7 -W3 47 SURFACE INFRARED SPECTROELECTROCHENISTRY

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INTERACTION OF THE ELECTRIC.. (U) UTAH UNIY SALT LAKEU Li IECITY DEPT OF CHEMISTRY S PONS ET AL. 39 JUL 86 TR-58

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Task No. NR 359-7180lTECHNICAL REPORT * 58

Surface Infrared Spectroelectrochemistry. The Interaction

of the Electric Field in the Electrical Double Layer withPyrene Adsorbed on a Platinum Electrode: Effects on the

Infrared Surface Difference Spectrum

By

Stanley Pons

C. Korzeniewski

Prepared for Publication in D T ICLangmuir ELECTE

AP 14 41988DUniversity of" Utah -*H

Department of Chemistry 0Salt Lake City, Utah 84112

July 30. 1986

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' ~fa""Tktrared Spectroelectrochemistry. Th $- TYPE OF REPORtT & PEMIO COVEIEO

Interaction of the Electric Field in the Electricat Technical Report#I 58Double Layer with Pyrene Adsorbed on a PlatinlElectrode: Effects on the infrared Surfac 6' PEFORMNING RG. RRLT u.4gX

Difference Soectrum7. AU~mok(s) S. CONTRACT OA4 GRANT 4UM41Efl(s)

Stanley Pons, C. Korzeniewski 14OO04-83K-O47O-PQOO03

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20. AftrRAST icffeine vnifs.&d*e I~tr nt o ' anidVnlf by horbe~at a platinum electrode isobtained by using SNIFTIRS._ ___

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sN I Surface Infrared Spectroelectrochemistry. The Interactionsame s of the Electric Field in the Electrical Double Layer with

3 Pyrene Adsorbed on a Platinum Electrode: Effects on the

D iInfrared Surface Difference SpectrumAL-r0 Carol Korzeniewski and Stanley Ponse

AASW Department of Chemistry. University of Utah, Salt Lake City, Utah 84112HDGa3RCVoi Received January 13, 1986. In Final Form: March 27, 1986ABSS03SEN03 I The surface infrared spectrum of pyrene adsorbed at a platinum electrode is obtained by using theSENS is SNIFTIRS technique. Activation of Raman modes by coupling of the polarizable electrons in the moleculeSEN09 is to the strong electric field field which exists across the electrical double laver is reported. SNIFT1RS spectra

4 are compared to both the solution IR and Raman spectra.rre

SENo3 i IntroductionPAMOstNO3 i The perturbation of infrared spectra by strong electricstme s fields wa s ggested by Condon in 1932.1 It was predicted FNT 1

* that a strong static external electric field could distort14 polarizable electrons in a molecule in the same way that

as in symmetric molecules, effects that could be observed byso v Raman spectroscopy. The selection rules for absorption

7 of infrared radiation require that the vibrational mode giveif rise to a dipole moment oscillating at the frequency of the

Sr12 r exciting radiation. Application of a static electric field cana distort polarizable electrons in a molecule resulting in an

sENis is induced dipole moment. Oscillation of this dipole in re-sponse to motion of the nuclei symmetrically about the

to molecular center of mass can be detected by using infraredSENIS 2s radiation. Thus, for highly polarizable molecules, in a

9 strong static electric field, it is possible to detect totallyis symmetric (A) vibrational modes by infrared spectroscopy.

SEN21 I Field-induced infrared absorption of this type has beenio shown convincingly for molecular hydrogen' and crystals FNT 2P " of diamond type.3 FNT 3

sro Ia Other types of perturbations caused by static electricsEme to fields have been observed in vibrational spectra. Changes

3 in the intensity of infrared-active bands have been ob-it served both in gas phastns--TeIaT-s lectrochemica sys- j FNT 4-7

stes 20 temr's The potential dependence of vibrational frequency FNT 8sEN12 a has also been investigated. t Attempts have been made

s to give a more quantitative explanation of the role of theA 7 electric field in such systems."'1 FNT 9-12PARO,

