SciELO - Scientific Electronic Library Online

 
vol.6 issue3A new route to process diamond wiresModeling of alkynes: synthesis and theoretical properties author indexsubject indexarticles search
Home Pagealphabetic serial listing  

Services on Demand

Journal

Article

Indicators

Related links

Share


Materials Research

Print version ISSN 1516-1439On-line version ISSN 1980-5373

Mat. Res. vol.6 no.3 São Carlos Apr./June 2003

http://dx.doi.org/10.1590/S1516-14392003000300006 

Dye incorporation in polyphosphate gels: synthesis and theoretical calculations

 

 

Jordan Del NeroI*; André GalembeckII; Sidicleia Bezerra Costa SilvaII; José Augusto Pereira da SivaII

IDepartamento de Física, Universidade Federal do Pará (UFPA), 66075-110 Belém - PA, Brazil
IIDepartamento de Química Fundamental, Universidade Federal de Pernambuco (UFPE), 50670-901 Recife - PE, Brazil

 

 


ABSTRACT

In this work we described theoretical calculations on the electronic structure and optical properties of the dyes crystal violet and malachite green based in semiempirical methods (Parametric Method 3 and Intermediate Neglect of Differential Overlap / Spectroscopic - Configuration Interaction) and the synthesis of a new hybrid material based upon the incorporation of these dyes in an aluminum polyphosphate gel network. The samples are nearly transparent, free-standing thick films. The optical properties of the entrapped dyes are sensitive to chemical changes within the matrix caused either by gel aging or external stimulli such as exposition to acidic and basic vapors that can percolate within the matrix. Our theoretical modeling is in good agreement with the experimental results for the dyes.

Keywords: sol-gel, electronic structure, theoretical and experimental absorption spectra, semiempirical/CI calculations, malachite green, crystal violet


 

 

1. Introduction

The sol-gel process provides interesting paths to synthesize organic-inorganic hybrid materials, in which one can take advantage of the properties of each component individually and, also, reach synergistic properties between them. The organic and inorganic components may either exchange weak interactions like hydrogen bonding, van de Waals forces and electrostatic forces or be linked through chemical bonds. The inorganic to organic relative amount may change significantly1.

Silica-based networks are the most widely used inorganic fraction because the precursors are commercially available and/or can be easily modified. Their chemical reactivity is well understood and the synthesis may be carried out to form transparent films, fibers or monoliths with good mechanical properties2.

Polyphosphate-based materials are also attractive as hosts for the design of inorganic hybrid composites as they can be synthesized as particles containing closed pores3, nanoparticle4, transparent gels5, glasses6 and hybrid net works7. These materials may present a broad range of chemical compositions, with many different morphologies which allow us to envisage the entrapment of compounds in mild reaction conditions, thus preventing degradation of the active species.

Polyphosphate gels can be synthesized as transparent, flexible free-standing films. The gelation derives from the association of the polyphosphate polyanions with metallic cations, leading to a supramolecular ionic swollen network. In fact, these cations (Ca, Zr, Al, Fe) act as bridges between different polyphosphate chains and, hence, the gel cohesion is a consequence of electrostatic interactions rather than the covalent bonding which develops as a result of the polycondensation reactions that proceed to give silica-based networks, starting from alkoxide precursors.

We have reported, recently, the synthesis of new hybrid materials in which a polyphosphate gel network was used as the host structure for the incorporation of rare-earth cryptates8, polyaniline9 and the dyes methyl orange10 and malachite green11, in order to develop new optical materials.

Crystal violet (CV) and malachite green (MG) are tri-aryl-methane dyes with similar chemical structures (Fig. 1). They are used as acidic-base indicators, stain compounds in histology and as flourophores in immunoassays.

 

 

CV tends to dimerize in aqueous solution depending upon the dye concentration. The monomer and dimer give different absorption bands in the visible spectrum. Also, two kinds of molecular orientation were described for CV dimerization in the literature: (i) the molecules are parallel, and; (ii) there is a superposition of the nitrogen atom from one dymethyl-amine group to the aromatic ring (anti-parallel). MG structure is very similar to CV, but no dimerization is reported in the literature12,13.

