Jablonski Diagram Notes | Explanation | How to Draw

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It demonstrates processes such as absorption, fluorescence, phosphorescence, and other non-radiative transitions. For example, this is useful for characterizing host materials in the emissive layers of organic light-emitting diodes (OLEDs). Understanding whether these materials exhibit fluorescence or phosphorescence informs device fabrication. In a Jablonski diagram, lines representing the different possible energy levels are stacked in two columns, with energy on the vertical axis. The levels are distributed horizontally according to energy state multiplicity. Jablonski diagrams are frequently used in optical spectroscopy, particularly fluorescence spectroscopy. 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Supplies</a> <a href="/collections/spectroscopy"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> Spectroscopy Equipment</a> <a href="/collections/solution-making"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> Solution Making Supplies</a> <a href="/collections/equipment-accessories"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> Equipment Accessories</a> <a href="/collections/general-laboratory-supplies"> <svg class="icon icon-navigate_next"><use xlink:href="#icon-navigate_next"></use></svg> General Laboratory Supplies</a> </div> </div> </ul> </li> </ul> </nav> </div> </div> </div>  <div class="container"> <div id="unsupported-browser-message" class="alert-warning"> <p>It looks like you are using an unsupported browser. You can still place orders by emailing us on <a href="mailto:info@ossila.com">info@ossila.com</a>, but you may experience issues browsing our website. Please consider upgrading to a modern browser for better security and an improved browsing experience.</p> </div> </div>  <main> <div id="informational-page"> <h1>The Jablonski Diagram</h1> <div class="container"> <img alt="The Jablonski Diagram" class="featured-image" height="280" loading="lazy" src="https://www.ossila.com/cdn/shop/files/broadband-white-light-source-breadboard.jpg?crop=center&width=1340&height=280" width="1340"> <p id="jablonski-diagrams">A Jablonski diagram is a simple and effective way to illustrate the energy transitions between the electronic and vibrational states of a molecule. It demonstrates processes such as absorption, fluorescence, phosphorescence, and other non-radiative transitions. For example, this is useful for characterizing <a href="/collections/host-materials" title="host materials">host materials</a> in the emissive layers of organic light-emitting diodes (OLEDs). Understanding whether these materials exhibit fluorescence or phosphorescence informs device fabrication.</p> <p>In a Jablonski diagram, lines representing the different possible energy levels are stacked in two columns, with energy on the vertical axis. The levels are distributed horizontally according to energy state multiplicity.</p> <p>Jablonski diagrams are frequently used in optical spectroscopy, particularly fluorescence spectroscopy. They are named after Polish physicist named Aleksander Jablonski, who introduced the concept in the 1930s to provide a visual representation and a theoretical framework for understanding the energy transitions and relaxation processes that occur in molecules after the absorption of light. The Jablonski diagram helped explain the mechanisms behind light-induced processes, contributing to a deeper understanding of fluorescence and phosphorescence spectroscopy.</p> <h2>How to Draw Energy States on a Jablonski Diagram</h2> <hr> <p>An example Jablonski diagram (without any energy transitions) is shown below. On the diagram, bold lines represent the base energy of each state (v<sub>0</sub>). Additional vibrational energy states (<span class="maths">v<sub>1</sub></span>, <span class="maths">v<sub>2</sub></span>, <span class="maths">v<sub>3 </sub></span>,etc) are represented by the thinner lines.</p> <figure><img alt="Jablonski diagram" height="634.234" loading="lazy" src="https://www.ossila.com/cdn/shop/files/Spectrometer_Diagrams-04.svg?v=1677850724" width="848.328"> <figcaption>Jablonski diagram showing the singlet ground state (<em>S<sub>0</sub></em>), the first two singlet excited states (<em>S<sub>1</sub></em> and <em>S<sub>2</sub></em>), and the first triplet excited state (<em>T<sub>1</sub></em>) (bold lines). The vibrational energy levels (<em>v<sub>0</sub></em>, <em>v<sub>1</sub></em>, <em>v<sub>2</sub></em>, and <em>v<sub>3</sub></em>) are denoted by the thinner lines.</figcaption> </figure> <p>The ground state is represented as <span class="maths">S<sub>0</sub></span> as spin angular momentum <span class="maths">S=0</span> in the ground state. When an electron enters an excited state, it can have different spin multiplicity, depending on if total spin angular momentum has been conserved. If spin has been conserved, the electron is said to be in a singlet excited state (<span class="maths">S<sub>1</sub></span>). If angular momentum is not conserved, then the electron enters a triplet energy state (T<sub>1</sub>).