1. 8-1 Ultraviolet-Visible Spectroscopy Introduction to UV-Visible §Absorption spectroscopy from 160 nm to 780 nm §Measurement of transmittance àConversion to absorbance *A=-logT=  bc Measurement of transmittance and absorbance Beer’s law Noise Instrumentation

2. 8-2 Measurement Scattering of light §Refraction at interfaces §Scatter in solution àLarge molecules àAir bubbles Normalized by comparison to reference cell §Contains only solvent àMeasurement for transmittance is compared to results from reference cell

3. 8-3 Beer’s Law Based on absorption of light by a sample §dP x /P x =dS/S àdS/S=ratio of absorbance area to total area *Proportional to number of absorbing particles àdS=adn *a is a constant, dn is number of particles §n is total number of particles within a sample

4. 8-4 Beer’s Law Area S can be described by volume and length §S=V/b (cm 2 ) §Substitute for S §n/V = concentration  Substitute concentration and collect constant into single term  Beer’s law can be applied to mixtures  A tot =  A x

5. 8-5 Beer’s Law Limitations Equilibrium shift §pH indicators àNeed to consider speciation àWeak acid equilibrium

6. 8-6 Beer’s Law Limitation Polychromatic Light §More than one wavelength

7. 8-7 Noise Limited readout resolution Dark current and electronic noise Photon detector shot noise Cell position uncertainty §Changing samples Flicker

8. 8-8 Instrumentation Light source §Deuterium and hydrogen lamps §W filament lamp §Xe arc lamps Sample containers §Cuvettes àPlastic àGlass àQuartz

9. 8-9 Spectrometers

10. 8-10 Spectrometer Time separated double beam

11. 8-11 Spectrometer Multichannel photodiode array Dip probe

12. 8-12 Application of UV-Visible Spectroscopy Identification of inorganic and organic species Widely used method Magnitude of molar absorptivities Absorbing species methods

13. 8-13 Molar Absorptivties Range from 0 to 1E5   =8.7E19PA àP=transition probability àA=target cross section (cm 2 ) *Allowed transitions 0.1>P>1  range 1E4 to 1E5 *Forbidden transition 0.01 Absorbing species  M+  ->M* àM * has a short lifetime (nanoseconds) àRelaxation processes *Heat *Photo emission Fluorescence or phosphorescence

14. 8-14 Absorbing species Electronic transitions   and n electrons §d and f electrons §Charge transfer reactions  and n (non-bonding) electrons

15. 8-15 Sigma and Pi orbitals

16. 8-16 Electron transitions

17. 8-17 Transitions  §UV photon required, high energy àMethane at 125 nm àEthane at 135 nm n->  §Saturated compounds with unshared e - àAbsorption between 150 nm to 250 nm   between 100 and 3000 L cm -1 mol -1 àShifts to shorter wavelengths with polar solvents *Minimum accessibility §Halogens, N, O, S

18. 8-18 Transitions n-> ,  §Organic compounds, wavelengths 200 to 700 nm §Requires unsaturated groups  n->  low  (10 to 100) *Shorter wavelengths   higher  (1000 to 10000)

19. 8-19 Solvent effects

20. 8-20 Transitions d-d §3d and 4d 1 st and 2 nd transitions series §Broad transitions àImpacted by solution

21. 8-21 Transitions

22. 8-22 D transitions Partially occupied d orbitals §Transitions from lower to higher energy levels àSplitting of levels due to spatial distribution similar Axial direction

23. 8-23 D transitions Binding ligands on axis have greater effect on axial orbitals

24. 8-24 D transitions  value dependent upon ligand field strength  <Br-<Cl-<F-<OH-<C2O42-~H2O<SCN- <NH3<en<NO2-<CN -   increases with increasing field strength f-f §4f and 5f (lanthanides and actinides) §Sharper transitions

25. 8-25 Actinide transitions Figure 2: UV-vis spectra of organic phases for 13M HNO 3 system

26. 8-26 Charge-transfer Transitions Electron donor and acceptor characteristics §Absorption involves e - transitions from donor to acceptor àSCN to Fe(III) *Fe(II) and neutral SCN §Metal is acceptor àReduced metals can be exception

27. 8-27 Electronic Spectra Cr(NH 3 ) 6 3+ §d 3 §Weak low energy transition àSpin forbidden §2 stronger transitions àSpin allowed *t 2g and e g transitions Lower energy to higher energy §CT at higher energy àLigand to metal transition

28. 8-28 Charge transfer bands High energy absorbance §Energy greater than d-d transition àElectron moves between orbitals *Metal to ligand *Ligand to metal àSensitive to solvent LMCT §High oxidation state metal ion §Lone pair ligand donor MLCT §Low lying pi, aromatic §Low oxidation state metal àHigh d orbital energy

29. 8-29 Solvent effect

30. 8-30 Methods Titration §Change of absorbance with solution variation àpH, ligand, metal Photoacoustic effect §Emission of sound