Why does benzene have 3 π–π* transitions in the UV range, but ethene, butadiene, and hexatriene each have...











up vote
3
down vote

favorite
1












Are the π and π* orbitals of benzene much closer together in energy which allows for multiple transitions? Why is this not the case for hexatriene if they both contain the same number of pi bonds?










share|improve this question




























    up vote
    3
    down vote

    favorite
    1












    Are the π and π* orbitals of benzene much closer together in energy which allows for multiple transitions? Why is this not the case for hexatriene if they both contain the same number of pi bonds?










    share|improve this question


























      up vote
      3
      down vote

      favorite
      1









      up vote
      3
      down vote

      favorite
      1






      1





      Are the π and π* orbitals of benzene much closer together in energy which allows for multiple transitions? Why is this not the case for hexatriene if they both contain the same number of pi bonds?










      share|improve this question















      Are the π and π* orbitals of benzene much closer together in energy which allows for multiple transitions? Why is this not the case for hexatriene if they both contain the same number of pi bonds?







      molecular-orbital-theory hydrocarbons symmetry group-theory uv-vis-spectroscopy






      share|improve this question















      share|improve this question













      share|improve this question




      share|improve this question








      edited Nov 18 at 2:36









      orthocresol

      37k7108219




      37k7108219










      asked Nov 18 at 2:19









      ETS

      544




      544






















          1 Answer
          1






          active

          oldest

          votes

















          up vote
          4
          down vote













          It seems that here we only need to consider the lowest energy transitions, i.e. HOMO–LUMO transitions. The difference between benzene and the linear polyenes is that both the HOMO and LUMO of benzene are doubly degenerate, whereas the linear polyenes do not have degeneracy.



          If we think about this HOMO–LUMO excitation in the case of benzene, we can schematically represent it like this:



          Electronic configurations of ground and first excited state of benzene



          The ground state has overall symmetry $mathrm{A_{1g}}$ because all electrons are paired, but the first excited electronic configuration above $(mathrm{e_{1g}})^3(mathrm{e_{2u}})^1$ corresponds to three different electronic states, each with a slightly different spatial distribution of electrons. The symmetries of these three states are obtained by taking a direct product of the relevant irreps:



          $$mathrm{E_{1g} times E_{2u} = B_{1u} oplus B_{2u} oplus E_{1u}}$$



          Because these three states arise from the same electronic configuration, their energies are going to be fairly close to each other, and all three electronic transitions from the ground state



          $$mathrm{A_{1g} to B_{1u}, quad A_{1g} to B_{2u}, quad A_{1g} to E_{1u}}$$



          should fall within the UV range.



          For any linear polyene (including ethene, butadiene, and hexatriene), both HOMO and LUMO are nondegenerate, so the $(pi)^3(pi^*)^1$ configuration will only correspond to one electronic state.



          This is a rather simplified analysis, because we are only considering transitions which conserve spin, i.e. singlet–singlet transitions. These are so-called "spin-allowed" transitions. The singlet–triplet transitions also occur within the UV range, but are technically "forbidden". On top of that, not all of the three singlet–singlet transitions in benzene are equal: two of them are also "forbidden", as the transition dipole moment $langle i | hat{mu} | j rangle$ vanishes. But that is a story for another day. The keen reader may wish to check out J. Mol. Struct. 1973, 19, 143–166 for an assignment of the electronic transitions of benzene.






          share|improve this answer























            Your Answer





            StackExchange.ifUsing("editor", function () {
            return StackExchange.using("mathjaxEditing", function () {
            StackExchange.MarkdownEditor.creationCallbacks.add(function (editor, postfix) {
            StackExchange.mathjaxEditing.prepareWmdForMathJax(editor, postfix, [["$", "$"], ["\\(","\\)"]]);
            });
            });
            }, "mathjax-editing");

            StackExchange.ready(function() {
            var channelOptions = {
            tags: "".split(" "),
            id: "431"
            };
            initTagRenderer("".split(" "), "".split(" "), channelOptions);

            StackExchange.using("externalEditor", function() {
            // Have to fire editor after snippets, if snippets enabled
            if (StackExchange.settings.snippets.snippetsEnabled) {
            StackExchange.using("snippets", function() {
            createEditor();
            });
            }
            else {
            createEditor();
            }
            });

            function createEditor() {
            StackExchange.prepareEditor({
            heartbeatType: 'answer',
            convertImagesToLinks: false,
            noModals: true,
            showLowRepImageUploadWarning: true,
            reputationToPostImages: null,
            bindNavPrevention: true,
            postfix: "",
            imageUploader: {
            brandingHtml: "Powered by u003ca class="icon-imgur-white" href="https://imgur.com/"u003eu003c/au003e",
            contentPolicyHtml: "User contributions licensed under u003ca href="https://creativecommons.org/licenses/by-sa/3.0/"u003ecc by-sa 3.0 with attribution requiredu003c/au003e u003ca href="https://stackoverflow.com/legal/content-policy"u003e(content policy)u003c/au003e",
            allowUrls: true
            },
            onDemand: true,
            discardSelector: ".discard-answer"
            ,immediatelyShowMarkdownHelp:true
            });