SENo3 I Since electric fields on the order of 0 V/m exist across13 the polarized electrode/solution interface," an electro- FNT 13is chemical system with absorbers in the interfacial region2s is ideally suited to study the effects of strong electric fields

same 37 on infrared spectra. Recently, several techniques have* been developed to obtain spectra of species in the electrical

sMils I double layer.14 5 In this report the SNIFTIRS (sub- FNT 14.157 tractively normalized interfacial Fourier transform infrared

13 spectroscopy) technique has been used to observe infrared21 absorption of pyrene at frequencies where, under external2s field free conditions, only Raman modes are active.ITrS

sEN03 I Experimental SectionPARi2SNO I Electrochemical cells used in the experiments were constructedSENN to from glass syringes JAS Instrument Systems, Inc.). An infra-

3 red-trmnsparent window (50 mm dismeter x 0.3 mm thicknessi12 made of single-crystal n-type silicon was fitted on the front of

SukiN 23 the cell. The working electrode was constructed from a platinum1o disk J9 mm diameter X 1 mm thick) sealed in glass and polished23 to mirror finish with alumina of decreasing sizes down to 0.05

S.Mi2 25jam. Final polishing was made from a bWs wood base to minimizeSEiS 13 the embedding of alumina particlet in the platinum surface. Cells

3 were cleaned by acid treatment (50/50 vol 91, sulfuric/ nitric acid)

PARIS followed by rinsing in triply distilled water.SEN0. i Acetonitrile (Burdick and Jackson. Muskegon. MI containing

less than 0.009% (nominal) water was handled under a dry argonSENt 20 atmosphere. Pyrene was obtained from Aldrich and purified bySENoI to vacuum sublimation. Tetra-n-butylammonium tetrafnuoroborate

UNIT NO. 379 860513Gal. 2 LAeM1S LA8607199 V002 1004

TX?"SPARIS

4(ThAF) was prepared by the metathesis of sodium tetrafluoro-12 bora (Aldrich) and tetra-n-butyLammonium hydrogen sulfate

SEN12 ie (Aldrich). It was dried in vacuo at 80 IC for a minimum of 24is h before use.

PARISSESMr 3 The electrochemistry was controlled by a potantiostat andSRIU to waveform generator (Hi-Tek Instruments). The instrumentation

4for phase-sensitive detection used in the differential capacitysz405 12 measurements was obtained from Bentham lzulyrumenta. Inhered

3 spectra were obtained with the use of an IBM ER/Be Serie FuRsrNLZ is spectrometer. Light from the sourc, was focused onto the elec-s&Nis to trode and then reflected out of the cell onto the detector. The

s spectrum was obtained by collecting interferograms at twos&Nis it electrode potentials. E, and E,. After transformation of the

4 interferograims to the frequency domain, the two spectra wereis raticed to give R,,'R,, where the R, correspond to the reflictance,

MZ21 36 at each potential E, The spectra an normally displayed sm 82/R

9on the spectrometer. and may be converted to the more commonSZN24 30 units of ER/ft through the ritlation ER!R - R2/R, - 1. This final

4 result represents the difference spectrum of the species being

iX0 3 observed between the two potentials.

StN~O3 I ResultsPAR21szri a Figure I is a plot of the differential capacity of the FIG 1 (003. 3- 4)

13 platinum electrode used in the SNIFTERS experiments in21 acetonitrile solutions (a) without end (b) with pyrene.

CaNoe Addition of pyrene to the system significantly lowers theit differential capacitance of the platinum electrode indi-17 cating adsorption of pyrene across the entire potential

sieNo Is rnge investigated. Reduction at large negative potentials7 results in the descorption of the species and increase in the

CR412 is capacitance as expected. Since we are working at pyrenea concentrations below 0.5 mM. it is likely that the pyrene

is is adsorbed in a flat orientation.PARD4sEIoa I Figure 2 shows the electrochemical behavior of pyrene FIG 2 1003. 3- 4)sEUos io in acetonitrile. It is noted that the current is constant and

ii essentially capacitive over the region of +0.5 to -1.5 V (vs.Satem n Ag/Ag*). Reduction of pyrene occurs at potentials more531412 : negative than -2.4 V. To study the effect that the electric

sfield has on the spectra independent of chemical effectsas such as reduction of pyrene. we have collected interfero-

srNis n Crams at potentials between +0.5 end -1.5 V. Thus, any4changes in the specta are due to changes induced by the

P 27is electric field rather than a chemical change.

