kim 2005, tio2 preparado capa a capa
DESCRIPTION
jhgjhTRANSCRIPT
-
of
f-a
Fuj
culty o
ama,
ne 16
nopar
abric
useful optical, electrical, and chemical properties such as high
mechanical instability, and high cost. However layer-by-layer
(LBL) self assembly method using sequential adsorptions of
thickness of thin film can be controlled with a nanoscale [16].
thin film comprising polyelectrolyte and TALH solution
which is stable and double negatively charged inorganic
precursor [21] shows high refractive index (n =1.68 1.8),e average thickness
Thin Solid Films 499 (200refractive index [1], high relative dielectric constant [2],
remarkable solar energy conversion [3,4], and photocatalysis
[5]. Therefore TiO2 thin film can be a promising material for
an optical filter [6], antireflection film [7], a self-cleaning
coating [8], a high efficient dielectric [9], and a solar cell [10].
TiO2 thin film has been fabricated by several methods such
as a solgel synthesis [11], sputtering [12] and chemical vapor
deposition (CVD) [13]. However, these processes that require
a high temperature, a high qualitative vacuum system and
intricate equipments have a limit of film area or thickness,
In previous reports, TiO2 thin films composed of
positively charged TiO2 nanoparticles [17] and oppositely
charged polyelectrolyte [18] or consisted of polyelectrolyte
and negatively charged titanium (IV) bis(ammonium lac-
tato) dihydroxide (TALH) [19] have been successfully
fabricated by a LBL self-assembly method. However the
refractive index of the film composed of TiO2 nanoparticles
and polyelectrolytes is significantly decreased because of
the presence of pores and polyelectrolyte with low refractive
index relatively [20]. On the other hand, although the TiO2applications and photocatalytic properties by decomposing methyl orange molecules gradually according to UV irradiation time. In addition, as
the pH of TALH was decreased from pH 5.5 to 2.0, the thickness of (TiO2 /TALH)30 film was increased from ca. 85 nm to ca. 442 nm.
D 2005 Elsevier B.V. All rights reserved.
Keywords: Layer-by-layer self-assembly method; TiO2 thin film; Polyelectrolyte; Quartz crystal microbalance
1. Introduction
In the past several years, there has been increasing interest
in the fabrication of TiO2 thin films because they present
ionized polyelectrolytes and oppositely charged materials in
aqueous solutions has lots of advantages such as a simple
process, low temperature deposition, no limit of thickness and
needless of complicated equipments [14,15]. In addition, thetemperature. Especially, by using the quartz crystal microbalance (QCM) to monitor the in-situ deposition phenomenon of TALH that is
saturated and then separated from the film before and after the deposition of 30 s at low pH, the anatase TiO2 multilayer films fabricated with 30
s deposition in TALH adjusted to pH 2.5 showed a higher refractive index (ca. n =1.75), a denser film growth, and a lower surface roughness
(ca. 10.5 nm) than those of the films deposited in different conditions. This film showed a high transmittance in visible range for opticalFabrication and characterization
layer-by-layer sel
Jin-Ho Kim *, Shiro
Department of Applied Physics and Physico-Informatics, Fa
Kohoku-ku, Yakoh
Available onli
Abstract
Titanium dioxide (TiO2) thin films assembled with TiO2 na
bis(ammonium lactato) dihydroxide (TALH) were successfully f0040-6090/$ - see front matter D 2005 Elsevier B.V. All rights reserved.
