{"id":2803,"date":"2016-08-24T18:33:02","date_gmt":"2016-08-24T18:33:02","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=2803"},"modified":"2017-08-28T22:55:59","modified_gmt":"2017-08-28T22:55:59","slug":"metallic-bonding","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/metallic-bonding\/","title":{"raw":"Metallic Bonding","rendered":"Metallic Bonding"},"content":{"raw":"<h1 id=\"x-ck12-SW9uaWMgYW5kIE1ldGFsbGljIEJvbmRpbmc.-chapter\">Ionic and Metallic Bonding<\/h1>\r\n<div class=\"x-ck12-data\"><\/div>\r\n<h1 id=\"x-ck12-RWxlY3Ryb24gRG90IERpYWdyYW1z\">Metallic Bonding<\/h1>\r\n<div class=\"x-ck12-data-objectives\">\r\n<ul id=\"x-ck12-MTczNmI2OTg1ODMzYTViMTQ0YmQ4ZTE5NWY1MTFmYjY.-bua\">\r\n \t<li>Define metallic bond.<\/li>\r\n \t<li>Describe properties of metals.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<p id=\"x-ck12-OTRiM2FiZmFlZGZmNjM0ZTAzMzFlZmFhNjFlMjgwYjU.-zsx\"><span class=\"x-ck12-img-inline\"><img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211415\/20140811155233583262.jpg\" alt=\"A copper plate has unique metallic properties\" width=\"200\" \/><\/span><\/p>\r\n<p id=\"x-ck12-MTA4ZTAxMGI3MzJmMTQzNDlmZDFmYmI2OTFmNjJkM2M.-viq\"><strong>Why do metals behave the way they do?<\/strong><\/p>\r\n<p id=\"x-ck12-NDhhYTc0ZDc2YTcyMDA1YjU4MzJlMjg5NjZmM2Y2MWM.-5uk\">The image above is of a copper plate that was made in 1893.\u00a0 The utensil has a great deal of elaborate decoration and the item is very useful.\u00a0 What would have happened if we decided that copper (I) chloride was just as good a material (well, it does have copper in it).\u00a0 The CuCl would end up as a powder when we pounded on it to shape it.\u00a0 Metals behave in unique ways. The bonding that occurs in a metal is responsible for its distinctive properties: luster, malleability, ductility, and excellent conductivity.<\/p>\r\n\r\n<h3>The Metallic Bond<\/h3>\r\n<p id=\"x-ck12-MGJlMjMyY2ZhYTkxYWU1NjUwZjVmNjQzNmUzOWJiOTc.-iv0\">Pure metals are crystalline solids, but unlike ionic compounds, every point in the crystal lattice is occupied by an identical atom.\u00a0 The electrons in the outer energy levels of a metal are mobile and capable of drifting from one metal atom to another.\u00a0 This means that the metal is more properly viewed as an array of positive ions surrounded by a sea of mobile valence electrons.\u00a0 Electrons which are capable of moving freely throughout the empty orbitals of the metallic crystal are called <strong>delocalized electrons <\/strong>(see <strong>Figure <\/strong>below ).\u00a0 A <strong>metallic bond <\/strong>is the attraction of the stationary metal cations to the surrounding mobile electrons.<\/p>\r\n\r\n<div id=\"x-ck12-MGE1M2U5YmEyMTY0NTdhODM1NWJhYWQwODNlOTU5Mzc.-t8o\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n<p id=\"x-ck12-tkq\"><img id=\"x-ck12-OTgwNDUtMTM2MjAxMTE5NS0wLTktQ2hlbUpSU19DaDE2X21ldGFsbGljYm9uZF9DQQ..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211416\/20140811155233745745.png\" alt=\"Diagram of metallic bonding\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/In%20a%20metal%2C%20the%20stationary%20metal%20cations%20are%20surrounded%20by%20a%20sea%20of%20mobile%20valence%20electrons%20that%20are%20not%20associated%20with%20any%20one%20cation.\" \/><\/p>\r\n<strong>Figure 8.16<\/strong>\r\n<p id=\"x-ck12-OGQwYTZiN2FjNTZjOWM3OGVlNTM1NWE4ZjA1YTkzNDg.-xr9\">In a metal, the stationary metal cations are surrounded by a sea of mobile valence electrons that are not associated with any one cation.<\/p>\r\n\r\n<\/div>\r\n<h4>Properties of Metals<\/h4>\r\n<p id=\"x-ck12-YTdkZDJkNTliY2E3OTU1MDU0Yjc0NDFmMDA5MzcxYTM.-yt6\">The metallic bonding model explains the physical properties of metals.