{"id":19499,"date":"2018-03-18T16:45:15","date_gmt":"2018-03-18T16:45:15","guid":{"rendered":"https:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/?p=19499"},"modified":"2018-03-25T08:12:14","modified_gmt":"2018-03-25T07:12:14","slug":"never-mind-main-group-hypervalency-what-about-transition-metal-hypervalency","status":"publish","type":"post","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=19499","title":{"rendered":"Never mind main group “hypervalency”, what about transition metal “hypervalency”?"},"content":{"rendered":"
\n

I have posted often on the chemical phenomenon known as hypervalency, being careful to state that as defined it applies just to “octet excess” in main group elements. But what about the next valence shell, occurring in transition metals and known as the “18-electron rule”? You rarely hear the term hypervalency being applied to such molecules, defined presumably by the 18-electron valence shell count being exceeded. So the following molecule (drawn in three possible valence bond representations) first made in 1992 intrigues.[1]<\/a><\/span><\/p>\n

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

The molecule comprises six phosphinidene ligands (RP:, R=tert-butyl), the P analogues of nitrenes and arranged around nickel to form an unusual hexagonal planar coordinate species and with three of the t-butyl groups facing up and three down. This arrangement totally obscures the two nickel diaxial positions, preventing any ligand from occupying them. One may even speculate that the dispersion attractions between the two pairs of three t-butyl groups might be unusually stabilising,\u2021<\/sup> maybe even on a par with those reported by Schreiner and co-workers for t-butyl substituted triphenylmethanes and noted on this blog.<\/a><\/p>\n

\"\"<\/p>\n

Nitrenes can be represented coordinating to a metal as RN=M. If the analogy extends to P, the valence bond structure 1<\/strong> above would result and the six P atoms would contribute 12 electrons to the Ni valence shell. Since the Ni shell is\u00a0 [Ar<\/strong>].3d<\/strong>8<\/sup>.4s<\/strong>2 <\/sup>adding another 12 electrons would make 22 electrons, thus exceeding the 18-electron rule. In fact it was never suggested as such; in the 1992 analysis of the bonding[1]<\/a><\/span>, the authors clearly state “The electronic structure … cannot be described in terms of the 18e rule”. To support this, they draw the structure in form 3<\/strong> above, which implies a Ni valence shell of 16e, albeit also implying a Ni bond index of ~6.<\/span><\/span><\/span><\/span><\/p>\n

Time I thought for calculations (wB97XD\/Def2-TZVPP).\u2020<\/sup> The calculated NBO bond index at Ni is in fact 2.38 and the individual Ni-P bond orders are 0.37. The P bond indices are each 3.24 and the P-P bond orders are 0.88. The final electronic configuration is\u00a0[Ar]3d9.53<\/sup>.4s0.22<\/sup>.4p0.64<\/sup>.4d0.01<\/sup>.5p0.01 <\/sup> and the natural charge on Ni is\u00a0-0.39.\u00a0I show one NBO orbital which illustrates the two-electron-three-centre interaction spanning two P atoms and the Ni and giving rise to the modest Ni-P bond order.<\/p>\n

\"\"<\/p>\n

The Ni electronic structure of\u00a0[Ar<\/strong>].3d<\/strong>8<\/sup>.4s<\/strong>2<\/sup> normally corresponds to its divalency, so in this sense it is mildly hypervalent. Overall, representation 2<\/strong> above is perhaps more accurate than 3<\/strong>. The ELF (Electron localisation function) of the electron density is shown below (t-butyl groups represented by a single carbon) with the ELF basins highlighted. Basin 2 is a P lone pair, with an integration close to 2e. Basin 1 is a P-P basin with an integration of 1.89 and finally 3 is indeed a P-Ni basin, but with an integration of only 0.06e.\u00a0<\/p>\n

\"\"<\/p>\n

So this molecule really is a ring of six P atoms, encapsulating at its centre a lone Ni(II) atom. Rather than being hypervalent, perhaps it is most interesting as a complex in which a metal atom is contained in and perturbed by a dispersion-stabilized sphere of ligands.[2]<\/a><\/span><\/span> We need more examples!<\/p>\n

\n

\u2021<\/sup>The original authors[1]<\/a><\/span> merely stated that electron correlation effects are decisive for the stability. Of course, dispersion attractions are indeed a form of electron correlation! \u2020<\/sup>FAIR data doi: 10.14469\/hpc\/3925<\/a><\/p>\n

References<\/h2>\n
  1. R. Ahlrichs, D. Fenske, H. Oesen, and U. Schneider, \"Synthesis and Structure of [Ni(P<i>t<\/i>Bu<sub>6<\/sub>)] and [Ni<sub>5<\/sub>(P<i>t<\/i>Bu)<sub>6<\/sub>(CO)<sub>5<\/sub>] and Calculations on the Electronic Structure of [Ni(P<i>t<\/i>Bu)<sub>6<\/sub>] and (PR)<sub>6<\/sub>, R = <i>t<\/i>Bu,Me\", Angewandte Chemie International Edition in English<\/i>, vol. 31, pp. 323-326, 1992. https:\/\/doi.org\/10.1002\/anie.199203231<\/a>\n\n<\/li>\n
  2. https:\/\/doi.org\/<\/a>\n\n<\/li>\n<\/ol>\n\n<\/div> ","protected":false},"excerpt":{"rendered":"