</p> <p>The excited singlet and triplet states are represented in Jablonski diagrams with different columns.</p> <h2>How to Show Energy Transitions on a Jablonski Diagram</h2> <hr> <p>Energy transitions are shown on Jablonski diagrams using either straight or wavy arrows. Radiative transitions (such as absorption and fluorescence) are shown with straight arrows, while non-radiative transitions (such as internal conversion and intersystem crossing) tend to be depicted as wavy arrows.</p> <figure><video title="Energy Transitions on a Jablonski Diagram" alt="Energy Transitions on a Jablonski Diagram" autoplay="autoplay" loop="loop" muted="muted" src="https://cdn.ossila.com/videos/Jablonski-stages-diagram-loop.mp4" type="video/mp4"></video> <figcaption>Examples of how different transitions are represented on Jablonski Diagrams showing absorption (1), vibrational relaxation (2), fluorescence (3), internal conversion (4), intersystem crossing (5) and phosphorescence (6)</figcaption> </figure> <div class="info-tip-box"> <p>Jablonski diagrams provide a convenient way to represent energy transitions in a molecule or system. However, it is important to note that most of the time, these diagrams are purely schematic and do not represent these energy levels quantitatively.</p> </div> <p>The Jablonski diagram above shows six different types of transitions.</p> <h3 class="blue-heading">1. Absorbance</h3> <p>This represents the absorbance of a photon by an electron. The energy of the photon is high enough that the electron can be excited into a higher energy state. Absorption between energy levels can be explored with an <a href="/products/optical-spectrometer" title="USB spectrometer">USB spectrometer</a> if this transition energy is between 1.1 – 3.8 eV.</p> <h3 class="blue-heading">2. Vibrational relaxation</h3> <p>Vibrational relaxation is a non-radiative loss of energy between vibrational energy levels. This excess vibrational energy is lost as kinetic energy to other vibrational modes, either of the same molecule or of a different molecule. This energy is loss happens very rapidly (10<sup>-14</sup> – 10<sup>-12</sup> seconds) and is often measured using Raman spectroscopy or IR spectroscopy.</p> <h3 class="blue-heading">3. Fluorescence</h3> <p>Fluorescence is a type of photoluminescence in which the spin state of the electron relaxes back into the ground state and a photon is emitted. It is represented on a Jablonski diagram by a straight line.</p> <p>The spin state of the electron stays the same from the excited state to the ground state, so this is a singlet-singlet transition (<span class="maths">S<sub>1</sub> → S<sub>0</sub></span>). This is an allowed transition, so fluorescence often occurs a very short time after the electron is excited.</p> <p>Fluorescence can be measured with optical spectroscopy if this transition energy is between 1.1 – 3.8 eV.</p> <h3 class="blue-heading">4. Internal conversion</h3> <p>Internal conversion is a type of non-radiative emission, where an electron moves from a higher energy excited state to a lower energy excited state. This occurs when the vibrational modes of different electronic levels overlap. No photon is emitted and the electrons spin state remains the same throughout the transition.</p> <h3 class="blue-heading">5. Intersystem crossing</h3> <p>Intersystem crossing is another form of non-radiative emission. Unlike internal conversion, the spin state of the excited electron changes. The Jablonski diagram above shows an electron moving from the excited singlet state (<span class="maths">S<sub>1</sub></span>) into the excited triplet state (<span class="maths">T<sub>1</sub></span>). Often intersystem crossing results in phosphorescence emission.</p> <h3 class="blue-heading">6. Phosphorescence</h3> <p>Phosphorescence<span> </span>is a type of fluorescence in which an electron relaxes into the ground state via emission of a photon. However, unlike in fluorescence, the electron must change spin states for this to occur. This is a forbidden transition, so happens over a much longer time scale. Phosphorescence can be measured with optical spectroscopy if the transition is between 1.1 – 3.8 eV.</p> <h2>Time Scales for Different Energy Transitions</h2> <table> <tbody> <tr> <td width="33.333%"><strong>Transition</strong></td> <td width="33.333%"><strong>Time Taken (s)</strong></td> <td width="33.333%"><strong>How to measure?