\u00a0 Metals conduct electricity and heat very well because of their free-flowing electrons.\u00a0 As electrons enter one end of a piece of metal, an equal number of electrons flow outward from the other end.\u00a0 When light is shone on to the surface of a metal, its electrons absorb small amounts of energy and become excited into one of its many empty orbitals.\u00a0 The electrons immediately fall back down to lower energy levels and emit light.\u00a0 This process is responsible for the high <strong>luster <\/strong>of metals.<\/p>\r\n\r\n<div id=\"x-ck12-MTY1NGRmM2QxZmZiOTgyNTBhMjgzYzJlODZmNmNhNGE.-nsf\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n<p id=\"x-ck12-u4a\"><img id=\"x-ck12-OTgwNDUtMTM2MjAxMTI0Ny05Ni00NC1JbnRDaC0wOC0xMi1Db2lucw..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211418\/20140811155233824080.png\" alt=\"An American platinum eagle\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/The%20American%20Platinum%20Eagle%20is%20the%20official%20platinum%20bullion%20coin%20of%20the%20United%20States%20and%20was%20first%20minted%20in%201997.%20The%20luster%20of%20a%20metal%20is%20due%20to%20its%20metallic%20bonds.\" \/><\/p>\r\n<strong>Figure 8.17<\/strong>\r\n<p id=\"x-ck12-M2VhZjliZjYyYzNkYjk3ZmUxZmVlYTA1ZGExMTFlZTE.-7pa\">The American Platinum Eagle is the official platinum bullion coin of the United States and was first minted in 1997. The luster of a metal is due to its metallic bonds.<\/p>\r\n\r\n<\/div>\r\n<p id=\"x-ck12-MzUwYWFjNTM3ZGFjZTc1OWUxZTk2NDU3NDVjMDM5MTE.-day\">Recall that ionic compounds are very brittle.\u00a0 Application of a force results in like-charged ions in the crystal coming too close to one another, causing the crystal to shatter.\u00a0 When a force is applied to a metal, the free-flowing electrons can slip in between the stationary cations and prevent them from coming in contact.\u00a0 Imagine ball bearings that have been coated with oil sliding past one another.\u00a0 As a result, metals are very <strong>malleable <\/strong>and <strong>ductile <\/strong>. They can be hammered into shapes, rolled into thin sheets, or pulled into thin wires.<\/p>\r\n\r\n<h4>Summary<\/h4>\r\n<ul id=\"x-ck12-ZWIzZDVmNGExZjVkNTBjMzA4Y2EwNDkzZTA5YTQ2MzQ.-kfj\">\r\n \t<li>The metallic bond is responsible for the properties of metals.<\/li>\r\n \t<li>Metals conduct electricity and heat well.<\/li>\r\n \t<li>Metals are ductile and malleable.<\/li>\r\n \t<li>Metals have luster.<\/li>\r\n<\/ul>\r\n<h4>Practice<\/h4>\r\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-txn\"><em>Questions<\/em><\/p>\r\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-tj9\">Use the link below to answer the following questions:<\/p>\r\n<p id=\"x-ck12-ZmYyYTM5YmEyMWY5ZTQ2ZjAzZjVkNWNkMTdkMGIwNGQ.-0j4\"><a href=\"http:\/\/www.chemguide.co.uk\/atoms\/bonding\/metallic.html\">http:\/\/www.chemguide.co.uk\/atoms\/bonding\/metallic.html<\/a><\/p>\r\n\r\n<ol id=\"x-ck12-MmQ3MWZhOTA0Mjk4NzA5OTcwNzVlNTdjZmYzMTU3Mzg.-rg6\">\r\n \t<li>What happens to valence electrons in metals?<\/li>\r\n \t<li>What holds the atoms of a metal together?<\/li>\r\n \t<li>What happens to the metallic bond when a metal is melted?<\/li>\r\n \t<li>What happens to the metallic bond when a metal boils?<\/li>\r\n<\/ol>\r\n<h4>Review<\/h4>\r\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-3pz\"><em>Questions<\/em><\/p>\r\n\r\n<ol id=\"x-ck12-ZGM4MjY5Yjc3NzA3MzhiNDllNGVhNzk0NTljY2Q4ODI.-kmk\">\r\n \t<li>What is a delocalized electron?<\/li>\r\n \t<li>Why do metals conduct electricity and heat well?<\/li>\r\n \t<li>Why do metals have luster?