SENGS I Figure 3 shows SNIFTIRS spectra in the region of the FIG 3 0013* 3- 4)12 ring stretching modes of pyrene as a function of the in-

sauios 22 tansity of potential modulation. A bend 1840 cin' is ob- ..t7 served, which is weakly dependent on tite magniiude or-

sEos Is the electrode potential. The position of the band appears& to shift to higher energy as the electrode potential is made

SEN412 1s more positive. This result was reproducible in severalSEKil s independent experiments. The SNIFTIRS spectra can be

7 compared to the Raman (Figure 4) and infrared (Figure FIG 4 015.12-11)SENIS 1s 5) Solution Spectra. The bends in the Raman Spectrum FIG 5 (015.16-17)

a are assigned to symmetric C-C stretching ring modesCLN2i 1s (A,)."6 The infrared spectrum has a strong bend at 1598 FNT 16

ii cm- assigned to the 83. ring mode end a strong band atPAN2 3049 cm-' assigned to the aromatic C-H stretch."

SEW I2 Figure 6is the SNIFTIRS difference spectra of the same FIG 68(003. 3- 4112 pyrene platinum electrode system in the region of the

SF-40 It pyrne aromatic C-H stretch. We note the absence of anyTT2sSNIFTrIRS absorption bands in the 3049-cm-' region.

53140 I DiscussionPARS:SrEreo I Pvrer- was chosen to study field-induced infrared ab-

I WoPti -,muse of its large molecular polarizability" ansd FNT 17-2017 the li- 'od that the molecule would undergo flat ad-25 soirptiur: % the platinum electrode under low bulk solution

SENN A conditt~rno (vide infra). Measurements have been madeCENNs 6 to ensure adsorption and flat orientation of pyrene. The

2 differential capacity of the electrode indicates that pyrerie531112 I I is adsorbed over the Potential range studied. Further, we

1 3k4 are working at Concentrations where pvrene should adsorb2145i flat on the surface rather then edgewise. Sorisga end, Hubbard have studied the concentration dependence of

R il !I N M ~ k 1N 11111jj!jj 1 1111111111111 i! 111 111 111111 1111ili l

3Il

UNIT NO. 380 860513Gal. 3 LA4MI5 LA8607199 V002 1004

TNT12PAR33

it the orientation of several w-electron-rich molecules ad-sENis 17 sorbed at platinum electrodes.

2 They have shown that FNT 21,22s in general, flat adsorption is the primary surface configu-

14 ration at bulk concentrations less than about 0.5 mM.PAXSEsxi* I The -bsence of an absorption band in the SNIFTIRS

ii spectra of Figure 6 provides further evidence that pyrenesL w is orientated flat on the surface. If the molecule were

1 orientated edgewise on the electrode s strong band atis about 3049 cm

"1 corresponding to the aromatic C-H

stas : stretch would be expected to appear. However, if the& molecule were orientated flat on the surface absorption

sENL 13 would be forbidden. This differential absorption is knowns LNIS 7 as the surface selection rule. The surface selection rule

s arises due to the properties of radiation reflection from asN s is metal surface. These properties may be derived through

a analysis of the Fresnel relations and have been discussedSEN21 17 in detail elsewhere."s When infrared radiation is reflected

7 from a metal surface, only the component polarized parallelis to the plane of incidence (p polarized) has any amplitude

srN2s u at the surface after reflection. Light polarized perpen-4 dicular to the plane of incidence (s polarized) undergoes

13 a phase shift of close to 180" for all angles of incidence2s resulting in a standing wave that has little amplitude near

sENr 3 the surface. Infrared radiation will interact with an os-s cillating dipole of a species when both the electric field of

its the radiation and the oscillator have spatial componentsSEN0 27 in the same direction. Thus, only molecules that have a

a component of the dipole derivative (the change in the17 dipole moment with respect to the normal coordinate)as oriented in a direction perpendicular to the surface can

SEN 34 interact with the p-polarized radiation. The s-polarizedSEN3 , radiation is blind to species adsorbed near the surface. For

3 a molecule adsorbed flat on the surface, absorption oft2 infrared radiation is forbidden by the surface selection rule.

