{"id":3059,"date":"2016-08-25T16:20:42","date_gmt":"2016-08-25T16:20:42","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=3059"},"modified":"2016-08-25T16:20:42","modified_gmt":"2016-08-25T16:20:42","slug":"single-covalent-bonds","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/single-covalent-bonds\/","title":{"raw":"Single Covalent Bonds","rendered":"Single Covalent Bonds"},"content":{"raw":"<div class=\"x-ck12-data-objectives\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\n<ul>\r\n \t<li>Define a single covalent bond.<\/li>\r\n \t<li>Draw Lewis dot structures of molecules containing single covalent bonds.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3><strong style=\"line-height: 1.5;\">What holds molecules together?<\/strong><\/h3>\r\n<p id=\"x-ck12-M2FiODcwYzcwZWE4NmU4N2ZhZTg0MWJlMTYzODIwZmI.-fgz\"><img class=\"alignright\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211432\/20140811155250435900.jpeg\" alt=\"Democritus believed atoms were held together by hooks\" width=\"300\" \/>In one form or another, the idea of atoms connecting to form larger substances has been with us for a long time. The Greek philosopher Democritus (460\u2013370 BC) believed that atoms had hooks on them that allowed atoms to connect with one another.<\/p>\r\nToday we believe that atoms are held together by bonds formed when two atoms share a set of electrons, a much more complicated picture than the simple hooks that Democritus preferred.\r\n\r\n<\/div>\r\n<\/div>\r\n<p id=\"x-ck12-NmUwNDYwZDZjZmIwYmVjNmNjZTk5ZWE4MTM5ZDUzZGY.-u3f\">A covalent bond forms when two orbitals with one electron each overlap each other. For the hydrogen molecule, this can be shown as:<\/p>\r\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-mem\"><img class=\"alignnone wp-image-3112\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/24231957\/hydrogen.png\" alt=\"Electronic configuration of a hydrogen molecule\" width=\"150\" height=\"111\" \/><\/p>\r\n<p id=\"x-ck12-NWM4YTNjYjJiNWI4N2JmNDVmYTlhZmI0NmNkOTZiNjk.-zxh\">Upon formation of the H<sub>2 <\/sub> molecule, the shared electrons must have opposite spin, so they are shown with opposite spin in the atomic 1 <em> s <\/em> orbital.<\/p>\r\n<p id=\"x-ck12-MWYwN2NiNWUxNzM0MjFlNDJiZjE1MTU0ZmQ4MjkxZTQ.-va7\">The halogens also form single covalent bonds in their diatomic molecules. An atom of any halogen, such as fluorine, has seven valence electrons. Its unpaired electron is located in the 2<em>p <\/em> orbital.<\/p>\r\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-duq\"><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\/19211434\/20140811155250721586.png\" alt=\"Electronic configuration of a fluorine molecule\" width=\"300\" \/><\/span><\/p>\r\n<p id=\"x-ck12-NzI3NTEyNTM1M2ZjNzNkZjY4MzIzMDM2OTI3OTA3NDU.-8tl\">The single electrons in the third 2 <em> p <\/em> orbital combine to form the covalent bond:<\/p>\r\n\r\n<div id=\"x-ck12-ZjM0YTU3YjY0NWRkZjg0NDZjZTVmYmMwMjA2OWM1N2M.-bfi\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"500\"]<img id=\"x-ck12-OTgwNDUtMTM2MTk1NjA2MC01OS02LUltYWdlLS0tNg..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211435\/20140811155250858641.png\" alt=\"Picture of electron distribution\u00a0in a fluorine molecule\" width=\"500\" height=\"212\" longdesc=\"On%20the%20left%20is%20a%20fluorine%20atom%20with%20seven%20valence%20electrons.%20On%20the%20right%20is%20the%20F%3Csub%3E2%3C\/sub%3E%20molecule.