Chemical Light Sources. Incoherent Light Sources Sylvia Bark SS 2013
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1 Chemical Light Sources Incoherent Light Sources
2 Content: Introduction History Chemiluminescence in nature and daily life Requirements General mechanism Most common reactions: - 1. Luminol - 2. Peroxyloxalat - 3. Singlet-Oxygen Comparison of the reactions References
3 Introduction: What is luminescence? emission of (mostly) visible light When does it happen? if excited electrons fall down to the ground state (between discrete energy levels) Types of luminescence: electroluminescence photoluminescence chemiluminescence = basis for chemical light sources (bioluminescence) All types are non-thermal radiators ( cold light ): only very small amount of energy is set free as heat.
4 History: documentation started since around 3500 years in China fascination of self glowing organism was described by Aristoteles, Robert Boyle, 1669 first anorganic chemiluminescence by Heinrich Brand: - evaporation + drying of urine: Phosphat got reduced to Phosphor - oxidation in air: blue to white luminescence appr. 100 years later: Chemist Carl Scheele found the corresponding reaction mechanism Eilhard Mitscherlich ( ): - development to detect the contamination of white phosphor
5 Chemiluminescence in nature and daily life: a) some fishes and jellyfishes in the ocean b) fireflies: lantern fish - released energy is set free as light c) glow sticks firefly
6 Requirements for Chemiluminescence: excitation energy: - for visible light: kj/mol - energy has to be set free in only one step, short time, small volume - exothermic process - mostly based on oxidation processes atoms or molecules: - easy to bring to an excited state under this condition quantum efficiency: - number of emitted photons per molecules (which react) - should be high (as usual)
7 General reaction mechanism: Oxidation A <BC> B + C* B + C + h*f reactant A is a Luminophor for oxidation: O 2 (oxygen), R 2 O 2 (peroxides), O 2 - (hyperoxide), RO 2 H (hydroperoxide) <BC>: sort of Luminophor-Dioextane, instable B + C*: carbonyl compounds; C* is the excited molecule by emission of a photon it dissociates into the ground state
8 Most common reactions: 1. Luminol reaction Luminol = 3 Aminophthalacidhydrazid alkaline hydrogen peroxide acts on Luminol according to oxidation nitrogen N 2 is set free out of Luminol reaction is catalysed by potassium-hexacyanoferrat now a long time, weak chemiluminescence can be seen still not the whole mechanism of the reaction is well-known
9 Most common reactions: 1. Luminol reaction Applications: detection of blood spots at crime scenes: in blood is an iron-ion as tracer to detect small amounts of heavy metals lifeboats use Luminol compounds to throw it into the water to see/ search at night
10 Most common reactions: 2. Peroxyoxalat systems; Glow Sticks Set up of Glow Sticks: 1: plastic cover 2: H 2 O 2 covered in glass 3: room, filled with dye/ fluorophor, oxal acid ester, solvent 4 + 5: bending + mixing of chemicals; emission of light Examples: dye: RhodaminB (red) Rhodamin6G (orange) Perylen (blue) Rubren (yellow) oxal acid ester: TCPO DNPO solvent: Phthalacidesters Ethylacetat
11 Most common reactions: 2. Peroxyoxalat systems; Glow Sticks e.g. reaction of TCPO (oxal acid ester) with H 2 O 2 also here the mechanism of the reaction is not well-known it might be explained by the following: - H 2 O 2 will dissociate TCPO to Trichlorphenol and Dioxetandion: - Dioxetandion dissociates to excited CO 2 - dye gets back to ground state by emission of light - reaction is catalysed by alkalines
12 Most common reactions: 2. Peroxyoxalat systems; Glow Sticks Applications: decoration fun emergency light (e.g. in coal mining, seafaring) marking scenes of accidents or airfields fishing at night...
13 Most common reactions: 3. Singlet-Oxygen a) Oxygen ground state: two unpaired e -, parallel spin; 3 O 2 is in the triplet state applying energy: spin of one e- is turned; 1 O 2 is in the singlet state deactivation (2*94,5 kj/mol are set free emission of red light): + h*f
14 Most common reactions: 3. Singlet-Oxygen b) Production - from peroxides: NaOCl + H 2 O 2 instable peroxohypochloride acid NaCl + H 2 O + 1 O 2 - alternative: Cl 2 + H 2 O OH - 2 H 2 O + 2 Cl O 2 1: reaction tube 2: glass frit 3: solution 4: safety bottle 5: beaker glass with ice water
15 Most common reactions: 3. Singlet-Oxygen c) Applications demonstration of the high reactivity of singlet-oxygen in organic chemistry as strong oxidant, e.g. to produce peroxides in processes of bleachings and disinfactions in the photodynamic therapy of tumors
16 Comparison of the three reactions: quantum efficiency: Singlet-O 2 < Luminol reaction < Peroxyoxalatsystems Singlet- : λ = 634 nm, lowest energy Luminol: Ф CL 0,01 Peroxyoxalatsystems: most intensive, higher Ф CL but expensive similarities: reaction mechanism: - addition of H 2 O 2 - instable key precursor - emission of light mechanisms are not very well-known
17 References
18 Thanks for your attention.
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