{"id":3065,"date":"2016-08-26T02:00:33","date_gmt":"2016-08-26T02:00:33","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=3065"},"modified":"2016-08-26T18:02:18","modified_gmt":"2016-08-26T18:02:18","slug":"bond-energy","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/bond-energy\/","title":{"raw":"Bond Energy","rendered":"Bond Energy"},"content":{"raw":"<div class=\"x-ck12-data-objectives\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\n<ul id=\"x-ck12-OGVkMGIzYWY5N2IxMjZmYWQyNjQ1NDg2YWY3OTczODI.-mq1\">\r\n \t<li>Define bond energy.<\/li>\r\n \t<li>Describe the relationship between reactivity and bond energy.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>How does smog form?<\/h3>\r\n<p id=\"x-ck12-YTk3NGUxMWJlNTEzODA0MTQ2ZjIzZWZhN2QyNmI4NmY.-jjh\"><span class=\"x-ck12-img-inline\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211505\/20140811155254198417.jpeg\" alt=\"Smog over Los Angeles\" width=\"400\" \/><\/span><\/p>\r\n<p id=\"x-ck12-ZjY3ZTZlOGNjOWU3NGZiOTBlNDI0Y2E0MjFjZmVjZGE.-kag\">We know that nitrogen makes up about 79% of the gases in the air and that this gas is chemically very inert.\u00a0 However, we also know that a major contributor to the production of \u00a0smog is a mixture of nitrogen compounds collectively referred to as NO <sub> x <\/sub> .\u00a0 Due to the high combustion temperatures in modern car engines (brought about by the need for better fuel efficiency), we make more NO <sub> x <\/sub> that will react with other materials to create smog.\u00a0 So, our inert nitrogen gas can be converted to other compounds if enough energy is available to break the triple bonds in the N <sub> 2 <\/sub> molecule.<\/p>\r\n\r\n<\/div>\r\n<h2 id=\"x-ck12-Yjk2ZjA4M2VjZjFlNjE4YWYwMzllNmE4NWY2OWM0MzM.-wez_8-srb\"><strong> Bond Energy <\/strong><\/h2>\r\n<p id=\"x-ck12-N2UwZTVmODZkOTVlYWYwNGZlMTQxNDdkMjRkZThlNjk.-en9\">The formation of a chemical bond results in a decrease in potential energy.\u00a0 Consequently, breaking a chemical bond requires an input of energy.\u00a0<strong>Bond energy <\/strong> is the energy required to break a covalent bond between two atoms.\u00a0 A high bond energy means that a bond is strong and the molecule that contains that bond is likely to be stable and less reactive.\u00a0 More reactive compounds will contain bonds that have generally lower bond energies.\u00a0 Some bond energies are listed in the\u00a0table below.<\/p>\r\n\r\n<table id=\"x-ck12-OGFlYjFkZmEyYmE4MjAxZWU2Y2U4NjAxNjEyY2YxMWQ.-vh7\" class=\"x-ck12-nofloat\" border=\"1\"><caption><strong> Bond Energies <\/strong><\/caption>\r\n<tbody>\r\n<tr>\r\n<td><strong> Bond <\/strong><\/td>\r\n<td><strong> Bond Energy (kJ\/mol) <\/strong><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H\u2013H<\/td>\r\n<td>436<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>C\u2013H<\/td>\r\n<td>414<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>C\u2013C<\/td>\r\n<td>347<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>C=C<\/td>\r\n<td>620<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>C\u2261C<\/td>\r\n<td>812<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>F\u2013F<\/td>\r\n<td>157<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Cl\u2013Cl<\/td>\r\n<td>243<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Br\u2013Br<\/td>\r\n<td>193<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>I\u2013I<\/td>\r\n<td>151<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>N\u2261N<\/td>\r\n<td>941<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"x-ck12-YzFkMDNiMjAzMjY3Y2IxM2JiMTcyYjY3YTgxMWQwMzE.-zht\">The halogen elements all exist naturally as diatomic molecules (F<sub>2 <\/sub> , Cl<sub>2 <\/sub> , Br<sub>2 <\/sub> , and I<sub>2<\/sub>).\u00a0 They are generally very reactive and thus have relatively low bond energies.<\/p>\r\n<p id=\"x-ck12-MmViNDE2OGE3MzdkMDhlNzg3Yjc2NzgyNzViYTAyZmM.-5bo\">As can be seen by a comparison of the bond energies for the various carbon-carbon bonds, double bonds are substantially stronger than single bonds. Likewise, triple bonds are even stronger. The triple bond that exists between the nitrogen atoms in nitrogen gas (N<sub>2<\/sub>) makes it very unreactive.\u00a0 All plants and animals require the element nitrogen, but it cannot be obtained from the direct absorption of nitrogen gas from the atmosphere because of its strong, unreactive triple bond.