CALCULATING THE CHANGE IN DIPOLE MOMENT 1 :

1. ~ ~ Where: ~ Reichardt’s Dye • Δf = the solvent factor (change in the reaction field) • ε = the solvent dielectric constant • n = the refractive index • h = Planck’s constant • c = speed of light • vct = frequency of maximum emission in cm-1 • vct (0)= frequency of maximum emission in the gaseous phase in cm-1 • Δμ = difference in excited and ground state • dipole moment • ρ = the radius of the solute cavity • 4πε0 = gas permittivity constant ~ 4-amino-N-methylphthalimide TABLE OF CONSTANTS k-ET, non-rad N A - D + ΔH Coumarin 153 kET h1 A- - D+ A* - D A - D Compound ρ (Ǻ) ε (@ 25˚C)5 η (@ 25˚C)5 3 k-ET, rad A-D + h2 Cu153 3.92 -- -- 4-ANMP 3.33 -- -- O Reichardt's Dye 7.84 -- -- Chlorobenzene -- 5.621 1.52185 A* —D Dichloromethane -- 8.93 1.42115 Electron Transfer A- —D+ Dimethyl Sulfoxide -- 46.45 (20˚C) 1.47933 (20˚C) Solvent Relaxation A- —D+ Acetonitrile -- 35.94 1.34163 hυ1 E hυ2 A—D A—D SAMPLE RESULTS COMPOUNDS STUDIED ABSTRACT Our proposed research is intended to develop a laboratory exercise for publication, suited for a physical chemistry class. The exercise centers around the study of solvatochromism, which affects both emission and absorption in intramolecular photo-induced electron transfer. The method itself involves steady state absorption and steady state fluorescence measurements and allows for the determination of the change in dipole moment between the excited and ground states of the covalently linked electron donor and acceptor. It also provides for an experimental measurement of polarity for solvents and solvent mixtures. (for Coumarin 153) Solvatochromism and Photo-Induced Intramolecular Electron TransferKatelyn J. Billings; Bret R. Findley11Department of Chemistry and Physics, Saint Michael’s College, Colchester, VT 05439 BACKGROUND • When dealing with intramolecular photo-induced electron transfer (PET), • An electron donor and acceptor are covalently linked together (A-D complex) • The donor or acceptor is locally excited by a photon (h1) • The complex undergoes electron transfer • As a result the positively charged donor cation is bonded to the negatively charged acceptor anion. • This A--D+ excited state complex follows one of two potential pathways • whereby it returns to the ground state D-A complex • releasing either a photon via fluorescence (h2) OR • heat Literature values1: Theoretical Δμ = 3.9D Experimental Δμ = 6.0D Our Experimental Δμ : 7.05D Given that: ρ= 3.9Ǻ LAB SETUP & CONCLUSIONS • Students will: • Run steady state absorption and fluorescence spectra for: • Reichardt’s Dye & • Coumarin 153 OR • 4-amino-N-methylphthalimide • Which will be dissolved in Chlorobenzene, DCM, DMSO, & Acetonitrile • Graph the results and calculate Δμ. • In conclusion this lab will help students as: • It gives them a good introduction to photo-induced intramolecular electron transfer, which has applications to photovoltaic and solar cells, nanotechnology and many chemical and biological processes. • It provides them with a quantitative method for analyzing solvatochromism. • It deepens their understanding of basic physical chemistry topics. • As one alters the polarity of the solvent, the fluorescence produced undergoes a wavelength (or color) change in a process known as solvatochromism. • Bathochromic shift: the wavelength of emission shifts towards • the red end of the spectrum (lower photon energy), • Hypsochromic shift: the wavelength shifts towards the blue end of • the spectrum (higher photon energy). CALCULATING THE CHANGE IN DIPOLE MOMENT1: • For solutes with non-polar ground states: • Changes with the solvent polarity stabilize the excited A-—D+ complex • This lowers the energy gap between excited A-—D+and ground A-D states • emission spectra for a particular D-A complex is indicative of the polarity of the solvent and the dipole moment of the excited A-—D+ complex. • FUTURE PLANS • Calculate the change in dipole moment for Reichardt’s Dye, as it does NOT have a non-polar ground state. • Reevaluate our data—Check Fluorimeter calibration/correction for accuracy. • Test lab and submit for publishing. ACKNOWLEDGEMENTS The authors would like to thank the NASA Vermont Space Grant initiative for funding this research project. SAMPLE DATA Fluorescence Spectra for Coumarin 153 REFERENCES (1)Hermant, R. M.; Bakker, N. A. C.; Scherer, T.; Krijnen, B.; Verhoeven, J. W. J. Am. Chem. Soc, 1990, 112, 1214-1221. (2) Maroncelli M., Fleming, G. R. J. Chem. Phys,1987, 86, 6221-6239. (3) Chapman, C. F.; Fee, R. S.; Maroncelli, M. J. Phys. Chem., 1995, 99, 4811-4819. (4) Mente, S. R.; Maroncelli, M. J. Phys. Chem B., 1999, 103, 7704-7719. (5) Riddick, J. A; Bunger, W. B.; Sakano, T. K. Organic Solvents: Physical Properties and Methods of Purification; Wiley Interscience: New York, 1986; Vol. 2. • EXPERIMENTAL PROCEDURE • Take fluorescence measurements for solvatochromic dyes in a variety of solvents (with different polarities). • Plot , the maximum emission frequency in cm-1, versus Δf, a solvent polarity parameter. • Slope of this line ultimately yields Δμ, the difference in excited and ground state dipole moment of the solute. **Note the Bathochromic Shift