Alberti et al. reported the intercalation of crystal violet both in the external surface and in the interlayer space of a-zirconium phosphate (a-ZrP). They observed both dimerization and protonation by the acidic P-OH groups within the dye host structure. Also, the design of optical sensors for ammonia and humidity detection were performed by dispersing this dye on Nafion® films14. Another chemical optical sensor for ammonia in which a sulfonephthalein (also a substituted triaryl-methane) dye was immobilized in sol-gel derived silica thin films was also reported. In the later, a glassy film of the organically modified silicate was deposited in optical fibers15.

In this work we investigated theoretically the CV, MG and CV-MG dimerization in order to optimize the dimer geometry and understanding its spectroscopic properties. We also synthesized new hybrid materials by the incorporation of these dyes within polyphosphate gels in order to get new optical sensors.

 

2. Methodology

2.1 CV-MG/Polyphosphate Hybrids Synthesis

Crystal violet + malachite green/aluminum polyphosphate (CV-MG/APP) composites were synthesized starting from sodium polyphosphate (2.0 mol/l, in P) and aluminum nitrate (1.0 mol/l) aqueous solutions. The MG to CV ratio in the dye aqueous solution was [MG]/[CV] = 5.0, which was adjusted in order to give similar absorbances from the two dye solutions. The total CV and MG concentration were, respectively, 2.0 × 10-5 and 1.0 × 10-4 mol/l. The average polyphosphate chain length was 10.6, determined by31 P NMR.

In a typical synthesis, the MG-CV (1 ml) solution was previously added to 10 ml of the polyphosphate solution, followed by the addition 10 ml of the Al3+ solution under strong stirring. In some cases, sodium hydroxide solution was also added to raise the pH. The phosphorus to aluminum ratio (P/Al) ranged from 2.0 to 2.8.

Gelation occurs under ambient atmosphere at room temperature within 1 min. The gel was stirred for 30 min and centrifuged for 1 h at 10,000 × g. Transparent greenish-blue samples form after 1 to 3 days. Free-standing films were prepared spreading the gel samples on a flat surface and letting them dry at room temperature in a moisture-controlled environment (50% relative humidity) for one week.

The samples were exposed to HCl and NH3 vapors, from 6 mol/l solutions heated at 60 °C, in a closed environment order to investigate their sensitivity to acidic and basic vapors.

The MG-CV/PP free-standing thick film samples were characterized by absorption spectra using a using an UV-visible spectrophotometer Perkin-Elmer LAMBDA 6 model 2688-002, within the 200-800 nm range.

2.2 Theoretical Calculations

Semiempirical calculations at the PM316 levels were performed for the guest molecules CV and MG and the corresponding fully optimized geometry could be determined. Standard MOPAC17 parameters were used, except for the convergence criterion, for which a maximum step size of 0.005 was adopted. For these molecules, a planar configuration was assumed as the starting point for the geometry optimization calculations. A RHF criterion was adopted because the compounds investigated have a positive ion in the second phenyl ring, which corresponds to a closed shell system.

Absorption spectrum calculations of the structures presented in Fig. 1 were performed using the ZINDO package18-21 with geometries fully optimized at the PM3 level and the absorption spectra were calculated at the Intermediate Neglect of Differential Overlap/Spectroscopic - Configuration Interaction (INDO/S-CI) level, and the parameters chosen to give the best description of the UV-visible-NIR optical transitions for those molecules22-25. In this case, the level of approximation was utilized within a restricted closed-shell Hartree-Fock approach to determine the ground state. Approximately 280 configurations were investigated for each molecule, including singlet and doublet states.

For molecule dimerization, we started from the geometries optimized with semiempirical calculations at the PM3 level and separated by 2.6 angstroms according with our previous calculations11.

 

3. Results And Discussions

Figure 2 presents the absorption spectra of CV, MG and the MG-CV aqueous solutions. The spectrum of the CV solution shows two maxima near 544 and 584 nm. The first one is attributed to CV dimerization26. The spectrum of the MG-CV mixture is the sum of the individual solutions.

