{"id":3707,"date":"2019-04-23T13:05:44","date_gmt":"2019-04-23T13:05:44","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/chapter\/catalysis-2\/"},"modified":"2019-04-29T13:28:00","modified_gmt":"2019-04-29T13:28:00","slug":"catalysis-2","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/chapter\/catalysis-2\/","title":{"raw":"Catalysis","rendered":"Catalysis"},"content":{"raw":"<div class=\"bcc-box bcc-highlight\">\r\n<h3>Learning Objectives<\/h3>\r\n<ul>\r\n \t<li>To gain an understanding of homogenous, heterogenous, and biological catalysts.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<b>Catalysts<\/b> are substances that lower the activation energy of a specific reaction by providing an alternate reaction pathway. Catalysts participate in a reaction, but are not permanently changed in the process, as they are regenerated to their original state. Many scientists classify catalysts into one of three categories: homogeneous catalysts, heterogeneous catalysts, and biological catalysts (enzymes).\r\n<h2>Homogeneous Catalysts<\/h2>\r\nA <b>homogeneous catalyst<\/b> is any catalyst that is present in the same phase as the reactant molecules. There are numerous examples of homogeneous catalysts, and we will examine one that is commonly used in textbooks.\r\n\r\nThe alkene but-2-ene can exist as one of two isomers: <em>cis<\/em> where the methyl groups are located on the same side of the double bond, and <em>trans<\/em> where the methyl groups are located on opposite sides of the double bond (Figure 17.14 \"Isomerization of\u00a0But-2-ene\"). To convert (isomerize) between the two structures, the carbon-carbon double bond must be broken and the molecule must rotate. This process has a relatively high activation energy of approximately 264 kJ\/mol and is therefore fairly slow to occur at room temperature.\r\n\r\n<span class=\"Apple-style-span\">Figure17.14. Isomerization of But-2-ene<\/span>\r\n\r\n<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/but-2-ene-isomerization-large.png\"><img class=\"alignnone wp-image-1299\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130531\/but-2-ene-isomerization-large-1.png\" alt=\"Figure17.7.1. Isomerization of but-2-ene.\" width=\"400\" height=\"104\" \/><\/a>\r\n\r\n<span class=\"Apple-style-span\">But-2-ene can exist as one of two isomers. This diagram shows the isomerization of but-2-ene.<\/span>\r\n\r\nA catalyst like iodine can be used to provide an alternate pathway for the reaction with a much lower activation energy of approximately 118 kJ\/mol (Figures 17.15 \"Catalyzed and\u00a0Uncatalyzed\u00a0Reaction\u00a0Pathways\").\r\n\r\n<span class=\"Apple-style-span\">Figure 17.15. Catalyzed and Uncatalyzed Reaction Pathways<\/span>\r\n\r\n<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/catalyzed-vs-uncatalyzed-reaction-mechanism.jpg\"><img class=\"alignnone wp-image-1300 size-full\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130534\/catalyzed-vs-uncatalyzed-reaction-mechanism-1.jpg\" alt=\"Figure 17.7.2. Potential energy diagram of catalyzed vs uncatalyzed reaction pathway.\" width=\"406\" height=\"333\" \/><\/a>\r\n\r\n<span class=\"Apple-style-span\">Potential energy diagrams of catalyzed and uncatalyzed reaction pathways.<\/span>\r\n\r\nIn the catalyzed pathway, an iodine atom is generated that reacts with cis-but-2-ene to produce a reaction intermediate that\u00a0has broken its carbon-carbon double bond and formed a new C-I bond and a radical (Figure 17.16 \"But-2-ene\u00a0Catalyzed\u00a0Isomerization\u00a0Steps\"). The molecule can rotate more easily and the C-I breaks to reform the double bond.\r\n\r\n<span class=\"Apple-style-span\">Figure 17.16. But-2-ene Catalyzed Isomerization Steps<\/span>\r\n\r\n[caption id=\"attachment_1313\" align=\"alignnone\" width=\"400\"]<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/butene-catalysis-reaction-steps-ver-2.jpg\"><img class=\"wp-image-1313\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130537\/butene-catalysis-reaction-steps-ver-2-1.jpg\" alt=\"17.7.3. But-2-ene catalyzed isomerization steps.