{"id":332,"date":"2017-10-04T15:17:42","date_gmt":"2017-10-04T15:17:42","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/?post_type=chapter&#038;p=332"},"modified":"2017-10-24T16:23:37","modified_gmt":"2017-10-24T16:23:37","slug":"drawing-chemical-structures","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/chapter\/drawing-chemical-structures\/","title":{"raw":"Drawing Chemical Structures","rendered":"Drawing Chemical Structures"},"content":{"raw":"<div class=\"elm-header\"><\/div>\r\n<div id=\"elm-main-content\" class=\"elm-content-container\">\r\n<div>\r\n<div id=\"skills\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Objectives<\/h3>\r\nAfter completing this section, you should be able to\r\n<ol>\r\n \t<li>propose one or more acceptable Kekul\u00e9 structures (structural formulas) for any given molecular formula<\/li>\r\n \t<li>write the molecular formula of a compound, given its Kekul\u00e9 structure.<\/li>\r\n \t<li>draw the shorthand structure of a compound, given its Kekul\u00e9 structure.<\/li>\r\n \t<li>interpret shorthand structures and convert them to Kekul\u00e9 structures.<\/li>\r\n \t<li>write the molecular formula of a compound, given its shorthand structure.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<div id=\"note\">\r\n<div class=\"textbox\">\r\n<h3 class=\"boxtitle\">Study Notes<\/h3>\r\nWhen drawing the structure of a neutral organic compound, you will find it helpful to remember that\r\n<ul>\r\n \t<li>each carbon atom has four bonds.<\/li>\r\n \t<li>each nitrogen atom has three bonds.<\/li>\r\n \t<li>each oxygen atom has two bonds.<\/li>\r\n \t<li>each hydrogen atom has one bond.<\/li>\r\n<\/ul>\r\n<\/div>\r\n\r\n\r\n<\/div>\r\nIt is necessary to draw structural formulas for organic compounds because in most cases a molecular formula does not uniquely represent a single compound. Different compounds having the same molecular formula are called <strong>isomers<\/strong>, and the prevalence of organic isomers reflects the extraordinary versatility of carbon in forming strong bonds to itself and to other elements. When the group of atoms that make up the molecules of different isomers are bonded together in fundamentally different ways, we refer to such compounds as <strong>constitutional isomers<\/strong>. There are seven constitutional isomers of C<sub>4<\/sub>H<sub>10<\/sub>O, and structural formulas for these are drawn in the following table. These formulas represent all known and possible C<sub>4<\/sub>H<sub>10<\/sub>O compounds, and display a common structural feature. <u>There are no double or triple bonds and no rings in any of these structures.<\/u>\r\n<table style=\"margin: auto;border-spacing: 2px\" border=\"0\" cellpadding=\"2\"><caption><em>Structural Formulas for C<sub>4<\/sub>H<sub>10O<\/sub> isomers<\/em><\/caption>\r\n<tbody>\r\n<tr>\r\n<td align=\"center\"><strong>Kekul\u00e9 Formula<\/strong><\/td>\r\n<td align=\"center\"><strong>Condensed Formula<\/strong><\/td>\r\n<td align=\"center\"><strong>Shorthand Formula <\/strong><\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"3\"><u><img class=\"internal default\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151633\/structure2.gif\" alt=\"structure2.gif\" width=\"429px\" height=\"475px\" \/><\/u><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nSimplification of structural formulas may be achieved without any loss of the information they convey. In <strong>condensed structural formulas<\/strong> the bonds to each carbon are omitted, but each distinct structural unit (group) is written with subscript numbers designating multiple substituents, including the hydrogens. <strong> Shorthand (line) formulas<\/strong> omit the symbols for carbon and hydrogen entirely. Each straight line segment represents a bond, the ends and intersections of the lines are carbon atoms, and the correct number of hydrogens is calculated from the tetravalency of carbon. Non-bonding valence shell electrons are omitted in these formulas.