{"id":1778,"date":"2017-10-10T15:29:36","date_gmt":"2017-10-10T15:29:36","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/?post_type=chapter&#038;p=1778"},"modified":"2018-10-05T19:53:42","modified_gmt":"2018-10-05T19:53:42","slug":"stability-of-conjugated-dienes-mo-theory","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/chapter\/stability-of-conjugated-dienes-mo-theory\/","title":{"raw":"Stability of Conjugated Dienes MO Theory","rendered":"Stability of Conjugated Dienes MO Theory"},"content":{"raw":"<div class=\"elm-header\">\r\n<div class=\"elm-header-custom\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Objectives<\/h3>\r\n<div id=\"elm-main-content\" class=\"elm-content-container\">\r\n<div>\r\n<div id=\"skills\">\r\n\r\nAfter completing this section, you should be able to\r\n<ol>\r\n \t<li>write a reaction sequence to show a convenient method for preparing a given conjugated diene from an alkene, allyl halide, alkyl dihalide or alcohol (diol).<\/li>\r\n \t<li>identify the reagents needed to prepare a given diene from one of the starting materials listed in Objective 1, above.<\/li>\r\n \t<li>compare the stabilities of conjugated and nonconjugated dienes, using evidence obtained from hydrogenation experiments.<\/li>\r\n \t<li>discuss the bonding in a conjugated diene, such as 1,3-butadiene, in terms of the hybridization of the carbon atoms involved.<\/li>\r\n \t<li>discuss the bonding in 1,3-butadiene in terms of the molecular orbital theory, and draw a molecular orbital for this and similar compounds.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Key TERMS<\/h3>\r\n<div class=\"elm-header\"><\/div>\r\n<div id=\"elm-main-content\" class=\"elm-content-container\">\r\n<div>\r\n<div>\r\n\r\nMake certain that you can define, and use in context, the key terms below.\r\n<ul>\r\n \t<li>delocalized electrons<\/li>\r\n \t<li>node<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox\">\r\n<div class=\"elm-header\">\r\n<div class=\"elm-header-custom\">\r\n<h3>Study Notes<\/h3>\r\n<\/div>\r\n<\/div>\r\n<div id=\"elm-main-content\" class=\"elm-content-container\">\r\n<div id=\"note\">\r\n\r\nThe two most frequent ways to synthesize conjugated dienes are dehydration of alcohols and dehydrohalogenation of organohalides, which were introduced in the preparation of alkenes (Section 8.1). The following scheme illustrates some ofthe routes to preparing a conjugated diene.<img class=\"aligncenter\" src=\"http:\/\/chem.libretexts.org\/@api\/deki\/files\/87116\/14-1a.png?origin=mt-web\" alt=\"various synthetic routes to 1,3-butadiene\" \/>\r\n\r\n&nbsp;\r\n\r\nThe formation of synthetic polymers from dienes such as 1,3-butadiene and isoprene is discussed in Section 14.6. Synthetic polymers are large molecules made up of smaller repeating units. You are probably somewhat familiar with a number of these polymers; for example, polyethylene, polypropylene, polystyrene and poly(vinyl chloride).\r\n\r\nAs the hydrogenation of 1,3-butadiene releases less than the predicted amount of energy, the energy content of 1,3-butadiene must be lower than we might have expected. In other words, 1,3-butadiene is more stable than its formula suggests.\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"391\"]<img src=\"http:\/\/chem.libretexts.org\/@api\/deki\/files\/87117\/14-1b.png?origin=mt-web\" alt=\"energy diagram for the hydrogenation of 1,3-butadiene\" width=\"391\" height=\"331\" \/> Figure 14.1: Energy diagram for the hydrogenation of 1,3-butadiene (not to scale).[\/caption]\r\n\r\n&nbsp;\r\n\r\n&nbsp;\r\n\r\nSome university-level general chemistry courses do not introduce the subject of molecular orbitals. If you have taken such a course, or forgotten what is meant by the term \u201cmolecular orbital,\u201d combine a review of Section 1.11 with your study of this section.