{"id":3058,"date":"2016-08-24T23:18:27","date_gmt":"2016-08-24T23:18:27","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=3058"},"modified":"2016-08-24T23:18:27","modified_gmt":"2016-08-24T23:18:27","slug":"lewis-electron-dot-structures","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/lewis-electron-dot-structures\/","title":{"raw":"Lewis Electron-Dot Structures","rendered":"Lewis Electron-Dot Structures"},"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 Lewis electron-dot structure.<\/li>\r\n \t<li>Define single covalent bond.<\/li>\r\n \t<li>Define structural formula.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>What does cholesterol really look like?<\/h3>\r\n<p id=\"x-ck12-Y2Y5Nzk4YWE1NGVjZjllYzc4NDk0MzU2NjYyNjM2NWQ.-3dq\"><span class=\"x-ck12-img-inline\"><img class=\"alignright\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211429\/20140811155249954998.png\" alt=\"Structure of cholesterol\" width=\"300\" \/><\/span><\/p>\r\n<p id=\"x-ck12-NzY2ZWNlOWEzNjUxZDRhOTcwNzVhODU5OTY3NGFmMWQ.-rl5\">We can write the structure of the cholesterol molecule a couple of different ways.\u00a0 The simplest approach is to just write C<sub>27<\/sub>H<sub>46<\/sub>O.\u00a0 This \u201cstructure\u201d is not very useful because it does not tell us how the carbons, hydrogens, and oxygen are connected to one another.<\/p>\r\nThe structure in the figure to the right\u00a0is much more helpful\u2014in it, we can see how the different atoms are connected together to form the molecule.\r\n\r\n<\/div>\r\n<p id=\"x-ck12-OTIwZmNkZGE1Yzg5YTNjYmQxNDUzMjA0NjA2Mjc4Mjk.-5s6\">In a previous chapter, you learned that the valence electrons of an atom can be shown in a simple way with an electron dot diagram.\u00a0 A hydrogen atom is shown as H\u2022 because of its one valence electron.\u00a0 The structures of molecules that are held together by covalent bonds can be diagrammed by <strong> Lewis electron-dot structures <\/strong> .\u00a0 The hydrogen molecule is shown in the <strong> Figure 1<\/strong>.<\/p>\r\n\r\n<div id=\"x-ck12-ZWVjZTQzNDVmZTc3MGFkY2Y2ZTVmY2I5N2QyYTZjYzM.-pn4\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"500\"]<img id=\"x-ck12-OTgwNDUtMTM2MTYwNDEyMC0yNC01OS0y\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211430\/20140811155250329647.png\" alt=\"Picture of a hydrogen atom and molecule\" width=\"500\" height=\"276\" longdesc=\"On%20the%20left%20is%20a%20single%20hydrogen%20atom%20with%20one%20electron.%20On%20the%20right%20is%20an%20H%3Csub%3E2%3C\/sub%3E%20molecule%20showing%20the%20electron%20cloud%20overlap.\" \/> Figure 1.\u00a0On the left is a single hydrogen atom with one electron. On the right is an H<sub>2<\/sub> molecule showing the electron cloud overlap.[\/caption]\r\n\r\n<\/div>\r\n<p id=\"x-ck12-ODBjYmY4MDRlZTQ0YWU3YjRkZmZjYWUzMGNlZWY1NDU.-cf1\">The shared pair of electrons is shown as two dots in between the two H symbols (H:H). This is called a <strong> single covalent bond<\/strong>, when two atoms are joined by the sharing of one pair of electrons. The single covalent bond can also be shown by a dash in between the two symbols (H\u2013H). A <strong> structural formula <\/strong> is a formula that shows the arrangement of atoms in a molecule and represents covalent bonds between atoms by dashes.<\/p>\r\n\r\n<h2 id=\"x-ck12-NzI4MGVlNTYyNDcyZWEzYjFmODM5MzY1N2ZiNzhiYTM.-anb_1-svk\"><strong> The Octet Rule and Covalent Bonds <\/strong><\/h2>\r\n<p id=\"x-ck12-YzAwNTFhMzg5NWZkNDk2NjA3YmFkMzdiN2Y0OWY2ZWE.-z6n\">When ions form, they conform to the <strong> octet rule <\/strong> by either losing or gaining electrons in order to achieve the electron configuration of the nearest noble gas. In a similar way, nonmetal atoms share electrons in the formation of a covalent in bond such a way that each of the atoms involved in the bond can attain a noble-gas electron configuration. The shared electrons are \u201ccounted\u201d for each of the atoms involved in the sharing. For hydrogen (H<sub>2<\/sub>), the shared pair of electrons means that each of the atoms is able to attain the electron configuration of helium, the noble gas with two electrons. For atoms other than hydrogen, the sharing of electrons will usually provide each of the atoms with eight valence electrons.<\/p>\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-MWUxYjE2Mjk0MjI5NDQ3OTZmOTU2NzUxNjc5ZjA0OTI.-aur\">\r\n \t<li>Lewis electron-dot structures show the bonding in covalent molecules.<\/li>\r\n \t<li>Covalent bonds between atoms can be indicated either with dots (:) or a dash (-).