 

 

After the centrifugation of the samples a supernatant solution is expelled from the solid gel, which is called synerisis liquid. A spectrum is also presented in Fig. 2e. As gelation proceeds in acidic medium (0.5 to 2.0), the supernatant solution spectrum is compared to MG and CV solutions spectra in the same conditions, which are very similar (Fig. 2c and 2d). This was done in order to investigate if one of the dyes is preferentially incorporated to the gel matrix, which is not the case as the supernatant spectrum showed contributions from both dyes.

The spectrum of the MG-CV/PP hybrid is presented in Fig. 3. The spectrum is similar to the MG-CV solution, which is greenish-blue. Both dyes were incorporated to the gel matrix. When these samples were exposed to HCl vapors, the films turned to green as presented in Fig. 3b. This sample presented two absorptions: (i) the first one has two maxima at 416 and 438 nm, ascribed to CV and MG in acidic media; (ii) 640 nm, due to CV protonation to give CV-H. The absorption at 640 nm has an asymmetry, which may result also from MG in acidic medium26. Hence, both dyes can be protonated by sample exposition to acidic vapors. Exposition to basic ammonia vapors leads to deprotonation of those dyes and the original color is restored.

 

 

MG-CV/PP samples presented the same color change if dried at 50% humidity (green samples). The spectrum of a dried MG-CV gels is presented in Fig. 3c. The maximum is centered at 630 nm and the band is broader than in the former case, in which the sample was exposed to acidic vapors. The original greenish-blue color is restored if the samples were exposed to moisture-rich (> 80%) environment.

The gel tends absorb and desorb water in reversible way. Fresh samples presents higher water content than samples dried under 50% relative humidity. As the sample dries, the water amount within the gel liquid phase decreases, which should increase the acidity of this phase. The color will develop if the pH change related to this process is enough to protonate/deprotonate the dye which is incorporated in the gel matrix.

CV presents a violet-blue to green color change when the pH decreases from 2.0 to 1.0. MG turns to yellow if the pH is lower than 1.0. This means that the dyes acted as internal sensors for the aqueous phase of the gel, which is within the 1.0 to 2.0 range.

Once CV and MG are cationic species, they should have affinity with polyphosphate polyanion chains. This interaction leads to a phenomenon called metachromasy in which the absorption bands of the dye is dislocated in relation to aqueous solution. In aqueous solution, the maximum absorption for CV is located at 590 nm11. A shift to 603 nm is observed (not shown) if CV is added to a 2.0 mol/lpolyphosphate solution, used to synthesize the gel,. This means that the guest molecule interacts with these chains even before its incorporation within the gel. After dye incorporation in the maximum shifts further to 611 (Fig. 3).

The interactions between host and guest molecules are electrostatic and contribute to stabilize the hybrid, but the optical properties of the guest molecule is not significantly altered upon its incorporation within the matrix, which is desirable if one is interested in a solid state chemical sensor based on CV and MG dyes.

Figure 4 presents the main transitions contributing to the optical spectra of dye molecules. The corresponding theoretical absorption spectra were obtained by broadening each of these principal transitions by a suitably weighted Gaussian function normalized to the calculated oscillator strengths27.

 

 

For both, CV+ and MG+, the first and second optical transitions are essentially a HOMO to LUMO transition (|H®L>) and HOMO-1 to LUMO transition (|H-1®L>), respectively. Those transitions appears at different regions of the spectra, the first one for CV+ [MG+] at 427.3 [448.2] nm with oscillator strength (o.s.) equal to 0.88 [1.06] and the second one for CV+[MG+] at 424.8 [360.7] and o.s. equal to 0.89 [0.48]. For this reason the band at this region of spectrum is more pronounced for CV+ molecule and it appears an extra band for MG+ molecule (360 nm region). Details for the three additional bands, it is presented in Table 1.