doi:10.1016/j.tsf.2005.07.001
* Correspondi
E-mail addresses: [email protected] (J.-H. Kim)
[email protected] (S. Shiratori).TiO2 thin film prepared by a
ssembly method
ita, Seimei Shiratori
f Science and Technology, Keio University, 3-14-1 Hiyoshi,
223-8522, Japan
August 2005
ticles and oppositely charged polyelectrolytes or titanium (IV)
ated via a layer-by-layer (LBL) self-assembly method at room
6) 83 89
www.elsevier.com/locate/tsfthis film has a small film growth with thng author. Fax: +81 45 566 1602.(ca.1.5 5 nm) of a bilayer [22,23]. In addition, the filmgrowth phenomenon between TALH and polyelectrolytes or
-
well as a gas sensor [25,26], because when material is
deposited on the electrode of QCM, frequency is decreased
used as a negatively charged polyelectrolyte. Titanium (IV)
bis(ammonium lactato) dihydroxide (TALH, 50 wt.%,
Aldrich) with double negative charges [21] was selected
as an inorganic precursor. The molecular structure of TALH
is shown in Fig. 1. The concentration of PPA and PDDA
were adjusted to 0.01 M using ultra pure water (>18 MVcm) and then the pH of solutions was adjusted with NaOH
or HCl. 0.1 wt.% of TiO2 colloidal solution was adjusted to
H HNH3
CH3
CH3
H
H
HH
C
C
C
CO
OO
OTi
OO
OO
J.-H. Kim et al. / Thin Solid Films 499 (2006) 838984in proportional to the mass change by the Sauerbrey
relation [27]:
df f2
NqAdm 1
In this study, we report that TiO2 thin films assembled
with TALH and TiO2 nanoparticles have been successfully
fabricated with a low surface roughness, high refractive
index, improved thickness growth and a high transmittance
by monitoring the deposition phenomenon depended on the
pH of solution as well as immersion time into TALH using a
QCM. In addition, the properties of these films were
compared with that of films comprising TiO2 nanoparticles
and polyelectrolyte.
2. Experimental details
2.1. Materials
The used starting materials were oppositely chargednanoparticles has not been sufficiently explored as functions
of the immersion time or the pH of solution [19].
Quartz crystal microbalance (QCM) has been used for
the monitoring of the in-situ deposition phenomenon of
materials on substrate in LBL assembly process [24] as
H3N
Fig. 1. Assumed molecular structure of the non-ionized form of TALH (the
arrows indicated electron pairs).poly(dimethyldiammonium chloride) (PDDA, 20 wt.%,
Aldrich) and TiO2 colloidal solution (ca. 7 nm in primary
particle size, anatase) obtained from Ishihara Sangyo, Ltd.
(Japan). Poly(phosphoric acid) (PPA, Wako) and poly(so-
dium 4-styrenesulfonate) (PSS, Mw=70,000, Aldrich) were
Fig. 2. Schematic illustration of the procedures to fabricatepH 2.5 and the pH of TALH solution was adjusted from 5.5
to 2.0 with HNO3. Glass, Si/SiO2, and QCM (AT-cut, 10
MHz) with a gold electrode were used as substrates.
2.2. Preparation of thin films
Negatively charged substrates, glass and Si/SiO2, were
obtained by KOH (1 wt.%) treatment in ultrasonication for 5
min and then rinsed in ultra pure water (pH 5.56.5). QCMwas also carried out KOH treatment and then the 3 bilayers
of (PDDA/PSS) were assembled on electrode to diminish
the surface influence of each QCM.
Substrates and QCM were immersed into TiO2 colloidal
solution and polyelectrolytes for 10 min and TALH solution
for 10 s 10 min. Fig. 2 depicts the schematic illustrationof the procedures to fabricate the (TiO2/TALH) multilayer
thin film. Rinse procedures (1 min3 times) weresubsequently carried out after immersion into solutions
using ultra pure water. These coating procedures were
repeated 30 times. When we deposit material B over A with
30 times, we describe as (A/B)30.
2.3. Characterization of multilayer thin films
The surface microstructure and the cross-section of thin
film deposited on glass substrate were investigated by a
field emission scanning electron microscope (FE-SEM,
Hitachi S-4700) and the root mean squared (RMS) surface
roughness was measured by an atomic force microscope
(AFM, Digital Instrument nanoscope ha) in a tapping mode.The RMS roughness was calculated according to the
following Eq. (2):
RMS ~ Zi Zave 2
N
s2
where Zi is the height on the Z-axis of feature i, Zave is the
average height of the entire image, and N is the number of
points in image.the multilayer thin film consisted of (TiO2/TALH).
-
The refractive index of film assembled on Si/SiO2substrate was determined by an ellipsometry (Film Tek
3000, Scientific Computing International) at the wavelength
of 632 nm. The absorbance and transmittance of prepared
TiO2 films deposited on glass were measured by a UV-vis
spectrophotometer (UV mini-1240, Shimadzu).
The photocatalytic properties of anatase TiO2 films to
decompose methyl orange molecules were measured.
Prepared thin film was put into the cell filled with methyl
orange solution that was adjusted to ca. 0.948 absorbance at
460 nm before UV irradiation and this cell was then exposed
to UV light (254 nm, 22 W, SUV-16, As One) for 30 min.
