MadSci Network: Chemistry |
To explain this, I will need to give a brief sketch of the electronic state of molecules. When a molecule is formed through the combination of atoms, it achieves an intertwining of all of the atomic energy levels to form new arrangements which are called "molecular orbitals". These are similar to the orbitals for atoms except that they are orbitals for the molecule. However, they follow the sorts of rules for filling as atomic orbitals - Hund's Rule of Maximum Spin Multiplicity, Pauli's Exclusion Principle, the Aufbau Principle, etc. So, when a molecule is put together, all of the molecular orbitals fill with all of the available electrons. The result is the "electronic ground state". That is, the "resting" or lowest energy state of the molecule. Above this state are higher energy configurations where, for example, spin pairing might occur that is not present in the ground state configuration. Fluorescence and Chemiluminescence have a common origin. They both result from the decay of a molecule in a higher energy or "excited" state back down to the ground state. This decay results in the release of energy and the emission of a photon. But they are caused by different phenomenon. Fluorescence results from electronic excitation - a consequence of the molecule absorbing a photon initially. That is, a photon of light is absorbed and very quickly re-emitted. However, the same colour is not necessarily re-emitted as the molecule can lose energy, while in the excited state, through vibrational deactivation. This is why fluorescence essentially changes the colour of the light - for example, blue in, green out. And why fluorescence takes UV light and converts it to visible. Chemiluminescence is caused by a molecular reaction of two (or more) ground state molecules producing a final molecule in an excited state. That is, the energy that is in the reactants is translated to the products and, while forming the products, it also excites them. All molecular interactions form products in "vibrationally" excited states - a bit like ringing a bell, it takes time for the vibrations to die away. This birational excitation leads to "infrared chemiluminescence. But reactions can also result in the formation of molecules in "electronic" excited states and, in this case, that results in the emission of a photon of light. Hope this answers your question.
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