SEN39 i However, if a dipole moment is induced in the species12 perpendicular to the surface, for example, by external fields21 or bonding effects, a vibrational transition can be observed3o by using infrared radiation.

s EoW I The appearance of symmetry-forbidden bands in thespectra of molecules adsorbed on metal surfaces has been

sE0 1s observed. The interpretation of such bands includesa mechanisms involving chemical bonding of the molecule --

is to the surface and interaction of the molecule with electricsENos 25 fields near the metal surface. The chemical mechanism 7-.

s suggests that bonding to the surface decreases the sym-13 metry of the molecule causing disallowed modes to become "

SLN12 22 active." In addition, distortion of the molecule by dona-s tion of electrons from the metal to orbitals on the molecule .

SENIS 2o has also been suggested. More quantitative explanationsa based on electric fields present near the metal surface have

SENIs is been discussed. Sass et al.' have shown that electric fieldio gradients arising from interaction of radiation with the __is metal surface are strong enough to couple with quadrupole c $ ion FO rr moments in the molecule, giving rise to activation of in- -_-

SE21 M frared-forbidden modes. In electrochemical systems, it has NTIS RA& &been shown quantitatively that large electric fields which

is exist across the electrical double layer are strong enough DTT C TAR El24 to interact with electrons of highly polarizable molecules. iuanotriounaed :1 W

SEN24 i This interaction results in a dipole moment which canSEN27 i1 oscillate normal to the metal surface." Applying this Justifloatio

4 calculations to pyrene predicts a AR/R on the order of 10- _

SEN30 is for an electric field strength of 10' V/cm. Therefore, we4 believe that the mechanism for appearance of bands in the By-

u SNIFTIRS difference spectrum of Figure 3 is through22 interaction of polarizable electrons in the molecule with DistribUtion/

SEN3 30 the large static electric field across the double layer. This r Availability Codesa interaction can induce a dipole moment normal to the

t2 surface which can oscillate at the vibrational frequency of . .. ail an/orsEN3e 21 the A, ring mode. The band appears at potentials very

&close in energy to those observed for ring stretching modes Dis Spe ia

PAR42 is in the Raman spectrum (which are infrared-forbidden).SEiO Thus. for adsorbed pyrene a dipole moment can be in-

i duced normal to the surface by coupling the highly po-20 larizable electrons in the aromatic ring of the molecule to

- ,V.0

UNIT NO. 381 860513Gal. 4 LA4MI5 LA8607199 V002 1004

TXTI2PAR42Svqos 3o the electric field across the double layer. The aromatic

4 C-H stretching modes would not be expected to be en-13 hanced by the electric field because of the small polariz-

T ability of the C-H bond.

SENo3 I ConclusionPAR4SSE-.o3 I This report demonstrates that the electric field in the

it double layer is sufficiently strong to induce infrared ac-ts tivity in modes which are forbidden by normal infrared

sEm 2s selection rules. Field induced absorption can be used tos study the electric field in the double layer.

TXF21

PARS IsENoo I Acknowledgment. We thank the Office of Naval Re-s NOs s search for support of this work. We thank John Foley for

7 many helpful discussions of the work, and we also ac-ts knowledge the assistance of and discussion with Dr. Mi-2 chael Hunnicutt and Professor Joel M. Harris regarding

srmeN 32 pyrene. These workers have investigated similar effectss of pyrene adsorbed at dielectric surfaces.n

SYF03ENO0 I *To whom correspondence should be addressed.

FNN02FNPM$EN03 1 (1) Condon. E. U. Phys. Rev. 1932. 41, 759.FNN03FNPOSENO3 1 (2) Crawford. M. F.; MacDonald. R. E. Can. J. Phys 1958. 36. 1022.FNN04FNPMSEN03 1 (3) Ansittiska. E; lwssa. S.; Burstein, E Phys. Rev. Lett. It". 17,

i3 1051.FNNOSFNPIZiEN03 1 (4) Stells. A.; Migho. L.; Palik. E. D.; HoLm. F. T.; Hughes. H. L.

