Open Access

Characterization of ZnO nanoparticles grown in presence of Folic acid template

Journal of Nanobiotechnology201210:29

Received: 28 February 2012

Accepted: 2 July 2012

Published: 12 July 2012



ZnO nanoparticles (grown in the template of folic acid) are biologically useful, luminescent material. It can be used for multifunctional purposes, e.g., as biosensor, bioimaging, targeted drug delivery and as growth promoting medicine.


Sol–gel chemical method was used to develop the uniform ZnO nanoparticles, in a folic acid template at room temperature and pH ~ 7.5. Agglomeration of the particles was prevented due to surface charge density of folic acid in the medium. ZnO nanoparticle was further characterized by different physical methods.


Nanocrystalline, wurtzite ZnO particles thus prepared show interesting structural as well as band gap properties due to capping with folic acid.


A rapid, easy and chemical preparative method for the growth of ZnO nanoparticles with important surface physical properties is discussed. Emphatically, after capping with folic acid, its photoluminescence properties are in the visible region. Therefore, the same can be used for monitoring local environmental properties of biosystems.


ZnO nanoparticles Folic acid Structural effects Spectroscopic study Charge transfer effects


Nanometer size multifunctional materials are gearing the biological fields in various ways [1]. One of the promising nontoxic and biocompatible semiconductor material is Zinc Oxide (ZnO), which has received extensive application due to its exceptional electrical and optical characteristics [2] in fabricating nanoscaled electronic and optoelectronic devices. ZnO is a kind of wide band gap (3.37 eV) semiconductor with large exciton binding energy (60 meV) [2]. In comparison to other wide band-gap semiconductors, ZnO possesses higher quantum efficiency [3] and higher exciton energy [4, 5]. Also, ZnO is a biofriendly oxide semiconductor and an inexpensive luminescent material. Owing to the properties stated above, it is expected to have a wide range of applications in room temperature ultraviolet (UV) lasing [6], biosensors [7], bioimaging [8], drug delivery [9] and piezoelectric transducers [10]. In general, ZnO is considered “generally recognized as safe” (GRAS) [11] but ZnO nanoparticle system may be toxic. ZnO nanosystem may be of important relevance in the context of nanomedicine, where targeted treatment of biological systems at molecular level is a necessity [12].

Recently, there are several physical or chemical synthetic methods of preparing ZnO, such as thermal evaporation [13], pulsed laser deposition (PLD) [14], ion implantation [15], reactive electron beam evaporation [16], thermal decomposition [17] and sol–gel technique [1822]. To obtain ZnO nanoparticle, we choose sol–gel method because of its simplicity, which offers a possibility of large-area yield at low cost.

In the present study, nano-sized ZnO sample has been prepared by chemical synthesis in presence of surface active biological substance, such as folic acid. Folic acid [23, 24] is a member of the Vitamin B family and is necessary for the healthy function of a variety of bodily processes. The structural aspect of the folic acid is shown in Figure 1. Folic acid is sparingly soluble in pure water, but is well dispersed under physiological pH ~ 7.5. Folic acid being a multi dentate ligand, helps in controlling ZnO nanoparticle size through its surface charge density [23]. Also, folic acid has a natural affinity towards Folate receptor protein, which is over expressed by a number of tumor cells [25]. Since ZnO nanoparticles are cytotoxic and can combat the growth of tumor cells, it is envisaged that such a capping would help in targeting tumor cells. In this article further, the structural effects and the influence of folic acid are discussed in detail with the help of physical methods and spectroscopic tools. It is envisioned that the simple preparative scheme of the compound and the physical characteristics as shown in this article, would find its vital pathway in biotechnological applications and as well as optoelectronic device forming material.
Figure 1

Molecular structure of folic acid.

Materials and methods

Chemical method

Chemical Synthesis of pure Zinc oxide (ZnO)

ZnO nanoparticles were prepared by the sol–gel technique (shown in Figure 2) from the zinc acetate (Zn(CH3COO)2. 2H2O, extra pure AR, grade material, from SRL, India). Desired weight of zinc acetate was dissolved in triple distilled water (TDW) and (1:1/vol) ammonia solution (Merck India) was added to this solution drop by drop, maintaining pH ~ 7.5; initially zinc precipitated as zinc hydroxide. After centrifugation, the precipitate has been collected and re-dispersed into TDW for removing of excess ions. Finally, the precipitate was recollected and dried at 100°C to get ZnO.
Figure 2