After taking the film out of the solution, the absorbance of
methyl orange solution was measured by UV-vis spectro-
photometer. These procedures were repeated until the total
irradiation time became 5.5 h.
resulted in the separation from TiO2 nanoparticles deposited
during previous procedure. We assume that this phenom-
larger clusters than that of Fig. 5 (ac). On the other hand,
the film fabricated using TALH adjusted to pH 5.5 showed
the formation of pores on film however the presence of pores
was remarkably decreased in TALH solution adjusted to pH
2.5 or 2.0 and these films contain ca. 70 100 nm clustersformed from the agglomeration of nanoparticles and TALH.
Fig. 5 (b) film showed a flat and dense surface morphology.
Fig. 6 shows the surface morphologies and cross-
sectional images of [(TiO2/TALH)(pH 2.5)]30 multilayers
as a function of immersion time into TALH. The prepared
thin films with 10 or 30 s immersion time present a dense
surface, however when the immersion time is increased to
10 min, the amount of pores is also increased on the film.
We consider that this result is caused by the separation of
TiO2 from film after 30 s from the film as shown in Fig. 3
(a). Fig. 6 (d) shows the cross-sectional image of Fig. 6 (b).
The thickness was ca. 275 nm, which was in good
accordance with an ellipsometry measurement.
J.-H. Kim et al. / Thin Solid F3. Results and discussion
3.1. Frequency shift of QCM
Fig. 3 shows the frequency shift of QCM deposited TiO2nanoparticles (pH 2.5) or PDDA (pH 2.5) in TALH solution
adjusted to pH 2.5 for 10 min. In this figure, the frequency
shift of QCM coated with PDDA that has a remarkably
larger charge density [28] than that of colloidal particles was
saturated in short time and then there is no large change of
frequency shift, however the frequency shift of QCM
deposited TiO2 nanoparticles was saturated after about 30
s and then decreased significantly. This decrease of
frequency shift after 30 s in TALH may be derived from
the separation of precipitated TiO2 on QCM because at low
pH, the destabilization of chelate results in TiO2 precipitate
or films and the TiO2 precipitates formed from titanium
lactate solution are charged positively [19], which hasFig. 3. Frequency shift of a QCM in TALH (pH 2.5) solution after the
deposition of TiO2 or PDDA: (a) TiO2 (pH 2.5) and (b) PDDA (pH 2.5).enon is gradually carried out after deposition for 30 s with
TiO2 nanoparticles. Therefore the deposition for 30 s in
TALH will be suitable for obtaining the reasonable TiO2thin film with high thickness growth.
The frequency shift for 30 s as a function of the pH of
TALH are given in Fig. 4. The frequency shift in TALH
adjusted to pH 5.5, 2.5, and 2.0 were 50, 145, and 210 Hz,
respectively. Hence, the thickest film can be assembled in
the pH 2.0 of TALH.
3.2. Surface morphology and thickness of films
Fig. 5 (a c) present the surface morphologies ofprepared (TiO2/TALH)30 multilayers thin films as a function
of the pH of TALH. Substrates were immersed into TALH
for 30 s. Fig. 5 (d) is the surface image of [(PDDA/
TALH)(pH 2.5)]30 thin film assembled using solutions
adjusted to pH 2.5. In this figure, the film was consisted of
Fig. 4. Frequency shifts of QCM in TALH solution as a function of the pH
of TALH after immersion into TiO2: (a) pH 5.5, (b) pH 2.5, and (c) pH 2.0.
ilms 499 (2006) 8389 85The RMS values of [(TiO2/TALH)(pH 2.5)]30 and
[(TiO2/PPA)(pH 2.5)]30 are shown in Fig. 7. In order to
-
Fig. 5. FE-SEM images of (TiO2/TALH)30 thin films as a function of the pH of TALH solution and (PDDA/TALH)30 film: (a) pH 5.5, (b) pH 2.5, (c) pH 2.0
pH 2
J.-H. Kim et al. / Thin Solid Films 499 (2006) 838986prepare films, glass substrates were immersed into TiO2colloidal and PPA solution for 10 min and TALH for 30 s.
The RMS of [(TiO2/TALH)(pH 2.5)]30 film as shown in Fig.