IS Ph)sco A 153. 17B. 777.FNN06FNPISiEN03 1 (5) Kuninasau, K.; Golden. W. G.; Seki. H.: Phdpott,. M R. Lormuvr

13 1,85.1.245.FNNO7FNPI$iEN03 1 (6) Kuatimastu. K.; Ski. H.; Golden. W. G. Chem. Phys. Lett. 1984.

13 108. 195.FNN03FNP21SEN03 1 (7) Lambert. D. Solid State Commun. 1964, 51. 29,FNNO9FNP24SEN03 1 (8) Konsiniswk. C.; Pow, S. J. Vac. Sri. Technol.. B. 1983. 3. 1421.FNNI0FNP27SEN03 1 (9) Korzeniewski. C.. Shaun. R. B.. Pons. S. J Phys. Chem, 1 8, 89.

14 2297.FNNIIFNP30SEN03 I (10) Brewer. R. G.. McLean. A. D. Ph.s Rev. Lett, 1948. 21. 271.FNN12FNP33SEN03 a (11) Holloway. S.. Norkakov. J. K. J Electroanal CteCem 1584, !61.

12 193.FNNI3FNP36SEN03 I (12) Ford, G. W.; Weber, W. H. Surf Sca. 1181. 109. 451,FNNI4FNP39sEN03 I (13) Bard. A. T. Fsulkner. L Ft. Electrorhemical Methoda; Wiley

12 New York. 1980FNNISFNP42iEN03 I (141 Foley. J K. Pons. S Anal. Chem Ies, 57, 45A,FNNI4FNP45SEN03 1 (151 Foley. J K. Komniewski. C. Daschbach. J D. Pons. S Elee-

12 tmor.al Chem 1904. 14."NNI?INP4&iEN03 I (16) Bro,. A. Kydd. R A. Mast. T N.Vilkho. V V B Spectrorham

IS Act&. Part A 1971. RTA. 2315.a FNNI5

"NPsI•E.103 I (]I Woe J. FPipadoupouss. M G. Nirolad". C A J Chem Ph,.

13 1 U2. 77, 2536.

FNPS4i%01 ' (I) Greenler, R J Chem PhI 19. 44. 110FNN2oFNPS7its",1 I 19) Lahwald. S. Ibach, H. Demuth. J E Surf Sc l98, 78. S"FN N21VNP6a1EN0s 1 f201 Sm. J K. Neff. H. Mookiit. M . Hollows, S J Ph-. Chi

14 ]1 . 95. 621IFNN i

SEINIO 1 (2

11 Solle M P.Hobbard.k T J As Chest Siw 1021, fE. 2-1,FNN2SPN',sI

j p1

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ENO~ 1 (22) Hunnicutt. M.. Harris. J1 M, LoChmuallfl. C J, Phtye Che".12 19U. 89. 5246

r f s. w i, Wpm Nor

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C,,

c~tm i Figure 1. Differential capacity curves for a platinum electrodecAm0 a in asolutioui of a)0.1 M TBAF in acetonitrile and bi same ascApos 23 (a) with 0-5mM pyrene. Results were obtained by using a 5 mV

to (pp amplitudet) 400 Hz sine wave superimposed on a 10 in'21 voltage ramp applied to the working electrode and measuing the

cAPo, 31 in and out of phase components of the ac current. All potentialsawe with reference to the Ag,/Ag* (0.01 M Ag* in acetonirile with

I,0.1 %1 TEAFI.

0law 00 so0 -1 -30

cAPODi Fgr 2. Cyclic voltammetry of the solution in Figure lb. SweepCAP% 3 rate is 50 mV, a.

-.~~ Is/

i

1"o '00 16C

cAPOO i Figure 3. SNIFTIRS difference spectrum of the %olution inCA"S 9 Figure lb betwenl.hgjnlicated potential regions Band., es-

tending down tr presers increased absorbance at the moreq12 negative electrioI'-pnrential

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S.o

AVEAS

CAPOO Figure 4. Solution inred spectrum of pyrene in acabonitie-

CAP7 regioridee Band a16n). aaetae rntrf

j 300 100

%

kws

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as -Ut

U-0.

as A

cA.p t Figure 6. SNIFTIRS difference spectrum in the aromatic C-H

CAPo3 S stretch region for the solution described in Figure lb.