Flow chart of chemical preparation of ZnO nanoparticle in presence of folic acid template.

a) ZnO grown under Folic acid template

Folic acid (M.F.: C19H19N7O6, procured from Sigma. life Science), was dissolved in mildly alkaline TDW [26] at different percentage concentrations. Folic acid solution of desired dilution was added to zinc acetate solution and the final pH was adjusted to 7.5. The samples are denoted as Z0.2, Z0.5, Z1.0, Z1.3, Z2.0, Z3.0 and Z4.8. The suffix (Zx) represents the percentage concentration (weight/volume) of folic acid solution. After centrifugation, the precipitate was collected and re-dispersed into TDW for removal of excess ions. Finally, the precipitates were recollected and dried at 100°C. The schematic representation of the chemical synthesis is given in Figure 2. The prepared samples have been characterized by various physical techniques as given in the following classified sections.

Physical methods of characterization of the ZnO nanoparticles

X-ray diffraction (XRD) measurements

The phase structures of the samples were identified by X-ray diffraction technique using Seifert XDAL 3000 diffractometer with CuKα radiation (wavelength of the radiation, k = 1.54 Å). The data have been collected in the range (2θ) 30° –80° with a step size of 0.06°. Si has been used as external standard to deconvolute the contribution of instrumental broadening [27]. The XRD pattern has been shown in Figure 3.
Figure 3

X-ray diffraction patterns with (hkl) values of as-grown ZnO nanoparticles by sol–gel method, where folic acid concentration (weight/volume) has been (a) 0%, (b) 0.5%, (c) 1.3%, (d) 4.8%.

The grain sizes of the synthesized samples have been calculated using Scherrer formula [27]:
D hkl = K λ β P cos θ

where, Dhkl is the average grain size, K the shape factor (taken as 0.9), λ is the X-ray wavelength, βP is the full width at half maximum (FWHM) intensity (here 101 peak of the ZnO spectrum fitted with a Gaussian, for precision measurement) and θ is the Bragg angle.

The nano crystalline material usually suffers from structural strain as the grain interior is relatively defect free but the grain boundary consists of high-density defect clusters [28, 29]. Thus, the strain in the lattice has been estimated through constructing Williamson–Hall (W–H) plot, with different Bragg peaks [30] taken in to consideration, such as:
β cos θ = K λ / D hkl + 2 ɛ sin θ

where, ϵ is the micro strain parameter.

Also, an estimation of the lattice parameters has been made by using FullProf program [31].

Transmission Electron Microscopic (TEM) study

The morphology of the synthesized product were characterized by transmission electron microscopy, TEM (Tecnai S-twin, FEI) using an accelerating voltage of 200 kV, having a resolution of ~ 1 Å. For this analysis, the ZnO sample has been dispersed in TDW through a probe sonicator; a drop of the same was placed onto a carbon coated copper grid and dried at room temperature. Furthermore, selected area electron diffraction (SAED) patterns are recorded to determine the growth orientation of the synthesized ZnO.

Spectroscopic Measurements

i) Fourier transmission infrared (FT-IR) spectra

Fourier transmission infrared (FT-IR) spectra of the powders (as pellets in KBr, without moisture) were recorded using a Fourier transform infrared spectrometer (Perkin Elmer FTIR system; Spectrum GX) in the range of 400–6000 cm-1 with a resolution of 0.2 cm-1.

ii) UV –Vis Spectroscopic measurements

The optical absorption spectra were measured in the range of 250–800 nm using a UV–VIS-NIR scanning spectrometer (Lamda 750, Perkin Elmer).

iii) Room temperature Photoluminescence (PL) Spectroscopy

Room temperature Photoluminescence (PL) measurement was carried out by a laser induced luminescence spectrometer (model IK3102R-G), the excitation source at room temperature being 325 nm line from a He-Cd laser.