7 (a and b) was ca. 10.5 nm and the RMS of [(TiO2/
PPA)(pH 2.5)]30 as shown in Fig. 7 (c and d) was ca. 22.4
nm. From this result, it was turned out that the thin film
consisted of TiO2 nanoparticles and TALH has a lower RMS
value and the denser surface of TiO2 than that of the film
fabricated with nanoparticles and PPA. The refractive
and (d) [(PDDA/TALH)(pH 2.5)]30. TiO2 colloidal solution was adjusted toindices of thin films consisted of (TiO2/TALH) and (TiO2/
Fig. 6. Surface morphologies of [(TiO2/TALH)(pH 2.5)]30 thin films as a function o
(d) cross-sectional image of (b). Immersion time into TiO2 solution is 10 min.PPA) were ca. 1.70 1.75 and ca. 1.45 1.50 at 632 nm,respectively. These results will be important information for
optical applications.
Table 1 summarizes the properties of prepared (TiO2/
TALH)30 films as functions of the pH value and the
immersion time of TALH solution as well as a rinse process
after TALH assemble. As the immersion was increased from
10 to 30 s, the thickness of films was also increased from ca.
162 nm to ca. 275 nm in the pH 2.5 of TiO2 colloidal and
.5.TALH solutions and was then gradually decreased to ca. 50
f the immersion time into TALH solution: (a) 10 s, (b) 30 s, (c) 10 min, and
-
ng mo
10 A.
J.-H. Kim et al. / Thin Solid Fnm as the deposition was increased from 30 s to 10 min.
From this data, we suppose that at low pH, the negative
charge density of film formed from titanium lactate was
gradually increased until 30 s, which became the driving
force to deposit lots of positively charged TiO2 nano-
particles during next deposition. However, as the deposition
time in TALH was increased from 30 s to 10 min, the
formation of cationic TiO2 from TALH was gradually
carried out on the surface of film, which decreased the
negative charge of surface and then, the cationic TiO2complexes were finally separated from film deposited with
cationic TiO2 nanoparticles. This thickness decrease of film
Fig. 7. AFM images of (TiO2/TALH)30 and (TiO2/PPA)30 thin films in tappi
view, and (d) section analysis of (TiO2/PPA)30. Scan size and height is 10solution and 30 s into TALH solution. All solutions are adjusted to pH 2.5with the deposition over 30 s is consistent with the
frequency shift of QCM as shown in Fig. 3 (a).
The RMS values of films assembled with an immersion
for 20 or 30 s in TALH were lower than that of other films.
As the immersion time was increased from 30 s, the RMS
values were also gradually increased. In addition, as the pH
value of TALH was decreased from pH 5.5 to pH 2.0, the
Table 1
Properties of prepared (TiO2/TALH)30 thin films as functions of the pH and
immersion time of TALH solution as well as rinse process after TALH
deposition
Sample pH of
(TiO2/TALH)
Immersion
time into
TAHL
Rinse process
after TALH
deposition
Thickness
(nm)
Surface
roughness
(nm)
T1 (2.5/2.5) 10 s 1 min1 162 14.2T2 (2.5/2.5) 20 s 1 min1 170 10.2T3 (2.5/2.5) 30 s 1 min1 275 10.5T4 (2.5/2.5) 1 min 1 min1 155 12.7T5 (2.5/2.5) 5 min 1 min1 105 13.2T6 (2.5/2.5) 10 min 1 min1 50 16.2T7 (2.5/2.5) 30 s 1 min1 442 27.5T8 (2.5/2.5) 30 s 1 min1 85 17.5T9 (2.5/2.5) 1 min 1 min3 62 20.6film thickness was increased. Especially, the thin film
deposited in TALH adjusted to pH 2.0 was showed a high
thickness growth with ca. 442 nm. However the RMS value
was also largest than that of thin film fabricated in TALH
adjusted to pH 5.5 or 2.5.
Rinse process after TALH deposition also influenced the
thickness of films. Comparing the T4 and T9, the thickness
of film was decreased by the addition of rinse steps and the
RMS roughness was also increased because the cationic
TiO2 complexes were formed and separated from film
during rinse procedure.
de: (a) surface view, and (b) section analysis of (TiO2/TALH)30, (c) surface
m and 200 nm, respectively. Immersion time is 10 min into TiO2 and PPA
ilms 499 (2006) 8389 873.3. Absorbance, transmittance, and refractive index of
films
Fig. 8 shows the absorbance of prepared thin films as
functions of the pH of TALH and immersion time into
TALH solution. As shown in Fig. 8 (a), as the pH of
TALH was decreased from pH 5.5 to 2.0, the maximum
absorbance of TiO2 multilayer thin films was increased.