<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Practice<\/h3>\r\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-ltj\">Use the link below to answer the following questions:<\/p>\r\n<p id=\"x-ck12-NTcwMjFhZjc3ZDhhYjNmZTU4YWI1MTg4ZjRmM2ZjNzk.-xkw\"><a href=\"http:\/\/chemistry.about.com\/od\/generalchemistry\/a\/lewisstructures.htm\"> http:\/\/chemistry.about.com\/od\/generalchemistry\/a\/lewisstructures.htm <\/a><\/p>\r\n\r\n<ol id=\"x-ck12-NzcxZTQ2MDQyODVjNTM5NDk3NzU5MDdjMGQ2MGZjOWI.-jdd\">\r\n \t<li>Who developed the electron-dot structure system?<\/li>\r\n \t<li>Are lines or dots more commonly used?<\/li>\r\n \t<li>How are unbounded electrons represented?<\/li>\r\n \t<li>Which atom is selected as the central atom?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-YWIwMjgwMzQ4YWIyNDc3ZjE2MzllOGNjYzM3ZTg4MDc.-vbr\">\r\n \t<li>What is a single covalent bond?<\/li>\r\n \t<li>How can covalently-bound atoms obey the octet rule?<\/li>\r\n \t<li>Does the hydrogen molecule obey the octet rule?<\/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-MmU0ZmYwZTc5NmI4ODUzODEyMWM3ZjNjNGVjMDMzZmI.-34m\">\r\n \t<li><strong> Lewis electron-dot structures: <\/strong> A way of representing covalent bonds in molecules.<\/li>\r\n \t<li><strong> octet rule: <\/strong> Ions form by adding or losing electrons to form an outer shell of eight.<\/li>\r\n \t<li><strong> single covalent bond: <\/strong> When two atoms are joined by the sharing of one pair of electrons.<\/li>\r\n \t<li><strong> structural formula: <\/strong> A formula that shows the arrangement of atoms in a molecule and represents covalent bonds between atoms by dashes.<\/li>\r\n<\/ul>\r\n[reveal-answer q=\"836080\"]Show References[\/reveal-answer]\r\n[hidden-answer a=\"836080\"]\r\n<h2>References<\/h2>\r\n<ol>\r\n \t<li>User:BorisTM\/Wikimedia Commons.<a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Cholesterol.svg\">http:\/\/commons.wikimedia.org\/wiki\/File:Cholesterol.svg <\/a>.<\/li>\r\n \t<li>CK-12 Foundation - Jodi So.<\/li>\r\n<\/ol>\r\n[\/hidden-answer]\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 Lewis electron-dot structure.<\/li>\n<li>Define single covalent bond.<\/li>\n<li>Define structural formula.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3>What does cholesterol really look like?<\/h3>\n<p id=\"x-ck12-Y2Y5Nzk4YWE1NGVjZjllYzc4NDk0MzU2NjYyNjM2NWQ.-3dq\"><span class=\"x-ck12-img-inline\"><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\/19211429\/20140811155249954998.png\" alt=\"Structure of cholesterol\" width=\"300\" \/><\/span><\/p>\n<p id=\"x-ck12-NzY2ZWNlOWEzNjUxZDRhOTcwNzVhODU5OTY3NGFmMWQ.-rl5\">We can write the structure of the cholesterol molecule a couple of different ways.\u00a0 The simplest approach is to just write C<sub>27<\/sub>H<sub>46<\/sub>O.\u00a0 This \u201cstructure\u201d is not very useful because it does not tell us how the carbons, hydrogens, and oxygen are connected to one another.<\/p>\n<p>The structure in the figure to the right\u00a0is much more helpful\u2014in it, we can see how the different atoms are connected together to form the molecule.<\/p>\n<\/div>\n<p id=\"x-ck12-OTIwZmNkZGE1Yzg5YTNjYmQxNDUzMjA0NjA2Mjc4Mjk.-5s6\">In a previous chapter, you learned that the valence electrons of an atom can be shown in a simple way with an electron dot diagram.\u00a0 A hydrogen atom is shown as H\u2022 because of its one valence electron.\u00a0 The structures of molecules that are held together by covalent bonds can be diagrammed by <strong> Lewis electron-dot structures <\/strong> .\u00a0 The hydrogen molecule is shown in the <strong> Figure 1<\/strong>.<\/p>\n<div id=\"x-ck12-ZWVjZTQzNDVmZTc3MGFkY2Y2ZTVmY2I5N2QyYTZjYzM.-pn4\" 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-OTgwNDUtMTM2MTYwNDEyMC0yNC01OS0y\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211430\/20140811155250329647.png\" alt=\"Picture of a hydrogen atom and molecule\" width=\"500\" height=\"276\" longdesc=\"On%20the%20left%20is%20a%20single%20hydrogen%20atom%20with%20one%20electron.%20On%20the%20right%20is%20an%20H%3Csub%3E2%3C\/sub%3E%20molecule%20showing%20the%20electron%20cloud%20overlap.\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 1.\u00a0On the left is a single hydrogen atom with one electron. On the right is an H<sub>2<\/sub> molecule showing the electron cloud overlap.<\/p>\n<\/div>\n<\/div>\n<p id=\"x-ck12-ODBjYmY4MDRlZTQ0YWU3YjRkZmZjYWUzMGNlZWY1NDU.