IR laser-induced process for chemical vapor deposition of polyselenocarbosilane films
-
Upload
magna-santos -
Category
Documents
-
view
212 -
download
0
Transcript of IR laser-induced process for chemical vapor deposition of polyselenocarbosilane films
IR laser-induced process for chemical vapor
deposition of polyselenocarbosilane films
Magna Santos a, Luis Dıaz a, Marketa Urbanova b, Dana Pokorna b,Zdenek Bastl c, Jan Subrt d, Josef Pola b,*
a Instituto de Estructura de la Materia, C.S.I.C., 28024 Madrid, Spainb Laboratory of Laser Chemistry, Institute of Chemical Process Fundamentals, A.S.C.R., 16502 Prague, Czech Republic
c J. Heyrovsky Institute of Physical Chemistry, A.S.C.R., 18223 Prague, Czech Republicd Institute of Inorganic Chemistry, A.S.C.R., 25068 Rez, Czech Republic
Received 24 June 2005; accepted 20 October 2005
Available online 28 December 2005
Abstract
TEA CO2 laser irradiation into gaseous mixtures of 1,3-disilacyclobutane (DSCB) and dimethyl selenide (DMS) results in infrared multiple
photon-induced, non-interacting homogeneous decompositions of both educts, one yielding silene (H2Si CH2) and the other elemental selenium
as major products. The reaction between polymerizing silene and agglomerizing Se leads to chemical vapor deposition of novel polyseleno-
carbosilane films which are unstable in atmosphere. The laser induced co-decomposition represents a new process in allowing (i) reaction between
thermally generated transient and element and (ii) chemical vapor deposition of the product of this reaction.
# 2005 Elsevier B.V. All rights reserved.
Keywords: Polyselenocarbosilane films; Selenium; Laser decomposition; 1,3-Disilacyclobutane; Dimethyl selenide
www.elsevier.com/locate/jaap
J. Anal. Appl. Pyrolysis 76 (2006) 178–185
1. Introduction
There is continuing interest in the production of heteroatom-
containing polycarbosilanes as polycarbosilazanes [1], poly-
oxacarbosilanes [2] and polyborocarbosiloxanes [3] which are
available through conventional solution chemistry and are
useful as precursors of ceramics, glasses, high temperature
supports, insulation and wear protection materials.
It was recently shown that IR or UV laser irradiation of some
volatile organosilicon compounds in the absence or presence of
heteroatom-containing compounds allows for chemical vapor
deposition of polycarbosilanes [4], polyoxacarbosilanes [5],
polyborocarbosiloxanes [6] and polythiacarbosilanes [7] and
can serve as a simple, one-step alternative to the conventional
solution-involved syntheses.
Polycarbosilanes [4], polyoxacarbosilanes [5e] and poly-
thiacarbosilanes [7] were produced through IR or UV laser
irradiation of silacyclobutane or 1,3-disilacyclobutane (DSCB,
c-Si2C2H8) and of its mixtures with heteroatom-containing
* Corresponding author. Tel.: +420 2 20390308; fax: +420 2 20920661.
E-mail address: [email protected] (J. Pola).
0165-2370/$ – see front matter # 2005 Elsevier B.V. All rights reserved.
doi:10.1016/j.jaap.2005.10.007
volatile compounds. In these instances, the IR or UV laser-
induced formation of intermediate silene allows gas-phase
chemistry dominated by polymerization of silene, or controlled
by a sequence of (i) silene intercepting heteroatom-containing
species (O2, CS2) and (ii) polymerization of the fragments from
the unstable adduct. These processes lead to gas-phase
deposition of the polycarbosilanes and polyheterocarbosilane
thin films of ultrafine powders (Scheme 1).
It is known that UV laser photolysis [8] or IR laser
thermolysis [9] of gaseous dimethyl selenide (DMS, (CH3)2Se)
occurs as extrusion of Se atoms and formation of Se
agglomerates (of which Se2 and Se5 dominate in the gas phase
[10]) and that it affords chemical vapor deposition of thin films
of elemental Se. Should such reaction occur simultaneously
with the decomposition of 1,3-disilacyclobutane into silene, it
lends possibility for Sen interception by silene and hence
chemical vapor deposition of the yet unknown polyseleno-
carbosilane. No reaction between the Sen and silene species
would, on the other hand, result in chemical vapor deposition of
nanosized Se particles embedded in polycarbosilanes.