\" \/> Figure 1. On the left is a fluorine atom with seven valence electrons. On the right is the F<sub>2<\/sub> molecule.[\/caption]\r\n\r\n<\/div>\r\n<p id=\"x-ck12-ZTM5ZmE0YTE4ZDU1MjZmZjVlZmNhYmVkM2ZlYTkxZWM.-vpf\">The diatomic fluorine molecule (F<sub>2<\/sub>) contains a single shared pair of electrons. Each F atom also has three pair of electrons that are not shared with the other atom. A <strong> lone pair <\/strong> is a pair of electrons in a Lewis electron-dot structure that is not shared between atoms. The oxygen atom in the water molecule shown below has two lone pair sets of electrons. Each F atom has three lone pairs. Combined with the two electrons in the covalent bond, each F atom follows the octet rule.<\/p>\r\n\r\n<div class=\"textbox shaded\">\r\n<h4 id=\"x-ck12-ZDI4ZWE3ZTA2ODAzOTg1MTU1ZDQ2M2FiMWEyMTE4OWI.-r41_2-vee\"><strong>Sample Problem: Lewis Electron Dot Structures <\/strong><\/h4>\r\n<p id=\"x-ck12-OTA1OTg3YWY0ZjQ1NWZlY2E2ZTQzNTI3NTVkOTYzYjc.-tvj\">Draw the Lewis electron dot structure for water.<\/p>\r\n<p id=\"x-ck12-M2U4ZTdjOGY3NjFhZjIzNGViMTQyODU0MWM0MTc3NzM.-5lq\"><em> Step 1: List the known quantities and plan the problem <\/em><\/p>\r\n<p id=\"x-ck12-MmY1NjUwZTQ4NGZhMTk1OTQ5YWM2YzhkMTFkY2E0ZmQ.-my5\"><span class=\"x-ck12-underline\"> Known <\/span><\/p>\r\n\r\n<ul id=\"x-ck12-YmI1NDNmOGRiODgzMTY3OGUwZGEyMzAyYWM5MTlmMzE.-mv6\">\r\n \t<li>molecular formula of water = H <sub> 2 <\/sub> O<\/li>\r\n \t<li>1 O atom = 6 valence electrons<\/li>\r\n \t<li>2 H atoms = 2 \u00d7 1 = 2 valence electrons<\/li>\r\n \t<li>total number of valence electrons = 8<\/li>\r\n<\/ul>\r\n<p id=\"x-ck12-YTc4ZWUzMjRhNDMyMTY3ODg4MzIwYmM5ZjhkN2M1ODA.-rcl\">Use the periodic table to determine the number of valence electrons for each atom and the total number of valence electrons.\u00a0 Arrange the atoms and distribute the electrons so that each atom follows the octet rule.\u00a0 The oxygen atom will have 8 electrons, while the hydrogen atoms will each have 2.<\/p>\r\n<p id=\"x-ck12-ZjZhN2M2ZWIzYjU5NWY1NDY2Yzg4ZDMxMDBjN2VkODc.-oq4\"><em> Step 2: Solve <\/em><\/p>\r\n<p id=\"x-ck12-NjJkYzJmYTU0Mjc2NDVkNzUyOThhZWU5OTM5Mzg4NDA.-da1\">Electron dot diagrams for each atom are:<\/p>\r\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-pju\"><img class=\"alignnone wp-image-3114\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/24232409\/electrondot-300x78.png\" alt=\"Lewis electron dot diagrams for hydrogen and oxygen\" width=\"250\" height=\"65\" \/><\/p>\r\n<p id=\"x-ck12-Mjc4MjM3ODMyNGY0YzdiMDIxYjkwYTQxMzAzZDIzNTM.-jlf\">Each hydrogen atom with its single electron will form a covalent bond with the oxygen atom where it has a single electron.\u00a0 The resulting Lewis electron dot structure is:<\/p>\r\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-v1w\"><img class=\"alignnone wp-image-3113\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/24232311\/lewisdot-300x150.png\" alt=\"Lewis electron dot structure of water\" width=\"100\" height=\"50\" \/><\/p>\r\n<p id=\"x-ck12-MGZhMzc5YjY2OWU0YzY0ZWM4YjYzZWNhYzc4OTQ3ZDA.-q6n\"><em> Step 3: \u00a0Think about your result. <\/em><\/p>\r\n<p id=\"x-ck12-NWE4MThiOTk0MzZmMjU4NjA4OGQ0NDM0NTc3NGE1ZWY.-5gf\">The oxygen atom follows the octet rule with two pairs of bonding electrons and two lone pairs.\u00a0 Each hydrogen atom follows the octet rule with one bonding pair of electrons.<\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-OTEyZWYyMDAzZjgzODJkMmE2YmJjZDA3N2I3MjEyODI.