\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"elm-main-content\" class=\"elm-content-container\">\r\n<div>\r\n\r\nConjugated dienes are more stable than non conjugated dienes (both isolated and cumulated) due to factors such as delocalization of charge through resonance and hybridization energy. This can also explain why <a title=\"Organic Chemistry\/Conjugation\/Overlap of Adjacent p Orbitals-Electron Delocalization\" href=\"https:\/\/chem.libretexts.org\/Core\/Organic_Chemistry\/Conjugation\/Overlap_of_Adjacent_p_Orbitals-Electron_Delocalization\" rel=\"internal\">allylic radicals<\/a> are much more stable than secondary or even tertiary carbocations. This is all due to the positioning of the pi orbitals and ability for overlap to occur to strengthen the single bond between the two double bonds.\r\n\r\nThe resonance structure shown below gives a good understanding of how the charge is delocalized across the four carbons in this conjugated diene. This delocalization of charges stablizes the conjugated diene:\r\n\r\n<img class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1608\/Resonance.bmp?revision=1#fixme\" alt=\"Resonance.bmp\" width=\"727\" height=\"104\" \/>\r\n\r\nAlong with resonance, hybridization energy effect the stability of the compound. For example in 1,3-butadiene the carbons with the single bond are sp2 hybridized unlike in nonconjugated dienes where the carbons with single bonds are sp3 hybridized. This difference in hybridization shows that the conjugated dienes have more 's' character and draw in more of the pi electrons, thus making the single bond stronger and shorter than an ordinary alkane C-C bond (1.54\u00c5).\r\n\r\n<img class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1601\/piorbitaloverlaps.bmp?revision=1&amp;size=bestfit&amp;width=603&amp;height=261#fixme\" alt=\"piorbitaloverlaps.bmp\" width=\"603px\" height=\"261px\" \/>\r\n\r\nAnother useful resource to consider are the heats of hydrogenation of different arrangements of double bonds. Since the higher the heat of hydrogenation the less stable the compound, it is shown below that conjugated dienes (~54 kcal) have a lower heat of hydrogenation than their isolated (~60 kcal) and cumulated diene (~70 kcal) counterparts.\r\n\r\nHere is an energy diagram comparing different types of bonds with their heats of hydrogenation to show relative stability of each molecule:\r\n\r\n<img class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1590\/energychart.bmp?revision=1#fixme\" alt=\"energychart.bmp\" width=\"613\" height=\"316\" \/>\r\n\r\nThe stabilization of dienes by conjugation is less dramatic than the aromatic stabilization of benzene. Nevertheless, similar resonance and molecular orbital descriptions of conjugation may be written.\r\n<div id=\"section_1\">\r\n<h3 class=\"editable\">Allylic Carbocation<\/h3>\r\nConjugation occurs when p orbital on three or more adjacent atoms can overlap\u00a0 Conjugation tends to stabilize molecules\r\n\r\nAllylic carbocations are a common conjugated system.\r\n\r\nThe positive charge of a carbocation is contained in a P orbital of a <em>sp<sup>2<\/sup><\/em> hybrizied carbon.\u00a0 This allows for overlap with double bonds.\u00a0 The positive charge is more stable because it is spread over 2 carbons.\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\/05154837\/allylic_ccarbocat.png\" alt=\"allylic ccarbocat.png\" width=\"355px\" height=\"233px\" \/>\r\n<div id=\"section_2\">\r\n<h4 class=\"editable\">Molecular Orbitals of an Allylic Carbocation<\/h4>\r\nThe stability of the carbocation of propene is due to a conjugated \u03c0 electron system. A \"double bond\" doesn't really exist. Instead, it is a group of 3 adjacent, overlapping, non-hybridized <em>p\u00a0<\/em>orbitals we call a <strong>conjugated \u03c0 electron system<\/strong>. You can clearly see the interactions between all three of the <em>p <\/em>orbitals from the three carbons resulting in a really stable cation. It all comes down to\u00a0 where the location of the electron-deficient carbon is.