use of spin traps to measure the addition and fragmentation rate coefficients of small molecule...
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COMMUNICATION www.rsc.org/polymers | Polymer Chemistry
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Use of spin traps to measure the addition and fragmentation rate coefficientsof small molecule RAFT-adduct radicals†
Elena Chernikova,*a Vladimir Golubev,a Anatoly Filippov,a Ching Yeh Linb and Michelle L. Coote*b
Received 2nd August 2010, Accepted 16th August 2010
DOI: 10.1039/c0py00245c
Spin traps have been used to obtain the first direct experimental
determination of the addition (5 � 106 L mol�1 s�1), fragmentation
(8 � 10�3 s�1) and self-termination (6.5 � 102 L mol�1 s�1) rate
coefficients in RAFT polymerization using the interaction of a tert-
butyl radical with tert-butyl dithiobenzoate at ambient temperature
as a model reaction.
Since the invention of the addition fragmentation chain-transfer
(RAFT) polymerization process,1 there has been an ongoing debate
about the origin of retardation and inhibition effects in polymeriza-
tions mediated by cumyl dithiobenzoate and related dithiobenzoate
agents.2,3 On the one hand, a kinetic model that assumes that inter-
mediate radical cross- and self-termination reactions (IRT) occur
with diffusion-controlled rate coefficients, similar to those for the
bimolecular termination of conventional propagating polymer radi-
cals (i.e. <kt> < ca. 107–108 L mol�1 s�1), can be fitted successfully to
experimentally determined overall reaction rates and ESR-derived
radical concentrations.4 However, this so-called IRT model predicts
that significant concentrations of the IRT products should be
produced even under standard RAFT conditions and these are not
observable in significant quantities in the resulting polymer except
under forcing conditions.5 Furthermore, the fragmentation rate
coefficient (kfr¼ 104 s�1) and equilibrium constants (K¼ kad/kfr¼ 55
mol L�1, where kad is the rate coefficient for addition) that are
obtained under the IRT model are incompatible with those predicted
from quantum chemistry,6 with radical storage experiments,7 and
with the kinetics of thioketone mediated polymerization.8 Many of
these problems can be addressed if one instead assumes that IRT is
not kinetically significant under normal polymerization conditions
(i.e., <kt> < ca. 104 L mol�1 s�1). In this case, model fitting to
experimental kinetic data indicates that the intermediate radicals are
much more stable (K¼ 1.06� 107 L mol�1) and there is no significant
IRT product formation.6c,9 However, this so-called slow fragmenta-
tion model also predicts intermediate radical concentrations that are
completely incompatible with the available ESR data, measured for
polymerizing systems. Resolving these inconsistencies and finding the
correct kinetic model for RAFT polymerization would improve our
aLenin Hills, 1, bld. 3, Polymer Department, Faculty of Chemistry,Lomonosov Moscow State University, Moscow, 119991, Russia. E-mail:[email protected]; Fax: +7 495 9390174; Tel: +7 495 9395409bARC Centre of Excellence for Free-radical Chemistry and Biotechnology,Research School of Chemistry, Australian National University, Canberra,ACT 0200, Australia. E-mail: [email protected]; Fax: +61 2 61250750
† Electronic supplementary information (ESI) available: Additionalkinetic and computational data, and full descriptions of theexperimental and theoretical procedures. See DOI: 10.1039/c0py00245c
This journal is ª The Royal Society of Chemistry 2010
understanding of the process and assist in process optimization and
control.