</strong></td> </tr> <tr> <td>Absorbance</td> <td>10<sup>-14</sup> – 10<sup>-12</sup> </td> <td>UV-Vis/Optical spectroscopy</td> </tr> <tr> <td>Vibrational relaxation</td> <td>10<sup>-14</sup> – 10<sup>-11</sup> </td> <td>Time resolved spectroscopy<br>IR spectroscopy<br>Raman spectroscopy</td> </tr> <tr> <td>Fluorescence</td> <td>10<sup>-9</sup> – 10<sup>-7</sup> </td> <td>UV-Vis/Optical spectroscopy</td> </tr> <tr> <td>Internal Conversion</td> <td>10<sup>-15</sup> </td> <td></td> </tr> <tr> <td>Intersystem Crossing</td> <td>10<sup>-8</sup> – 10<sup>-3</sup> </td> <td></td> </tr> <tr> <td>Phosphorescence</td> <td>10<sup>-4</sup> – 10<sup>-1</sup> </td> <td>UV-Vis/Optical spectroscopy</td> </tr> </tbody> </table> <h2>Example Energy Transitions on Jablonski Diagram</h2> <figure><img alt="Jablonski diagram showing vibrational relaxation, internal conversion and intersystem crossing" height="658.25" loading="lazy" src="https://www.ossila.com/cdn/shop/files/Spectrometer_Diagrams.svg" width="848.33"> <figcaption>Jablonski diagram illustrating vibrational relaxation, internal conversion and intersystem crossing</figcaption> </figure> <p>In the Jablonski diagram above, a photon is absorbed, exciting a ground state electron to an excited vibrational state of the second singlet excited state, <span class="maths">S<sub>2</sub></span> (dark blue straight arrow pointing upwards). It then relaxes through internal conversion to an excited vibrational state of <span class="maths">S<sub>1</sub></span> (faint blue wavy arrow) and further relaxes to the ground vibrational state of <span class="maths">S<sub>1</sub></span> through vibrational relaxation (LHS light blue wavy arrow).</p> <p>The electron then undergoes intersystem crossing (green wavy arrow on the Jablonski diagram) to an excited vibrational state of the first excited triplet state (<span class="maths">T<sub>1</sub></span>) and undergoes vibrational relaxation once more (RHS light blue wavy arrow) to the <span class="maths">T<sub>1</sub></span> vibrational ground state. After a time (can be seconds or even hours), the electron relaxes back down to an excited vibrational state of the singlet ground state, <span class="maths">S<sub>0</sub></span>, via phosphorescence (angled blue arrow).</p> <a class="green-banner" data-track-content="" href="https://www.ossila.com/products/optical-spectrometer"> <p data-content-name="/pages/jablonski-diagrams" data-content-piece="cta-optical-spectrometer">Optical Spectrometer</p> <img alt="Optical Spectrometer" height="120" loading="lazy" src="https://www.ossila.com/cdn/shop/files/Ossila-Optical-Spectrometer-Kit-Fluorescence.jpg?crop=center&width=600&height=120" width="600"> <button>Browse now</button> </a> <h3>Learn More</h3> <hr> <div class="row button-row"> <div class="col-xs-12 col-sm-6 button-col"> <div class="card-box card-truncate"> <a href="/pages/fluorescence-phosphorescence"><img alt="Fluorescence and Phosphorescence" height="160" loading="lazy" src="https://www.ossila.com/cdn/shop/files/Fluorescence-Phosphorescence.svg?v=1718710450" width="160"></a> <a href="/pages/fluorescence-phosphorescence">Fluorescence and Phosphorescence</a> <p>Fluorescence and phosphorescence are types of photoluminescence. Photoluminescence refers to radiative emissions where the absorbance of a photon is followed by the emission of a lower energy photon. The main empirical difference between fluorescence and phosphorescence is the time in between absorbance and the emission of photons. Fluorescence is where a material absorbs a photon, and almost immediately emits a lower energy photon.</p> <a href="/pages/fluorescence-phosphorescence">Read more...</a> </div> </div> <div class="col-xs-12 col-sm-6 button-col"> <div class="card-box card-truncate"> <a href="/pages/what-is-an-exciton"><img alt="Exciton: An Introduction" height="160" loading="lazy" src="https://www.ossila.com/cdn/shop/files/Ossila-Optical-Spectrometer-Kit-Fluorescence.jpg?crop=center&width=160&height=160" width="160"></a> <a href="/pages/what-is-an-exciton">Exciton: An Introduction</a> <p>Excitons are quasi-particles made up of bound electron and hole pairs. Having a clear understanding of exciton theory is essential in order to understand semiconductor behaviour. Exitonic behaviour can be examined using various spectroscopy techniques, including an optical spectrometer. Excitonic properties will often determine the potential application of a material in optoelectronic devices, for example as photovoltaics, light-emitting diodes or even as lasers.</p> <a href="/pages/what-is-an-exciton">Read more...</a> </div> </div> </div> <div class="panel panel-default"> <div class="panel-body"> <h3>Contributing Authors</h3> <hr> <p>Written by</p> <p class="no-margin"><a href="/pages/our-writers#other-authors" title="Contributing Authors">Kirsty McGhee</a></p> <p class="text-muted">PhD Student Collaborator</p> <p>Reviewed and edited by</p> <p class="no-margin"><a href="/pages/our-writers#mary-okane" title="Author Biography: Mary O'Kane">Dr. Mary O'Kane</a></p> <p class="text-muted">Application Scientist</p> </div> </div> <script type="application/ld+json"> { "@context": "https://schema.org", "@type": "Article", "abstract": "A Jablonski diagram is a simple and effective way to illustrate the energy transitions between the electronic and vibrational states of a molecule. 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Jablonski Diagram Notes | Explanation | How to Draw | Ossila