-gi8\">\r\n \t<li>Covalent bonds form when electrons in two atoms form overlapping orbitals.<\/li>\r\n \t<li>Lone pair electrons in an atom are not shared with another atom.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Practice<\/h3>\r\n<p id=\"x-ck12-MzUyOWM1NWU0ZjdmMDIyNTNkOTViZThmZTJlMjU5YmE.-cbb\">Read the article and practice drawing Lewis structures for some of the single covalent bond compounds listed at the end.<\/p>\r\n<p id=\"x-ck12-NWZjZWU2OGI4ZWY3ZWU1MmE2ZDIwNGNkNTE1OWFjN2Y.-dlm\"><a href=\"http:\/\/www2.fiu.edu\/~landrumj\/LewisStructures.pdf\"> http:\/\/www2.fiu.edu\/~landrumj\/LewisStructures.pdf<\/a><\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-MDdlNTQ0MGM4NDdiMWYwMDllNzNhMjYyZmIwMWMxOTI.-mxa\">\r\n \t<li>How does a covalent bond form?<\/li>\r\n \t<li>What do the spins of the shared electrons need to be?<\/li>\r\n \t<li>Do lone pair electrons form covalent bonds?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<h2>Glossary<\/h2>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-ZGU2NjliMzY1ODU3ZjM0N2U5MzMwOWU5ZGZiNTAxNjk.-bc8\">\r\n \t<li><strong> lone pair: <\/strong> A pair of electrons in a Lewis electron-dot structure that is not shared between atoms.<\/li>\r\n<\/ul>\r\n&nbsp;\r\n\r\n<\/div>","rendered":"<div class=\"x-ck12-data-objectives\">\n<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<ul>\n<li>Define a single covalent bond.<\/li>\n<li>Draw Lewis dot structures of molecules containing single covalent bonds.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox examples\">\n<h3><strong style=\"line-height: 1.5;\">What holds molecules together?<\/strong><\/h3>\n<p id=\"x-ck12-M2FiODcwYzcwZWE4NmU4N2ZhZTg0MWJlMTYzODIwZmI.-fgz\"><img decoding=\"async\" class=\"alignright\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211432\/20140811155250435900.jpeg\" alt=\"Democritus believed atoms were held together by hooks\" width=\"300\" \/>In one form or another, the idea of atoms connecting to form larger substances has been with us for a long time. The Greek philosopher Democritus (460\u2013370 BC) believed that atoms had hooks on them that allowed atoms to connect with one another.<\/p>\n<p>Today we believe that atoms are held together by bonds formed when two atoms share a set of electrons, a much more complicated picture than the simple hooks that Democritus preferred.<\/p>\n<\/div>\n<\/div>\n<p id=\"x-ck12-NmUwNDYwZDZjZmIwYmVjNmNjZTk5ZWE4MTM5ZDUzZGY.-u3f\">A covalent bond forms when two orbitals with one electron each overlap each other. For the hydrogen molecule, this can be shown as:<\/p>\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-mem\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-3112\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/24231957\/hydrogen.png\" alt=\"Electronic configuration of a hydrogen molecule\" width=\"150\" height=\"111\" \/><\/p>\n<p id=\"x-ck12-NWM4YTNjYjJiNWI4N2JmNDVmYTlhZmI0NmNkOTZiNjk.-zxh\">Upon formation of the H<sub>2 <\/sub> molecule, the shared electrons must have opposite spin, so they are shown with opposite spin in the atomic 1 <em> s <\/em> orbital.<\/p>\n<p id=\"x-ck12-MWYwN2NiNWUxNzM0MjFlNDJiZjE1MTU0ZmQ4MjkxZTQ.-va7\">The halogens also form single covalent bonds in their diatomic molecules. An atom of any halogen, such as fluorine, has seven valence electrons. Its unpaired electron is located in the 2<em>p <\/em> orbital.