\u00a0 Instead, bacteria convert the nitrogen to a more usable form such as ammonium and nitrate ions, which is then absorbed by plants from the soil.\u00a0 Animals only obtain nitrogen by eating those plants.<\/p>\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-NGI2YmMzNmQyMGEwNjkyMzUxYjk4ZjBjM2E4NzM0YzE.-ree\">\r\n \t<li>Bond energy is an indication of the amount of energy needed for a chemical reaction.<\/li>\r\n \t<li>The higher the bond energy, the less reactive the bond is.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Practice<\/h3>\r\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-qv8\">Use the link below to answer the following questions:<\/p>\r\n<p id=\"x-ck12-OWY5YjE3YjYxYzBkYjJhNGEzY2Q1YWFmYmU5MmJjMmM.-v6v\"><a href=\"http:\/\/chemwiki.ucdavis.edu\/Theoretical_Chemistry\/Chemical_Bonding\/General_Principles\/Bond_Energies\"> http:\/\/chemwiki.ucdavis.edu\/Theoretical_Chemistry\/Chemical_Bonding\/General_Principles\/Bond_Energies <\/a><\/p>\r\n\r\n<ol id=\"x-ck12-MmRkMWVhYmFlOWU3MGZmMWYzOGY5NWFlYzY3Y2ZiOGI.-z32\">\r\n \t<li>What is needed for bonds to break or form?<\/li>\r\n \t<li>The shorter the bond length, the ______ the bond energy.<\/li>\r\n \t<li>A higher bond energy means what?<\/li>\r\n \t<li>Why is the energy change positive when a bond is broken?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-OWU5YzMzMDc0MjJmZmQ2N2I2MzZmNzVjM2JhZmRkNjc.-pa5\">\r\n \t<li>What does a high bond energy mean?<\/li>\r\n \t<li>What kind of bonds do more reactive compounds have?<\/li>\r\n \t<li>Which will react more readily: a C-H bond or a Cl-Cl bond?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<h2 class=\"x-ck12-data-problem-set\">\u00a0Glossary<\/h2>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-MjQ0N2FmMmNmNjYwNjE4MjRmMGVjN2UyMjYwYmVlOGE.-dic\">\r\n \t<li><strong> bond energy: <\/strong> The energy required to break a covalent bond between two atoms.<\/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>Warner Hocker (Flickr: TravelingOtter).<a href=\"http:\/\/www.flickr.com\/photos\/travelingotter\/1552289685\/\">http:\/\/www.flickr.com\/photos\/travelingotter\/1552289685\/ <\/a>.<\/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 id=\"x-ck12-OGVkMGIzYWY5N2IxMjZmYWQyNjQ1NDg2YWY3OTczODI.-mq1\">\n<li>Define bond energy.<\/li>\n<li>Describe the relationship between reactivity and bond energy.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3>How does smog form?<\/h3>\n<p id=\"x-ck12-YTk3NGUxMWJlNTEzODA0MTQ2ZjIzZWZhN2QyNmI4NmY.-jjh\"><span class=\"x-ck12-img-inline\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211505\/20140811155254198417.jpeg\" alt=\"Smog over Los Angeles\" width=\"400\" \/><\/span><\/p>\n<p id=\"x-ck12-ZjY3ZTZlOGNjOWU3NGZiOTBlNDI0Y2E0MjFjZmVjZGE.-kag\">We know that nitrogen makes up about 79% of the gases in the air and that this gas is chemically very inert.\u00a0 However, we also know that a major contributor to the production of \u00a0smog is a mixture of nitrogen compounds collectively referred to as NO <sub> x <\/sub> .\u00a0 Due to the high combustion temperatures in modern car engines (brought about by the need for better fuel efficiency), we make more NO <sub> x <\/sub> that will react with other materials to create smog.\u00a0 So, our inert nitrogen gas can be converted to other compounds if enough energy is available to break the triple bonds in the N <sub> 2 <\/sub> molecule.<\/p>\n<\/div>\n<h2 id=\"x-ck12-Yjk2ZjA4M2VjZjFlNjE4YWYwMzllNmE4NWY2OWM0MzM.-wez_8-srb\"><strong> Bond Energy <\/strong><\/h2>\n<p id=\"x-ck12-N2UwZTVmODZkOTVlYWYwNGZlMTQxNDdkMjRkZThlNjk.-en9\">The formation of a chemical bond results in a decrease in potential energy.\u00a0 Consequently, breaking a chemical bond requires an input of energy.\u00a0<strong>Bond energy <\/strong> is the energy required to break a covalent bond between two atoms.\u00a0 A high bond energy means that a bond is strong and the molecule that contains that bond is likely to be stable and less reactive.\u00a0 More reactive compounds will contain bonds that have generally lower bond energies.\u00a0 Some bond energies are listed in the\u00a0table below.<\/p>\n<table id=\"x-ck12-OGFlYjFkZmEyYmE4MjAxZWU2Y2U4NjAxNjEyY2YxMWQ.