 

 

Figure 5 shows the theoretical absorption spectra for parallel dimer of (a) CV+/CV+, (b) MG+/MG+ and (c) CV+/MG+ molecules interacting. The way of interaction for these molecules is following the steps discussed by theoretical methodology. For CV+/CV+ (Fig. 5a) molecules interacting we can see the strongest band at » 400 nm. The most important transitions for this interaction correspond to a mixing of the transitions |H®L>, |H-1®L>, |H-2®L>, |H®L+1> and |H-1®L+1>. Note that, those transitions came from the interaction between the two CV+ molecules because for a single molecule the first transition is composed by only a |H®L> transition.

 

 

For the parallel MG+/MG+ (Fig. 5b) interaction the most important absorption line corresponds to the |H®L> transition (coefficient 0.67 and o.s.= 0.12), while the band at » 232 nm has contributions from the |H-1®L+2> transition (with coefficients of 0.48) and o.s.= 0.27 and the first two bands are composed by only lower transitions.

For the parallel CV+/MG+ (Fig. 5c) interaction there are five main bands centered respectively in: (i)453 nm region, composed by a |H®L > transition with o.s. = 0.15, (ii) 422 nm, with o.s.= 0.68 (0.5|H-1 ® L+1> and-0.3|H2 ® L+1> transitions), (iii)407 nm, with o.s. = 1.93 (the most important and corresponding to 0.3|H®L> and -0.5|H-2®L+1> transitions), (iv and v) 358 nm and 243 corresponding by a |H-3 ® L> and an overlapping of -0.33|H-1 ® L+6> and 0.33|H-2 ® L+3> with o.s. = 0.80 and 0.22, respectively.

Figure 6 represents the theoretical absorption spectra for anti-parallel dimer of (a) CV+/CV+, (b) MG+/MG+ and (c) CV+/MG+ molecules interacting following the propose of Coon et al.28. A different behavior is followed by anti-parallel structures. There is a pronounced red shift for all species proportioned by strong charge interaction between the rings29. For CV+/CV+ (Fig. 6a) the band at » 430 nm has an o.s. equal to 0.68 and corresponds to a mixing of the transitions |H®L+1> and |H-1®L> (with coefficients of 0.35 and -0.59, respectively). In Table 1, note that the in the main transitions shows the importance of deeper and lower orbitals. For MG+/MG+ (Fig. 6b) appears a more pronounced red shift than the others two spectra and this behavior is according to the appearance of only lower orbitals. Similar analysis for CV+/MG+ (Fig. 6c) is done and it can see with Table 1.

 

 

4. Conclusions

The organic dyes crystal violet and malachite green were successfully incorporated within the aluminum polyphosphate gel inorganic matrix. The dyes are sensitive to changes in the chemical environment such as drying and exposure to acidic and basic vapors, which led optical responses (color changes) on the samples.

Theoretical investigation for the ground state and first excited states of MG and CV molecules, and examined the corresponding absorption spectra.

 

Acknowledgments

Support by the Brazilian agency PIBIC for JAPS (10060/2001) and Pernambuco state agency FACEPE for the fellowship for SBCS and financial support is gratefully acknowledged.

 

References

1. Sanchez, C.; Soler–illia, G.J.A.A.; Ribot, F.; Lalot, T.; Mayer, C.R.; Cabuil, V. Chem. Mater, n. 12, p. 3061, 2001.        [ Links ]

2. Lebeau, B.; Sanchez, C. Curr. Op. Solid State Mat. Sci, n. 4, p. 11, 1999.         [ Links ]

3. Lima, E.C.O.; Galembeck, F. Colloid Surface A, n. 75, p. 65, 1993.         [ Links ]

4. Galembeck, F.; Lima, E.C.O.; Beppu, M.M.; Sassaki, R.M.; Masson, N.C.; Monteiro, V.A.R.; Souza, E.F. "Fine Particles Science and Technology­: From Micro to Nanoparticles" (E. Pellizetti, Ed.), p. 267. Kluwer, Amsterdam, 1996.         [ Links ]

5. Lima, E.C.O.; Galembeck, F.; Colloid, J. Interf. Sci., n. 166, p. 309, 1994.         [ Links ]

6. Corbridge, D.E.C. Phosphorus, and Outline of its Chemistry, Biochemistry and Technology. Elsevier, Amsterdam, 1990.         [ Links ]