Both phenomena – the formation of polyselenocarbosilane
and that of Se/polycarbosilanes nanocomposite – are of interest
due to potential applications of these materials and due to
M. Santos et al. / J. Anal. Appl. Pyrolysis 76 (2006) 178–185 179
Scheme 1.
elucidation of the reaction between silene and Sen. We note that
the silene interception of many reagents is well known [11], but
that of Se has not been yet attempted.
We now report that IR laser irradiation of gaseous mixtures
of DSCB and DMS induces decomposition of both compounds,
involves interception of elemental Se by transient silene and is
an efficient way for the production of novel polyselenocarbo-
silanes that are unstable in atmosphere.
2. Experimental
The experiments were carried out using two different TEA
CO2 lasers. The CO2 Plovdiv University and a Lumonics K-103
lasers operated on the P(14) line of the 0001 ! 1000 transition
(949.48 cm�1) with a repetition frequency of 1 Hz and
respective energy 1 and 2 J in a pulse. For the irradiation of
gaseous DSCB–DMS mixtures in 140 and 95 ml Pyrex
reactors, the laser beam was focused by NaCl lenses to
achieve incident fluences of 4 and 50 J cm�2 (f.l. 15 cm) and
200 J cm�2 (f.l. 10 cm). The 140 ml Pyrex reactor (total
pressure of both reactants 13–28 mbar) consisted of two
orthogonal positioned Pyrex tubes (both 3 cm in diameter, one
9 cm and the other 13 cm long) fitted with KBr windows and it
was equipped with a sleeve with a rubber septum and PTFE
valve connecting it to a vacuum manifold. The 95 ml Pyrex
reactor (total pressure of both reactants 10 mbar) was a Pyrex
tube (3 cm in diameter, 10 cm long) furnished with NaCl
windows and a stopcock.
The progress of the decomposition of both compounds
was monitored by periodically removing the reactor and
placing it in the cell compartment of an FTIR spectrometer
(a Nicolet Impact or Perkin-Elmer 1600 spectrometer) using
absorption band of DSCB at 650 cm�1 and that of DMS at
1431 cm�1, and also by gas chromatography (a Shimadzu 14 B
chromatograph) and gas chromatography–mass spectroscopy
(a Shimadzu QP 5050 mass spectrometer) both using 25 m long
PoraBOND capillary column, programmed (30–160 8C) tem-
perature and sampling by a gas-tight syringe. These analyses
were conducted several minutes after the irradiation has been
ceased. This allowed the fog formed upon the irradiation descend
to the reactor bottom. The chromatograph was equipped with
flame-ionization detector and connected with a Shimadzu CR-
8A Chromatopac data processor. Decomposition products were
identified through their mass spectra using the NIST library.
The solid films were deposited from the gas phase on KBr,
Al and Au-plated Fe substrates accommodated in the reactors
before the irradiation.
The FTIR spectra of the films deposited on the KBr
substrates were measured directly in the reactor after
evacuation of gaseous products. The samples on Al and Au-
coated Fe substrates were transferred for the X-ray photoelec-
tron spectra (XPS) and electron microscopy measurements
using a double and single glove-box (argon inert gas) technique.
(The sample was transferred under argon to a sealed vial and
from it under argon to the XP spectrometer, or transferred under
argon to a sealed vial and exposed to air for 25 s and introduced
to an electron microscope.)
The XP spectra were measured using ESCA 310 (Gamma-
data Scienta) electron spectrometer. The pressure of residual
gases in the analyzer chamber during measurements was in the
low 10�9 mbar range. The spectra of Si (2p), C (1s), O (1s) and
Se (3d) and the spectra of Se L3M45M45 Auger electrons were
recorded. The curve fitting of the spectra was accomplished
using a Gaussian–Lorentzian line-shape. The decomposition of
Se (3d) profiles was made subject to the constraints of the
constant 3d5/2–3d3/2 doublet separation (0.9 eV) [12] and the
constant intensity ratio (3d5/2/3d3/2 = 1.45). Quantification of
the surface concentrations of elements was accomplished by
correcting the photoelectron peak areas for their cross-sections
[13].
