, often being hydrogen bonds and other unusual interactions such as a π-π stacking region (rather than a bond). So here, we see that below the single bond type, we get a continuum of interactions rather than bonds as such. The resulting NCI analysis is shown below for firstly the radical cation and then the di-cation at the same geometry.<\/p>\n

\"\"<\/p>\n

The colour coding in the NCI surface analysis above means that dark blue are strong non-covalent interactions such as hydrogen bonds, paler blue or cyan areas are weaker ones and green is weaker still and typical of π-π stacking regions rather than bonds between two atoms. These are all deemed stabilising, whereas orange and red regions are destabilising. Click on the image above to inspect the full three dimensional surface of this NCI function and you will find the π-π stacking features, but also three cyan regions. Enclosed by two of the cyan regions are dark blue ones, whilst the third cyan region contains only a small blue part. This third cyan region is indeed in the C-C one-electron bond region, but using this analysis it emerges as only a “weak” interaction. <\/p>\n

But a surprise! The two dark blue regions, deemed strong “interactions” are between a C-H of an aryl group and the two carbon atoms shown with blue dots in the diagram above and these are apparently more stabilizing than the one-electron C-C “bond”. Should they not also be bonds then?<\/p>\n

\"\"<\/p>\n

The plot above is for the di-cation at the radical cation geometry. It emerges as very similar to the radical cation itself, although the C-C cyan NCI region is less intense than that for the latter and now contains little trace of the dark blue inner core. <\/p>\n

We might conclude from this inspection of the newly reported molecule containing a one-electron C-C bond, is that it probably belongs to the class known as an “interaction” rather than an actual bond. Even as an interaction, it is not particularly strong – in part this is probably because only a proportion of that one electron is actually located in the C-C region, with the rest being distributed around the aromatic rings. However, I rather suspect that despite it resembling an interaction, it will no doubt become known as a bond!<\/p>\n

Added in response to comment<\/b><\/p>\n

\nBelow is shown the Laplacian of the electron density (a definition can be found at eg [6]<\/a><\/span>). Negative values of the Laplacian appear here in purple and positive values in orange (contour value 0.125 a.u). The regular C-C bonds are all enclosed in a negative region of the Laplacian, whilst the one-electron C-C bond lies in the orange region.<\/p>\n

\"\"<\/p>\n

\n
\n

‡<\/sup> Note added 4\/03\/2026. The archived crystal structures at CCDC are shown without a bond in the C-C region.[7]<\/a><\/span>,[8]<\/a><\/span>,[9]<\/a><\/span>,[10]<\/a><\/span><\/p>\n

References<\/h2>\n
  1. G.N. Lewis, \"THE ATOM AND THE MOLECULE.\", Journal of the American Chemical Society<\/i>, vol. 38, pp. 762-785, 1916. https:\/\/doi.org\/10.1021\/ja02261a002<\/a>\n\n<\/li>\n
  2. S. Shaik, D. Danovich, W. Wu, P. Su, H.S. Rzepa, and P.C. Hiberty, \"Quadruple bonding in C2 and analogous eight-valence electron species\", Nature Chemistry<\/i>, vol. 4, pp. 195-200, 2012. https:\/\/doi.org\/10.1038\/nchem.1263<\/a>\n\n<\/li>\n
  3. T. Shimajiri, S. Kawaguchi, T. Suzuki, and Y. Ishigaki, \"Direct evidence for a carbon\u2013carbon one-electron \u03c3-bond\", Nature<\/i>, vol. 634, pp. 347-351, 2024. https:\/\/doi.org\/10.1038\/s41586-024-07965-1<\/a>\n\n<\/li>\n
  4. H. Rzepa, \"A carbon-carbon one-electron bond! Or a weak carbon-carbon interaction?\", 2024. https:\/\/doi.org\/10.14469\/hpc\/14642<\/a>\n\n<\/li>\n
  5. E.R. Johnson, S. Keinan, P. Mori-S\u00e1nchez, J. Contreras-Garc\u00eda, A.J. Cohen, and W. Yang, \"Revealing Noncovalent Interactions\", Journal of the American Chemical Society<\/i>, vol. 132, pp. 6498-6506, 2010. https:\/\/doi.org\/10.1021\/ja100936w<\/a>\n\n<\/li>\n
  6. H. Rzepa, \"Looking at bonds in a different way: the Laplacian.\", 2010. https:\/\/doi.org\/10.59350\/bk5zm-6rk67<\/a>\n\n<\/li>\n
  7. Shimajiri, Takuya., Kawaguchi, Soki., Suzuki, Takanori., and Ishigaki, Yusuke., \"CCDC 2301033: Experimental Crystal Structure Determination\", 2024. https:\/\/doi.org\/10.5517\/ccdc.csd.cc2h7dw1<\/a>\n\n<\/li>\n
  8. Shimajiri, Takuya., Kawaguchi, Soki., Suzuki, Takanori., and Ishigaki, Yusuke., \"CCDC 2301032: Experimental Crystal Structure Determination\", 2024. https:\/\/doi.org\/10.5517\/ccdc.csd.cc2h7dv0<\/a>\n\n<\/li>\n
  9. Shimajiri, Takuya., Kawaguchi, Soki., Suzuki, Takanori., and Ishigaki, Yusuke., \"CCDC 2301034: Experimental Crystal Structure Determination\", 2024. https:\/\/doi.org\/10.5517\/ccdc.csd.cc2h7dx2<\/a>\n\n<\/li>\n
  10. Shimajiri, Takuya., Kawaguchi, Soki., Suzuki, Takanori., and Ishigaki, Yusuke., \"CCDC 2301035: Experimental Crystal Structure Determination\", 2024. https:\/\/doi.org\/10.5517\/ccdc.csd.cc2h7dy3<\/a>\n\n<\/li>\n<\/ol>\n\n<\/div> ","protected":false},"excerpt":{"rendered":"