\r\n\r\nMolecular orbital descriptions can explain allylic stability in yet another way using 2-propenyl. Fig.6\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\/05154839\/MO_diagram_of_3_orbitals.png\" alt=\"MO diagram of 3 orbitals.png\" width=\"383px\" height=\"395px\" \/>\r\n\r\n<strong>Fig.6 Shows the 3 possible Molecular orbitals of 2-propenyl<\/strong>\r\n\r\nIf we just take the \u03c0 molecular orbital and not any of the s, we get three of them. \u03c0<sub>1 <\/sub>is bonding with no nodes,\u00a0 \u03c0<sub>2<\/sub> is nonbonding (In other words, the same energy as a regular <em>p<\/em>-orbital) with a node, and \u03c0<sub>3<\/sub> is antibonding with 2 nodes (none of the orbitals are interacting). The first two electrons will go into the\u00a0 \u03c0<sub>1 <\/sub>molecular orbital, regardless of whether it is a cation, radical, or anion. If it is a radical or anion, the next electron goes into the\u00a0 \u03c0<sub>2<\/sub> molecular orbital. The last anion electron goes into the nonbonding orbital also. So no matter what kind of carbon center exists, no electron will ever go into the antibonding orbital.\r\n\r\nThe Bonding orbitals are the lowest energy orbitals and are favorable, which is why they are filled first. Even though the nonbonding orbitals can be filled, the overall energy of the system is still lower and more stable due to the filled bonding molecular orbitals.\r\n\r\nThis figure also shows that \u03c0<sub>2 <\/sub>is the only molecular orbital where the electrion differs, and it is also where a single node passes through the middle. Because of this, the charges of the molecule are mainly on the two terminal carbons and not the middle carbon.\r\n\r\nThis molecular orbital description can also illustrate the stability of allylic carbon centers in figure 7.\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\/05154841\/energy_diagram.png\" alt=\"energy diagram.png\" width=\"495\" height=\"268\" \/>\r\n\r\n<em><strong>Fig. 7: <\/strong>diagram showing how the electrons fill based on the Aufbau principle.<\/em>\r\n\r\nThe \u03c0 bonding orbital is lower in energy than the nonbonding <em>p <\/em>orbital. Since every carbon center shown has two electrons in the lower energy, bonding \u03c0 orbitals, the energy of each system is lowered overall (and thus more stable), regardless of cation, radical, or anion.\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"section_3\">\r\n<h3 class=\"editable\">1,3-Dienes<\/h3>\r\nConjugated double bonds are separated by a single bond. 1,3-dienes are an excellent example of a conjugated system.\u00a0 Each carbon in 1,3 dienes are<em> sp<sup>2<\/sup><\/em> hybridized and therefore have one <em>p<\/em> orbital. The four <em>p <\/em>orbitals in 1,3-butadiene overlap to form a conjugated system.\r\n\r\n<img class=\"size-medium wp-image-1886 aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/10152806\/13-diene-300x286.png\" alt=\"\" width=\"300\" height=\"286\" \/>\r\n\r\n<img src=\"https:\/\/chem.libretexts.org\/LibreTexts\/Athabasca_University\/Chemistry_350%3A_Organic_Chemistry_I\/Chapter_14%3A_Conjugated_Compounds_and_Ultraviolet_Spectroscopy\/denied:data:image\/png;base64,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#fixme\" alt=\"\" width=\"195\" height=\"188\" \/><img class=\"size-medium wp-image-1885 aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/10152731\/13-dienes-300x179.png\" alt=\"\" width=\"300\" height=\"179\" \/>\r\n\r\n<\/div>\r\n<div id=\"section_4\">\r\n<h3 class=\"editable\"><strong>Conjugated vs. Nonconjugated Dienes<\/strong><\/h3>\r\nConjugated dienes are two double bonds separated by a single bond\r\n\r\n<img class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1586\/conjugated_diene2_(1).bmp?revision=1&amp;size=bestfit&amp;width=182&amp;height=64#fixme\" alt=\"conjugated_diene2 (1).bmp\" width=\"182px\" height=\"64px\" \/>\r\n\r\nNonconjugated (Isolated) Dienes are two double bonds are separated by more than one single bond.\r\n\r\n<img class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1598\/nonconjugated_diene_(1).bmp?revision=1&amp;size=bestfit&amp;width=159&amp;height=64#fixme\" alt=\"nonconjugated_diene (1).bmp\" width=\"159px\" height=\"64px\" \/>\r\n\r\nWhen using electrostatic potential maps, it is observed that the pi electron density overlap is closer together and delocalized in conjugated dienes, while in non conjugated dienes the pi electron density is located differently across the molecule. Since having more electron density delocalized makes the molecule more stable conjugated dienes are more stable than non conjugated\r\n\r\nFor example in 1,3-butadiene the carbons with the single bond are sp2 hybridized unlike in nonconjugated dienes where the carbons with single bonds are sp3 hybridized. This difference in hybridization shows that the conjugated dienes have more 's' character and draw in more of the pi electrons, thus making the single bond stronger and shorter than an ordinary alkane C-C bond (1.54\u00c5).