<\/p>\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-duq\"><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\/19211434\/20140811155250721586.png\" alt=\"Electronic configuration of a fluorine molecule\" width=\"300\" \/><\/span><\/p>\n<p id=\"x-ck12-NzI3NTEyNTM1M2ZjNzNkZjY4MzIzMDM2OTI3OTA3NDU.-8tl\">The single electrons in the third 2 <em> p <\/em> orbital combine to form the covalent bond:<\/p>\n<div id=\"x-ck12-ZjM0YTU3YjY0NWRkZjg0NDZjZTVmYmMwMjA2OWM1N2M.-bfi\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\n<div style=\"width: 510px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTk1NjA2MC01OS02LUltYWdlLS0tNg..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211435\/20140811155250858641.png\" alt=\"Picture of electron distribution\u00a0in a fluorine molecule\" width=\"500\" height=\"212\" longdesc=\"On%20the%20left%20is%20a%20fluorine%20atom%20with%20seven%20valence%20electrons.%20On%20the%20right%20is%20the%20F%3Csub%3E2%3C\/sub%3E%20molecule.\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 1. On the left is a fluorine atom with seven valence electrons. On the right is the F<sub>2<\/sub> molecule.<\/p>\n<\/div>\n<\/div>\n<p id=\"x-ck12-ZTM5ZmE0YTE4ZDU1MjZmZjVlZmNhYmVkM2ZlYTkxZWM.-vpf\">The diatomic fluorine molecule (F<sub>2<\/sub>) contains a single shared pair of electrons. Each F atom also has three pair of electrons that are not shared with the other atom. A <strong> lone pair <\/strong> is a pair of electrons in a Lewis electron-dot structure that is not shared between atoms. The oxygen atom in the water molecule shown below has two lone pair sets of electrons. Each F atom has three lone pairs. Combined with the two electrons in the covalent bond, each F atom follows the octet rule.<\/p>\n<div class=\"textbox shaded\">\n<h4 id=\"x-ck12-ZDI4ZWE3ZTA2ODAzOTg1MTU1ZDQ2M2FiMWEyMTE4OWI.-r41_2-vee\"><strong>Sample Problem: Lewis Electron Dot Structures <\/strong><\/h4>\n<p id=\"x-ck12-OTA1OTg3YWY0ZjQ1NWZlY2E2ZTQzNTI3NTVkOTYzYjc.-tvj\">Draw the Lewis electron dot structure for water.<\/p>\n<p id=\"x-ck12-M2U4ZTdjOGY3NjFhZjIzNGViMTQyODU0MWM0MTc3NzM.-5lq\"><em> Step 1: List the known quantities and plan the problem <\/em><\/p>\n<p id=\"x-ck12-MmY1NjUwZTQ4NGZhMTk1OTQ5YWM2YzhkMTFkY2E0ZmQ.-my5\"><span class=\"x-ck12-underline\"> Known <\/span><\/p>\n<ul id=\"x-ck12-YmI1NDNmOGRiODgzMTY3OGUwZGEyMzAyYWM5MTlmMzE.-mv6\">\n<li>molecular formula of water = H <sub> 2 <\/sub> O<\/li>\n<li>1 O atom = 6 valence electrons<\/li>\n<li>2 H atoms = 2 \u00d7 1 = 2 valence electrons<\/li>\n<li>total number of valence electrons = 8<\/li>\n<\/ul>\n<p id=\"x-ck12-YTc4ZWUzMjRhNDMyMTY3ODg4MzIwYmM5ZjhkN2M1ODA.-rcl\">Use the periodic table to determine the number of valence electrons for each atom and the total number of valence electrons.\u00a0 Arrange the atoms and distribute the electrons so that each atom follows the octet rule.\u00a0 The oxygen atom will have 8 electrons, while the hydrogen atoms will each have 2.<\/p>\n<p id=\"x-ck12-ZjZhN2M2ZWIzYjU5NWY1NDY2Yzg4ZDMxMDBjN2VkODc.-oq4\"><em> Step 2: Solve <\/em><\/p>\n<p id=\"x-ck12-NjJkYzJmYTU0Mjc2NDVkNzUyOThhZWU5OTM5Mzg4NDA.-da1\">Electron dot diagrams for each atom are:<\/p>\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-pju\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-3114\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/24232409\/electrondot-300x78.png\" alt=\"Lewis electron dot diagrams for hydrogen and oxygen\" width=\"250\" height=\"65\" \/><\/p>\n<p id=\"x-ck12-Mjc4MjM3ODMyNGY0YzdiMDIxYjkwYTQxMzAzZDIzNTM.-jlf\">Each hydrogen atom with its single electron will form a covalent bond with the oxygen atom where it has a single electron.