-vh7\" class=\"x-ck12-nofloat\">\n<caption><strong> Bond Energies <\/strong><\/caption>\n<tbody>\n<tr>\n<td><strong> Bond <\/strong><\/td>\n<td><strong> Bond Energy (kJ\/mol) <\/strong><\/td>\n<\/tr>\n<tr>\n<td>H\u2013H<\/td>\n<td>436<\/td>\n<\/tr>\n<tr>\n<td>C\u2013H<\/td>\n<td>414<\/td>\n<\/tr>\n<tr>\n<td>C\u2013C<\/td>\n<td>347<\/td>\n<\/tr>\n<tr>\n<td>C=C<\/td>\n<td>620<\/td>\n<\/tr>\n<tr>\n<td>C\u2261C<\/td>\n<td>812<\/td>\n<\/tr>\n<tr>\n<td>F\u2013F<\/td>\n<td>157<\/td>\n<\/tr>\n<tr>\n<td>Cl\u2013Cl<\/td>\n<td>243<\/td>\n<\/tr>\n<tr>\n<td>Br\u2013Br<\/td>\n<td>193<\/td>\n<\/tr>\n<tr>\n<td>I\u2013I<\/td>\n<td>151<\/td>\n<\/tr>\n<tr>\n<td>N\u2261N<\/td>\n<td>941<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"x-ck12-YzFkMDNiMjAzMjY3Y2IxM2JiMTcyYjY3YTgxMWQwMzE.-zht\">The halogen elements all exist naturally as diatomic molecules (F<sub>2 <\/sub> , Cl<sub>2 <\/sub> , Br<sub>2 <\/sub> , and I<sub>2<\/sub>).\u00a0 They are generally very reactive and thus have relatively low bond energies.<\/p>\n<p id=\"x-ck12-MmViNDE2OGE3MzdkMDhlNzg3Yjc2NzgyNzViYTAyZmM.-5bo\">As can be seen by a comparison of the bond energies for the various carbon-carbon bonds, double bonds are substantially stronger than single bonds. Likewise, triple bonds are even stronger. The triple bond that exists between the nitrogen atoms in nitrogen gas (N<sub>2<\/sub>) makes it very unreactive.\u00a0 All plants and animals require the element nitrogen, but it cannot be obtained from the direct absorption of nitrogen gas from the atmosphere because of its strong, unreactive triple bond.\u00a0 Instead, bacteria convert the nitrogen to a more usable form such as ammonium and nitrate ions, which is then absorbed by plants from the soil.\u00a0 Animals only obtain nitrogen by eating those plants.<\/p>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-NGI2YmMzNmQyMGEwNjkyMzUxYjk4ZjBjM2E4NzM0YzE.-ree\">\n<li>Bond energy is an indication of the amount of energy needed for a chemical reaction.<\/li>\n<li>The higher the bond energy, the less reactive the bond is.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-qv8\">Use the link below to answer the following questions:<\/p>\n<p id=\"x-ck12-OWY5YjE3YjYxYzBkYjJhNGEzY2Q1YWFmYmU5MmJjMmM.-v6v\"><a href=\"http:\/\/chemwiki.ucdavis.edu\/Theoretical_Chemistry\/Chemical_Bonding\/General_Principles\/Bond_Energies\"> http:\/\/chemwiki.ucdavis.edu\/Theoretical_Chemistry\/Chemical_Bonding\/General_Principles\/Bond_Energies <\/a><\/p>\n<ol id=\"x-ck12-MmRkMWVhYmFlOWU3MGZmMWYzOGY5NWFlYzY3Y2ZiOGI.-z32\">\n<li>What is needed for bonds to break or form?<\/li>\n<li>The shorter the bond length, the ______ the bond energy.<\/li>\n<li>A higher bond energy means what?<\/li>\n<li>Why is the energy change positive when a bond is broken?<\/li>\n<\/ol>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-OWU5YzMzMDc0MjJmZmQ2N2I2MzZmNzVjM2JhZmRkNjc.-pa5\">\n<li>What does a high bond energy mean?<\/li>\n<li>What kind of bonds do more reactive compounds have?<\/li>\n<li>Which will react more readily: a C-H bond or a Cl-Cl bond?<\/li>\n<\/ol>\n<\/div>\n<h2 class=\"x-ck12-data-problem-set\">\u00a0Glossary<\/h2>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-MjQ0N2FmMmNmNjYwNjE4MjRmMGVjN2UyMjYwYmVlOGE.-dic\">\n<li><strong> bond energy: <\/strong> The energy required to break a covalent bond between two atoms.<\/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>Warner Hocker (Flickr: TravelingOtter).<a href=\"http:\/\/www.flickr.com\/photos\/travelingotter\/1552289685\/\">http:\/\/www.flickr.com\/photos\/travelingotter\/1552289685\/ <\/a>.<\/li>\n<\/ol>\n<\/div>\n<\/div>\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-3065\">\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":10,"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-3065","chapter","type-chapter","status-publish","hentry"],"part":2330,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3065","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":6,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3065\/revisions"}],"predecessor-version":[{"id":3305,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3065\/revisions\/3305"}],"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\/3065\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=3065"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=3065"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=3065"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=3065"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}