This result is in accordance with the thickness increase of
film as shown in Table 1. However, the absorbance of
films was not increased in proportional to the thickness of
film. Although the T7 film was fabricated with ca. 442 nm
in thickness, the absorbance was not remarkably higher
than that of T3 film. This means that the T7 film has a
high thickness growth with high RMS roughness during
deposition. Therefore some pores may be formed inside of
film.
Fig 8 (b) shows that the absorbance of films prepared
with deposition time from 10 to 30 s was gradually
increased and was then decreased from 30 s to 10 min at
285 nm. These data are in good accordance with the
thickness of films prepared in different conditions as shown
in Table 1.
-
Fig. 9. Transmittance of prepared (TiO2/TALH)30 thin films as a function of
the pH value of TALH with TiO2 solution adjusted to pH 2.5: (a) pH 2.5
and (b) pH 2.0. Immersion time is 10 min into TiO2 and 30 s into TALH,
respectively.
Fig. 8. UV-vis spectra of (TiO2/TALH)30 thin films prepared as functions as
(a) the pH of TALH solution with 30 s immersion time and (b) the
immersion time into TALH solution adjusted to pH 2.5. The pH and
immersion time of TiO2 solution are pH 2.5 and 10 min.
J.-H. Kim et al. / Thin Solid F88Fig. 9 presents the transmittances of sample T3 and T7
multilayers thin films. Sample T3 film showed a high
transmittance in a visible range, therefore this film may be
suitable for an optical application as a high refractive layer
because the refractive index of thin film was ca. 1.70 1.75at 632 nm. On the other hand, the transmittance of sample
T7 film was decreased in visible range. Even if it is clearly
difficult to identify the volume of pores and the roughness in
Fig. 5 (c) compared with Fig. 5 (b). When we compare the
thickness and absorbance of films, T7 film has a lower
density of TiO2 than that of T3 film by the formation of
pores, high roughness and thick film thickness. In fact, a
few cracks were shown on film. Therefore we think that the
T7 film may show a higher light reflectance in visible range
than that of T3 film.
3.4. Photocatalysis of film
Fig. 10. Absorbance at 460 nm in UV-vis spectra of aqueous methyl orange
solution decomposited by the (TiO2/TALH)30 thin film as a function of UV
irradiation time.ilms 499 (2006) 8389The absorbance changes of methyl orange solution by the
anatase TiO2 thin film (T3) were measured. The absorbance
of methyl orange solution at 460 nm as a function of UV
irradiation time was shown in Fig. 10. The absorbance of
methyl orange in UV-vis spectra was gradually decreased
from ca. 0.948 according to the increase of irradiation time
because methyl orange molecules were decomposed by
anatase TiO2 with UV irradiation. After 3 h, the decom-
position rate of methyl orange was slightly decreased since
the concentration of methyl orange remained was gradually
decreased. The film irradiated for 5.5 h still showed the
reproducible photocatalytic performance in new methyl
orange solution.
4. Conclusions
(TiO2/TALH)30 multilayer thin films consisted of TiO2nanoparticles and TALH were successfully fabricated via
LBL-SA method with an advanced growth in thickness ( ca.
-
275 nm) by adjusting the pH and the immersion time of
TALH solution. The in situ assembly of TALH that shows
the phenomenon to be saturated and separated before and
after 30 s was clearly monitored by a QCM. As the pH of
TALH was decreased, the thickness of films was increased.
Finally, by using TiO2 colloidal solution and TALH adjusted
to pH 2.5 with the immersion of 30 s into TALH, we
fabricated an anatase TiO2 thin film that has a lower RMS
roughness (ca. 10.5 nm), a higher refractive index (ca. 1.75)
than that of the film composed of TiO2 nanoparticles and
PPA. In addition, this film showed a high transmittance in
visible range for optical applications as well as good
photocatalytic performances to decompose the methyl
orange molecules with UV light irradiation.
Acknowledgements
This work was partially supported by Grant-in-Aid for
the 21st Century COE program KEIO Life Conjugate
Chemistry from the Ministry of Education, Culture, Sports,
6382.