\r\n\r\nDeveloping the ability to visualize a three-dimensional structure from two-dimensional formulas requires practice, and in most cases the aid of molecular models. As noted earlier, many kinds of model kits are available to students and professional chemists, and the beginning student is encouraged to obtain one.\r\n<div id=\"section_1\">\r\n\r\n\r\n<h4 class=\"editable\">Kekul\u00e9 Formula<\/h4>\r\nA structural formula displays the atoms of the molecule in the order they are bonded. \u00a0It also depicts how the atoms are bonded to one another, for example single, double, and triple covalent bond. \u00a0 Covalent bonds are shown using lines. \u00a0The number of dashes indicate whether the bond is a single, double, or triple covalent bond.\u00a0 Structural formulas are helpful because they explain the properties and structure of the compound which empirical and molecular formulas cannot always represent.\r\n\r\nEx. \u00a0Kekul\u00e9 Formula for Ethanol:\u00a0<a class=\"lightbox\" title=\"Ethanol Jean NEW.gif\" href=\"\/Wikitexts\/Purdue\/Purdue_CHM_26100\/Chapter_01%3A_Introduction_and_Review\/@api\/deki\/files\/4771\/=Ethanol_Jean_NEW.gif?size=webview\" rel=\"image-gallery\"><img class=\"image internal\" title=\"Ethanol Jean NEW.gif\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151635\/Ethanol_Jean_NEW.gif\" alt=\"File:Physical_Chemistry\/Quantum_Mechanics\/Atomic_Theory\/Chemical_Compounds\/Formulas_of_Inorganic_and_Organic_Compounds\/Ethanol_Jean_NEW.gif\" \/><\/a>\r\n\r\n<\/div>\r\n<div id=\"section_2\">\r\n\r\n\r\n<h4 class=\"editable\">Condensed Formula<\/h4>\r\nCondensed structural formulas show the order of atoms like a structural formula but are written in a single line to save space and make it more convenient and faster to write out. Condensed structural formulas are also helpful when showing that a group of atoms is connected to a single atom in a compound. When this happens, parenthesis are used around the group of atoms to show they are together.\r\n\r\nEx. Condensed Structural Formula for Ethanol: CH<sub>3<\/sub>CH<sub>2<\/sub>OH (Molecular Formula for Ethanol\u00a0C<sub>2<\/sub>H<sub>6<\/sub>O).\r\n\r\n<\/div>\r\n<div id=\"section_3\">\r\n\r\n\r\n<h4 class=\"editable\">Shorthand Formula<\/h4>\r\nBecause organic compounds can be complex at times, line-angle formulas are used to write carbon and hydrogen atoms more efficiently by replacing the letters with lines.\u00a0 A carbon atom is present wherever a line intersects another line.\u00a0 Hydrogen atoms are then assumed to complete each of carbon's four bonds.\u00a0 All other atoms that are connected to carbon atoms are written out.\u00a0 Line angle formulas help show structure and order of the atoms in a compound making the advantages and disadvantages similar to structural formulas.\r\n\r\nEx.Shorthand\u00a0 Formula for Ethanol: \u00a0<a class=\"lightbox\" title=\"Line Angle Ethanol Jean.gif\" href=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/4746\/image181.png?revision=1\" rel=\"internal\"><img class=\"image internal\" title=\"Line Angle Ethanol Jean.gif\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151636\/Line_Angle_Ethanol_Jean.gif\" alt=\"File:Physical_Chemistry\/Quantum_Mechanics\/Atomic_Theory\/Chemical_Compounds\/Formulas_of_Inorganic_and_Organic_Compounds\/Line_Angle_Ethanol_Jean.gif\" \/><\/a>\r\n\r\n<\/div>\r\n<div id=\"section_4\">\r\n\r\n\r\n<div class=\"textbox exercises\">\r\n<h3>Exercises<\/h3>\r\n<h3>Question<\/h3>\r\n<div id=\"section_4\">\r\n\r\nWrite down the molecular formula for each of the compounds shown here.