{"id":3066,"date":"2016-08-25T17:37:23","date_gmt":"2016-08-25T17:37:23","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=3066"},"modified":"2016-08-26T18:01:04","modified_gmt":"2016-08-26T18:01:04","slug":"vsepr-theory","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/vsepr-theory\/","title":{"raw":"VSEPR Theory","rendered":"VSEPR Theory"},"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 the VSEPR theory.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3><strong style=\"line-height: 1.5\">What do I do now?<\/strong><\/h3>\r\n<p id=\"x-ck12-MDdiNDM1MWQ0OTM1Y2RkZWFlZGU5Y2ZmYzRlMWNmMzU.-feb\">In every scientist\u2019s life comes that moment when you realize that you were wrong.\u00a0 Sometimes you think about a problem and recognize where you went astray.\u00a0 Other times you find out when you go into the lab and the experiment doesn\u2019t work (or gets way too exciting). What has to happen then is a change in direction.\u00a0 The good scientist sees the problem and comes up with a new answer.\u00a0 Then that answer has to be tested to see how it works.<\/p>\r\nPutting atoms together to form compounds can be done on paper or in the lab.\u00a0 However, when the shape of the molecule made in the lab is different from the shape of the molecule drawn on paper, then we need to rethink our ideas and find better explanations.\r\n\r\n<\/div>\r\n<p id=\"x-ck12-OTRlYzFmN2E3YWE5ZGI3NzFjNTUyYmI4OTA4NzhkNjY.-mmd\">In 1956, British scientists R.J. Gillespie and R.S. Nyholm recognized that the current model for explaining bond angles did not work well.\u00a0 The theory at that time relied on hybrid orbitals to explain all aspects of bonding.\u00a0 The problem was that the theory gave incorrect prediction of bond angles for many compounds.\u00a0 They developed a new approach based on earlier work by other scientists that incorporated a consideration of electron pairs in predicting three-dimensional structure.<\/p>\r\n<p id=\"x-ck12-ZTkyNDVjNTFmYWNlODliYWRhMmYyYTVhMjk4Y2Y1N2I.-1h9\">The <strong> valence shell <\/strong> is the outermost electron-occupied shell of an atom.\u00a0 The valence shell holds the electrons that are involved in bonding and are the electrons shown in a Lewis structure.\u00a0 The acronym VSEPR stands for the <strong> valence-shell electron pair repulsion <\/strong> model.\u00a0 The model states that electron pairs will repel each other such that the shape of the molecule will adjust so that the valence electron-pairs stay as far apart from each other as possible. Molecules can be systematically classified according to the number of bonding pairs of electrons as well as the number of nonbonding or lone pairs around the central atom. For the purposes of the VSEPR model, a double or triple bond is no different in terms of repulsion than a single bond.<\/p>\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-NGU1NDczMjFlNjgzMzMxMGY2YTI3YzBlM2ViYjYzMWE.-omr\">\r\n \t<li>VSEPR theory allows more accurate predictions of molecular shape.<\/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.-mbe\">Use the link below to answer the following questions:<\/p>\r\n<p id=\"x-ck12-NzE2NjU3NTUxY2M5YzBhZmFmOTc3ZjgzZjY2OGQyM2U.-vuf\"><a href=\"http:\/\/www.ehow.com\/about_4739704_what-vsepr-model.html\"> http:\/\/www.ehow.com\/about_4739704_what-vsepr-model.html <\/a><\/p>\r\n\r\n<ol id=\"x-ck12-ZGEyNzJmNTkyZGU0YzlmODYzZWU0ZDk2Y2Q1M2UwOGI.-ai0\">\r\n \t<li>When was the VSEPR model first proposed?<\/li>\r\n \t<li>What is the basic theory behind the model?<\/li>\r\n \t<li>What is the significance of this theory?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-Yjg4YzYyYWI1YTljZjg3N2VhZTg1NTY2MTNmZTFlZWQ.-z0q\">\r\n \t<li>Who did the major work in developing the VSEPR theory?<\/li>\r\n \t<li>Where are the electrons that are involved in bonding?<\/li>\r\n \t<li>What is the basic idea behind the VSEPR theory?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<h2 class=\"x-ck12-data-problem-set\">Glossary<\/h2>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-MDgzNWE3MDU2Y2JiZjY2ZTRmMDkyMGRjNmY3YTljODg.-slp\">\r\n \t<li><strong> valence shell: <\/strong> The outermost electron-occupied shell of an atom.<\/li>\r\n \t<li><strong> valence-shell electron pair repulsion (VSEPR): <\/strong> Electron pairs will repel each other such that the shape of the molecule will adjust so that the valence electron-pairs stay as far apart from each other as possible.<\/li>\r\n<\/ul>\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 the VSEPR theory.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3><strong style=\"line-height: 1.5\">What do I do now?<\/strong><\/h3>\n<p id=\"x-ck12-MDdiNDM1MWQ0OTM1Y2RkZWFlZGU5Y2ZmYzRlMWNmMzU.