Raman spectra of the samples exposed to air were measured
on a Renishaw RM2000 confocal micro-Raman spectrometer.
The excitation source was an Ar+ laser (514 nm); laser power
on the sample was kept at 0.2 mW. The scattered radiation from
the surface was collected in backscattering (1808) geometry at a
resolution of 4 cm�1.
M. Santos et al. / J. Anal. Appl. Pyrolysis 76 (2006) 178–185180
Fig. 1. Infrared spectra of DSCB and DMS (optical path, 10 cm; Me2Se,
13.3 mbar; DSCB, 1.3 mbar).
Table 1
Laser-induced decompositiona of DSCB and DMS in DSCB–DMS mixtures at
total pressure 10 mbar
Initial mixture (mbar) Depletion (in mol%)
DMS DSCB DMS DSCB
10 0 55
0 10 82
9 1 25 39
8 2 54 64
7 3 65 68
6 4 51 57
5 5 52 75
3 7 57 74
a 30 pulses, f = 120 J cm�2.
SEM photographs were obtained using a Philips XL30 CP
scanning electron microscope equipped with an energy
dispersive analyzer of X-ray radiation Edax DX4.
DMS (purity better than 98%) was purchased from Aldrich
and DSCB (purity better than 99%) was prepared in the lab
according to the earlier reported procedure [14].
Fig. 2. Depletion of DSCB (&) and DMS (^) upon irradiation with fluence of 200
and (c) DSCB (2 mbar)–DMS (8 mbar).
3. Results and discussion
The IR bands of DSCB (d(SiH2) mode [15]) and DMS
(rCH3 mode [16]) (overlapping in the region of the CO2 laser
emission (Fig. 1) allow infrared multiple-photon excitation of
both compounds.
3.1. Features of the DSCB–DMS co-decomposition
The irradiation of the gaseous DSCB–DMS mixtures (both
1–21 mbar) results in the decomposition of both educts and the
formation of gaseous products and a whitish fog depositing on
the reactor surface as whitish or orange films. The relative
depletion of DSCB and DMS depends on the initial ratio of
these educts. The illustrative examples are given in Fig. 2 and
Table 1.
The activation energy of the DSCB decomposition
(230 kJ mole�1 [17]) and the mean Se–C bond dissociation
energy (�250 kJ mole�1 [18]) are very similar, but the ground
state optical absorption coefficients (in cm�1 mbar�1) at
944 cm�1 for DSCB (1.5 � 10�2) and DMS (6.8 � 10�4)
significantly differ. These features are in keeping with more
mJ cm�2 of (a) DSCB–DMS (each 5 mbar), (b) DSCB (8 mbar)–DMS (2 mbar)
M. Santos et al. / J. Anal. Appl. Pyrolysis 76 (2006) 178–185 181
Fig. 3. Typical GC/MS trace of gaseous products of laser-induced co-decom-
position of DSCB and DMS: (1) CH4, (2) C2H2, (3) C2H4, (4) C2H6, (5) H2Se,
(6) CH3SiH3, (7) C3H6, (8) C3H6, (9) (CH3)2SiH2, (10) C4H4, (11) CH3SeH,
(12) (CH3)3SiH, (13) C4H8, (14) DMS, (15) DSCB, (16) CH3SeC2H5 and (17)
CSe2.
feasible IR multiple photon decomposition of DSCB. The
relative depletions of DSCB and DMS observed in different
mixtures (Fig. 2 and Table 1) reveal, however, that the
decomposition progress of each educt is enhanced at its higher
partial pressure. In other words, depletion of both educts (in
mol%) reaches very similar values independent of fluence and
the educts ratio. This observation is compatible with a collision-
assisted energy transfer between DSCB and DMS molecules,
bringing both DMS and DSCB molecules to a thermal
equilibrium.
The total distribution of the gaseous products (Fig. 3) is little
affected with the decomposition progress and depends to a
small extent on the initial educts ratio (Table 2).
The major products (in relative mol%) are methane (�52–
57), ethane (�3–22) and ethene (�14–28) which are
accompanied with very small quantities of ethyne, higher
hydrocarbons (C3H4, C4H4, C3H6 and C3H8), methylsilanes
((CH3)nSiH4 – n, n = 1–3) and Se-containing compounds
(CH3SeH, CH3SeC2H5, H2Se and CSe2). Very importantly,
(i) the total yields of methylsilanes correspond to less than 3%
of the DSCB decomposed, (ii) the total yield of methane, ethane
Table 2
Distribution of gaseous products in TEA CO2 laser co-decomposition of DSCB an
Initial mixture
(mbar)
Incident fluence
(J cm�2) (pulse no.)