Results and discussions

X-ray Diffraction (XRD) study

XRD results give us the characteristic diffraction pattern of the crystallites under the particular configuration, through a Bragg angle. Figure 3 shows the XRD patterns of the synthesized ZnO powder samples in presence of folic acid template. The appearance of characteristic diffraction peaks for pure ZnO sample corresponding to (1 0 0), (0 0 2), (1 0 1), (1 0 2), (1 1 0), (1 0 3) and (1 1 2) planes is in good agreement with the standard XRD peaks of crystalline bulk ZnO with hexagonal wurtzite structure [JCPDS card No. 36–1451, a = 3.2501 Å, c = 5.2071 Å, space group: P63mc (1 8 6)], except for Z4.8 sample, where partial crystallinity has been found. No characteristic peaks from the intermediates such as Zn(OH)2 can be detected in the samples stated above. The amorphous nature in Z4.8 sample is only due to the ensconced folic acid molecules due to its high concentration [32]. All the XRD data of the samples have been analyzed by FullProf programming as shown in Table 1. In order to have a clear idea of the partial crystallinity observed in the case of Z4.8 sample, the analysis (through FullProf programming) has been clearly shown in Figure 4 and Table 2. The analysis depicts that partial crystallinity of ZnO remains, despite the strong folic acid influence in the medium. The lattice parameters given in Table 1 for the synthesized ZnO samples are in accordance with standard data of ZnO wurtzite structure except for Z1.0 sample. The deviation here is ~ 11% in a-parameter and ~25% in c-parameter. This could be due to the structural transition in the crystallite, which we discuss later in detail.
Table 1

Lattice constant calculated from Fullprof programming


a (Å)

b (Å)

c (Å)

Pure ZnO
































Figure 4

XRD peak fitting for Z 4.8 sample using FullProf programming, notice Bragg position for crystallinity assessment.

Table 2

Miller indices (hkl) and corresponding peak position for Z 4.8 sample

h k l

peak position

1 0 0


0 0 2


1 0 1


1 0 2


1 1 0


1 0 3


2 0 0


1 1 2


2 0 1


0 0 4


2 0 2


Further, the average grain sizes of the ZnO samples were estimated from X-ray line broadening using Scherrer’s equation [27]. The particle size of pure ZnO is 41 nm, whereas it decreases to 20 nm with increase in folic acid concentration, shown in Figure 5. A sharp decrease in grain size (grain size ~ 18 nm) for Z1 sample has been shown in the results. The use of folic acid template has been effective after a certain concentration in controlling the Ostwald ripening [33] process in the growth rate of the crystallites. From the size effect of the ZnO shown the agglomeration number of the molecules in the case of each samples can be explained through simple relationship (assuming the small crystallites are roughly spherical for a minimal surface to volume ratio):
n = 4 / 3 ( πr 3 p ) N A / M
where, density of ZnO (ρ) = 5.606 gm/cm3, NA is the Avogadro’s number, molecular weight (M) = 81.389 gm/mole.
Figure 5

Relationship between ZnO grain size development and folic acid concentration (weight/volume), added during sol–gel preparation method.

It has been noticed from the results (Table 3), shown that the grain size decreases with folic acid concentration with a consequent decrease in agglomeration number of ZnO crystallites. One can estimate the strain in ZnO structure due to its size effect (grown in the presence of folic acid) by W-H plot, shown in Figure 6. Considerable anisotropy in structure has been noticed since unambiguous linear plot of the strain from all Bragg angles were not possible, the reason possibly lies with the surface effect of the crystallites. Although the results have been shown for only two representative samples [for pure ZnO (~ 21 nm) and Z1.3 samples (~ 29 nm)] but the trend has been maintained in case of all the samples.
Table 3

Average grain size, agglomeration number (n), surface to volume ratio of the crystallites and the molecular organization of ZnO crystallites grown without and with folic acid template

Avg. grain size



No. of molecules in the surface

40 nm (pure ZnO)




20 nm




(with 3% folic acid concentration)

Figure 6

Williamson–Hall plots for (a) pure ZnO and (b) Z 1.3 samples, for structural strain analysis. Error bar indicates the structural broadening of particular peak.

Morphological Investigation by TEM

Typical TEM images of different ZnO samples grown under folic acid template (pure, Z1.3, Z4.8) has been shown in Figure 7. TEM analysis was carried out for the determination of morphology, size and crystalline nature of the synthesized ZnO crystals. It can be estimated that the average size of ZnO lies nearly around 10 nm (from Figure 7(a)), which appears lower than the estimated results from Scherrer analysis. The fringes (shown in Figure 7(b)) in the microscopic analysis depicts the crystallinity of the selected zone in pure ZnO sample. Similarly, the wurtzite pattern has been shown in Z1.3 sample, shown in Figure 7(c) but with in the emblem of folic acid. Changes in the structure and size due to encapsulation by folic acid are quite evident from the Figure 7(c). However, the crystallinity pattern is maintained as shown in the subsequent results, in Figure 7(d) and (e). With increase in folic acid concentration, such as Z4.8 sample, a complete change in morphological structure has been found (shown in Figure 7(f)). The organization of nano-rods is evident. Further, the electron beam was focused on the nano-rods, fringe structure was repeatedly observed, as shown in Figure 7(g). Thus, we find at higher concentration of folic acid, although the ZnO granules are organized into nano-rod like structure yet a part of intrinsic crystallinity is retained.
Figure 7