<\/li>\r\n<\/ol>\r\n<div class=\"x-ck12-data-problem-set\"><\/div>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-NDVjZWI0YjBiM2FjOTJjMmY5ZmE5MWFiZjkwN2EyNzM.-ij2\">\r\n \t<li><strong>delocalized electrons: <\/strong>Electrons which are capable of moving freely throughout the empty orbitals of the metallic crystal.<\/li>\r\n \t<li><strong>ductile: <\/strong>Able to be drawn out into a thin wire.<\/li>\r\n \t<li><strong>luster: <\/strong>A gentle sheen or soft glow, especially that of a partly reflective surface.<\/li>\r\n \t<li><strong>malleable: <\/strong>Able to be hammered or pressed permanently out of shape without breaking or cracking.<\/li>\r\n \t<li><strong>metallic bond: <\/strong>The attraction of the stationary metal cations to the surrounding mobile electrons.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<h1><\/h1>\r\n[reveal-answer q=\"836080\"]Show References[\/reveal-answer]\r\n[hidden-answer a=\"836080\"]\r\n<h2>References<\/h2>\r\n<ul>\r\n \t<li>John Pearson. <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:John_Pearson01.png\"> http:\/\/commons.wikimedia.org\/wiki\/File:John_Pearson01.png<\/a>.<\/li>\r\n \t<li>CK-12 Foundation - Christopher Auyeung.<\/li>\r\n \t<li>Courtesy of the US Mint. Front: <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:2005_AEPlat_Proof_Obv.png\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:2005_AEPlat_Proof_Obv.png<\/a>; Back: <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:American_Platinum_Eagle_2008_Proof_Rev.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:American_Platinum_Eagle_2008_Proof_Rev.jpg<\/a>.<\/li>\r\n<\/ul>\r\n[\/hidden-answer]","rendered":"<h1 id=\"x-ck12-SW9uaWMgYW5kIE1ldGFsbGljIEJvbmRpbmc.-chapter\">Ionic and Metallic Bonding<\/h1>\n<div class=\"x-ck12-data\"><\/div>\n<h1 id=\"x-ck12-RWxlY3Ryb24gRG90IERpYWdyYW1z\">Metallic Bonding<\/h1>\n<div class=\"x-ck12-data-objectives\">\n<ul id=\"x-ck12-MTczNmI2OTg1ODMzYTViMTQ0YmQ4ZTE5NWY1MTFmYjY.-bua\">\n<li>Define metallic bond.<\/li>\n<li>Describe properties of metals.<\/li>\n<\/ul>\n<\/div>\n<p id=\"x-ck12-OTRiM2FiZmFlZGZmNjM0ZTAzMzFlZmFhNjFlMjgwYjU.-zsx\"><span class=\"x-ck12-img-inline\"><img decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211415\/20140811155233583262.jpg\" alt=\"A copper plate has unique metallic properties\" width=\"200\" \/><\/span><\/p>\n<p id=\"x-ck12-MTA4ZTAxMGI3MzJmMTQzNDlmZDFmYmI2OTFmNjJkM2M.-viq\"><strong>Why do metals behave the way they do?<\/strong><\/p>\n<p id=\"x-ck12-NDhhYTc0ZDc2YTcyMDA1YjU4MzJlMjg5NjZmM2Y2MWM.-5uk\">The image above is of a copper plate that was made in 1893.\u00a0 The utensil has a great deal of elaborate decoration and the item is very useful.\u00a0 What would have happened if we decided that copper (I) chloride was just as good a material (well, it does have copper in it).\u00a0 The CuCl would end up as a powder when we pounded on it to shape it.\u00a0 Metals behave in unique ways. The bonding that occurs in a metal is responsible for its distinctive properties: luster, malleability, ductility, and excellent conductivity.<\/p>\n<h3>The Metallic Bond<\/h3>\n<p id=\"x-ck12-MGJlMjMyY2ZhYTkxYWU1NjUwZjVmNjQzNmUzOWJiOTc.-iv0\">Pure metals are crystalline solids, but unlike ionic compounds, every point in the crystal lattice is occupied by an identical atom.\u00a0 The electrons in the outer energy levels of a metal are mobile and capable of drifting from one metal atom to another.\u00a0 This means that the metal is more properly viewed as an array of positive ions surrounded by a sea of mobile valence electrons.\u00a0 Electrons which are capable of moving freely throughout the empty orbitals of the metallic crystal are called <strong>delocalized electrons <\/strong>(see <strong>Figure <\/strong>below ).