\r\n\r\n<\/div>\r\n<div id=\"section_5\">\r\n<h3 class=\"editable\">Stability of Conjugated Dienes<\/h3>\r\nConjugated dienes are more stable than non conjugated dienes (both isolated and cumulated) due to factors such as delocalization of charge through resonance and hybridization energy. This can also explain why allylic radicals are much more stable than secondary or even tertiary carbocations. This is all due to the positioning of the pi orbitals and ability for overlap to occur to strengthen the single bond between the two double bonds.\r\n\r\nThe resonance structure shown below gives a good understanding of how the charge is delocalized across the four carbons in this conjugated diene. This delocalization of charges stablizes the conjugated diene:\r\n\r\n<img class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1608\/Resonance.bmp?revision=1#fixme\" alt=\"Resonance.bmp\" width=\"636\" height=\"91\" \/>\r\n\r\nAlong with resonance, hybridization energy effect the stability of the compound. For example in 1,3-butadiene the carbons with the single bond are sp2 hybridized unlike in nonconjugated dienes where the carbons with single bonds are sp3 hybridized. This difference in hybridization shows that the conjugated dienes have more 's' character and draw in more of the pi electrons, thus making the single bond stronger and shorter than an ordinary alkane C-C bond (1.54\u00c5).\r\n\r\n<\/div>\r\n<div id=\"section_6\">\r\n<h3 class=\"editable\">Molecular Orbitals of 1,3 Dienes<\/h3>\r\nA molecular orbital model for 1,3-butadiene is shown below. Note that the lobes of the four p-orbital components in each pi-orbital are colored differently and carry a plus or minus sign. This distinction refers to different phases, defined by the mathematical wave equations for such orbitals. Regions in which adjacent orbital lobes undergo a phase change are called <strong>nodes<\/strong>. Orbital electron density is zero in such regions. Thus a single p-orbital has a node at the nucleus, and all the pi-orbitals shown here have a nodal plane that is defined by the atoms of the diene. This is the only nodal surface in the lowest energy pi-orbital, \u03c0<sub>1<\/sub>. Higher energy pi-orbitals have an increasing number of nodes.\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\/05154845\/budienmo.gif\" alt=\"budienmo.gif\" width=\"530\" height=\"305\" \/>\r\n\r\n<\/div>\r\n<div id=\"section_7\">\r\n<div class=\"textbox exercises\">\r\n<h3 class=\"editable\">Exercise<\/h3>\r\n<div id=\"s61719\">\r\n<div>\r\n<h4 id=\"Questions-61719\">Question<\/h4>\r\nThe heat of hydrogenation for allene is about 300 kJ\/mol. Order a conjugated diene, a non-conjugated diene, and allene in increasing stability.\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\/05154847\/14.1.png\" alt=\"\" width=\"153\" height=\"173\" \/>\r\n\r\n<\/div>\r\n<h3>Solution<\/h3>\r\n<div>\r\n\r\n[reveal-answer q=\"224739\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"224739\"]\u00a0allene &lt; non-conjugated \u00a0diene &lt; conjugated diene (most stable)[\/hidden-answer]\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"section_8\">\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\">\n<div class=\"elm-header-custom\">\n<div class=\"textbox learning-objectives\">\n<h3>Objectives<\/h3>\n<div id=\"elm-main-content\" class=\"elm-content-container\">\n<div>\n<div id=\"skills\">\n<p>After completing this section, you should be able to<\/p>\n<ol>\n<li>write a reaction sequence to show a convenient method for preparing a given conjugated diene from an alkene, allyl halide, alkyl dihalide or alcohol (diol).