TEM images for structural morphology of (a) pure ZnO sample and (b) the corresponding fringe patterns; (c) Z 1.3 sample and the corresponding (d) SAED and (e) fringe pattern; (f) Z 4.8 sample and (g) the corresponding fringe pattern of rod-like structure.

However, the size estimate of nanoparticles from Scherrer method differs considerably, but it may be a rough estimate from the Dhkl values in the Scherrer’s formula. Both TEM and XRD method justifies the crystalline nature of the nanoparticles.

Spectroscopic study

FTIR investigation

The structural analysis of wurtzite ZnO was further supported through FTIR investigation, shown in Figure 8. Figure 8(a) corresponds to the wurtzite oxide stretching frequencies of ZnO. The main absorption bands at ~ 450–500 cm-1(~ 4473x10-10- 4970 x10-10 joule), which is the stretching mode of ZnO, was considered [3436]. In this context, it is observed that there is an influence of folic acid as the stretching modes have been shifted to higher energy states (with decrease in size of nanocrystallites). The effect of folic acid concentration on the starching frequencies of ZnO can be sensed through the calculation of the force constant
v = 1 / 2 πc [ K / μ ] 1 / 2
and is tabulated as under Table 4[37]. These shifts may be related to change in bond length of Zn-O in the nanoparticles [37]. Further the FTIR spectra show absorption bands corresponding to the residual functional groups of folic acid template, as shown in Figure 8(b) and Table 5. Thus, it can be inferred that the influence of the template exists and ZnO electronic environment has been modified.
Figure 8

FTIR spectra of ZnO nanoparticles grown under the template of folic acid solution in (a) lower wave number and (b) higher wave number range (to show the residual effect of folic acid).

Table 4

IR frequency shift of Zn-O stretching frequency under the influence of folic acid


IR frequency (cm-1)

Pure ZnO










Table 5

FTIR absorption frequencies for residual groups of folic acid

Wave number (cm-1)

Absorption band

~ 3400

O-H mode

~ 2900

C-H mode

~ 1600

Symmetric C = O stretching mode

~ 1380

asymmetric C = O stretching mode

UV–vis spectrum analysis

The electronic absorption spectrum of ZnO samples in the UV–vis range enables to characterize the absorption edge related to semiconductor band structure. Figure 9 shows the UV–visible spectra of ZnO nanoparticles synthesized under folic acid template. The spectral absorption coefficient α(λ) has been evaluated [38] from the measured spectral extinction coefficient, k(λ), using the following expression:
α λ = 4 π k λ / λ
where λ is the wavelength of the absorbed photon. The optical band gap (Eg) of the samples have been estimated from the well known expression [39] for direct transition, by fitting experimental absorption data with the equation
α E = A ( E Eg ) n
where E (=hc/λ) is the photon energy and A is a constant and ‘n’ depends on the kind of optical transition that prevails. Specifically, with n =1/2, a good linearity has been observed for the direct allowed transition, the most preferable one in the system studied here. Standard extrapolation of absorption onset (as shown in Figure 10) [39] to αE = 0 (where E = E g) has been made for each samples. The band gap of pure ZnO is ~ 3.3 eV, which is good agreement with other studies [40]. Overall decreasing nature of optical band gap (from 3.30 eV to 3.22 eV) has been observed in Figure 11, except for Z1.0 and Z1.3 samples, which lies in the structural transition zone. This effect is in corroboration with the XRD results, as referred in Figure 5. The red shift of the band gap due to systematic increase of folic acid concentration in the medium (at the sample preparation state) could be attributed to some defect state between valence band and conduction band (O2p → Zn3d) [41]. The overall effect of this red shift of the band gap energy due to increase in folic acid concentration also relates to structural morphologies, particle size and surface microstructures [40]. However, a structural transition around Z1 and Z1.3 is evident from the result of XRD study (Figure 5) and optical absorption study (Figure 11). It would be worthwhile perhaps to recall the effect of subtle electronic environmental changes from IR spectroscopic data that conforms to this kind of structural changes.
Figure 9

Optical absorbance spectra for pure ZnO (a representative spectrum in the range of 250–500 nm).

