{"id":23588,"date":"2021-05-08T15:10:58","date_gmt":"2021-05-08T14:10:58","guid":{"rendered":"https:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/?p=23588"},"modified":"2021-05-16T10:00:44","modified_gmt":"2021-05-16T09:00:44","slug":"two-new-reality-based-suggestions-for-molecules-with-a-metal-m%e2%a9%b8c-quadruple-bond","status":"publish","type":"post","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=23588","title":{"rendered":"Two new reality-based suggestions for molecules with a metal M\u2a78C quadruple bond."},"content":{"rendered":"
\n

Following from much discussion over the last decade about the nature of C2<\/sub>, a diatomic molecule which some have suggested sustains a quadruple bond between the two carbon atoms, new ideas<\/a> are now appearing for molecules in which such a bond may also exist between carbon and a transition metal atom. A suggested, albeit hypothetical example was C\u2a78Fe(CO)3<\/sub>[1]<\/a><\/span>. Iron has a\u00a0[Ar<\/strong>].3d<\/strong>6<\/sup>.4s<\/strong>2<\/sup>\u00a0electronic configuration and if we ionise to balance a C4-<\/sup> ligand, the iron becomes formally FeVI<\/sup> or [Ar<\/strong>].3d<\/strong>4<\/sup>. By adding 14 electrons deriving from the seven “bonds” to the 3d<\/strong>4<\/sup>,\u00a0including a quadruple count from carbon, the Fe formally completes its 18-electron valence shell, as also found in e.g.<\/em> Ferrocene.<\/p>\n

\"\"<\/a><\/p>\n

A search for crystal structures containing the very simple query structure shown below, where C is defined as having one atom only attached, TR is any transition metal and the structure is non-polymeric, was undertaken to see if any examples of this motif might already exist.\u00a0\"\"<\/a><\/p>\n

Zero hits with 4-coordinate metal atoms, but 11<\/strong>\u00a0real examples were found (FAIR DOI 10.14469\/hpc\/8190<\/a>), all of which exhibit a five-coordinate transition metal centre, where X is a mono-anionic ligand (CN, halogen, etc) and L is a neutral ligand (PR3<\/sub> etc). The most common metal was M = Ru, the electronic configuration of which is [Kr<\/strong>].4d<\/strong>7<\/sup>5s<\/strong>1<\/sup>, becoming [Kr<\/strong>].4d<\/strong>2<\/sup> by ionising to balance a C4-<\/sup> ligand and the two X–<\/sup> ligands. There are now 16 electrons from the eight “bonds” surrounding the atom, including again a quadruple one from the carbon and forming a filled 18-electron valence shell around the metal.<\/p>\n

\"\"<\/a><\/p>\n

So could these 11 constitute known examples of quadruple bonds from a transition metal to carbon? I will investigate using M=Ru, L = PH3<\/sub> and X = CN–<\/sup>, which represents a simplified form of one of the 11 examples[2]<\/a><\/span> using the following electronic model: \u03c9B97XD\/Def2-SVPD. The focus will be on five localised NBO orbitals (the procedure I used previously<\/a> to count the number of bonds at carbon\u00a0for C\u2a78Fe(CO)3<\/sub>).<\/p>\n

For M=Ru, the NBOs emerge as follows (click on any orbital thumbnail to convert to a 3D rotatable model).<\/p>\n\n\n\n\n\n\n\n\n\n
M=Ru, r = 1.624\u00c5.<\/th>\n<\/tr>\n
NBO 42, Occupied, Non-bonding d-orbital<\/th>\nNBO 41 \u03c0 bond<\/th>\n<\/tr>\n
\"\"<\/td>\n\"\"<\/td>\n<\/tr>\n
NBO 36 \u03c0 bond<\/th>\nNBO 35 \u03c3 bond<\/th>\n<\/tr>\n
\"\"<\/td>\n\"\"<\/td>\n<\/tr>\n
NBO 34 non-bonding carbon lone pair<\/th>\nOverlap of orbitals 42 and 34<\/th>\n<\/tr>\n
\"\"<\/td>\n \"\"\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