<\/li>\n<li>identify the reagents needed to prepare a given diene from one of the starting materials listed in Objective 1, above.<\/li>\n<li>compare the stabilities of conjugated and nonconjugated dienes, using evidence obtained from hydrogenation experiments.<\/li>\n<li>discuss the bonding in a conjugated diene, such as 1,3-butadiene, in terms of the hybridization of the carbon atoms involved.<\/li>\n<li>discuss the bonding in 1,3-butadiene in terms of the molecular orbital theory, and draw a molecular orbital for this and similar compounds.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox key-takeaways\">\n<h3>Key TERMS<\/h3>\n<div class=\"elm-header\"><\/div>\n<div id=\"elm-main-content\" class=\"elm-content-container\">\n<div>\n<div>\n<p>Make certain that you can define, and use in context, the key terms below.<\/p>\n<ul>\n<li>delocalized electrons<\/li>\n<li>node<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox\">\n<div class=\"elm-header\">\n<div class=\"elm-header-custom\">\n<h3>Study Notes<\/h3>\n<\/div>\n<\/div>\n<div id=\"elm-main-content\" class=\"elm-content-container\">\n<div id=\"note\">\n<p>The two most frequent ways to synthesize conjugated dienes are dehydration of alcohols and dehydrohalogenation of organohalides, which were introduced in the preparation of alkenes (Section 8.1). The following scheme illustrates some ofthe routes to preparing a conjugated diene.<img decoding=\"async\" class=\"aligncenter\" src=\"http:\/\/chem.libretexts.org\/@api\/deki\/files\/87116\/14-1a.png?origin=mt-web\" alt=\"various synthetic routes to 1,3-butadiene\" \/><\/p>\n<p>&nbsp;<\/p>\n<p>The formation of synthetic polymers from dienes such as 1,3-butadiene and isoprene is discussed in Section 14.6. Synthetic polymers are large molecules made up of smaller repeating units. You are probably somewhat familiar with a number of these polymers; for example, polyethylene, polypropylene, polystyrene and poly(vinyl chloride).<\/p>\n<p>As the hydrogenation of 1,3-butadiene releases less than the predicted amount of energy, the energy content of 1,3-butadiene must be lower than we might have expected. In other words, 1,3-butadiene is more stable than its formula suggests.<\/p>\n<div style=\"width: 401px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/chem.libretexts.org\/@api\/deki\/files\/87117\/14-1b.png?origin=mt-web\" alt=\"energy diagram for the hydrogenation of 1,3-butadiene\" width=\"391\" height=\"331\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 14.1: Energy diagram for the hydrogenation of 1,3-butadiene (not to scale).<\/p>\n<\/div>\n<p>&nbsp;<\/p>\n<p>&nbsp;<\/p>\n<p>Some university-level general chemistry courses do not introduce the subject of molecular orbitals. If you have taken such a course, or forgotten what is meant by the term \u201cmolecular orbital,\u201d combine a review of Section 1.11 with your study of this section.<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"elm-main-content\" class=\"elm-content-container\">\n<div>\n<p>Conjugated dienes are more stable than non conjugated dienes (both isolated and cumulated) due to factors such as delocalization of charge through resonance and hybridization energy. This can also explain why <a title=\"Organic Chemistry\/Conjugation\/Overlap of Adjacent p Orbitals-Electron Delocalization\" href=\"https:\/\/chem.libretexts.org\/Core\/Organic_Chemistry\/Conjugation\/Overlap_of_Adjacent_p_Orbitals-Electron_Delocalization\" rel=\"internal\">allylic radicals<\/a> are much more stable than secondary or even tertiary carbocations. This is all due to the positioning of the pi orbitals and ability for overlap to occur to strengthen the single bond between the two double bonds.<\/p>\n<p>The resonance structure shown below gives a good understanding of how the charge is delocalized across the four carbons in this conjugated diene. This delocalization of charges stablizes the conjugated diene:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1608\/Resonance.bmp?revision=1#fixme\" alt=\"Resonance.bmp\" width=\"727\" height=\"104\" \/><\/p>\n<p>Along with resonance, hybridization energy effect the stability of the compound. For example in 1,3-butadiene the carbons with the single bond are sp2 hybridized unlike in nonconjugated dienes where the carbons with single bonds are sp3 hybridized. This difference in hybridization shows that the conjugated dienes have more &#8216;s&#8217; character and draw in more of the pi electrons, thus making the single bond stronger and shorter than an ordinary alkane C-C bond (1.54\u00c5).