    More than 100 years ago, before the quantum mechanical treatment of molecules had been formulated, G. N. Lewis proposed a simple model for chemical bonding that is still taught today. 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N. Lewis suggested a model for single and double bonds that involved sharing either 2 or 4 electrons between a pair of atoms. We tend to think\u2026","rel":"","context":"In "Interesting chemistry"","block_context":{"text":"Interesting chemistry","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=4"},"img":{"alt_text":"Click for 3D","src":"https:\/\/i0.wp.com\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2013\/03\/PYRDRE.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":27870,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=27870","url_meta":{"origin":27788,"position":1},"title":"The one-electron carbon-carbon bond: Hexafluoroethane and ethane radical cations.","author":"Henry Rzepa","date":"October 3, 2024","format":false,"excerpt":"In the previous post, I looked at the recently reported hexa-arylethane containing a carbon-carbon one-electron bond, its structure having been determined by x-ray diffraction (XRD). The measured C-C bond length was ~2.9a\u00c5 and my conclusion was that the C...C region represented more of a weak \"interaction\" than of a bond\u2026","rel":"","context":"In "Interesting chemistry"","block_context":{"text":"Interesting chemistry","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=4"},"img":{"alt_text":"","src":"","width":0,"height":0},"classes":[]},{"id":28187,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=28187","url_meta":{"origin":27788,"position":2},"title":"Molecules of the Year 2024: A crystal structure perspective on anti-Bredt olefins.","author":"Henry Rzepa","date":"January 8, 2025","format":false,"excerpt":"Each year C&E News publishes a list of candidates for the Molecule of the Year. For 2024 the list is (in order of votes cast for each) Mirror-image cyclodextrin Molecular shuttle in a box Rule-bending strained alkene First soluble promethium complex Single-electron carbon-carbon bond Hot MOF for capturing carbon I\u2026","rel":"","context":"In "Interesting chemistry"","block_context":{"text":"Interesting chemistry","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=4"},"img":{"alt_text":"","src":"","width":0,"height":0},"classes":[]},{"id":17829,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=17829","url_meta":{"origin":27788,"position":3},"title":"First, hexacoordinate carbon – now pentacoordinate nitrogen?","author":"Henry Rzepa","date":"March 25, 2017","format":false,"excerpt":"A few years back I followed a train of thought here which ended with hexacoordinate carbon, then a hypothesis rather than a demonstrated reality. That reality was recently confirmed via a crystal structure,\u00a0DOI:10.5517\/CCDC.CSD.CC1M71QM. Here is a\u00a0similar proposal for\u00a0penta-coordinate nitrogen. First, a search of the CSD (Cambridge structure database) for such\u00a0nitrogen.\u2026","rel":"","context":"In "Bond slam"","block_context":{"text":"Bond slam","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=2237"},"img":{"alt_text":"","src":"","width":0,"height":0},"classes":[]},{"id":8048,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=8048","url_meta":{"origin":27788,"position":4},"title":"Trimethylenemethane Ruthenium benzene","author":"Henry Rzepa","date":"October 17, 2012","format":false,"excerpt":"Every once in a while, one encounters a molecule which instantly makes an interesting point. Thus Ruthenium is ten electrons short of completing an 18-electron shell, and it can form a complex with benzene on one face and a ligand known as trimethylenemethane on the other. This four-carbon molecule has\u2026","rel":"","context":"In "Interesting chemistry"","block_context":{"text":"Interesting chemistry","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=4"},"img":{"alt_text":"","src":"https:\/\/i0.wp.com\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2012\/10\/JODLIX.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":19251,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=19251","url_meta":{"origin":27788,"position":5},"title":"Are diazomethanes hypervalent molecules? Probably, but in an unexpected way!","author":"Henry Rzepa","date":"December 23, 2017","format":false,"excerpt":"A recently published review on hypervalency introduced a very simple way of quantifying the effect. One of the molecules which was suggested to be hypervalent using this method was diazomethane. Here I take a closer look. The new method is called the valence electron equivalent \u03b3. It is defined as\u00a0\"the\u2026","rel":"","context":"In "Hypervalency"","block_context":{"text":"Hypervalency","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=7"},"img":{"alt_text":"","src":"","width":0,"height":0},"classes":[]}],"jetpack_likes_enabled":false,"authors":[{"term_id":2661,"user_id":1,"is_guest":0,"slug":"admin","display_name":"Henry Rzepa","avatar_url":"https:\/\/secure.gravatar.com\/avatar\/897b6740f7f599bca7942cdf7d7914af5988937ae0e3869ab09aebb87f26a731?s=96&d=blank&r=g","0":null,"1":"","2":"","3":"","4":"","5":"","6":"","7":"","8":""}],"_links":{"self":[{"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/27788","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fcomments&post=27788"}],"version-history":[{"count":77,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/27788\/revisions"}],"predecessor-version":[{"id":31030,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/27788\/revisions\/31030"}],"wp:attachment":[{"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fmedia&parent=27788"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fcategories&post=27788"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Ftags&post=27788"},{"taxonomy":"author","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fppma_author&post=27788"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}