Figure 10

Plots of (αhν) 2 vs photon energy for ZnO sample.

Figure 11

Dependence of the band gap (Eg) of all samples as a function of folic acid concentration.

Photoluminescence spectroscopy (PL)

The room-temperature PL spectroscopic study enables to determine the electronic energy levels from where emission is particularly observed which in turn helps to corroborate the band structure of the ZnO nanoparticles [42]. The results of PL spectrum of ZnO nanoparticles are presented in Figure 12. The pure ZnO spectrum shows a broad emission spectrum covering from near UV to whole of the visible region. With introduction of very low concentration of folic acid in the medium (Z0.5), a double peak emission spectrum becomes existent. This double peak structure is very prominent at Z1.3 sample, which is also the region exactly where a structural transition was observed with the size effect (vide Figures 5 and 11, band gap ~3.17 eV). The ultraviolet emission peak (UV) corresponds to an exciton emission band, whereas the visible peak is believed to be due to an electronic transition from a level close to the conduction band edge to a defect-associated trap state, such as an oxygen vacancy [43, 44]. The UV emission is known as a near-band-edge (NBE) emission, originating from the recombination of free exciton through an exciton–exciton collision process [45].
Figure 12

Photoluminescence spectra of (a) pure ZnO, (b) Z 0.5 , (c) Z 1.3 , (d) Z 2.0 , (e) Z 3.0 , (f) Z 4.8 samples.

In pure ZnO spectrum, a weak emission peak at 440 nm (blue emission) has been observed due to surface defect in ZnO, mainly due to Zn vacancy and broad green emission band (~ 550 nm), known as a deep level emission, relates to the deep-level defect states [46]. Singly ionized oxygen vacancy is responsible for this green emission in the ZnO [47]. It results from the recombination of the photo-generated hole with an electron, occupying the oxygen vacancy and interstitials of zinc.

In all samples, green light emission is most prominent. With increase in folic acid concentration in the medium (above 1.3%) a dramatic change in emission spectrum is observed. The spectrum now shows the emission peak only ~ 464 nm (for Z2.0) to 472 nm (Z3.0 and Z4.8) (with the blue shift of single emission peak), which is a signature of charge transfer reaction [48]. This clear transition is in corroborative confirmation of the effect of folic acid concentration on ZnO particle size and band gap properties shown by Figures 5 and 11. ZnO is now virtually ensconced structure with folic acid and the effect is drastic. The effect is also evident from FTIR (Tables 4 and 5) and TEM (Figure 7) study. The surface defects of ZnO are in the proximity of the functional groups of folic acid. Therefore, charge transfer effect becomes prominent and viable.

However, the physical mechanism behind visible light emission in ZnO is claimed by different authors in different ways and is still under controversy [4952]. Therefore, it is important to investigate the luminescent mechanism caused by the defects of ZnO thin films, since they are the key factors for obtaining the visible luminescence. In our case, we find that the ZnO nanoparticle size decreases under influence of folic acid, there is a structural transition and finally the nano rod like structure is formed under the strong influence of folic acid. As a consequence to this the emission spectrum has shown the pronounced green light emission, which is conferred to photon induced charge transfer transition state.


Influence of folic acid in controlling the structural effects of ZnO nanoparticle under physiological conditions of temperature and pH has been studied as a novel method. The physical investigations with XRD, TEM and spectroscopic tools have been carried out in order to understand the interesting structural changes involved in the system which may find important biomedical applications. Photo induced charge transfer due to folic acid ensconced ZnO nanosystem is particularly a noticeable effect as seen from our results.



The author acknowledge the technical help in measurements received from Solid State Physics Division, Indian Association for the Cultivation of Science for XRD data, Biophysics Division, Saha Institute of Nuclear Physics (SINP) (Mr. Pulak Ray) for TEM measurement, Surface Physics Division, SINP (Smita Mukherjee, Dr. Satyaban Bhunia) for FTIR and PL measurements. The author also thanks Prof. P. M. G. Nambissan for UV–vis spectroscopy and Soma Roy for all kinds of technical help.

