{"id":4479,"date":"2011-06-26T18:30:55","date_gmt":"2011-06-26T18:30:55","guid":{"rendered":"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/?p=4479"},"modified":"2011-06-27T06:35:38","modified_gmt":"2011-06-27T06:35:38","slug":"hexavalent-carbon-revisited","status":"publish","type":"post","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479","title":{"rendered":"Hexavalent carbon revisited (and undecavalent boron thrown in)."},"content":{"rendered":"<div class=\"kcite-section\" kcite-section-id=\"4479\">\n<p>A little while ago, <a href=\"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/?p=878\" target=\"_blank\">I speculated<\/a> (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 the lines: <em>what about carboranes?<\/em> So here I have decided to explore that portal into boron chemistry. The starting point is the reported crystal structure of a molecule containing a CH<sub>12<\/sub>B<sub>11<\/sub><sup>&#8211; <\/sup>anion<sup> <\/sup>(DOI:\u00a0<a href=\"http:\/\/dx.doi.org\/10.1021\/ja00201a073\" target=\"_blank\">10.1021\/ja00201a073<\/a>). This differs from the molecule I previously reported in having not so much 5C-C + 1C-H bonds around a single carbon, but instead 5B-C + 1C-H bonds. The basic cluster is much in fashion (as\u00a0B<sub>12<\/sub>Cl<sub>12<\/sub><sup>2-<\/sup>) for its properties as a non-coordinating counterion.<\/p>\n<p><div id=\"attachment_4483\" style=\"width: 229px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" aria-describedby=\"caption-attachment-4483\" class=\"size-full wp-image-4483 \" title=\"CB11\" onclick=\"jmolInitialize('..\/Jmol\/',true);jmolSetAppletColor('white');jmolApplet([450,450],'load wp-content\/uploads\/2011\/06\/VEFMAU-aim.mol;');\" src=\"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg\" alt=\"\" width=\"219\" height=\"217\" srcset=\"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg 365w, https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11-150x150.jpg 150w, https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11-300x297.jpg 300w\" sizes=\"auto, (max-width: 219px) 100vw, 219px\" \/><p id=\"caption-attachment-4483\" class=\"wp-caption-text\">The CH12B11 (-) anion. AIM analysis. Click for 3D.<\/p><\/div>Above is the QTAIM topological analysis of the electron density (<a href=\"http:\/\/hdl.handle.net\/10042\/to-9118\" target=\"_blank\">B3LYP\/6-311G(d,p) calculation<\/a>) which reveals all 11 borons and the single carbon atom as being surrounded by six bond critical points. ELF tells us how many electrons populate the synaptic basins.<\/p>\n<p><div id=\"attachment_4489\" style=\"width: 341px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" aria-describedby=\"caption-attachment-4489\" class=\"size-full wp-image-4489 \" title=\"CB11-elf\" onclick=\"jmolInitialize('..\/Jmol\/',true);jmolSetAppletColor('white');jmolApplet([450,450],'load wp-content\/uploads\/2011\/06\/CB11.mol;');\" src=\"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11-elf.jpg\" alt=\"\" width=\"331\" height=\"335\" srcset=\"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11-elf.jpg 551w, https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11-elf-295x300.jpg 295w\" sizes=\"auto, (max-width: 331px) 100vw, 331px\" \/><p id=\"caption-attachment-4489\" class=\"wp-caption-text\">The CH12B11 (-) anion ELF basins. Click for 3D.<\/p><\/div>This clearly reveals that the bonding to the carbon and all the boron atoms is non-Lewis, <em>i.e.<\/em> that of the six bonds to each of the non-hydrogens, five are not of the Lewis two-electron pair type. The carbon for example is surrounded by five C-B basins, each of 1.02e, with its valence shell occupied by ~7.2e in total. The boron involved in each of the C-B bonds also has five bonds, with basins corresponding to 1.01, 2*0.95 and 2*0.73e. The boron directly opposite the carbon has five basins corresponding to five B-B two-centre bonds of 0.6e each, and a further five basins of 0.3e corresponding to 3-centre BBB bonds (shown as yellow spheres above). Arguably, that particular boron atom has eleven bonds to it!<\/p>\n<p>This molecule reveals quite clearly how sterile the debate is about whether carbon can be hypervalent.\u00a0If the Lewis definition of a bond as an electron pair is removed, then hypervalency exceeding four can easily be obtained. What is certainly sacrosanct is the valence shell octet for carbon (and boron).