This reveals only a triple Ru\u2261C bond plus a non-bonding lone pair on carbon. It turns out that bonding σ-orbital 34<\/strong>\u00a0is “surrounded” by the non-bonding Ru d-orbital 42. The electron-electron repulsions between the pair causes the electrons in orbital 34<\/strong> to locate onto the carbon to form a non-bonding lone pair, as thus:<\/p>\n

\"\"<\/a><\/p>\n

So might it be possible to persuade this carbon lone pair to instead donate into the M-C bond to form that fully-fledged quadruple bond?<\/p>\n

\"\"<\/a><\/p>\n

One simple strategy is to remove the two electrons in orbital 42<\/strong>, preventing the Pauli repulsions from occuring and this can be done by using Mo instead of Ru.<\/p>\n\n\n\n\n\n\n\n\n\n
M=Mo, r = 1.673\u00c5<\/th>\n<\/tr>\n
NBO 42 unoccupied Non-bonding d-orbital<\/th>\nNBO 41 \u03c3 bond<\/th>\n<\/tr>\n
\"\"<\/td>\n\"\"<\/td>\n<\/tr>\n
NBO 40 \u03c0 bond<\/th>\nNBO 39 \u03c0 bond<\/th>\n<\/tr>\n
\"\"<\/td>\n\"\"<\/td>\n<\/tr>\n
NBO 22 \u03c3 bond<\/th>\n<\/tr>\n
\"\"<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

By removing the repulsions to the non-bonding d-orbital, we have now transformed the erstwhile carbon lone pair into a fully fledged bond as in orbital 22<\/strong>, thus forming the quadruple motif. There are two electrons less, so this time the Mo valence shell is a 16-electron system.<\/p>\n

So, SUGGESTION 1<\/span><\/strong>:<\/p>\n

\"\"<\/a><\/p>\n

The second possibility is to increase the size of the non-bonding d-orbital 42<\/strong> by changing from Ru to Os. Here again, orbital 22<\/strong> is less repelled by the electrons in orbital 42<\/strong> due to the larger size of the latter and so can again become C-Os bonding rather than non-bonding carbon lone pair.<\/p>\n\n\n\n\n\n\n\n\n\n
M=Os, r = 1.679\u00c5<\/th>\n<\/tr>\n
NBO 42 Occupied Non-bonding d-orbital<\/th>\nNBO 41 \u03c0 bond<\/th>\n<\/tr>\n
\"\"<\/td>\n\"\"<\/td>\n<\/tr>\n
\nNBO 40 \u03c3 bond <\/th>\n\nNBO 35 \u03c0 bond<\/th>\n<\/tr>\n
\n\"\"<\/td>\n\n\"\"<\/td>\n<\/tr>\n
NBO 22 \u03c3 bond<\/th>\n<\/tr>\n
\n\"\"<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

So, SUGGESTION 2<\/span><\/strong><\/p>\n

\"\"<\/a><\/p>\n

This approach also reveals the binary decision in the NBO analysis, either an orbital is classified as “LP” and hence is not considered a bond, or it is classified as “BD” and is a bond. Reality is certainly more nuanced, with weights needing to be assigned to each valence bond representation (rather than just 1.0 or 0.0). Probably also these weights will depend on a number of factors, such as basis set quality and the method applied (e.g. the DFT procedure used). So the binary terms “triple” or “quadruple” do not carry the full measure of the bonding behaviour, which may be a continuum between these two extremes. But the two molecules shown above do represent molecules that could be realistically synthesized, since they are but small variations of already known molecules. Once made, they could then be subjected to appropriate experimental analysis to test the bonding hypotheses made here.<\/p>\n