\" width=\"400\" height=\"135\" \/><\/a> But-2-ene catalyzed isomerization steps using iodine as the catalyst.[\/caption]\r\n<h2>Heterogeneous Catalysts<\/h2>\r\n<b>Heterogeneous catalysts<\/b> are those that are in a different phase from one or more of the reactants. Commonly solid metals and metal oxides are used to catalyze the reactions of gaseous or liquid reactants. Solid catalysts often serve as a surface on which\u00a0reactions can\u00a0occur, where one or more reactants will <b>adsorb<\/b> (bind to the surface) to the solid.\r\n\r\nA common example of heterogeneous catalysis is the hydrogenation reaction of simple alkenes. The conversion of ethene (C<sub>2<\/sub>H<sub>4<\/sub>) to ethane (C<sub>2<\/sub>H<sub>6<\/sub>) can be performed with hydrogen gas in the presence of a metal catalyst such as palladium (Figure 17.17 \"Conversion of\u00a0Ethene to\u00a0Ethane with Hydrogen and a Metal Catalyst\").\r\n\r\nC<sub>2<\/sub>H<sub>4<\/sub>(g) + H<sub>2<\/sub>(g) \u2192\u00a0C<sub>2<\/sub>H<sub>6<\/sub>(g)\r\n\r\n<span class=\"Apple-style-span\">Figure 17.17 Conversion of Ethene to Ethane with Hydrogen and a Metal Catalyst<\/span>\r\n\r\n[caption id=\"attachment_1312\" align=\"alignnone\" width=\"401\"]<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/heterogeneous-catalysis.jpg\"><img class=\"size-full wp-image-1312\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130540\/heterogeneous-catalysis-1.jpg\" alt=\"Figure 17.7.4. Heterogeneous catalysis mechanisms of reaction for ethene with hydrogen on a catalytic metal surface.\" width=\"401\" height=\"360\" \/><\/a> Heterogeneous catalysis mechanisms of reaction for ethene with hydrogen on a catalytic metal surface[\/caption]\r\n\r\nEthene and hydrogen adsorb onto the metal surface, where the H<sub>2<\/sub> breaks into two individual hydrogen atoms bonded to the metal surface. A reaction occurs between adjacent ethene and hydrogen atoms on the metal surface, first to generate a C<sub>2<\/sub>H<sub>5<\/sub> intermediate, then to generate ethane, C<sub>2<\/sub>H<sub>6<\/sub>, which desorbs from the surface.\r\n<h2>Biological Catalysts<\/h2>\r\nCatalysts within living things facilitate the vast and intricate system of chemical reactions required for life. There are two main types of naturally occurring catalytic biomolecules: ribozymes and enzymes.\r\n\r\n<strong>Ribozymes<\/strong> are ribonucleic acid (RNA) molecules capable of catalyzing certain chemical reactions. Ribozymes are a relatively recent discovery, first reported in 1982, but their importance was demonstrated by the awarding of the 1989 Nobel Prize to the discoverers Sidney Altman and Thomas Cech. Research is ongoing to better understand these catalysts and develop new therapeutics and medicines using them.\r\n\r\n<strong>Enzymes<\/strong> are protein molecules that\u00a0catalyze biochemical reactions. They are remarkably specific for the reactants they can use, known as <b>substrates, <\/b>and many dramatically increase reaction rate by factors of 10<sup>7<\/sup> to 10<sup>14<\/sup>. A simple model often used to describe enzyme activity is known as the lock-and-key model (Figure 17.18 \"Lock-and-Key Model of Enzymatic Catalysis\"). In this model, enzymes accelerate reactions by providing a tight-fitting area, known as the\u00a0<b>active site,<\/b> where substrate molecules can react. Hydrophobicity and intermolecular forces such as hydrogen bonding, London-dispersion forces, and dipole-dipole interactions facilitate the binding of substrate molecules to the active site, forming an <b>enzyme-substrate complex<\/b>. When the\u00a0reaction is completed\u00a0at the active site, the product is released.\r\n\r\n<span class=\"Apple-style-span\">Figure 17.18. Lock-and-Key Model of Enzymatic Catalysis<\/span>\r\n\r\n<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/Enzyme_mechanism_1.jpg\"><img class=\"alignnone wp-image-1317\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130542\/Enzyme_mechanism_1-1.jpg\" alt=\"Figure 17.7.5. &quot;Lock-and-Key&quot; model of enzymatic catalysis.\" width=\"400\" height=\"155\" \/><\/a>\r\n\r\n<span class=\"Apple-style-span\">Lock-and-key model of enzymatic catalysis showing the tight-fitting area where substrate molecules react.