<\/p>\n<p>Finally, I throw\u00a0<a href=\"http:\/\/hdl.handle.net\/10042\/to-9119\" target=\"_blank\">B<sub>12<\/sub>H<sub>12<\/sub><sup>2-<\/sup><\/a> in. This has the wonderful icosahedral symmetry, and as you might expect, each boron is defined by five two-centre B-B bonds (~0.66e) and five three-centre BBB bonds (~0.24e), as well as a conventional two-electron B-H bond. Each boron is <strong>undecavalent<\/strong>! Not seen that particular valency before!!<\/p>\n<!-- kcite active, but no citations found -->\n<\/div> <!-- kcite-section 4479 -->","protected":false},"excerpt":{"rendered":"<p>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 the lines: what about carboranes? [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_jetpack_newsletter_access":"","_jetpack_dont_email_post_to_subs":false,"_jetpack_newsletter_tier_id":0,"_jetpack_memberships_contains_paywalled_content":false,"_jetpack_memberships_contains_paid_content":false,"activitypub_content_warning":"","activitypub_content_visibility":"","activitypub_max_image_attachments":5,"activitypub_interaction_policy_quote":"anyone","activitypub_status":"","footnotes":"","jetpack_publicize_message":"","jetpack_publicize_feature_enabled":true,"jetpack_social_post_already_shared":false,"jetpack_social_options":{"image_generator_settings":{"template":"highway","default_image_id":0,"font":"","enabled":false},"version":2},"jetpack_post_was_ever_published":false},"categories":[7],"tags":[11,571],"ppma_author":[2661],"class_list":["post-4479","post","type-post","status-publish","format-standard","hentry","category-hypervalency","tag-elf","tag-qtaim"],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v27.6 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Hexavalent carbon revisited (and undecavalent boron thrown in). - Henry Rzepa&#039;s Blog<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479\" \/>\n<meta property=\"og:locale\" content=\"en_GB\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Hexavalent carbon revisited (and undecavalent boron thrown in). - Henry Rzepa&#039;s Blog\" \/>\n<meta property=\"og:description\" content=\"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 the lines: what about carboranes? [&hellip;]\" \/>\n<meta property=\"og:url\" content=\"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479\" \/>\n<meta property=\"og:site_name\" content=\"Henry Rzepa&#039;s Blog\" \/>\n<meta property=\"article:published_time\" content=\"2011-06-26T18:30:55+00:00\" \/>\n<meta property=\"article:modified_time\" content=\"2011-06-27T06:35:38+00:00\" \/>\n<meta property=\"og:image\" content=\"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg\" \/>\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=\"2 minutes\" \/>\n<!-- \/ Yoast SEO plugin. -->","yoast_head_json":{"title":"Hexavalent carbon revisited (and undecavalent boron thrown in). - Henry Rzepa&#039;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=4479","og_locale":"en_GB","og_type":"article","og_title":"Hexavalent carbon revisited (and undecavalent boron thrown in). - Henry Rzepa&#039;s Blog","og_description":"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 the lines: what about carboranes? [&hellip;]","og_url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479","og_site_name":"Henry Rzepa&#039;s Blog","article_published_time":"2011-06-26T18:30:55+00:00","article_modified_time":"2011-06-27T06:35:38+00:00","og_image":[{"url":"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg","type":"","width":"","height":""}],"author":"Henry Rzepa","twitter_card":"summary_large_image","twitter_misc":{"Written by":"Henry Rzepa","Estimated reading time":"2 minutes"},"schema":{"@context":"https:\/\/schema.org","@graph":[{"@type":"Article","@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#article","isPartOf":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479"},"author":{"name":"Henry Rzepa","@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/#\/schema\/person\/2b40f7b9c872a4dc1547e040a11b6281"},"headline":"Hexavalent carbon revisited (and undecavalent boron thrown in).","datePublished":"2011-06-26T18:30:55+00:00","dateModified":"2011-06-27T06:35:38+00:00","mainEntityOfPage":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479"},"wordCount":443,"commentCount":1,"image":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#primaryimage"},"thumbnailUrl":"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg","keywords":["ELF","QTAIM"],"articleSection":["Hypervalency"],"inLanguage":"en-GB","potentialAction":[{"@type":"CommentAction","name":"Comment","target":["https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#respond"]}]},{"@type":"WebPage","@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479","url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479","name":"Hexavalent