Decomposition
progress (mol%)
Volatile productsa (rel
CH4 C2H2 C2H4
DSCB (3) 4 DSCB (52)
DMS (11) (70) DMS (38) 55.5 0.6 16
DSCB (7) 4 DSCB (43)
DMS (21) (40) DMS (35) 56.9 0 14.3
DSCB (3) 50 DSCB (53)
DMS (11) (100) DMS (37) 55.4 0 17.6
DSCB (21) 4 DSCB (38)
DMS (7) (50) DMS (35) 55.1 4.8 21.4
DSCB (13) 25 DSCB (29)
DMS (13) (40) DMS (28) 52.2 0 27.6
DSCB (13) 2 DSCB (30)
DMS (13) (40) DMS (27) 53.6 2.4 20.5
a Trace products: C3H4, C4H4, H2Se and CSe2.
and ethene correspond to more than 95% of the DMS
decomposed and (iii) the yield of methyl selenide corresponds
to less than 3% of the DMS decomposed.
Such distribution of volatile products is in line with
practically non-interacting, homogeneous decompositions of
DSCB and DMS. The CO2 laser-induced decomposition of
DSCB is known [19] to yield minute amounts of methane,
ethene, ethyne, propene and methylsilanes and large amounts of
a solid polycarbosilanes. It was accounted for [19] as
dominated by the formation of silene and its dehydrogenative
polymerization (DSCB ! 2H2Si CH2, polymerization, loss of
H2 ! polycarbosilane). The CO2 laser-induced decomposition
of DMS [20] yielding ethane, methane and ethene (the main
products) along with elemental selenium (main product) and
polyselenoformaldehyde (minor product) was explained [20] as
extrusion of selenium (and transient selenoformaldehyde)
through radical paths. The observed methylethyl selenide not
only confirms the occurrence of the previously reported radical
steps [20], but also proves a transient CH3Se radical [21] and its
reaction with C2H4 (produced upon decomposition of the
reported selenoformaldehyde [20]).
It thus appears that the only significant interference between
both decompositions consists of reactions between the species
producing the solid deposit, i.e. those between silene and
elemental selenium (a main route) and between silene and
selenoformaldehyde (a minor route). It is shown below that this
view is proved by the identification of the solid deposits.
3.2. Properties of solid deposits
The SEM analysis (Fig. 4) reveals that the deposited films
show, regardless of the irradiation conditions and the educts
ratio, a fluffy morphology consisting of irregularly shaped
agglomerates. These features were also observed with the
deposits from IR laser decomposition of DSCB alone [19] and
are very different from the round-shape and oval particles of
elemental selenium deposited by IR laser-induced decomposi-
tion of DMS [20].
d DMS
ative mol%)
C2H6 CH3SiH3 C3H6 C3H8 (CH3)2SiH2 CH3SeH (CH3)3SiH
21.5 0.20 0.40 0.80 0.50 0.10 0.10
21 0.40 0.40 2.2 1.30 2.10 0.40
21.7 0 0.5 0.6 0.40 3.7 0
3.2 6.2 0.20 0.40 6.30 0.40 1.60
7.9 2.1 0.3 0.7 3.5 3.5 1.7
8.8 2.9 0.3 0.8 4.6 3.2 2.3
M. Santos et al. / J. Anal. Appl. Pyrolysis 76 (2006) 178–185182
Fig. 4. SEM images of solid deposit. Irradiation of (a, b) DSCB (21 mbar)–DMS (7 mbar) at 4 J cm�2, (c, d) DSCB (7 mbar)–DMS (21 mbar) at 50 J cm�2 and of (e,
f) DSCB–DMS (5 mbar each) at 200 J cm�2.