<\/p>\n<p><img decoding=\"async\" class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1601\/piorbitaloverlaps.bmp?revision=1&amp;size=bestfit&amp;width=603&amp;height=261#fixme\" alt=\"piorbitaloverlaps.bmp\" width=\"603px\" height=\"261px\" \/><\/p>\n<p>Another useful resource to consider are the heats of hydrogenation of different arrangements of double bonds. Since the higher the heat of hydrogenation the less stable the compound, it is shown below that conjugated dienes (~54 kcal) have a lower heat of hydrogenation than their isolated (~60 kcal) and cumulated diene (~70 kcal) counterparts.<\/p>\n<p>Here is an energy diagram comparing different types of bonds with their heats of hydrogenation to show relative stability of each molecule:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1590\/energychart.bmp?revision=1#fixme\" alt=\"energychart.bmp\" width=\"613\" height=\"316\" \/><\/p>\n<p>The stabilization of dienes by conjugation is less dramatic than the aromatic stabilization of benzene. Nevertheless, similar resonance and molecular orbital descriptions of conjugation may be written.<\/p>\n<div id=\"section_1\">\n<h3 class=\"editable\">Allylic Carbocation<\/h3>\n<p>Conjugation occurs when p orbital on three or more adjacent atoms can overlap\u00a0 Conjugation tends to stabilize molecules<\/p>\n<p>Allylic carbocations are a common conjugated system.<\/p>\n<p>The positive charge of a carbocation is contained in a P orbital of a <em>sp<sup>2<\/sup><\/em> hybrizied carbon.\u00a0 This allows for overlap with double bonds.\u00a0 The positive charge is more stable because it is spread over 2 carbons.<\/p>\n<p><img decoding=\"async\" class=\"internal default aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/05154837\/allylic_ccarbocat.png\" alt=\"allylic ccarbocat.png\" width=\"355px\" height=\"233px\" \/><\/p>\n<div id=\"section_2\">\n<h4 class=\"editable\">Molecular Orbitals of an Allylic Carbocation<\/h4>\n<p>The stability of the carbocation of propene is due to a conjugated \u03c0 electron system. A &#8220;double bond&#8221; doesn&#8217;t really exist. Instead, it is a group of 3 adjacent, overlapping, non-hybridized <em>p\u00a0<\/em>orbitals we call a <strong>conjugated \u03c0 electron system<\/strong>. You can clearly see the interactions between all three of the <em>p <\/em>orbitals from the three carbons resulting in a really stable cation. It all comes down to\u00a0 where the location of the electron-deficient carbon is.<\/p>\n<p>Molecular orbital descriptions can explain allylic stability in yet another way using 2-propenyl. Fig.6<\/p>\n<p><img decoding=\"async\" class=\"internal default aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/05154839\/MO_diagram_of_3_orbitals.png\" alt=\"MO diagram of 3 orbitals.png\" width=\"383px\" height=\"395px\" \/><\/p>\n<p><strong>Fig.6 Shows the 3 possible Molecular orbitals of 2-propenyl<\/strong><\/p>\n<p>If we just take the \u03c0 molecular orbital and not any of the s, we get three of them. \u03c0<sub>1 <\/sub>is bonding with no nodes,\u00a0 \u03c0<sub>2<\/sub> is nonbonding (In other words, the same energy as a regular <em>p<\/em>-orbital) with a node, and \u03c0<sub>3<\/sub> is antibonding with 2 nodes (none of the orbitals are interacting). The first two electrons will go into the\u00a0 \u03c0<sub>1 <\/sub>molecular orbital, regardless of whether it is a cation, radical, or anion. If it is a radical or anion, the next electron goes into the\u00a0 \u03c0<sub>2<\/sub> molecular orbital. The last anion electron goes into the nonbonding orbital also. So no matter what kind of carbon center exists, no electron will ever go into the antibonding orbital.