The number of words in this manuscript is 2491.

The manuscript type is A.

Running Heads

Surface Infrared Spectroelectrochernistry

Korzenieuwski and Pons

Author Index Entries

Korzenieski, C.

Pons. S.

Text Page Size Estimate = 2.3 Pages

Graphic Page Size Estimate = 0.8 Pages

Total Page Size Estimate - 3.1 Pages

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University of Pennsylvania University of CaliforniaPhiladelphia, Pennsylvania 19104 Los Angeles, California 90024

M. L. Robertson Dr. Elton CairnsManager, Electrochemical Energy & Environment Division

and Power Sources Division Lawrence Berkeley LaboratoryNaval Weapons Support Center University of CaliforniaCrane, Indiana 47522 Berkeley, California 94720

Dr. T. Marks Dr. Richard PollardDepartment of Chemistry Department of Chemical EngineeringNorthwestern University University of HoustonEvanston, Illinois 60201 Houston, Texas 77004

Dr. Micha Tomkiewicz Dr. M. PhilpottDepartment of Physics IBM CorporationBrooklyn College 5600 Cottle RoadBrooklyn, New York 11210 San Jose, California 95193

Dr. Lesser Blum Dr. Donald SandstromDepartment of Physics Boeing Aerospace Co.University of Puerto Rico P.O. Box 3999Rio Piedras, Puerto Rico 00931 Seattle, Washington 98124

Dr. Joseph Gordon, I Dr. Carl KarnewurfIBM Corporation Department of Electrical Engineering5600 Cattle Road and Computer ScienceSan Jose, California 95193 Northwestern University

Evanston, Illinois 60201Dr. Nathan LewisDepartment of Chemistry Dr. Joel HarrisStanford University Department of ChemistryStanford, California 94305 University of Utah

Salt Lake City, Utah 84112

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Dr. M. Wrighton Dr. M. M. NicholsonChemistry Department Electronics Research CenterMassachusetts Institute Rockwell International

of Technology 3370 Miraloma AvenueCambridge, Massachusett 02139 Amuheim, California

Dr. B. Stanle ns Dr. Michael J. WeaverDepartmen Chemistry Department of ChemistryUnive ty of Utah Purdue UniversitySa Lake City, Utah 84.12 West Lafayette, Indiana 47907

Donald E. Mains Dr. R. David RauhNaval Weapons Support Center EIC Laboratories, Inc.Electrochemical Power Sources Division 111 Downey StreetCrane, Indiana 47522 Norwood, Massachusetts 02062

S. Ruby Dr. Aaron WoldDOE (STOR) Department of ChemistryRoom 5E036 Forrestal Bldg., CE-14 Brown UniversityWashington, D.C. 20595 Providence, Rhode Island 02192

Dr. A. J. Bard Dr. Martin FleischmannDepartment of Chemistry Department of ChemistryUniversity of Texas University of SouthamptonAustin, Texas 78712 Southampton S09 5NH ENGLAND

Dr. Janet Osteryoung Dr. R. A. OsteryoungDepartment of Chemistry Department of ChemistryState University of New York State University of New YorkBuffalo, New York 14214 Buffalo, New York 14214

Dr. Donald W. Ernst Dr. John WilkesNaval Surface Weapons Center Air Force Office of ScientificCode R-33 ResearchWhite Oak Laboratory Bolling AFBSilver Spring, Maryland 20910 Washington, D.C. 20332

Mr. James R. Moden Dr. R. NowakNaval Underwater Systems Center Naval Research LaboratoryCode 3632 Code 6171Newport, Rhode Island 02840 Washington, D.C. 20375

Dr. Bernard Spielvogel Dr. 0. F. Shrive-U.S. Amy Research Office Department of ChemistryP.O. Box 12211 Northwestern UniversityResearch Triangle Park, NC 27709 Evanston, Illinois 60201

Dr. Aaron FletcherNaval Weapons CenterCode 3852China Lake, California 93555

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