The XPS surface stoichiometry (of ca. 5 nm superficial
layers) calculated from intensities of photoemission lines
together with the bulk stoichiometry calculated from the EDX–
SEM analysis of several films deposited under different
conditions (Table 3) reveal similar compositions of these
films, i.e. similar amounts of Si and C, small amounts of Se and
significant contents of O. The incorporation of oxygen and the
small amounts of Se indicate that the films are extremely
sensitive to moisture and that they react with ubiquitous traces
of water directly in the reactor and/or with traces of atmosphere
upon transfer of the films from the reactor to the XP
spectrometer. The EDX-determined compositions of the films
exposed for 15 s and 1 h to atmosphere do not differ and they
Table 3
Core level binding energies (eV) and composition of some solid films deposited f
Initial mixture (mbar) Fluence (J cm�2) XPS analysis
DMS DSCB Stoichiometry
21 7 50 Si1.0 C1.04Se0.18O0.72
7 21 4 Si1.0 C0.86Se0.16O0.30
7 7 200 Si1.0 C0.87Se0.18O0.63
show lower content of Se and higher content of O. The reaction
of the films with traces of water is thus responsible for both
incorporation of O and a substantial removal of Se. The Se
observed by the EDX analysis corresponds to a form of Se not
reacting with water and is tentatively assigned to the elemental
form.
The high reactivity of the solid materials towards air
moisture was confirmed by the XP spectra (Table 3) and FTIR
spectra (Figs. 6 and 7) and also in additional experiments when
the films accumulated from several runs were exposed to air
and the volatile products formed were identified by GC and
GC–MS analysis [mass spectrum, m/z (relative intensity in
percent)] as H2Se [84 (13), 83 (6), 82 (86), 81 (31), 80 (100), 79
rom DSCB–DMS mixtures
EDX analysis
Si (2p) (eV)
(population, %)
Se (3d) (eV)
(population, %)
102.0 (74) 55.0 (44) Si1.0 C0.64Se0.03O1.39
103.5 (26) 56.1 (56)
102.0 (91) 55.1 (25) Si1.0 C1.05Se0.07O0.48
103.5 (9) 56.2 (75)
102.2 (74) 55.0 (22) Si1.0 C0.83Se0.09O1.46
103.6 (26) 56.1 (78)
M. Santos et al. / J. Anal. Appl. Pyrolysis 76 (2006) 178–185 183
Fig. 5. The fitted spectra of Se 3d spectra of the deposits obtained from
(a) DSCB (7 mbar)–DMS (21 mbar), (b) DSCB (21 mbar)–DMS (7 mbar)
and (c) DSCB–DMS (each 5 mbar) with corresponding fluence 50, 4 and
200 J cm�2.
Fig. 6. FTIR spectra of films deposited upon irradiation of (a) DSCB (7 mbar)–
DMS (21 mbar) ( f = 50 J cm�2) and (b) DSCB (21 mbar)–DMS (7 mbar)
( f = 4 J cm�2).
(28), 78 (50), 77 (16), 76 (15)] and CH3SeH [98 (17), 97 (8), 96
(100), 95 (51), 94 (65), 93 (77), 92 (41), 91 (33), 90 (15), 89 (9),
82 (9), 81 (19), 80 (52), 79 (9), 78 (28), 77 (12), 76 (11)]
compounds.
As to the XP spectra, that of Si 2p electrons is best fitted as
contributions of two components located at 102.2 and
103.5 eV which are, respectively, assignable [22,23]) to
RxSiOy (R Si, C; y = 2, 3) and SiO4 structures. The spectra
of Se 3d electrons are fitted as two components with Se 3d5/2peaks located at 55.0 � 0.2 and 56.1 � 0.2 eV. The Auger
parameter a (calculated as a sum of the binding energy of
Se 3d5/2 electrons and kinetic energy of corresponding Se
L3M45M45 (1G) Auger electrons amount to 1361.7 and
1360.2 eV. The values at 55 and 1361.7 eV correspond to
elemental selenium [24,25] and the values at 56.1 and
1360.2 eV are tentatively assigned to a polymer containing
Se–X (X = Si, C) bonds. The contributions of the Se 3d
electrons reveal that the elemental form is less abundant than
the Se in the Se–X bonds (Table 3 and Fig. 5) and that the
proportion of the Se–X form increases with increasing portion
of DSCB in the initial mixtures.
The presence of elemental selenium is also revealed by
Raman spectra measured after exposing the films to air, which
show a peak at 254 cm�1 (a-Se form, [26]) whose intensity is
more pronounced for deposits obtained from DSCB–DMS
mixtures with higher DMS content.