<\/p>\n<p>The Bonding orbitals are the lowest energy orbitals and are favorable, which is why they are filled first. Even though the nonbonding orbitals can be filled, the overall energy of the system is still lower and more stable due to the filled bonding molecular orbitals.<\/p>\n<p>This figure also shows that \u03c0<sub>2 <\/sub>is the only molecular orbital where the electrion differs, and it is also where a single node passes through the middle. Because of this, the charges of the molecule are mainly on the two terminal carbons and not the middle carbon.<\/p>\n<p>This molecular orbital description can also illustrate the stability of allylic carbon centers in figure 7.<\/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\/05154841\/energy_diagram.png\" alt=\"energy diagram.png\" width=\"495\" height=\"268\" \/><\/p>\n<p><em><strong>Fig. 7: <\/strong>diagram showing how the electrons fill based on the Aufbau principle.<\/em><\/p>\n<p>The \u03c0 bonding orbital is lower in energy than the nonbonding <em>p <\/em>orbital. Since every carbon center shown has two electrons in the lower energy, bonding \u03c0 orbitals, the energy of each system is lowered overall (and thus more stable), regardless of cation, radical, or anion.<\/p>\n<\/div>\n<\/div>\n<div id=\"section_3\">\n<h3 class=\"editable\">1,3-Dienes<\/h3>\n<p>Conjugated double bonds are separated by a single bond. 1,3-dienes are an excellent example of a conjugated system.\u00a0 Each carbon in 1,3 dienes are<em> sp<sup>2<\/sup><\/em> hybridized and therefore have one <em>p<\/em> orbital. The four <em>p <\/em>orbitals in 1,3-butadiene overlap to form a conjugated system.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"size-medium wp-image-1886 aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/10152806\/13-diene-300x286.png\" alt=\"\" width=\"300\" height=\"286\" \/><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chem.libretexts.org\/LibreTexts\/Athabasca_University\/Chemistry_350%3A_Organic_Chemistry_I\/Chapter_14%3A_Conjugated_Compounds_and_Ultraviolet_Spectroscopy\/denied:data:image\/png;base64,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#fixme\" alt=\"\" width=\"195\" height=\"188\" \/><img loading=\"lazy\" decoding=\"async\" class=\"size-medium wp-image-1885 aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/1518\/2017\/10\/10152731\/13-dienes-300x179.png\" alt=\"\" width=\"300\" height=\"179\" \/><\/p>\n<\/div>\n<div id=\"section_4\">\n<h3 class=\"editable\"><strong>Conjugated vs. Nonconjugated Dienes<\/strong><\/h3>\n<p>Conjugated dienes are two double bonds separated by a single bond<\/p>\n<p><img decoding=\"async\" class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1586\/conjugated_diene2_(1).bmp?revision=1&amp;size=bestfit&amp;width=182&amp;height=64#fixme\" alt=\"conjugated_diene2 (1).bmp\" width=\"182px\" height=\"64px\" \/><\/p>\n<p>Nonconjugated (Isolated) Dienes are two double bonds are separated by more than one single bond.<\/p>\n<p><img decoding=\"async\" class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1598\/nonconjugated_diene_(1).bmp?revision=1&amp;size=bestfit&amp;width=159&amp;height=64#fixme\" alt=\"nonconjugated_diene (1).bmp\" width=\"159px\" height=\"64px\" \/><\/p>\n<p>When using electrostatic potential maps, it is observed that the pi electron density overlap is closer together and delocalized in conjugated dienes, while in non conjugated dienes the pi electron density is located differently across the molecule. Since having more electron density delocalized makes the molecule more stable conjugated dienes are more stable than non conjugated<\/p>\n<p>For example in 1,3-butadiene the carbons with the single bond are sp2 hybridized unlike in nonconjugated dienes where the carbons with single bonds are sp3 hybridized. This difference in hybridization shows that the conjugated dienes have more &#8216;s&#8217; character and draw in more of the pi electrons, thus making the single bond stronger and shorter than an ordinary alkane C-C bond (1.54\u00c5).