\u00a0 The resulting Lewis electron dot structure is:<\/p>\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-v1w\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-3113\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/24232311\/lewisdot-300x150.png\" alt=\"Lewis electron dot structure of water\" width=\"100\" height=\"50\" \/><\/p>\n<p id=\"x-ck12-MGZhMzc5YjY2OWU0YzY0ZWM4YjYzZWNhYzc4OTQ3ZDA.-q6n\"><em> Step 3: \u00a0Think about your result. <\/em><\/p>\n<p id=\"x-ck12-NWE4MThiOTk0MzZmMjU4NjA4OGQ0NDM0NTc3NGE1ZWY.-5gf\">The oxygen atom follows the octet rule with two pairs of bonding electrons and two lone pairs.\u00a0 Each hydrogen atom follows the octet rule with one bonding pair of electrons.<\/p>\n<\/div>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-OTEyZWYyMDAzZjgzODJkMmE2YmJjZDA3N2I3MjEyODI.-gi8\">\n<li>Covalent bonds form when electrons in two atoms form overlapping orbitals.<\/li>\n<li>Lone pair electrons in an atom are not shared with another atom.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-MzUyOWM1NWU0ZjdmMDIyNTNkOTViZThmZTJlMjU5YmE.-cbb\">Read the article and practice drawing Lewis structures for some of the single covalent bond compounds listed at the end.<\/p>\n<p id=\"x-ck12-NWZjZWU2OGI4ZWY3ZWU1MmE2ZDIwNGNkNTE1OWFjN2Y.-dlm\"><a href=\"http:\/\/www2.fiu.edu\/~landrumj\/LewisStructures.pdf\"> http:\/\/www2.fiu.edu\/~landrumj\/LewisStructures.pdf<\/a><\/p>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-MDdlNTQ0MGM4NDdiMWYwMDllNzNhMjYyZmIwMWMxOTI.-mxa\">\n<li>How does a covalent bond form?<\/li>\n<li>What do the spins of the shared electrons need to be?<\/li>\n<li>Do lone pair electrons form covalent bonds?<\/li>\n<\/ol>\n<\/div>\n<h2>Glossary<\/h2>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-ZGU2NjliMzY1ODU3ZjM0N2U5MzMwOWU5ZGZiNTAxNjk.-bc8\">\n<li><strong> lone pair: <\/strong> A pair of electrons in a Lewis electron-dot structure that is not shared between atoms.<\/li>\n<\/ul>\n<p>&nbsp;<\/p>\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-3059\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Shared previously<\/div><ul class=\"citation-list\"><li>Chemistry Concepts Intermediate. <strong>Authored by<\/strong>: Calbreath, Baxter, et al.. <strong>Provided by<\/strong>: CK12.org. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/\">http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc\/4.0\/\">CC BY-NC: Attribution-NonCommercial<\/a><\/em><\/li><\/ul><div class=\"license-attribution-dropdown-subheading\">Public domain content<\/div><ul class=\"citation-list\"><li>Fishhook. <strong>Authored by<\/strong>: Fluri. <strong>Provided by<\/strong>: English Wikipedia. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Fishhook.jpg\">https:\/\/commons.wikimedia.org\/wiki\/File:Fishhook.jpg<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/about\/pdm\">Public Domain: No Known Copyright<\/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>","protected":false},"author":17,"menu_order":4,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Chemistry Concepts Intermediate\",\"author\":\"Calbreath, Baxter, et al.\",\"organization\":\"CK12.org\",\"url\":\"http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/\",\"project\":\"\",\"license\":\"cc-by-nc\",\"license_terms\":\"\"},{\"type\":\"pd\",\"description\":\"Fishhook\",\"author\":\"Fluri\",\"organization\":\"English 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