\r\n<p><img src=\"https:\/\/chem.libretexts.org\/LibreTexts\/Athabasca_University\/Chemistry_350%3A_Organic_Chemistry_I\/Chapter_1%3A_Structure_and_Bonding\/\/LibreTexts\/Athabasca_University\/Chemistry_350:_Organic_Chemistry_I\/Chapter_1:_Structure_and_Bonding\/1.12_Drawing_Chemical_Structures##fixme\" alt=\"compounds A through D for naming\" \/><\/p>\r\n\r\n<div id=\"section_5\">\r\n<h3 class=\"editable\">Solution<\/h3>\r\n[reveal-answer q=\"319921\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"319921\"]\r\n\r\n1. C7H7N\r\n\r\n2. C5H10\r\n\r\n3. C5H4O\r\n\r\n4. C5H6Br2[\/hidden-answer]\r\n<div id=\"s61688\">\r\n<div id=\"section_39\">\r\n<h3 id=\"Questions-61688\">Question<\/h3>\r\n<span><span>Below is the molecule for caffeine. Give the molecular formula for it.<\/span><\/span>\r\n\r\n<img class=\"internal default aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151637\/1.12.png\" alt=\"\" width=\"190\" height=\"152\" \/>\r\n\r\n<\/div>\r\n<div id=\"section_40\">\r\n\r\n\r\n<h3 id=\"Solutions-61688\">Solution<\/h3>\r\n[reveal-answer q=\"206416\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"206416\"]C8H10O2N4[\/hidden-answer]\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"section_6\"><\/div>\r\n<\/div>\r\n\r\n\r\n<\/div>\r\n<div id=\"section_6\">\r\n<h3 class=\"editable\">Contributors<\/h3>\r\n<ul>\r\n \t<li><a class=\"external\" title=\"http:\/\/science.athabascau.ca\/staff-pages\/dietmark\" href=\"http:\/\/science.athabascau.ca\/staff-pages\/dietmark\" target=\"_blank\" rel=\"external nofollow noopener\">Dr. Dietmar Kennepohl<\/a> FCIC (Professor of Chemistry, <a class=\"external\" title=\"http:\/\/www.athabascau.ca\/\" href=\"http:\/\/www.athabascau.ca\/\" target=\"_blank\" rel=\"external nofollow noopener\">Athabasca University<\/a>)<\/li>\r\n \t<li>Prof. Steven Farmer (<a class=\"external\" title=\"http:\/\/www.sonoma.edu\" href=\"http:\/\/www.sonoma.edu\" target=\"_blank\" rel=\"external nofollow noopener\">Sonoma State University<\/a>)<\/li>\r\n \t<li>William Reusch, Professor Emeritus (<a class=\"external\" title=\"http:\/\/www.msu.edu\/\" href=\"http:\/\/www.msu.edu\/\" target=\"_blank\" rel=\"external nofollow noopener\">Michigan State U.<\/a>), <a class=\"external\" title=\"http:\/\/www.cem.msu.edu\/~reusch\/VirtualText\/intro1.htm\" href=\"http:\/\/www.cem.msu.edu\/%7Ereusch\/VirtualText\/intro1.htm\" target=\"_blank\" rel=\"external nofollow noopener\">Virtual Textbook of\u00a0Organic\u00a0Chemistry<\/a><\/li>\r\n \t<li><a title=\"Organic_Chemistry_With_a_Biological_Emphasis\" href=\"https:\/\/chem.libretexts.org\/Textbook_Maps\/Organic_Chemistry_Textbook_Maps\/Map%3A_Organic_Chemistry_with_a_Biological_Emphasis_(Soderberg)\" rel=\"internal\">Organic Chemistry With a Biological Emphasis <\/a>by\u00a0<a class=\"external\" title=\"http:\/\/facultypages.morris.umn.edu\/~soderbt\/\" href=\"http:\/\/facultypages.morris.umn.edu\/%7Esoderbt\/\" target=\"_blank\" rel=\"external nofollow noopener\">Tim Soderberg<\/a>\u00a0(University of Minnesota, Morris)<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"<div class=\"elm-header\"><\/div>\n<div id=\"elm-main-content\" class=\"elm-content-container\">\n<div>\n<div id=\"skills\">\n<div class=\"textbox learning-objectives\">\n<h3>Objectives<\/h3>\n<p>After completing this section, you should be able to<\/p>\n<ol>\n<li>propose one or more acceptable Kekul\u00e9 structures (structural formulas) for any given molecular formula<\/li>\n<li>write the molecular formula of a compound, given its Kekul\u00e9 structure.