\u00a0 A <strong>metallic bond <\/strong>is the attraction of the stationary metal cations to the surrounding mobile electrons.<\/p>\n<div id=\"x-ck12-MGE1M2U5YmEyMTY0NTdhODM1NWJhYWQwODNlOTU5Mzc.-t8o\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\n<p id=\"x-ck12-tkq\"><img decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MjAxMTE5NS0wLTktQ2hlbUpSU19DaDE2X21ldGFsbGljYm9uZF9DQQ..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211416\/20140811155233745745.png\" alt=\"Diagram of metallic bonding\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/In%20a%20metal%2C%20the%20stationary%20metal%20cations%20are%20surrounded%20by%20a%20sea%20of%20mobile%20valence%20electrons%20that%20are%20not%20associated%20with%20any%20one%20cation.\" \/><\/p>\n<p><strong>Figure 8.16<\/strong><\/p>\n<p id=\"x-ck12-OGQwYTZiN2FjNTZjOWM3OGVlNTM1NWE4ZjA1YTkzNDg.-xr9\">In a metal, the stationary metal cations are surrounded by a sea of mobile valence electrons that are not associated with any one cation.<\/p>\n<\/div>\n<h4>Properties of Metals<\/h4>\n<p id=\"x-ck12-YTdkZDJkNTliY2E3OTU1MDU0Yjc0NDFmMDA5MzcxYTM.-yt6\">The metallic bonding model explains the physical properties of metals.\u00a0 Metals conduct electricity and heat very well because of their free-flowing electrons.\u00a0 As electrons enter one end of a piece of metal, an equal number of electrons flow outward from the other end.\u00a0 When light is shone on to the surface of a metal, its electrons absorb small amounts of energy and become excited into one of its many empty orbitals.\u00a0 The electrons immediately fall back down to lower energy levels and emit light.\u00a0 This process is responsible for the high <strong>luster <\/strong>of metals.<\/p>\n<div id=\"x-ck12-MTY1NGRmM2QxZmZiOTgyNTBhMjgzYzJlODZmNmNhNGE.-nsf\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\n<p id=\"x-ck12-u4a\"><img decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MjAxMTI0Ny05Ni00NC1JbnRDaC0wOC0xMi1Db2lucw..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211418\/20140811155233824080.png\" alt=\"An American platinum eagle\" longdesc=\"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-admin\/The%20American%20Platinum%20Eagle%20is%20the%20official%20platinum%20bullion%20coin%20of%20the%20United%20States%20and%20was%20first%20minted%20in%201997.%20The%20luster%20of%20a%20metal%20is%20due%20to%20its%20metallic%20bonds.\" \/><\/p>\n<p><strong>Figure 8.17<\/strong><\/p>\n<p id=\"x-ck12-M2VhZjliZjYyYzNkYjk3ZmUxZmVlYTA1ZGExMTFlZTE.-7pa\">The American Platinum Eagle is the official platinum bullion coin of the United States and was first minted in 1997. The luster of a metal is due to its metallic bonds.<\/p>\n<\/div>\n<p id=\"x-ck12-MzUwYWFjNTM3ZGFjZTc1OWUxZTk2NDU3NDVjMDM5MTE.-day\">Recall that ionic compounds are very brittle.\u00a0 Application of a force results in like-charged ions in the crystal coming too close to one another, causing the crystal to shatter.\u00a0 When a force is applied to a metal, the free-flowing electrons can slip in between the stationary cations and prevent them from coming in contact.\u00a0 Imagine ball bearings that have been coated with oil sliding past one another.\u00a0 As a result, metals are very <strong>malleable <\/strong>and <strong>ductile <\/strong>. They can be hammered into shapes, rolled into thin sheets, or pulled into thin wires.<\/p>\n<h4>Summary<\/h4>\n<ul id=\"x-ck12-ZWIzZDVmNGExZjVkNTBjMzA4Y2EwNDkzZTA5YTQ2MzQ.-kfj\">\n<li>The metallic bond is responsible for the properties of metals.<\/li>\n<li>Metals conduct electricity and heat well.<\/li>\n<li>Metals are ductile and malleable.<\/li>\n<li>Metals have luster.