The FTIR spectra of the deposits show the typical pattern of
polycarbosilanes, and are very similar to those of the films
produced upon laser-induced decomposition of DSCB [19].
Those of the deposits obtained from the DSCB–DMS mixtures
rich in DSCB consist of strong bands at 780–845 cm�1, a weak
band at 1246–1250 cm�1, a medium band at 2127–2148 cm�1
and very weak bands between ca. 2860 and 2960 cm�1 which
are, in the given order, assignable [27] to n(Si–C) + r(CHx),
d(CHxSi), n(Si–H) and n(C–H) modes. The films deposited
from mixtures rich in DMS show also a band at 1048 cm�1 due
to n(SiOSi) mode and a very weak band at 615–625 cm�1, a
band at 953 cm�1 and a shoulder at 1262 cm�1 that are,
respectively, due to n(C–Se), r(CH3Se) and d(CH3Se) modes
[16]. The differences between the FTIR spectra obtained at the
different initial ratio of DMS and DSCB is illustrated in Fig. 6.
The selenium does not have active infrared modes and
stretching Si–Se modes [28] display themselves below
400 cm�1. The presence of the Si–Se bond is indirectly proved
by the shift of the n(Si–H) band which is located at 2148 cm�1
(deposits from DMS-rich mixtures) and 2127 cm�1 (deposits
from DSCB-rich mixtures). This change is compatible with
incorporation of electronegative Se (as Se–Si) inducing a shift
of the n(Si–H) band to higher wavenumbers [29]. Very high
sensitivity of the deposited films to atmosphere (illustrated on
Fig. 7) serves as another evidence for the formation of the Si–Se
bonds, since the enormous build-up of the n(SiOSi) absorption
band at 1070 cm�1 can only be explained by the well-known
[30] hydrolysis of the Si–Se bond to siloxane.
3.3. Gas-phase chemistry
The distribution of gaseous products strongly suggests that
homogeneous decompositions of DSCB and DMS take place
M. Santos et al. / J. Anal. Appl. Pyrolysis 76 (2006) 178–185184
Scheme 2.
Scheme 3.
rather independently and that the extents of reaction steps of
CH3 radical formed from DMS are virtually the same as during
the decomposition of DMS itself. The practical non-inter-
ference of both decompositions (Scheme 2) leads to the
deposition of solid materials that can be described as a blend of
elemental Se and a polymer containing Si–Se and C–Se bonds.
The polymer materials are mostly formed by reactions of the
dominating species (silene and Sen molecules). We assume that
the Sen (mostly Se2) is incorporated in polymerizing silene
via Se-nucleophilic attack initiated 2 + 2 cycloaddition
and cleavage of the adduct into transient silaneselone and
selenoformaldehyde. The latter species are very reactive
Fig. 7. FTIR spectra of the film after its deposition (a) and exposure to air (b).
Conditions: DMS (21 mbar)–DSCB (7 mbar) ( f = 25 or 50 J cm�2).
and undergo polymerization producing polyselenocarbosilane
films (Scheme 2). Other minor steps, i.e. reaction of Se2 with the
less stable isomer of silene, methylsilylene and 1,2-dimethylsi-
lene (the dimethylsilylene dimer), as well as insertion of Se into
the Si–Si and Si–H bonds, are also feasible [31–34].
We stress that the increasing proportion of DSCB in the initial
DSCB–DMS mixtures is beneficial for production of higher
amounts of silene and hence for more efficient Sen interception,
leading to the formation of higher relative amounts of
polyselenocarbosilane compared to elemental selenium.
3.4. Hydrolysis of films
The contact of the deposited films to atmosphere leading to
the formation of volatile hydrogen selenide and methyl
selenide and resulting in the development of the Si–O–Si
bonds in the FTIR spectra (Fig. 7) is accounted for by the
reaction of the Si–Se bonds with air moisture [30]. The
formation of the H2Se and CH3SeH is in line with the presence
of the Si–Se–Si and Si–Se–CH3 structures in the deposited
solid (Scheme 3).
4. Conclusion
The TEACO2 laser irradiation into gaseous mixtures of 1,3-
disilacyclobutane and dimethyl selenide induces independent
decomposition of both compounds and affords chemical vapor
deposition of solid films which are a blend of elemental
selenium and a polymer whose structure is assessed as
polyselenocarbosilane.