<\/li>\n<li>draw the shorthand structure of a compound, given its Kekul\u00e9 structure.<\/li>\n<li>interpret shorthand structures and convert them to Kekul\u00e9 structures.<\/li>\n<li>write the molecular formula of a compound, given its shorthand structure.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<div id=\"note\">\n<div class=\"textbox\">\n<h3 class=\"boxtitle\">Study Notes<\/h3>\n<p>When drawing the structure of a neutral organic compound, you will find it helpful to remember that<\/p>\n<ul>\n<li>each carbon atom has four bonds.<\/li>\n<li>each nitrogen atom has three bonds.<\/li>\n<li>each oxygen atom has two bonds.<\/li>\n<li>each hydrogen atom has one bond.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<p>It is necessary to draw structural formulas for organic compounds because in most cases a molecular formula does not uniquely represent a single compound. Different compounds having the same molecular formula are called <strong>isomers<\/strong>, and the prevalence of organic isomers reflects the extraordinary versatility of carbon in forming strong bonds to itself and to other elements. When the group of atoms that make up the molecules of different isomers are bonded together in fundamentally different ways, we refer to such compounds as <strong>constitutional isomers<\/strong>. There are seven constitutional isomers of C<sub>4<\/sub>H<sub>10<\/sub>O, and structural formulas for these are drawn in the following table. These formulas represent all known and possible C<sub>4<\/sub>H<sub>10<\/sub>O compounds, and display a common structural feature. <u>There are no double or triple bonds and no rings in any of these structures.<\/u><\/p>\n<table style=\"margin: auto;border-spacing: 2px\" cellpadding=\"2\">\n<caption><em>Structural Formulas for C<sub>4<\/sub>H<sub>10O<\/sub> isomers<\/em><\/caption>\n<tbody>\n<tr>\n<td align=\"center\"><strong>Kekul\u00e9 Formula<\/strong><\/td>\n<td align=\"center\"><strong>Condensed Formula<\/strong><\/td>\n<td align=\"center\"><strong>Shorthand Formula <\/strong><\/td>\n<\/tr>\n<tr>\n<td colspan=\"3\"><u><img decoding=\"async\" class=\"internal default\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151633\/structure2.gif\" alt=\"structure2.gif\" width=\"429px\" height=\"475px\" \/><\/u><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Simplification of structural formulas may be achieved without any loss of the information they convey. In <strong>condensed structural formulas<\/strong> the bonds to each carbon are omitted, but each distinct structural unit (group) is written with subscript numbers designating multiple substituents, including the hydrogens. <strong> Shorthand (line) formulas<\/strong> omit the symbols for carbon and hydrogen entirely. Each straight line segment represents a bond, the ends and intersections of the lines are carbon atoms, and the correct number of hydrogens is calculated from the tetravalency of carbon. Non-bonding valence shell electrons are omitted in these formulas.<\/p>\n<p>Developing the ability to visualize a three-dimensional structure from two-dimensional formulas requires practice, and in most cases the aid of molecular models. As noted earlier, many kinds of model kits are available to students and professional chemists, and the beginning student is encouraged to obtain one.