<\/span>[footnote]\"Enzyme mechanism\" by Aejahnke\/CC-BY-SA-3.0[\/footnote]\r\n<div class=\"bcc-box bcc-success\">\r\n<h3>Key Takeaways<\/h3>\r\n<ul>\r\n \t<li>Catalysts provide an alternate, lower-energy reaction pathway.<\/li>\r\n \t<li>A\u00a0homogeneous catalyst\u00a0is any catalyst that is present in the same phase as the reactant molecules.<\/li>\r\n \t<li>Heterogeneous catalysts\u00a0are in a different phase from one or more of the reactants, and often act as a surface on which\u00a0the reaction can\u00a0occur.<\/li>\r\n \t<li>According to the lock-and-key model,\u00a0enzymes accelerate reactions by providing a tight-fitting area, where substrate molecules can react.<\/li>\r\n<\/ul>\r\n<\/div>","rendered":"<div class=\"bcc-box bcc-highlight\">\n<h3>Learning Objectives<\/h3>\n<ul>\n<li>To gain an understanding of homogenous, heterogenous, and biological catalysts.<\/li>\n<\/ul>\n<\/div>\n<p><b>Catalysts<\/b> are substances that lower the activation energy of a specific reaction by providing an alternate reaction pathway. Catalysts participate in a reaction, but are not permanently changed in the process, as they are regenerated to their original state. Many scientists classify catalysts into one of three categories: homogeneous catalysts, heterogeneous catalysts, and biological catalysts (enzymes).<\/p>\n<h2>Homogeneous Catalysts<\/h2>\n<p>A <b>homogeneous catalyst<\/b> is any catalyst that is present in the same phase as the reactant molecules. There are numerous examples of homogeneous catalysts, and we will examine one that is commonly used in textbooks.<\/p>\n<p>The alkene but-2-ene can exist as one of two isomers: <em>cis<\/em> where the methyl groups are located on the same side of the double bond, and <em>trans<\/em> where the methyl groups are located on opposite sides of the double bond (Figure 17.14 &#8220;Isomerization of\u00a0But-2-ene&#8221;). To convert (isomerize) between the two structures, the carbon-carbon double bond must be broken and the molecule must rotate. This process has a relatively high activation energy of approximately 264 kJ\/mol and is therefore fairly slow to occur at room temperature.<\/p>\n<p><span class=\"Apple-style-span\">Figure17.14. Isomerization of But-2-ene<\/span><\/p>\n<p><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/but-2-ene-isomerization-large.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-1299\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130531\/but-2-ene-isomerization-large-1.png\" alt=\"Figure17.7.1. Isomerization of but-2-ene.\" width=\"400\" height=\"104\" \/><\/a><\/p>\n<p><span class=\"Apple-style-span\">But-2-ene can exist as one of two isomers. This diagram shows the isomerization of but-2-ene.<\/span><\/p>\n<p>A catalyst like iodine can be used to provide an alternate pathway for the reaction with a much lower activation energy of approximately 118 kJ\/mol (Figures 17.15 &#8220;Catalyzed and\u00a0Uncatalyzed\u00a0Reaction\u00a0Pathways&#8221;).<\/p>\n<p><span class=\"Apple-style-span\">Figure 17.15. Catalyzed and Uncatalyzed Reaction Pathways<\/span><\/p>\n<p><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/catalyzed-vs-uncatalyzed-reaction-mechanism.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-1300 size-full\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130534\/catalyzed-vs-uncatalyzed-reaction-mechanism-1.jpg\" alt=\"Figure 17.7.2. Potential energy diagram of catalyzed vs uncatalyzed reaction pathway.\" width=\"406\" height=\"333\" \/><\/a><\/p>\n<p><span class=\"Apple-style-span\">Potential energy diagrams of catalyzed and uncatalyzed reaction pathways.<\/span><\/p>\n<p>In the catalyzed pathway, an iodine atom is generated that reacts with cis-but-2-ene to produce a reaction intermediate that\u00a0has broken its carbon-carbon double bond and formed a new C-I bond and a radical (Figure 17.16 &#8220;But-2-ene\u00a0Catalyzed\u00a0Isomerization\u00a0Steps&#8221;). The molecule can rotate more easily and the C-I breaks to reform the double bond.