carbon revisited (and undecavalent boron thrown in). - Henry Rzepa&#039;s Blog","isPartOf":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/#website"},"primaryImageOfPage":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#primaryimage"},"image":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#primaryimage"},"thumbnailUrl":"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg","datePublished":"2011-06-26T18:30:55+00:00","dateModified":"2011-06-27T06:35:38+00:00","author":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/#\/schema\/person\/2b40f7b9c872a4dc1547e040a11b6281"},"breadcrumb":{"@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#breadcrumb"},"inLanguage":"en-GB","potentialAction":[{"@type":"ReadAction","target":["https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479"]}]},{"@type":"ImageObject","inLanguage":"en-GB","@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#primaryimage","url":"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg","contentUrl":"http:\/\/www.ch.imperial.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2011\/06\/CB11.jpg"},{"@type":"BreadcrumbList","@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4479#breadcrumb","itemListElement":[{"@type":"ListItem","position":1,"name":"Home","item":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog"},{"@type":"ListItem","position":2,"name":"Hexavalent carbon revisited (and undecavalent boron thrown in)."}]},{"@type":"WebSite","@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/#website","url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/","name":"Henry Rzepa&#039;s Blog","description":"Chemistry with a twist","potentialAction":[{"@type":"SearchAction","target":{"@type":"EntryPoint","urlTemplate":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?s={search_term_string}"},"query-input":{"@type":"PropertyValueSpecification","valueRequired":true,"valueName":"search_term_string"}}],"inLanguage":"en-GB"},{"@type":"Person","@id":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/#\/schema\/person\/2b40f7b9c872a4dc1547e040a11b6281","name":"Henry Rzepa","image":{"@type":"ImageObject","inLanguage":"en-GB","@id":"https:\/\/secure.gravatar.com\/avatar\/897b6740f7f599bca7942cdf7d7914af5988937ae0e3869ab09aebb87f26a731?s=96&d=blank&r=g370be3a7397865e4fd161aefeb0a5a85","url":"https:\/\/secure.gravatar.com\/avatar\/897b6740f7f599bca7942cdf7d7914af5988937ae0e3869ab09aebb87f26a731?s=96&d=blank&r=g","contentUrl":"https:\/\/secure.gravatar.com\/avatar\/897b6740f7f599bca7942cdf7d7914af5988937ae0e3869ab09aebb87f26a731?s=96&d=blank&r=g","caption":"Henry Rzepa"},"description":"Henry Rzepa is Emeritus Professor of Computational Chemistry at Imperial College London.","sameAs":["https:\/\/orcid.org\/0000-0002-8635-8390"],"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?author=1"}]}},"jetpack_publicize_connections":[],"jetpack_featured_media_url":"","jetpack_sharing_enabled":true,"jetpack_shortlink":"https:\/\/wp.me\/pDef7-1af","jetpack-related-posts":[{"id":961,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=961","url_meta":{"origin":4479,"position":0},"title":"Pentavalent nitrogen and boron","author":"Henry Rzepa","date":"October 3, 2009","format":false,"excerpt":"The previous posts have seen how a molecule containing a hypervalent carbon atom can be designed by making a series of logical chemical connections. Another logical step is to investigate whether the adjacent atoms in the periodic table may exhibit similar effects (C2+ \u2261 B+ \u2261 N3+ \u2261 Be \u2261\u2026","rel":"","context":"In &quot;Hypervalency&quot;","block_context":{"text":"Hypervalency","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=7"},"img":{"alt_text":"Pentavalency across a series","src":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2009\/10\/C4.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":878,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=878","url_meta":{"origin":4479,"position":1},"title":"It&#8217;s Hexa-coordinate carbon Spock &#8211; but not as we know it!","author":"Henry Rzepa","date":"October 2, 2009","format":false,"excerpt":"Science is about making connections. And these can often be made between the most unlikely concepts. Thus in the posts I have made about pentavalent carbon, one can identify a series of conceptual connections. The\u00a0first, by Matthias\u00a0Bickelhaupt and co, resulted in the suggestion of a possible frozen\u00a0SN2 transition state. They\u2026","rel":"","context":"In &quot;Hypervalency&quot;","block_context":{"text":"Hypervalency","link":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?cat=7"},"img":{"alt_text":"The HOMO orbital","src":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2009\/09\/C5-homo1.