<\/p>\n<div id=\"section_1\">\n<h4 class=\"editable\">Kekul\u00e9 Formula<\/h4>\n<p>A structural formula displays the atoms of the molecule in the order they are bonded. \u00a0It also depicts how the atoms are bonded to one another, for example single, double, and triple covalent bond. \u00a0 Covalent bonds are shown using lines. \u00a0The number of dashes indicate whether the bond is a single, double, or triple covalent bond.\u00a0 Structural formulas are helpful because they explain the properties and structure of the compound which empirical and molecular formulas cannot always represent.<\/p>\n<p>Ex. \u00a0Kekul\u00e9 Formula for Ethanol:\u00a0<a class=\"lightbox\" title=\"Ethanol Jean NEW.gif\" href=\"\/Wikitexts\/Purdue\/Purdue_CHM_26100\/Chapter_01%3A_Introduction_and_Review\/@api\/deki\/files\/4771\/=Ethanol_Jean_NEW.gif?size=webview\" rel=\"image-gallery\"><img decoding=\"async\" class=\"image internal\" title=\"Ethanol Jean NEW.gif\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151635\/Ethanol_Jean_NEW.gif\" alt=\"File:Physical_Chemistry\/Quantum_Mechanics\/Atomic_Theory\/Chemical_Compounds\/Formulas_of_Inorganic_and_Organic_Compounds\/Ethanol_Jean_NEW.gif\" \/><\/a><\/p>\n<\/div>\n<div id=\"section_2\">\n<h4 class=\"editable\">Condensed Formula<\/h4>\n<p>Condensed structural formulas show the order of atoms like a structural formula but are written in a single line to save space and make it more convenient and faster to write out. Condensed structural formulas are also helpful when showing that a group of atoms is connected to a single atom in a compound. When this happens, parenthesis are used around the group of atoms to show they are together.<\/p>\n<p>Ex. Condensed Structural Formula for Ethanol: CH<sub>3<\/sub>CH<sub>2<\/sub>OH (Molecular Formula for Ethanol\u00a0C<sub>2<\/sub>H<sub>6<\/sub>O).<\/p>\n<\/div>\n<div id=\"section_3\">\n<h4 class=\"editable\">Shorthand Formula<\/h4>\n<p>Because organic compounds can be complex at times, line-angle formulas are used to write carbon and hydrogen atoms more efficiently by replacing the letters with lines.\u00a0 A carbon atom is present wherever a line intersects another line.\u00a0 Hydrogen atoms are then assumed to complete each of carbon&#8217;s four bonds.\u00a0 All other atoms that are connected to carbon atoms are written out.\u00a0 Line angle formulas help show structure and order of the atoms in a compound making the advantages and disadvantages similar to structural formulas.<\/p>\n<p>Ex.Shorthand\u00a0 Formula for Ethanol: \u00a0<a class=\"lightbox\" title=\"Line Angle Ethanol Jean.gif\" href=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/4746\/image181.png?revision=1\" rel=\"internal\"><img decoding=\"async\" class=\"image internal\" title=\"Line Angle Ethanol Jean.gif\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151636\/Line_Angle_Ethanol_Jean.gif\" alt=\"File:Physical_Chemistry\/Quantum_Mechanics\/Atomic_Theory\/Chemical_Compounds\/Formulas_of_Inorganic_and_Organic_Compounds\/Line_Angle_Ethanol_Jean.gif\" \/><\/a><\/p>\n<\/div>\n<div id=\"section_4\">\n<div class=\"textbox exercises\">\n<h3>Exercises<\/h3>\n<h3>Question<\/h3>\n<div id=\"section_4\">\n<p>Write down the molecular formula for each of the compounds shown here.<\/p>\n<p><img decoding=\"async\" src=\"https:\/\/chem.libretexts.org\/LibreTexts\/Athabasca_University\/Chemistry_350%3A_Organic_Chemistry_I\/Chapter_1%3A_Structure_and_Bonding\/\/LibreTexts\/Athabasca_University\/Chemistry_350:_Organic_Chemistry_I\/Chapter_1:_Structure_and_Bonding\/1.12_Drawing_Chemical_Structures##fixme\" alt=\"compounds A through D for naming\" \/><\/p>\n<div id=\"section_5\">\n<h3 class=\"editable\">Solution<\/h3>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q319921\">Show Answer<\/span><\/p>\n<div id=\"q319921\" class=\"hidden-answer\" style=\"display: none\">\n<p>1. C7H7N<\/p>\n<p>2. C5H10<\/p>\n<p>3. C5H4O<\/p>\n<p>4. C5H6Br2<\/p><\/div>\n<\/div>\n<div id=\"s61688\">\n<div id=\"section_39\">\n<h3 id=\"Questions-61688\">Question<\/h3>\n<p><span><span>Below is the molecule for caffeine. Give the molecular formula for it.