            }
            });














             

            draft saved


            draft discarded


















            StackExchange.ready(
            function () {
            StackExchange.openid.initPostLogin('.new-post-login', 'https%3a%2f%2fchemistry.stackexchange.com%2fquestions%2f104479%2fwhy-does-benzene-have-3-%25cf%2580-%25cf%2580-transitions-in-the-uv-range-but-ethene-butadiene%23new-answer', 'question_page');
            }
            );

            Post as a guest















            Required, but never shown

























            1 Answer
            1






            active

            oldest

            votes








            1 Answer
            1






            active

            oldest

            votes









            active

            oldest

            votes






            active

            oldest

            votes








            up vote
            4
            down vote













            It seems that here we only need to consider the lowest energy transitions, i.e. HOMO–LUMO transitions. The difference between benzene and the linear polyenes is that both the HOMO and LUMO of benzene are doubly degenerate, whereas the linear polyenes do not have degeneracy.



            If we think about this HOMO–LUMO excitation in the case of benzene, we can schematically represent it like this:



            Electronic configurations of ground and first excited state of benzene



            The ground state has overall symmetry $mathrm{A_{1g}}$ because all electrons are paired, but the first excited electronic configuration above $(mathrm{e_{1g}})^3(mathrm{e_{2u}})^1$ corresponds to three different electronic states, each with a slightly different spatial distribution of electrons. The symmetries of these three states are obtained by taking a direct product of the relevant irreps:



            $$mathrm{E_{1g} times E_{2u} = B_{1u} oplus B_{2u} oplus E_{1u}}$$



            Because these three states arise from the same electronic configuration, their energies are going to be fairly close to each other, and all three electronic transitions from the ground state



            $$mathrm{A_{1g} to B_{1u}, quad A_{1g} to B_{2u}, quad A_{1g} to E_{1u}}$$



            should fall within the UV range.



            For any linear polyene (including ethene, butadiene, and hexatriene), both HOMO and LUMO are nondegenerate, so the $(pi)^3(pi^*)^1$ configuration will only correspond to one electronic state.



            This is a rather simplified analysis, because we are only considering transitions which conserve spin, i.e. singlet–singlet transitions. These are so-called "spin-allowed" transitions. The singlet–triplet transitions also occur within the UV range, but are technically "forbidden". On top of that, not all of the three singlet–singlet transitions in benzene are equal: two of them are also "forbidden", as the transition dipole moment $langle i | hat{mu} | j rangle$ vanishes. But that is a story for another day. The keen reader may wish to check out J. Mol. Struct. 1973, 19, 143–166 for an assignment of the electronic transitions of benzene.






            share|improve this answer



























              up vote
              4
              down vote













              It seems that here we only need to consider the lowest energy transitions, i.e. HOMO–LUMO transitions. The difference between benzene and the linear polyenes is that both the HOMO and LUMO of benzene are doubly degenerate, whereas the linear polyenes do not have degeneracy.



              If we think about this HOMO–LUMO excitation in the case of benzene, we can schematically represent it like this:



              Electronic configurations of ground and first excited state of benzene



              The ground state has overall symmetry $mathrm{A_{1g}}$ because all electrons are paired, but the first excited electronic configuration above $(mathrm{e_{1g}})^3(mathrm{e_{2u}})^1$ corresponds to three different electronic states, each with a slightly different spatial distribution of electrons. The symmetries of these three states are obtained by taking a direct product of the relevant irreps:



              $$mathrm{E_{1g} times E_{2u} = B_{1u} oplus B_{2u} oplus E_{1u}}$$



              Because these three states arise from the same electronic configuration, their energies are going to be fairly close to each other, and all three electronic transitions from the ground state



              $$mathrm{A_{1g} to B_{1u}, quad A_{1g} to B_{2u}, quad A_{1g} to E_{1u}}$$



              should fall within the UV range.



              For any linear polyene (including ethene, butadiene, and hexatriene), both HOMO and LUMO are nondegenerate, so the $(pi)^3(pi^*)^1$ configuration will only correspond to one electronic state.



              This is a rather simplified analysis, because we are only considering transitions which conserve spin, i.e. singlet–singlet transitions. These are so-called "spin-allowed" transitions. The singlet–triplet transitions also occur within the UV range, but are technically "forbidden". On top of that, not all of the three singlet–singlet transitions in benzene are equal: two of them are also "forbidden", as the transition dipole moment $langle i | hat{mu} | j rangle$ vanishes. But that is a story for another day. The keen reader may wish to check out J. Mol. Struct. 1973, 19, 143–166 for an assignment of the electronic transitions of benzene.






              share|improve this answer

























                up vote
                4
                down vote










                up vote
                4
                down vote









                It seems that here we only need to consider the lowest energy transitions, i.e. HOMO–LUMO transitions. The difference between benzene and the linear polyenes is that both the HOMO and LUMO of benzene are doubly degenerate, whereas the linear polyenes do not have degeneracy.