Authors’ Affiliations

Applied Nuclear Physics Division, Saha Institute of Nuclear Physics


  1. Salata OV: Applications of nanoparticles in biology and medicine. J Nanobiotechnology. 2004, 2: 3-8. 10.1186/1477-3155-2-3.View ArticleGoogle Scholar
  2. Dutta S, Chattopadhyay S, Sarkar A: Role of defects in tailoring structural, electrical and optical properties of ZnO. Prog Mater Sci. 2009, 54: 89-136. 10.1016/j.pmatsci.2008.07.002.View ArticleGoogle Scholar
  3. Yu P, Tang ZK, Wong GKL: Proc. 23rd Int. Conf. on Physics of Semiconductors. Edited by: Scheffler M, Zimmermann R. 1996, World Scientific, Singapore, 1453-BerlinGoogle Scholar
  4. Cracium V, Elders J, Gardeniers JGE: Growth of ZnO thin films on GaAs by pulsed laser deposition. Thin Solid Films. 1995, 259: 1-4. 10.1016/0040-6090(94)09479-9.View ArticleGoogle Scholar
  5. Look DC: Recent advances in ZnO materials and devices. Mater Sci Eng B. 2001, 80: 383-387. 10.1016/S0921-5107(00)00604-8.View ArticleGoogle Scholar
  6. Tang ZK, Wong GKL, Yu P: Room-temperature ultraviolet laser emission from self-assembled ZnO microcrystallite thin films. Appl Phys Lett. 1998, 72: 3270-3272. 10.1063/1.121620.View ArticleGoogle Scholar
  7. Zhao Z, Lei W, Zhang X: ZnO-Based Amperometric Enzyme Biosensors. Sensors. 2010, 10: 1216-1231. 10.3390/s100201216.View ArticleGoogle Scholar
  8. Senthilkumar K, Senthilkumar O, Yamauchi K: Phys. Preparation of ZnO nanoparticles for bio-imaging applications. Status Solidi b. 2009, 246: 885-888. 10.1002/pssb.200880606.View ArticleGoogle Scholar
  9. Wang Y, Chen L: Quantum dots, lighting up the research and development of nanomedicine. Nanomedicine: Nanotechnology, Biology, and Medicine. 2011, 7: 385-402. 10.1016/j.nano.2010.12.006.View ArticleGoogle Scholar
  10. Oertel DC, Bawendia MG, Arango AC: Photodetectors based on treated CdSe quantum-dot films. Appl Phys Lett. 2005, 87: 213505-213507. 10.1063/1.2136227.View ArticleGoogle Scholar
  11. Rasmussen JW, Martinez E, Louka P, Wingett DG: Zinc Oxide Nanoparticles for Selective Destruction of Tumor cells and Potential for Drug delivery Applications. Expt Opin Drug Deliv. 2010, 7: 1063-1077. 10.1517/17425247.2010.502560.View ArticleGoogle Scholar
  12. Clarke DR: Varistor ceramics. J Am Ceram Soc. 1999, 82: 485-502.View ArticleGoogle Scholar
  13. Masaki T, Kim SJ, Watanabe H: Synthesis of Nano-Sized ZnO Powders Prepared by Precursor Process. J Ceram Process Res. 2003, 4: 135-139.Google Scholar
  14. Chen L, Chen ZQ, Shang XZ: Effect of annealing temperature on density of ZnO quantum dots. Solid State Commun. 2006, 137: 561-565. 10.1016/j.ssc.2005.12.039.View ArticleGoogle Scholar
  15. Wang ZL: Zinc oxide nanostructures: growth, properties and applications. J Phys Condens Matter. 2004, 16: R829-R858. 10.1088/0953-8984/16/25/R01.View ArticleGoogle Scholar
  16. Wu HZ, Qiu DJ, Cai YJ: Optical studies of ZnO quantum dots grown on Si(0 0 1). J Cryst Growth. 2002, 245: 50-55. 10.1016/S0022-0248(02)01711-6.View ArticleGoogle Scholar
  17. Yang LL, Yang JH, Liu XY: Low-temperature synthesis and characterization of ZnO quantum dots. J Alloys Compd. 2008, 463: 92-95. 10.1016/j.jallcom.2007.12.006.View ArticleGoogle Scholar
  18. Spanhel L, Anderson MA: Semiconductor Clusters in the Sol–gel Process: Quantized Aggregation, Gelation, and Crystal Growth in Concentrated ZnO Colloids. J Am Chem Soc. 1991, 113: 2826-2833. 10.1021/ja00008a004.View ArticleGoogle Scholar