[5] A.L. Linsebigler, L. Guangquan, J.T. Yates Jr., Chem. Rev. 95 (1995)
735.
[6] Y. Lin, A. Wang, R. Claus, J. Phys. Chem., B 101 (1997) 1385.
[7] K. Yeng, Y. Lam, Thin Solid Films 109 (1983) 169.
[8] Y. Kikuchi, K. Sunada, T. Iyoda, K. Hashimoto, A. Fujishima, J.
Photochem. Photobiol., A Chem. 106 (1997) 51.
[9] C.J. Taylor, D.C. Gilmer, D.G. Colombo, G.D. Wilk, S.A. Campbell,
J. Robert, W.L. Gladfelter, J. Am. Chem. Soc. 121 (1991) 5220.
[10] Y. Saito, S. Kambe, T. Kitamura, Y. Wada, S. Yanagida, Sol. Energy
Mater. Sol. Cells 83 (2004) 1.
[11] P. Chrysicopoulou, D. Davazoglou, Chr. Trapalis, G. Kordas, Thin
Solid Films 323 (1998) 188.
[12] M. Takeuchi, T. Itoh, H. Nagasaka, Thin Solid Films 51 (1978) 83.
[13] K.S. Yeung, Y.W. Lam, Thin Solid Films 109 (1983) 169.
[14] G. Decher, J.D. Hong, J. Schmitt, Thin Solid Films 831 (1992) 210.
[15] G. Decher, Science 277 (1997) 1232.
[16] S. Shiratori, T. Ito, T. Yamada, Colloids Surf., A Physicochem. Eng.
Asp. 198 (2002) 415.
[17] M.R. Hoffmann, S.T. Martin, W. Choi, D.W. Bahnemann, Chem. Rev.
95 (1995) 69.
[18] T.H. Kim, B.H. Sohn, Appl. Surf. Sci. 201 (2002) 109.
[19] S. Baskaran, L. Song, J. Liu, Y.I. Chen, G.L. Graff, J. Am. Ceram.
Soc. 81 (1998) 401.
[20] N. Kovtyukhova, P.J. Ollivier, S. Chizhik, A. Dubravin, E. Buzaneva,
A. Gorchinskiy, A. Marchenko, N. Smirnova, Thin Solid Films 337
(1999) 166.
[21] H. Mockel, M. Giersig, F. Willig, J. Mater. Chem. 9 (1999) 3051.
[22] J.H. Rouse, G.S. Ferguson, Adv. Mater. 14 (2002) 151.
J.-H. Kim et al. / Thin Solid Films 499 (2006) 8389 89References
[1] E.T. Fitzgibbons, K.J. Sladek, W.H. Hartwig, J. Electrochem. Soc. 119
(1972) 735.
[2] G.V. Samsonov, The Oxide Handbook, Plenum, New York, 1973.
[3] B. ORegan, M. Gratzel, Nature 353 (1991) 737.
[4] M.K. Nazeeruddin, A. Kay, I. Rodicio, R. Humphry-Baker, E. Muller,
P. Liska, N. Vlachopoulos, M. Gratzel, J. Am. Chem. Soc. 115 (1993)[23] X. Shi, T. Cassagneau, F. Caruso, Langmuir 18 (2002) 904.
[24] F. Caruso, X. Shi, R.A. Caruso, A. Susha, Adv. Mater. 13 (2001) 740.
[25] J.H. Kim, S.H. Kim, S. Shiratori, Sens. Actuators, B, Chem. 102
(2004) 241.
[26] B. Ding, J.H. Kim, Y. Miyazaki, S. Shiratori, Sens. Actuators, B,
Chem. 101 (2004) 373.
[27] G. Sauerbrey, Z. Phys. 155 (1955) 206.
[28] Y. Lvov, K. Ariga, M. Onda, I. Ichinose, T. Kunitake, Langmuir 13
(1997) 6195.Science, and Technology, Japan.
Fabrication and characterization of TiO2 thin film prepared by a layer-by-layer self-assembly methodIntroductionExperimental detailsMaterialsPreparation of thin filmsCharacterization of multilayer thin films
Results and discussionFrequency shift of QCMSurface morphology and thickness of filmsAbsorbance, transmittance, and refractive index of filmsPhotocatalysis of film
ConclusionsAcknowledgementsReferences