The formation of these polymers takes place as reaction(s)
between the species which are dominating products of each
decomposition. These are silene and Sen molecules.
The described process is an extension of previous laser
induced decomposition of silacycles (silacyclobutane and
M. Santos et al. / J. Anal. Appl. Pyrolysis 76 (2006) 178–185 185
1,3-disilacyclobutane) with molecular oxygen [5e] and
carbon disulfide [7] and represents a new thermolytic pro-
cess by allowing reaction between thermally generated
transient and element, each of them being produced from the
decomposition of different precursor.
Polyselenocarbosilane films are unstable in atmosphere and
are readily hydrolyzed into polycarbosiloxanes and hydrogen
selenide and methyl selenide.
The low content of elemental Se determined after the
exposure of the polyselenocarbosilane films to air by the EDX
analysis is consistent with high ability of silene to intercept Sen
species.
The laser-induced co-decomposition of DSCB and DMS
represents the novel way for formation of Si–Se bond and
allows the deposition of novel selenocarbosilane polymer.
Acknowledgement
The work was supported by the Ministry of Education,
Youth and Sports of the Czech Republic (grant ME 684) and by
Spanish DGI, MCyT (BQU2003-08531-C02-02).
References
[1] For example
(a) M. Birot, J.-P. Pillot, J. Dunogues, Chem. Rev. 95 (1995) 1443;
(b) M. Peuckert, T. Vaahs, M. Bruck, Adv. Mater. 2 (1990) 398;
(c) A. Soum in Silicon-Containing Polymers, Kluwer Academic Publish-
ers, Dodrecht, 2000. (Chapter 11 and references therein.)
(d) R. Riedel, G. Passing, H. Schonefelder, R.J. Brook, Nature 355 (1992)
714.
[2] For example
(a) A.M. Wilson, G. Zank, K. Eguchi, W. Xing, B. Yates, J.R. Dahn,
Chem. Mater. 9 (1997) 1601;
(b) G.D. Soraru, Q. Lin, L.V. Interrante, T. Apple, Chem.Mater. 10 (1998)
4047.
[3] (a) A. Kasgoz, M. Kuramata, Y. Abe, J. Mater. Sci. 34 (1999) 6137;
(b) G.D. Soraru, N. Dallabona, C. Gervais, F. Babonneau, Chem. Mater.
11 (1999) 910.
[4] For example
(a) J. Pola, Radiat. Phys. Chem. 49 (1997) 151, and references therein;
(a) J. Pola, Surf. Coat. Technol. 100–101 (1998) 408, and refs. therein.
[5] For example
(a) Y.E. Kortobi, J.B. Espinose la Caillerie, A.P. Legrand, X. Armand, N.
Herlin, M. Cauchetier, Chem. Mater. 9 (1997) 632;
(b) J. Pola, A. Ouchi, Z. Bastl, J. Subrt, M. Sakuragi, A. Galıkova, A.
Galık, Chem. Vap. Deposition 7 (2001) 19;
(c) J. Pola, A. Ouchi, K. Vacek, A. Galikova, V. Blechta, J. Bohacek, Solid
State Sci. 5 (2003) 1079;
(d) J. Pola, A. Galikova, A. Galik, V. Blechta, Z. Bastl, J. Subrt, A. Ouchi,
Chem. Mater. 14 (2002) 144;
(e) J. Pola, J. Vitek, Z. Bastl, J. Subrt, J. Organomet. Chem. 640 (2001) 170.
[6] J. Pola, N. Herlin-Boime, J. Brus, Z. Bastl, K. Vacek, J. Subrt, V. Vorlicek,
Solid State Sci. 7 (2005) 123.
[7] M. Urbanova, J. Pola, J. Organomet. Chem. 689 (2004) 2697.
[8] J. Pola, Z. Bastl, J. Subrt, A. Ouchi, Appl. Surf. Sci. 172 (2001) 220.
[9] D. Pokorna, M. Urbanova, Z. Bastl, J. Subrt, J. Pola, J. Anal. Appl. Pyrol.
71 (2004) 635.