  19. Meulenkamp EA: Synthesis and Growth of ZnO Nanoparticles. J Phys Chem B. 1998, 102: 5566-5572. 10.1021/jp980730h.View ArticleGoogle Scholar
  20. Wu YL, Tok AIY, Boey FYC: Surface modification of ZnO nanocrystals. Appl Surf Sci. 2007, 253: 5473-5479. 10.1016/j.apsusc.2006.12.091.View ArticleGoogle Scholar
  21. Guo L, Yang SH, Yang CL: Highly monodisperse polymer-capped ZnO nanoparticles: Preparation and optical properties. Appl Phys Lett. 2000, 76: 2901-2903. 10.1063/1.126511.View ArticleGoogle Scholar
  22. Tong YH, Liu YC, Lu SX: The Optical Properties of ZnO Nanoparticles Capped with Polyvinyl Butyral. J Sol Gel Sci Technol. 2004, 30: 157-161.View ArticleGoogle Scholar
  23. Ke CY, Mathias CJ, Green MA: Folate-receptor-targeted radionuclide imaging agents. Adv Drug Deliv Rev. 2004, 56: 1143-1160. 10.1016/j.addr.2004.01.004.View ArticleGoogle Scholar
  24. Zhang J, Rana S, Srivastava RS: On the chemical synthesis and drug delivery response of folate receptor-activated, polyethylene glycol-functionalized magnetite nanoparticles. Acta Biomaterialia. 2008, 4: 40-48. 10.1016/j.actbio.2007.06.006.View ArticleGoogle Scholar
  25. Campbell IG, Jones TA, Foulkes WD, Trowsdale J: Folate-binding Protein Is a Maker for Ovarian Cencer. Cancer Res. 1991, 51: 5329-5338.Google Scholar
  26. Wu Z, Li X, Hou C: Solubility of Folic Acid in Water at pH Values between 0 and 7 at Temperatures (298.15, 303.15, and 313.15) K. J Chem Eng Data. 2010, 55: 3958-3961. 10.1021/je1000268.View ArticleGoogle Scholar
  27. Cullity BD, Stock SR: Elements of X-ray Diffraction. 2001, Prentice-Hall, Englewood Cliffs, New JerseyGoogle Scholar
  28. Staab TEM, Krause-Rehberg R, Kieback B: Review Positron annihilation in fine-grained materials and fine powders—an application to the sintering of metal powders. J Mater Sci. 1999, 34: 3833-3851. 10.1023/A:1004666003732.View ArticleGoogle Scholar
  29. Ungár T, Tichy G, Gubicza J: Correlation between subgrains and coherently scattering domains. Powder Diffr. 2005, 20: 366-375. 10.1154/1.2135313.View ArticleGoogle Scholar
  30. Williamson GK, Hall WH: X-ray line broadening from field aluminium and Wolfram. Acta Metall. 1953, 1: 22-31. 10.1016/0001-6160(53)90006-6.View ArticleGoogle Scholar
  31. Bilecka I, Luo L, Djerdj I: Microwave-Assisted Nonaqueous Sol–gel Chemistry for Highly Concentrated ZnO-Based Magnetic Semiconductor Nanocrystals. J Phys Chem C. 2011, 115: 1484-1495. 10.1021/jp108050w.View ArticleGoogle Scholar
  32. Vora A, Riga A, Dollimore D: Thermal stability of folic acid. Thermochim Acta. 2002, 392–393: 209-220.View ArticleGoogle Scholar
  33. Mantzaris NV: Liquid-phase synthesis of nanoparticles: Particle size distribution dynamics and control. Chem Eng Sci. 2005, 60: 4749-4770. 10.1016/j.ces.2005.04.012.View ArticleGoogle Scholar
  34. Kwon YJ, Kim KH, Lim CS: Characterization of ZnO nanopowders synthesized by the polymerized complex method via an organochemical route. J Ceram Proc Res. 2002, 3: 146-149.Google Scholar
  35. Silva RF, Zaniquelli MED: Morphology of nanometric size particulate aluminium-doped zinc oxide films. Colliod Surf Physicochem Eng Aspect. 2002, 198–200: 551-558.View ArticleGoogle Scholar
  36. Li H, Wang J, Liu H: Sol–gel preparation of transparent zinc oxide films with highly preferential crystal orientation. Vacuum. 2004, 77: 57-62. 10.1016/j.vacuum.2004.08.003.View ArticleGoogle Scholar