<\/span><\/span><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"internal default aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/04151637\/1.12.png\" alt=\"\" width=\"190\" height=\"152\" \/><\/p>\n<\/div>\n<div id=\"section_40\">\n<h3 id=\"Solutions-61688\">Solution<\/h3>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q206416\">Show Answer<\/span><\/p>\n<div id=\"q206416\" class=\"hidden-answer\" style=\"display: none\">C8H10O2N4<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"section_6\"><\/div>\n<\/div>\n<\/div>\n<div id=\"section_6\">\n<h3 class=\"editable\">Contributors<\/h3>\n<ul>\n<li><a class=\"external\" title=\"http:\/\/science.athabascau.ca\/staff-pages\/dietmark\" href=\"http:\/\/science.athabascau.ca\/staff-pages\/dietmark\" target=\"_blank\" rel=\"external nofollow noopener\">Dr. Dietmar Kennepohl<\/a> FCIC (Professor of Chemistry, <a class=\"external\" title=\"http:\/\/www.athabascau.ca\/\" href=\"http:\/\/www.athabascau.ca\/\" target=\"_blank\" rel=\"external nofollow noopener\">Athabasca University<\/a>)<\/li>\n<li>Prof. Steven Farmer (<a class=\"external\" title=\"http:\/\/www.sonoma.edu\" href=\"http:\/\/www.sonoma.edu\" target=\"_blank\" rel=\"external nofollow noopener\">Sonoma State University<\/a>)<\/li>\n<li>William Reusch, Professor Emeritus (<a class=\"external\" title=\"http:\/\/www.msu.edu\/\" href=\"http:\/\/www.msu.edu\/\" target=\"_blank\" rel=\"external nofollow noopener\">Michigan State U.<\/a>), <a class=\"external\" title=\"http:\/\/www.cem.msu.edu\/~reusch\/VirtualText\/intro1.htm\" href=\"http:\/\/www.cem.msu.edu\/%7Ereusch\/VirtualText\/intro1.htm\" target=\"_blank\" rel=\"external nofollow noopener\">Virtual Textbook of\u00a0Organic\u00a0Chemistry<\/a><\/li>\n<li><a title=\"Organic_Chemistry_With_a_Biological_Emphasis\" href=\"https:\/\/chem.libretexts.org\/Textbook_Maps\/Organic_Chemistry_Textbook_Maps\/Map%3A_Organic_Chemistry_with_a_Biological_Emphasis_(Soderberg)\" rel=\"internal\">Organic Chemistry With a Biological Emphasis <\/a>by\u00a0<a class=\"external\" title=\"http:\/\/facultypages.morris.umn.edu\/~soderbt\/\" href=\"http:\/\/facultypages.morris.umn.edu\/%7Esoderbt\/\" target=\"_blank\" rel=\"external nofollow noopener\">Tim Soderberg<\/a>\u00a0(University of Minnesota, Morris)<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<\/div>\n","protected":false},"author":311,"menu_order":16,"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-332","chapter","type-chapter","status-publish","hentry"],"part":76,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/332","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/users\/311"}],"version-history":[{"count":4,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/332\/revisions"}],"predecessor-version":[{"id":2125,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/332\/revisions\/2125"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/parts\/76"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/332\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/media?parent=332"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=332"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/contributor?post=332"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/license?post=332"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}