<\/p>\n<p><span class=\"Apple-style-span\">Figure 17.16. But-2-ene Catalyzed Isomerization Steps<\/span><\/p>\n<div id=\"attachment_1313\" style=\"width: 410px\" class=\"wp-caption alignnone\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/butene-catalysis-reaction-steps-ver-2.jpg\"><img loading=\"lazy\" decoding=\"async\" aria-describedby=\"caption-attachment-1313\" class=\"wp-image-1313\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130537\/butene-catalysis-reaction-steps-ver-2-1.jpg\" alt=\"17.7.3. But-2-ene catalyzed isomerization steps.\" width=\"400\" height=\"135\" \/><\/a><\/p>\n<p id=\"caption-attachment-1313\" class=\"wp-caption-text\">But-2-ene catalyzed isomerization steps using iodine as the catalyst.<\/p>\n<\/div>\n<h2>Heterogeneous Catalysts<\/h2>\n<p><b>Heterogeneous catalysts<\/b> are those that are in a different phase from one or more of the reactants. Commonly solid metals and metal oxides are used to catalyze the reactions of gaseous or liquid reactants. Solid catalysts often serve as a surface on which\u00a0reactions can\u00a0occur, where one or more reactants will <b>adsorb<\/b> (bind to the surface) to the solid.<\/p>\n<p>A common example of heterogeneous catalysis is the hydrogenation reaction of simple alkenes. The conversion of ethene (C<sub>2<\/sub>H<sub>4<\/sub>) to ethane (C<sub>2<\/sub>H<sub>6<\/sub>) can be performed with hydrogen gas in the presence of a metal catalyst such as palladium (Figure 17.17 &#8220;Conversion of\u00a0Ethene to\u00a0Ethane with Hydrogen and a Metal Catalyst&#8221;).<\/p>\n<p>C<sub>2<\/sub>H<sub>4<\/sub>(g) + H<sub>2<\/sub>(g) \u2192\u00a0C<sub>2<\/sub>H<sub>6<\/sub>(g)<\/p>\n<p><span class=\"Apple-style-span\">Figure 17.17 Conversion of Ethene to Ethane with Hydrogen and a Metal Catalyst<\/span><\/p>\n<div id=\"attachment_1312\" style=\"width: 411px\" class=\"wp-caption alignnone\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/heterogeneous-catalysis.jpg\"><img loading=\"lazy\" decoding=\"async\" aria-describedby=\"caption-attachment-1312\" class=\"size-full wp-image-1312\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130540\/heterogeneous-catalysis-1.jpg\" alt=\"Figure 17.7.4. Heterogeneous catalysis mechanisms of reaction for ethene with hydrogen on a catalytic metal surface.\" width=\"401\" height=\"360\" \/><\/a><\/p>\n<p id=\"caption-attachment-1312\" class=\"wp-caption-text\">Heterogeneous catalysis mechanisms of reaction for ethene with hydrogen on a catalytic metal surface<\/p>\n<\/div>\n<p>Ethene and hydrogen adsorb onto the metal surface, where the H<sub>2<\/sub> breaks into two individual hydrogen atoms bonded to the metal surface. A reaction occurs between adjacent ethene and hydrogen atoms on the metal surface, first to generate a C<sub>2<\/sub>H<sub>5<\/sub> intermediate, then to generate ethane, C<sub>2<\/sub>H<sub>6<\/sub>, which desorbs from the surface.<\/p>\n<h2>Biological Catalysts<\/h2>\n<p>Catalysts within living things facilitate the vast and intricate system of chemical reactions required for life. There are two main types of naturally occurring catalytic biomolecules: ribozymes and enzymes.<\/p>\n<p><strong>Ribozymes<\/strong> are ribonucleic acid (RNA) molecules capable of catalyzing certain chemical reactions. Ribozymes are a relatively recent discovery, first reported in 1982, but their importance was demonstrated by the awarding of the 1989 Nobel Prize to the discoverers Sidney Altman and Thomas Cech. Research is ongoing to better understand these catalysts and develop new therapeutics and medicines using them.<\/p>\n<p><strong>Enzymes<\/strong> are protein molecules that\u00a0catalyze biochemical reactions. They are remarkably specific for the reactants they can use, known as <b>substrates, <\/b>and many dramatically increase reaction rate by factors of 10<sup>7<\/sup> to 10<sup>14<\/sup>. A simple model often used to describe enzyme activity is known as the lock-and-key model (Figure 17.18 &#8220;Lock-and-Key Model of Enzymatic Catalysis&#8221;). In this model, enzymes accelerate reactions by providing a tight-fitting area, known as the\u00a0<b>active site,<\/b> where substrate molecules can react. Hydrophobicity and intermolecular forces such as hydrogen bonding, London-dispersion forces, and dipole-dipole interactions facilitate the binding of substrate molecules to the active site, forming an <b>enzyme-substrate complex<\/b>. When the\u00a0reaction is completed\u00a0at the active site, the product is released.