                If we think about this HOMO–LUMO excitation in the case of benzene, we can schematically represent it like this:



                Electronic configurations of ground and first excited state of benzene



                The ground state has overall symmetry $mathrm{A_{1g}}$ because all electrons are paired, but the first excited electronic configuration above $(mathrm{e_{1g}})^3(mathrm{e_{2u}})^1$ corresponds to three different electronic states, each with a slightly different spatial distribution of electrons. The symmetries of these three states are obtained by taking a direct product of the relevant irreps:



                $$mathrm{E_{1g} times E_{2u} = B_{1u} oplus B_{2u} oplus E_{1u}}$$



                Because these three states arise from the same electronic configuration, their energies are going to be fairly close to each other, and all three electronic transitions from the ground state



                $$mathrm{A_{1g} to B_{1u}, quad A_{1g} to B_{2u}, quad A_{1g} to E_{1u}}$$



                should fall within the UV range.



                For any linear polyene (including ethene, butadiene, and hexatriene), both HOMO and LUMO are nondegenerate, so the $(pi)^3(pi^*)^1$ configuration will only correspond to one electronic state.



                This is a rather simplified analysis, because we are only considering transitions which conserve spin, i.e. singlet–singlet transitions. These are so-called "spin-allowed" transitions. The singlet–triplet transitions also occur within the UV range, but are technically "forbidden". On top of that, not all of the three singlet–singlet transitions in benzene are equal: two of them are also "forbidden", as the transition dipole moment $langle i | hat{mu} | j rangle$ vanishes. But that is a story for another day. The keen reader may wish to check out J. Mol. Struct. 1973, 19, 143–166 for an assignment of the electronic transitions of benzene.






                share|improve this answer














                It seems that here we only need to consider the lowest energy transitions, i.e. HOMO–LUMO transitions. The difference between benzene and the linear polyenes is that both the HOMO and LUMO of benzene are doubly degenerate, whereas the linear polyenes do not have degeneracy.



                If we think about this HOMO–LUMO excitation in the case of benzene, we can schematically represent it like this:



                Electronic configurations of ground and first excited state of benzene



                The ground state has overall symmetry $mathrm{A_{1g}}$ because all electrons are paired, but the first excited electronic configuration above $(mathrm{e_{1g}})^3(mathrm{e_{2u}})^1$ corresponds to three different electronic states, each with a slightly different spatial distribution of electrons. The symmetries of these three states are obtained by taking a direct product of the relevant irreps:



                $$mathrm{E_{1g} times E_{2u} = B_{1u} oplus B_{2u} oplus E_{1u}}$$



                Because these three states arise from the same electronic configuration, their energies are going to be fairly close to each other, and all three electronic transitions from the ground state



                $$mathrm{A_{1g} to B_{1u}, quad A_{1g} to B_{2u}, quad A_{1g} to E_{1u}}$$



                should fall within the UV range.



                For any linear polyene (including ethene, butadiene, and hexatriene), both HOMO and LUMO are nondegenerate, so the $(pi)^3(pi^*)^1$ configuration will only correspond to one electronic state.



                This is a rather simplified analysis, because we are only considering transitions which conserve spin, i.e. singlet–singlet transitions. These are so-called "spin-allowed" transitions. The singlet–triplet transitions also occur within the UV range, but are technically "forbidden". On top of that, not all of the three singlet–singlet transitions in benzene are equal: two of them are also "forbidden", as the transition dipole moment $langle i | hat{mu} | j rangle$ vanishes. But that is a story for another day. The keen reader may wish to check out J. Mol. Struct. 1973, 19, 143–166 for an assignment of the electronic transitions of benzene.







                share|improve this answer














                share|improve this answer



                share|improve this answer








                edited Nov 18 at 3:19

























                answered Nov 18 at 2:50









                orthocresol

                37k7108219




                37k7108219






























                     

                    draft saved


                    draft discarded



















































                     


                    draft saved


                    draft discarded














                    StackExchange.ready(
                    function () {
                    StackExchange.openid.initPostLogin('.new-post-login', 'https%3a%2f%2fchemistry.stackexchange.com%2fquestions%2f104479%2fwhy-does-benzene-have-3-%25cf%2580-%25cf%2580-transitions-in-the-uv-range-but-ethene-butadiene%23new-answer', 'question_page');
                    }
                    );

                    Post as a guest















                    Required, but never shown





















































                    Required, but never shown














                    Required, but never shown












                    Required, but never shown







                    Required, but never shown

































                    Required, but never shown














                    Required, but never shown












                    Required, but never shown







                    Required, but never shown







                    Popular posts from this blog

                    Сан-Квентин

                    Алькесар

                    Josef Freinademetz