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":2469,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=2469","url_meta":{"origin":4479,"position":2},"title":"Solid carbon dioxide: hexacoordinate carbon?","author":"Henry Rzepa","date":"September 17, 2010","format":false,"excerpt":"Carbon dioxide is much in the news, not least because its atmospheric concentration is on the increase. How to sequester it and save the planet is a hot topic. Here I ponder its solid state structure, as a hint to its possible reactivity, and hence perhaps for clues as to\u2026","rel":"","context":"In &quot;Hypervalency&quot;","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\/09\/CO2-solid.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":4719,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=4719","url_meta":{"origin":4479,"position":3},"title":"A stable borylene. An exercise in lateral thinking.","author":"Henry Rzepa","date":"August 7, 2011","format":false,"excerpt":"I have often heard the question posed \"how much of chemistry has been discovered?\" Another might be \"has most of chemistry, like low-hanging fruit, already been picked?\". Well, time and time again, one comes across examples which are only a simple diagram or so away from what might be found\u2026","rel":"","context":"In &quot;Interesting chemistry&quot;","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\/2011\/08\/borylene.jpg?resize=350%2C200","width":350,"height":200},"classes":[]},{"id":21798,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=21798","url_meta":{"origin":4479,"position":4},"title":"Can a carbon radical act as a hydrogen bond acceptor?","author":"Henry Rzepa","date":"December 28, 2019","format":false,"excerpt":"Having shown that carbon as a carbene centre, C:\u00a0can act as a hydrogen bond acceptor, as seen from a search of crystal structures, I began to wonder if there is any chance that carbon as a radical centre, C\u2022 could do so as well.\u00a0Definitely a subversive thought, since radical centres\u2026","rel":"","context":"In &quot;crystal_structure_mining&quot;","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\/2019\/12\/CH-1024x940.jpg?resize=350%2C200&ssl=1","width":350,"height":200},"classes":[]},{"id":26962,"url":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/?p=26962","url_meta":{"origin":4479,"position":5},"title":"Detecting anomeric effects in tetrahedral boron bearing four oxygen substituents.","author":"Henry Rzepa","date":"April 30, 2024","format":false,"excerpt":"In an earlier post, I discussed a phenomenon known as the \"anomeric effect\" exhibited by tetrahedral carbon compounds with four C-O bonds. Each oxygen itself bears two bonds and has two lone pairs, and either of these can align with one of three other C-O bonds to generate an anomeric\u2026","rel":"","context":"Similar post","block_context":{"text":"Similar post","link":""},"img":{"alt_text":"","src":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2024\/04\/Screenshot-304.jpg?resize=350%2C200&ssl=1","width":350,"height":200,"srcset":"https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2024\/04\/Screenshot-304.jpg?resize=350%2C200&ssl=1 1x, https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2024\/04\/Screenshot-304.jpg?resize=525%2C300&ssl=1 1.5x, https:\/\/i0.wp.com\/www.ch.ic.ac.uk\/rzepa\/blog\/wp-content\/uploads\/2024\/04\/Screenshot-304.jpg?resize=700%2C400&ssl=1 2x"},"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\/4479","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=4479"}],"version-history":[{"count":0,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=\/wp\/v2\/posts\/4479\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fmedia&parent=4479"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fcategories&post=4479"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Ftags&post=4479"},{"taxonomy":"author","embeddable":true,"href":"https:\/\/www.ch.ic.ac.uk\/rzepa\/blog\/index.php?rest_route=%2Fwp%2Fv2%2Fppma_author&post=4479"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}