7. Souza, E.F.; Bezerra, C.C.; Galembeck, F. Polymer, n. 38, p. 6285, 1997.         [ Links ]

8. Amorim, M.S.; Galembeck, A.; Bazin, H.; Mathis, G.; Donegá, C.M.; Sá, G.F.; Junior, S.A. Mol. Cryst. Liq. Cryst., n. 374, p. 267, 2002.         [ Links ]

9. Castro, E.G.; Zarbin, A.J.G.; Galembeck, A.; Del Nero, J. International Conference of Synthetic Metals 2002, Xangai, China, 2002.         [ Links ]

10. Galembeck, A.; Silva, S.B.C.; Silva, J.A.P.; Del Nero, J. Opt. Mat., accepted, 2002.         [ Links ]

11. Del Nero, J.; Silva, J.A.P.; Silva, S.B.C.; Galembeck, A. Synth. Met., in press.         [ Links ]

12. Lovell, S.; Marquardt, B.J.; Kahr, B. J Chem. Soc. Perk. T. 2, p. 2241, 1999.         [ Links ]

13. Lueck, H.B.; Rice, B.L.; McHale, J.L. Spectrochimica Acta, 48A, p. 819, 1992.         [ Links ]

14. Raimundo Jr., I.M.; Narayanaswamy, R. Sensors Actuators, B 74, p. 60, 2001.         [ Links ]

15. Malins, C.; Butler, T.M.; MacCraith, B.D. Thin Solid Films, n. 368, p. 105, 2000.         [ Links ]

16. Dewar, M.J.S.; Zoebisch, E.G.; Healy, E.F.; Stewart, J.P. J. Am. Chem. Soc., n. 107, p. 3902, 1985.         [ Links ]

17. Stewart, J.J.P. MOPAC Program Version 6 (QCEP 455).         [ Links ]

18. Head, J.D.; Zerner, M.C. Chem. Phys. Lett., n. 122, p. 264, 1985.         [ Links ]

19. Head, J.D.; Zerner, M.C. Chem. Phys. Lett., n. 131, p. 359, 1986.         [ Links ]

20. Ridley, J.; Zerner, M.C. Theoret. Chim. Acta, n. 42, p. 223, 1976.         [ Links ]

21. Edwards, W.D.; Zerner, M.C. Theoret. Chim. Acta, n. 72, p. 347, 1987.         [ Links ]

22. Del Nero, J.; Laks, B. Synth. Met., n. 101, p. 440, 1999.         [ Links ]

23. Del Nero, J.; Laks, B. Synth. Met., n. 101, p. 379, 1999.         [ Links ]

24. Doretto, R.L.; Del Nero, J.; Laks, B. Synth. Met., n. 101, p. 178, 1999.         [ Links ]

25. Del Nero, J.; Melo, C.P. Synth. Met. n. 121, p. 1741, 2001.         [ Links ]

26. Hoppe, R.; Alberti, G.; Costantino, U.; Dionigi, C.; Schulz-Ekloff, G.; Vivani, R. Langmuir, n. 13, p. 7252, 1997.         [ Links ]

27. Del Nero, J.; Melo, C.P. Mol. Cryst.-Liq.Cryst., n. 374, p. 555, 2002.         [ Links ]

28. Coon, S.R.; Zakharian, T.Y.; Littlefield, N.L.; Loheide, S.P.; Puchkova, E.J.; Freeney, R.M.; Pak, V.N. Langmuir, n. 16, p. 9690, 2000.         [ Links ]

29. Lueck, H.B.; McHale, J.L.; Edwards, W.D. J. Am. Chem. Soc., n. 114, p. 2342, 1992.         [ Links ]

 

 

Received: October 10, 2002
Revised: February 23, 2003
Trabalho apresentado no 1º Congresso da Sociedade Brasileira em Materiais, Rio de Janeiro, Julho de 2002.

 

 

*e-mail: jordan@ufpa.br

Creative Commons License All the contents of this journal, except where otherwise noted, is licensed under a Creative Commons Attribution License