    I have posted often on the chemical phenomenon known as hypervalency, being careful to state that as defined it applies just to “octet excess” in main group elements. But what about the next valence shell, occurring in transition metals and known as the “18-electron rule”? 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You rarely hear the term hypervalency being applied to such […]\" \/>\n<meta property=\"og:url\" content=\"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=19499\" \/>\n<meta property=\"og:site_name\" content=\"Henry Rzepa's Blog\" \/>\n<meta property=\"article:published_time\" content=\"2018-03-18T16:45:15+00:00\" \/>\n<meta property=\"article:modified_time\" content=\"2018-03-25T07:12:14+00:00\" \/>\n<meta property=\"og:image\" content=\"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2018\/03\/Ni-page001.svg\" \/>\n<meta name=\"author\" content=\"Henry Rzepa\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"Henry Rzepa\" \/>\n\t<meta name=\"twitter:label2\" content=\"Estimated reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"3 minutes\" \/>\n<!-- \/ Yoast SEO plugin. -->","yoast_head_json":{"title":"Never mind main group \"hypervalency\", what about transition metal \"hypervalency\"? - Henry Rzepa's Blog","robots":{"index":"index","follow":"follow","max-snippet":"max-snippet:-1","max-image-preview":"max-image-preview:large","max-video-preview":"max-video-preview:-1"},"canonical":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=19499","og_locale":"en_GB","og_type":"article","og_title":"Never mind main group \"hypervalency\", what about transition metal \"hypervalency\"? - Henry Rzepa's Blog","og_description":"I have posted often on the chemical phenomenon known as hypervalency, being careful to state that as defined it applies just to “octet excess” in main group elements. 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The definition there, \u00a0is \"a molecule that contains one or more\u00a0main group elements formally bearing more than eight\u00a0electrons in their\u00a0valence shells\" (although it could equally apply to e.g. transition elements\u2026","rel":"","context":"In "Hypervalency"","block_context":{"text":"Hypervalency","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=7"},"img":{"alt_text":"","src":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2010\/10\/IH7.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":1103,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=1103","url_meta":{"origin":19499,"position":1},"title":"Hypervalency: a reality check","author":"Henry Rzepa","date":"October 5, 2009","format":false,"excerpt":"We have seen in the series of posts on the topic of hypervalency\u00a0how the first row main group elements such as\u00a0Be, B, C and N can sustain apparent hypercoordination and arguably hypervalency. The latter is defined not so much by expanding the total valence shell of electrons surrounding the hypervalent\u2026","rel":"","context":"In "Hypervalency"","block_context":{"text":"Hypervalency","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=7"},"img":{"alt_text":"YOCVIV: Crystal structure of hexacoordinate boron","src":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2009\/10\/BBr.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":18975,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=18975","url_meta":{"origin":19499,"position":2},"title":"Hypervalence revisited. The odd case of hexamethyl selenium.","author":"Henry Rzepa","date":"November 7, 2017","format":false,"excerpt":"One thread that runs through this blog is that of hypervalency. It was therefore nice to come across a recent review of the concept which revisits the topic, and where a helpful summary is given of the evolving meanings over time of the term hypervalent. The key phrase \"it soon\u2026","rel":"","context":"In "Hypervalency"","block_context":{"text":"Hypervalency","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=7"},"img":{"alt_text":"","src":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2017\/11\/165-1024x1008.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":2619,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=2619","url_meta":{"origin":19499,"position":3},"title":"Hypervalency: I(CN)7 is not hypervalent!","author":"Henry Rzepa","date":"October 17, 2010","format":false,"excerpt":"In the last post, IH7 was examined to see if it might exhibit true hypervalency. The iodine, despite its high coordination, turned out not to be hypervalent, with its (s\/p) valence shell not exceeding eight electrons (and its d-shell still with 10, and the 6s\/6p shells largely unoccupied). Instead, 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":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2010\/10\/ICN7.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":19279,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=19279","url_meta":{"origin":19499,"position":4},"title":"Can any hypervalence in diazomethanes be amplified?","author":"Henry Rzepa","date":"December 23, 2017","format":false,"excerpt":"In the previous post, I referred to a recently published review on hypervalency which introduced a very simple way (the\u00a0valence electron equivalent \u03b3)\u00a0of quantifying the effect.\u00a0Diazomethane was cited as one example of a small molecule exhibiting hypervalency (on nitrogen) by this measure. Here I explore the effect of substituting diazomethane\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":[]},{"id":4479,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479","url_meta":{"origin":19499,"position":5},"title":"Hexavalent carbon revisited (and undecavalent boron thrown in).","author":"Henry Rzepa","date":"June 26, 2011","format":false,"excerpt":"A little while ago, I speculated (blogs are good for that sort of thing) about hexavalent carbon, and noted how one often needs to make (retrospectively) obvious connections between two different areas of chemistry. That post has attracted a number of comments in the two years its been up, along\u2026","rel":"","context":"In "Hypervalency"","block_context":{"text":"Hypervalency","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=7"},"img":{"alt_text":"","src":"https:\/\/i0.wp.com\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg?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\/19499","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=19499"}],"version-history":[{"count":20,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/19499\/revisions"}],"predecessor-version":[{"id":19538,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/19499\/revisions\/19538"}],"wp:attachment":[{"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fmedia&parent=19499"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fcategories&post=19499"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Ftags&post=19499"},{"taxonomy":"author","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fppma_author&post=19499"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}