[10] (a) V.V. Illarionov, L.M. Lapina, Dokl. Akad. Nauk SSSR 114 (1957)
1021;
V.V. Illarionov, L.M. Lapina, Chem. Abstr. 52 (1958) 3439f;
(b) R.F. Brebrick, J. Chem. Phys. 43 (1965) 3031;
(c) J. Berkowitz, W. Chupka, J. Chem. Phys. 48 (1968) 5743;
(d) R.F. Brebrick, J. Chem. Phys. 48 (1968) 5741.
[11] For example
G. Raabe, J. Michl, in: S. Patai, Z. Rappoport (Eds.), The Chemistry of
Organic Compounds, Wiley, Chichester, 1989 (Chapter 17).
[12] NIST X-ray Photoelectron Spectroscopy Database, version 2, U.S.
Department of Commerce, NIST, Gaithersburg, MD 20899, 1997.
[13] J.H. Scofield, J. Electron Spectrosc. Relat. Phenom. 8 (1976) 129.
[14] R.M. Irwin, J. Cooke, J. Laane, J. Am. Chem. Soc. 99 (1977) 3273.
[15] Infrared Structural Correlation Tables and Data Cards, Heyden & Son
Ltd., Spectrum House, London, Table 9, 1969.
[16] J.R. Allkins, P.J. Hendra, Spectrochim. Acta 22 (1966) 2075.
[17] N. Auner, I.M.T. Davidson, S. Ijadi-Maghsoodi, T. Lawrence, Organo-
metallics 5 (1986) 431.
[18] L. Batt, in: S. Patai, Z. Rappoport (Eds.), The Chemistry of Organic
Selenium and Tellurium Compounds, vol. 1, Wiley, Chichester, 1986.
[19] Z. Bastl, H. Burger, R. Fajgar, D. Pokorna, J. Pola, M. Senzlober, J. Subrt,
M. Urbanova, Appl. Organomet. Chem. 10 (1996) 83.
[20] D. Pokorna, M. Urbanova, Z. Bastl, J. Subrt, J. Pola, J. Anal. Appl. Pyrol.
71 (2004) 635.
[21] J.J. BelBruno, J. Spacek, E. Christophy, J. Phys. Chem. 95 (1991) 6928.
[22] C.D. Wagner, in: D. Briggs, M.P. Seah (Eds.), Practical Surface Analysis,
Auger and X-ray Photoelectron Spectroscopy, vol. 1, Wiley, Chichester,
1994, p. 595.
[23] M.R. Alexander, R.D. Short, F.R. Jones, M. Stollenwerk, J. Zabold, W.
Michaeli, J. Mater. Sci. 31 (1996) 1879.
[24] Z. Bastl, I. Spirovova, J. Horak, Solid State Ionics 95 (1997) 315.
[25] I. Ikemoto, K. Kikuchi, K. Yakuschi, H. Kuroda, Solid State Commun. 42
(1982) 257.
[26] G. Lucovsky, A. Mooradian, W. Taylor, G.B. Wright, R.C. Keezer, Solid
State Commun. 5 (1967) 113.
[27] Infrared Structural Correlation Tables and Data Cards, R.G.J. Miller, H.A.
Willis (Eds.), Heyden & Son Ltd., Spectrum House, London, Table 9,
1969.
[28] H. Burger, U. Goetze, W. Sawodny, Spectrochim. Acta A 24 (1968) 2003.
[29] S. Al-Dallal, S. Aljishi, M. Hammam, S.M. Al-Alawi, M. Stutzmann, S.
Jin, T. Muschik, R. Schwarz, J. Appl. Phys. 70 (1991) 4926.
[30] D.A. Armitage, in: G. Wilkinson, G.A. Stone, E.W. Abel (Eds.),
Comprehensive Organometallic Chemistry, vol. 2, Pergamon Press,
Oxford, 1982.
[31] R.P.K. Tan, G.R. Gillette, D.R. Powell, R. West, Organometallics 10
(1991) 546.
[32] B. Gehrhus, P.B. Hitchcock, M.F. Lappert, J. Heinicke, R. Boese, D.
Blaser, J. Organomet. Chem. 521 (1996) 211.
[33] R. West, D.J. De Young, K.J. Haller, J. Am. Chem. Soc. 107 (1985) 4942.
[34] U. Herzog, H. Borrmann, J. Organomet. Chem. 689 (2004) 564, and
references therein.