  37. He YY, Wang XC, Jin PK: Complexation of anthracene with folic acid studied by FTIR and UV spectroscopies. Spectrochim Acta Part A. 2009, 72: 876-879. 10.1016/j.saa.2008.12.021.View ArticleGoogle Scholar
  38. Dutta S, Chattopadhyay S, Jana D: Annealing effect on nano-ZnO powder studied from positron lifetime and optical absorption spectroscopy. J Appl Phys. 2006, 100: 114328-114333. 10.1063/1.2401311.View ArticleGoogle Scholar
  39. Pancove J: Optical Processes in Semiconductors. 1979, Prentice-Hall, New JerseyGoogle Scholar
  40. Zak AK, Abrishami ME, Abd Majid WH: Effects of annealing temperature on some structural and optical properties of ZnO nanoparticles prepared by a modified sol–gel combustion method. Ceram Int. 2011, 37: 393-398. 10.1016/j.ceramint.2010.08.017.View ArticleGoogle Scholar
  41. Sahoo T, Kim M, Baek JH: Synthesis and characterization of porous ZnO nanoparticles by hydrothermal treatment of a pure aqueous precursor. Mater Research Bull. 2011, 46: 525-530. 10.1016/j.materresbull.2011.01.002.View ArticleGoogle Scholar
  42. Xu F, Chen J, Guo L, Lei S, Ni Y: In situ electrochemically etching-derived ZnO nanotube arrays for highly efficient and facilely recyclable photocatalyst. Appl Surf Sci. 2012, In PressGoogle Scholar
  43. Dijken AV, Meulenkamp EA, Vanmaekelbergh D: The Kinetics of the Radiative and Nonradiative Processes in Nanocrystalline ZnO Particles upon Photoexcitation. J Phys Chem B. 2007, 104: 1715-1723.View ArticleGoogle Scholar
  44. Norberg NS, Gamelin DR: Influence of Surface Modification on the Luminescence of Colloidal ZnO Nanocrystals. J Phys Chem B. 2005, 109: 20810-20816. 10.1021/jp0535285.View ArticleGoogle Scholar
  45. Tang ZK, Kawasaki M, Ohtomo A: Self-assembled ZnO nano-crystals and exciton lasing at room temperature. J Crys Growth. 2006, 287: 169-179. 10.1016/j.jcrysgro.2005.10.062.View ArticleGoogle Scholar
  46. Wang D, Seo HW, Tin C-C: Effects of postgrowth annealing treatment on the photoluminescence of zinc oxide nanorods. J Appl Phys. 2006, 99: 113509-113513. 10.1063/1.2200593.View ArticleGoogle Scholar
  47. Vanheusden K, Warren WL, Seager CH: Mechanisms behind green photoluminescence in ZnO phosphor powders. J Appl Phys. 1996, 79: 7983-7990. 10.1063/1.362349.View ArticleGoogle Scholar
  48. Spalenka JW, Paoprasert P, Franking R: Molecular control of pentacene/ZnO photoinduced charge transfer. Appl Phys Lett. 2011, 98: 103303-103305. 10.1063/1.3560481.View ArticleGoogle Scholar
  49. Cho S, Ma J, Kim Y: Photoluminescence and ultraviolet lasing of polycrystalline ZnO thin films prepared by the oxidation of the metallic Zn. Appl Phys Lett. 1999, 75: 2761-2763. 10.1063/1.125141.View ArticleGoogle Scholar
  50. Liu M, Kitai AH, Mascher P: Point defects and luminescence centres in zinc oxide and zinc oxide doped with manganese. J Lumin. 1992, 54: 35-42. 10.1016/0022-2313(92)90047-D.View ArticleGoogle Scholar
  51. Lin B, Fu Z, Jia Y: Defect Photoluminescence of Undoping ZnO Films and Its Dependence on Annealing Conditions. J Electrochem Soc. 2001, 148: G110-G113. 10.1149/1.1346616.View ArticleGoogle Scholar
  52. Water W, Chu S-Y: Physical and structural properties of ZnO sputtered films. Mater Lett. 2002, 55: 67-72. 10.1016/S0167-577X(01)00621-8.View ArticleGoogle Scholar


© Dutta and Ganguly.; licensee BioMed Central Ltd. 2012

This article is published under license to BioMed Central Ltd. This is an Open Access article distributed under the terms of the Creative Commons Attribution License (, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.