-feb\">In every scientist\u2019s life comes that moment when you realize that you were wrong.\u00a0 Sometimes you think about a problem and recognize where you went astray.\u00a0 Other times you find out when you go into the lab and the experiment doesn\u2019t work (or gets way too exciting). What has to happen then is a change in direction.\u00a0 The good scientist sees the problem and comes up with a new answer.\u00a0 Then that answer has to be tested to see how it works.<\/p>\n<p>Putting atoms together to form compounds can be done on paper or in the lab.\u00a0 However, when the shape of the molecule made in the lab is different from the shape of the molecule drawn on paper, then we need to rethink our ideas and find better explanations.<\/p>\n<\/div>\n<p id=\"x-ck12-OTRlYzFmN2E3YWE5ZGI3NzFjNTUyYmI4OTA4NzhkNjY.-mmd\">In 1956, British scientists R.J. Gillespie and R.S. Nyholm recognized that the current model for explaining bond angles did not work well.\u00a0 The theory at that time relied on hybrid orbitals to explain all aspects of bonding.\u00a0 The problem was that the theory gave incorrect prediction of bond angles for many compounds.\u00a0 They developed a new approach based on earlier work by other scientists that incorporated a consideration of electron pairs in predicting three-dimensional structure.<\/p>\n<p id=\"x-ck12-ZTkyNDVjNTFmYWNlODliYWRhMmYyYTVhMjk4Y2Y1N2I.-1h9\">The <strong> valence shell <\/strong> is the outermost electron-occupied shell of an atom.\u00a0 The valence shell holds the electrons that are involved in bonding and are the electrons shown in a Lewis structure.\u00a0 The acronym VSEPR stands for the <strong> valence-shell electron pair repulsion <\/strong> model.\u00a0 The model states that electron pairs will repel each other such that the shape of the molecule will adjust so that the valence electron-pairs stay as far apart from each other as possible. Molecules can be systematically classified according to the number of bonding pairs of electrons as well as the number of nonbonding or lone pairs around the central atom. For the purposes of the VSEPR model, a double or triple bond is no different in terms of repulsion than a single bond.<\/p>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-NGU1NDczMjFlNjgzMzMxMGY2YTI3YzBlM2ViYjYzMWE.-omr\">\n<li>VSEPR theory allows more accurate predictions of molecular shape.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-mbe\">Use the link below to answer the following questions:<\/p>\n<p id=\"x-ck12-NzE2NjU3NTUxY2M5YzBhZmFmOTc3ZjgzZjY2OGQyM2U.-vuf\"><a href=\"http:\/\/www.ehow.com\/about_4739704_what-vsepr-model.html\"> http:\/\/www.ehow.com\/about_4739704_what-vsepr-model.html <\/a><\/p>\n<ol id=\"x-ck12-ZGEyNzJmNTkyZGU0YzlmODYzZWU0ZDk2Y2Q1M2UwOGI.-ai0\">\n<li>When was the VSEPR model first proposed?<\/li>\n<li>What is the basic theory behind the model?<\/li>\n<li>What is the significance of this theory?<\/li>\n<\/ol>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-Yjg4YzYyYWI1YTljZjg3N2VhZTg1NTY2MTNmZTFlZWQ.-z0q\">\n<li>Who did the major work in developing the VSEPR theory?<\/li>\n<li>Where are the electrons that are involved in bonding?<\/li>\n<li>What is the basic idea behind the VSEPR theory?<\/li>\n<\/ol>\n<\/div>\n<h2 class=\"x-ck12-data-problem-set\">Glossary<\/h2>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-MDgzNWE3MDU2Y2JiZjY2ZTRmMDkyMGRjNmY3YTljODg.-slp\">\n<li><strong> valence shell: <\/strong> The outermost electron-occupied shell of an atom.<\/li>\n<li><strong> valence-shell electron pair repulsion (VSEPR): <\/strong> Electron pairs will repel each other such that the shape of the molecule will adjust so that the valence electron-pairs stay as far apart from each other as possible.<\/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-3066\">\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>\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":11,"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\":\"\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-3066","chapter","type-chapter","status-publish","hentry"],"part":2330,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3066","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":8,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3066\/revisions"}],"predecessor-version":[{"id":3397,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3066\/revisions\/3397"}],"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\/3066\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=3066"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=3066"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=3066"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=3066"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}