<\/li>\n<\/ul>\n<h4>Practice<\/h4>\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-txn\"><em>Questions<\/em><\/p>\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-tj9\">Use the link below to answer the following questions:<\/p>\n<p id=\"x-ck12-ZmYyYTM5YmEyMWY5ZTQ2ZjAzZjVkNWNkMTdkMGIwNGQ.-0j4\"><a href=\"http:\/\/www.chemguide.co.uk\/atoms\/bonding\/metallic.html\">http:\/\/www.chemguide.co.uk\/atoms\/bonding\/metallic.html<\/a><\/p>\n<ol id=\"x-ck12-MmQ3MWZhOTA0Mjk4NzA5OTcwNzVlNTdjZmYzMTU3Mzg.-rg6\">\n<li>What happens to valence electrons in metals?<\/li>\n<li>What holds the atoms of a metal together?<\/li>\n<li>What happens to the metallic bond when a metal is melted?<\/li>\n<li>What happens to the metallic bond when a metal boils?<\/li>\n<\/ol>\n<h4>Review<\/h4>\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-3pz\"><em>Questions<\/em><\/p>\n<ol id=\"x-ck12-ZGM4MjY5Yjc3NzA3MzhiNDllNGVhNzk0NTljY2Q4ODI.-kmk\">\n<li>What is a delocalized electron?<\/li>\n<li>Why do metals conduct electricity and heat well?<\/li>\n<li>Why do metals have luster?<\/li>\n<\/ol>\n<div class=\"x-ck12-data-problem-set\"><\/div>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-NDVjZWI0YjBiM2FjOTJjMmY5ZmE5MWFiZjkwN2EyNzM.-ij2\">\n<li><strong>delocalized electrons: <\/strong>Electrons which are capable of moving freely throughout the empty orbitals of the metallic crystal.<\/li>\n<li><strong>ductile: <\/strong>Able to be drawn out into a thin wire.<\/li>\n<li><strong>luster: <\/strong>A gentle sheen or soft glow, especially that of a partly reflective surface.<\/li>\n<li><strong>malleable: <\/strong>Able to be hammered or pressed permanently out of shape without breaking or cracking.<\/li>\n<li><strong>metallic bond: <\/strong>The attraction of the stationary metal cations to the surrounding mobile electrons.<\/li>\n<\/ul>\n<\/div>\n<h1><\/h1>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q836080\">Show References<\/span><\/p>\n<div id=\"q836080\" class=\"hidden-answer\" style=\"display: none\">\n<h2>References<\/h2>\n<ul>\n<li>John Pearson. <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:John_Pearson01.png\"> http:\/\/commons.wikimedia.org\/wiki\/File:John_Pearson01.png<\/a>.<\/li>\n<li>CK-12 Foundation &#8211; Christopher Auyeung.<\/li>\n<li>Courtesy of the US Mint. Front: <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:2005_AEPlat_Proof_Obv.png\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:2005_AEPlat_Proof_Obv.png<\/a>; Back: <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:American_Platinum_Eagle_2008_Proof_Rev.jpg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:American_Platinum_Eagle_2008_Proof_Rev.jpg<\/a>.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n","protected":false},"author":1507,"menu_order":11,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-2803","chapter","type-chapter","status-publish","hentry"],"part":2329,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2803","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/users\/1507"}],"version-history":[{"count":5,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2803\/revisions"}],"predecessor-version":[{"id":3644,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2803\/revisions\/3644"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/parts\/2329"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2803\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=2803"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=2803"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=2803"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=2803"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}