\n

This post has DOI: https:\/\/doi.org\/gbq3<\/p>\n

\n

References<\/h2>\n
  1. A.J. Kalita, S.S. Rohman, C. Kashyap, S.S. Ullah, and A.K. Guha, \"Transition metal carbon quadruple bond: viability through single electron transmutation\", Physical Chemistry Chemical Physics<\/i>, vol. 22, pp. 24178-24180, 2020. https:\/\/doi.org\/10.1039\/d0cp03436c<\/a>\n\n<\/li>\n
  2. T.J. Morsing, A. Reinholdt, S.P.A. Sauer, and J. Bendix, \"Ligand Sphere Conversions in Terminal Carbide Complexes\", Organometallics<\/i>, vol. 35, pp. 100-105, 2015. https:\/\/doi.org\/10.1021\/acs.organomet.5b00803<\/a>\n\n<\/li>\n<\/ol>\n\n<\/div> ","protected":false},"excerpt":{"rendered":"

    Following from much discussion over the last decade about the nature of C2, a diatomic molecule which some have suggested sustains a quadruple bond between the two carbon atoms, new ideas are now appearing for molecules in which such a bond may also exist between carbon and a transition metal atom. 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I had previously mooted that the Fe\u2a78C combination might be\u2026","rel":"","context":"In "crystal_structure_mining"","block_context":{"text":"crystal_structure_mining","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=1745"},"img":{"alt_text":"","src":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2021\/05\/Screenshot-703-1024x818.jpg?resize=350%2C200&ssl=1","width":350,"height":200},"classes":[]},{"id":23777,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=23777","url_meta":{"origin":23588,"position":1},"title":"A suggestion for a molecule with a M\u2a78C quadruple bond with trigonal metal coordination.","author":"Henry Rzepa","date":"May 13, 2021","format":false,"excerpt":"The proposed identification of molecules with potential metal to carbon quadruple bonds, in which the metal exhibits trigonal bipyramidal coordination rather than the tetrahedral modes which have been proposed in the literature,, leads on to asking whether simple trigonal coordination at the metal can also sustain this theme? The rational\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":22971,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=22971","url_meta":{"origin":23588,"position":2},"title":"A new example of a quadruple bond from carbon – to Fe.","author":"Henry Rzepa","date":"November 7, 2020","format":false,"excerpt":"Way back in 2010, I was writing about an experience I had just had during an organic chemistry tutorial, which morphed into speculation as to whether a carbon atom might sustain a quadruple bond to nitrogen. A decade on, and possibly approaching 100 articles by many authors on the topic,\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.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2020\/11\/NMn_33a-1024x839.jpg?resize=350%2C200&ssl=1","width":350,"height":200},"classes":[]},{"id":9973,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=9973","url_meta":{"origin":23588,"position":3},"title":"A (very) short history of shared-electron bonds.","author":"Henry Rzepa","date":"March 26, 2013","format":false,"excerpt":"The concept of a shared electron bond and its property of an order is almost 100 years old in modern form, when G. 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":8048,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=8048","url_meta":{"origin":23588,"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":10733,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=10733","url_meta":{"origin":23588,"position":5},"title":"Is dicarbon (C2) a molecule of chemical interest?","author":"Henry Rzepa","date":"July 3, 2013","format":false,"excerpt":"C2\u00a0(dicarbon) is certainly interesting from a theoretical point of view. Whether or not it can be described as having a quadruple bond has induced much passionate discussion,,,. Its occurrence in space and in flames is also well-known. But does it have what might be called a conventional chemistry? Other highly\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\/07\/LaOsC1.jpeg?resize=350%2C200","width":350,"height":200},"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\/23588","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=23588"}],"version-history":[{"count":44,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/23588\/revisions"}],"predecessor-version":[{"id":23853,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/23588\/revisions\/23853"}],"wp:attachment":[{"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fmedia&parent=23588"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fcategories&post=23588"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Ftags&post=23588"},{"taxonomy":"author","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fppma_author&post=23588"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}