-cf1\">The shared pair of electrons is shown as two dots in between the two H symbols (H:H). This is called a <strong> single covalent bond<\/strong>, when two atoms are joined by the sharing of one pair of electrons. The single covalent bond can also be shown by a dash in between the two symbols (H\u2013H). A <strong> structural formula <\/strong> is a formula that shows the arrangement of atoms in a molecule and represents covalent bonds between atoms by dashes.<\/p>\n<h2 id=\"x-ck12-NzI4MGVlNTYyNDcyZWEzYjFmODM5MzY1N2ZiNzhiYTM.-anb_1-svk\"><strong> The Octet Rule and Covalent Bonds <\/strong><\/h2>\n<p id=\"x-ck12-YzAwNTFhMzg5NWZkNDk2NjA3YmFkMzdiN2Y0OWY2ZWE.-z6n\">When ions form, they conform to the <strong> octet rule <\/strong> by either losing or gaining electrons in order to achieve the electron configuration of the nearest noble gas. In a similar way, nonmetal atoms share electrons in the formation of a covalent in bond such a way that each of the atoms involved in the bond can attain a noble-gas electron configuration. The shared electrons are \u201ccounted\u201d for each of the atoms involved in the sharing. For hydrogen (H<sub>2<\/sub>), the shared pair of electrons means that each of the atoms is able to attain the electron configuration of helium, the noble gas with two electrons. For atoms other than hydrogen, the sharing of electrons will usually provide each of the atoms with eight valence electrons.<\/p>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-MWUxYjE2Mjk0MjI5NDQ3OTZmOTU2NzUxNjc5ZjA0OTI.-aur\">\n<li>Lewis electron-dot structures show the bonding in covalent molecules.<\/li>\n<li>Covalent bonds between atoms can be indicated either with dots (:) or a dash (-).<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-ltj\">Use the link below to answer the following questions:<\/p>\n<p id=\"x-ck12-NTcwMjFhZjc3ZDhhYjNmZTU4YWI1MTg4ZjRmM2ZjNzk.-xkw\"><a href=\"http:\/\/chemistry.about.com\/od\/generalchemistry\/a\/lewisstructures.htm\"> http:\/\/chemistry.about.com\/od\/generalchemistry\/a\/lewisstructures.htm <\/a><\/p>\n<ol id=\"x-ck12-NzcxZTQ2MDQyODVjNTM5NDk3NzU5MDdjMGQ2MGZjOWI.-jdd\">\n<li>Who developed the electron-dot structure system?<\/li>\n<li>Are lines or dots more commonly used?<\/li>\n<li>How are unbounded electrons represented?<\/li>\n<li>Which atom is selected as the central atom?<\/li>\n<\/ol>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-YWIwMjgwMzQ4YWIyNDc3ZjE2MzllOGNjYzM3ZTg4MDc.-vbr\">\n<li>What is a single covalent bond?<\/li>\n<li>How can covalently-bound atoms obey the octet rule?<\/li>\n<li>Does the hydrogen molecule obey the octet rule?<\/li>\n<\/ol>\n<\/div>\n<h2>Glossary<\/h2>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-MmU0ZmYwZTc5NmI4ODUzODEyMWM3ZjNjNGVjMDMzZmI.-34m\">\n<li><strong> Lewis electron-dot structures: <\/strong> A way of representing covalent bonds in molecules.<\/li>\n<li><strong> octet rule: <\/strong> Ions form by adding or losing electrons to form an outer shell of eight.<\/li>\n<li><strong> single covalent bond: <\/strong> When two atoms are joined by the sharing of one pair of electrons.<\/li>\n<li><strong> structural formula: <\/strong> A formula that shows the arrangement of atoms in a molecule and represents covalent bonds between atoms by dashes.<\/li>\n<\/ul>\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<ol>\n<li>User:BorisTM\/Wikimedia Commons.<a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Cholesterol.svg\">http:\/\/commons.wikimedia.org\/wiki\/File:Cholesterol.svg <\/a>.<\/li>\n<li>CK-12 Foundation &#8211; Jodi So.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n","protected":false},"author":17,"menu_order":2,"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-3058","chapter","type-chapter","status-publish","hentry"],"part":2330,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3058","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\/17"}],"version-history":[{"count":3,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3058\/revisions"}],"predecessor-version":[{"id":3110,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3058\/revisions\/3110"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/parts\/2330"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3058\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=3058"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=3058"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=3058"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=3058"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}