<\/p>\n<\/div>\n<div id=\"section_5\">\n<h3 class=\"editable\">Stability of Conjugated Dienes<\/h3>\n<p>Conjugated dienes are more stable than non conjugated dienes (both isolated and cumulated) due to factors such as delocalization of charge through resonance and hybridization energy. This can also explain why allylic radicals are much more stable than secondary or even tertiary carbocations. This is all due to the positioning of the pi orbitals and ability for overlap to occur to strengthen the single bond between the two double bonds.<\/p>\n<p>The resonance structure shown below gives a good understanding of how the charge is delocalized across the four carbons in this conjugated diene. This delocalization of charges stablizes the conjugated diene:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"internal aligncenter\" src=\"https:\/\/chem.libretexts.org\/@api\/deki\/files\/1608\/Resonance.bmp?revision=1#fixme\" alt=\"Resonance.bmp\" width=\"636\" height=\"91\" \/><\/p>\n<p>Along with resonance, hybridization energy effect the stability of the compound. For example in 1,3-butadiene the carbons with the single bond are sp2 hybridized unlike in nonconjugated dienes where the carbons with single bonds are sp3 hybridized. This difference in hybridization shows that the conjugated dienes have more &#8216;s&#8217; character and draw in more of the pi electrons, thus making the single bond stronger and shorter than an ordinary alkane C-C bond (1.54\u00c5).<\/p>\n<\/div>\n<div id=\"section_6\">\n<h3 class=\"editable\">Molecular Orbitals of 1,3 Dienes<\/h3>\n<p>A molecular orbital model for 1,3-butadiene is shown below. Note that the lobes of the four p-orbital components in each pi-orbital are colored differently and carry a plus or minus sign. This distinction refers to different phases, defined by the mathematical wave equations for such orbitals. Regions in which adjacent orbital lobes undergo a phase change are called <strong>nodes<\/strong>. Orbital electron density is zero in such regions. Thus a single p-orbital has a node at the nucleus, and all the pi-orbitals shown here have a nodal plane that is defined by the atoms of the diene. This is the only nodal surface in the lowest energy pi-orbital, \u03c0<sub>1<\/sub>. Higher energy pi-orbitals have an increasing number of nodes.<\/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\/05154845\/budienmo.gif\" alt=\"budienmo.gif\" width=\"530\" height=\"305\" \/><\/p>\n<\/div>\n<div id=\"section_7\">\n<div class=\"textbox exercises\">\n<h3 class=\"editable\">Exercise<\/h3>\n<div id=\"s61719\">\n<div>\n<h4 id=\"Questions-61719\">Question<\/h4>\n<p>The heat of hydrogenation for allene is about 300 kJ\/mol. Order a conjugated diene, a non-conjugated diene, and allene in increasing stability.<\/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\/05154847\/14.1.png\" alt=\"\" width=\"153\" height=\"173\" \/><\/p>\n<\/div>\n<h3>Solution<\/h3>\n<div>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q224739\">Show Answer<\/span><\/p>\n<div id=\"q224739\" class=\"hidden-answer\" style=\"display: none\">\u00a0allene &lt; non-conjugated \u00a0diene &lt; conjugated diene (most stable)<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"section_8\">\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":44985,"menu_order":14,"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-1778","chapter","type-chapter","status-publish","hentry"],"part":29,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/1778","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\/44985"}],"version-history":[{"count":10,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/1778\/revisions"}],"predecessor-version":[{"id":2363,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/1778\/revisions\/2363"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/parts\/29"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapters\/1778\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/media?parent=1778"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=1778"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/contributor?post=1778"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-organicchemistry\/wp-json\/wp\/v2\/license?post=1778"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}