<\/p>\n<p><span class=\"Apple-style-span\">Figure 17.18. Lock-and-Key Model of Enzymatic Catalysis<\/span><\/p>\n<p><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/05\/Enzyme_mechanism_1.jpg\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-1317\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/4084\/2019\/04\/23130542\/Enzyme_mechanism_1-1.jpg\" alt=\"Figure 17.7.5. &quot;Lock-and-Key&quot; model of enzymatic catalysis.\" width=\"400\" height=\"155\" \/><\/a><\/p>\n<p><span class=\"Apple-style-span\">Lock-and-key model of enzymatic catalysis showing the tight-fitting area where substrate molecules react.<\/span><a class=\"footnote\" title=\"&quot;Enzyme mechanism&quot; by Aejahnke\/CC-BY-SA-3.0\" id=\"return-footnote-3707-1\" href=\"#footnote-3707-1\" aria-label=\"Footnote 1\"><sup class=\"footnote\">[1]<\/sup><\/a><\/p>\n<div class=\"bcc-box bcc-success\">\n<h3>Key Takeaways<\/h3>\n<ul>\n<li>Catalysts provide an alternate, lower-energy reaction pathway.<\/li>\n<li>A\u00a0homogeneous catalyst\u00a0is any catalyst that is present in the same phase as the reactant molecules.<\/li>\n<li>Heterogeneous catalysts\u00a0are in a different phase from one or more of the reactants, and often act as a surface on which\u00a0the reaction can\u00a0occur.<\/li>\n<li>According to the lock-and-key model,\u00a0enzymes accelerate reactions by providing a tight-fitting area, where substrate molecules can react.<\/li>\n<\/ul>\n<\/div>\n\n\t\t\t <section class=\"citations-section\" role=\"contentinfo\">\n\t\t\t <h3>Candela Citations<\/h3>\n\t\t\t\t\t <div>\n\t\t\t\t\t\t <div id=\"citation-list-3707\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Original<\/div><ul class=\"citation-list\"><li><strong>Authored by<\/strong>: Jessie A. Key. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/opentextbc.ca\/introductorychemistry\/\">https:\/\/opentextbc.ca\/introductorychemistry\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc-sa\/4.0\/\">CC BY-NC-SA: Attribution-NonCommercial-ShareAlike<\/a><\/em><\/li><\/ul><\/div>\n\t\t\t\t\t\t <\/div>\n\t\t\t\t\t <\/div>\n\t\t\t <\/section><hr class=\"before-footnotes clear\" \/><div class=\"footnotes\"><ol><li id=\"footnote-3707-1\">\"Enzyme mechanism\" by Aejahnke\/CC-BY-SA-3.0 <a href=\"#return-footnote-3707-1\" class=\"return-footnote\" aria-label=\"Return to footnote 1\">&crarr;<\/a><\/li><\/ol><\/div>","protected":false},"author":89971,"menu_order":8,"template":"","meta":{"_candela_citation":"[{\"type\":\"original\",\"description\":\"\",\"author\":\"Jessie A. Key\",\"organization\":\"\",\"url\":\"https:\/\/opentextbc.ca\/introductorychemistry\/\",\"project\":\"\",\"license\":\"cc-by-nc-sa\",\"license_terms\":\"\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":["jessie-a-key"],"pb_section_license":"cc-by"},"chapter-type":[],"contributor":[59],"license":[50],"class_list":["post-3707","chapter","type-chapter","status-publish","hentry","contributor-jessie-a-key","license-cc-by"],"part":3670,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/3707","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/wp\/v2\/users\/89971"}],"version-history":[{"count":2,"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/3707\/revisions"}],"predecessor-version":[{"id":3887,"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/3707\/revisions\/3887"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/pressbooks\/v2\/parts\/3670"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/3707\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/wp\/v2\/media?parent=3707"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=3707"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/wp\/v2\/contributor?post=3707"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/wp-json\/wp\/v2\/license?post=3707"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}