Various proposals have been made to reconcile these conflicting
observations. Buback et al.10 have suggested that the absence of IRT
products could be explained if the IRT product reacts with another
propagating radical to form a terminated chain and re-form the
intermediate radical; however, direct evidence for the existence of this
reaction has yet to be provided. Moreover, such a revised IRT model
still predicts fragmentation rates and equilibrium constants that are
incompatible with the results from quantum chemistry, with radical
storage experiments and thioketone-mediated polymerization. In
a further alternative, Konkolewicz et al.11 recently suggested that all
incompatible observations might be reconciled by allowing for
a strongly chain length dependent version of the IRT model with
concomitant slow fragmentation; however, the physical basis for such
strong chain length effects has been questioned in the literature.3 This
is not to say that either of these proposals are incorrect, rather more
evidence is required, preferably based on direct experimental
measurements of model compounds.3
To date, experimental measurements of the individual rate
coefficients have taken place within the context of a polymerizing
system and have necessarily involved the fitting of some type of
assumed kinetic model to the experimental data. As illustrated
above, these kinetic assumptions can have a large influence on the
resulting estimated parameters. In that regard, the use of quantum
chemistry is particularly attractive as, unlike experiments, such
calculations depend only on the laws of quantum mechanics and
the numerical approximations that are introduced to solve the
resulting equations. However, since the accuracy of such calcula-
tions can vary considerably with the level of theory chosen, external
experimental benchmarking is important. Experimentally, one can
reduce the dependence on model-based assumptions by carrying
out experiments in situations where the kinetic effects of these
assumptions are minimal, or by studying the reactions in isolation,
usually on much simpler model compounds. A promising example
of the former approach is a laser flash photolysis technique recently
introduced by Buback et al. and used to measure the fragmentation
rate and equilibrium constants for S–S0-bis(methyl-2-propionate)-
trithiocarbonate mediated polymerization of butyl acrylate in
toluene at�30 �C.12 It is worth noting that results generated in this
study, which were shown to be insensitive to the assumed rate of
IRT termination, are in very good agreement with the quantum-
chemical calculations.13 However, this experimental technique has
not as yet been applied to the more controversial dithiobenzoate
mediated polymerizations as the dithiobenzoate chromophore
absorbs in the UV region and undergoes photo-induced decom-
position. To study these systems an alternative approach is
required.
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To this end, in the present work we use a spin trapping technique
based on electron spin resonance (ESR) spectrometry to study the
kinetics and mechanism of the elementary steps of RAFT polymeri-
zation. Spin traps are strong inhibitors of radical reactions; hence
they are useful when the need arises to examine processes involving
unstable radicals in a wide range of temperatures. Once added to the
reaction mixture, the spin trap starts to capture active radicals
forming relatively inactive radical species, i.e. spin adducts, which
have characteristic ESR-spectra. It is important to note in this context
that spin traps do not react with stable or relatively stable radicals.14
These spin adducts are stable enough to be observed by ESR-spec-
troscopy; by integration of each of these signals, one can measure the
concentrations of each species and thereby study the kinetics of the
process. At the same time, the spin traps themselves act as a constant
‘‘radical vacuum cleaner’’, mopping up the released radicals and
preventing side reactions, such as termination processes or re-addi-
tion of radicals to the RAFT agent. This implies that the reaction
scheme can be greatly simplified. Using the model compounds
employed herein – rather than a full polymerizing system – the rate
and equilibrium constants can thus be measured more directly, with
significantly reduced dependence on model-based assumptions than
the previous ESR studies.4,12
A key challenge to applying this approach to dithioester RAFT
agents is the need to avoid the problem of photo-induced decom-
position. To this end, in contrast to experiments described before,12 all
of the experiments were carried out at room temperature using a spin
trap, 2-methyl-2-nitrosopropane (MNP) that functions simulta-
neously as a visible-light photoinitiator.
When irradiated by visible light, MNP decomposes and forms an
active tert-butyl radical (Scheme 1, reaction 1); in solvents like
benzene the tert-butyl radical rapidly interacts with another MNP
species and forms the stable nitroxide radical di-tert-butylnitroxide
(DTBN), which has its own specific ESR-spectrum (reaction 2).
When a RAFT agent such as tert-butyl dithiobenzoate (TB) is added
to the system, the tert-butyl radical can interact with it (reaction 3). It
is important to note that the presence of RAFT agent does not
influence the MNP decomposition under visible light; the use of
visible light (instead of UV) also avoids the problems of RAFT agent
absorbance and – importantly – its decomposition.
Scheme 1 The reactions taking place upon irradiation of the MNP–TB–
benzene system at 20 �C.
1438 | Polym. Chem., 2010, 1, 1437–1440
The observed ESR-spectrum for the system TB–MNP–benzene at
20 �C is given in Fig. 1, and is evidently a result of the superposition
of the signals attributed to the spin adduct DTBN (triplet with AN¼15.1 G) and multiplet (g ¼ 2.0041 G, AdH
¼ 0.42 G, AoH ¼ 3.65 G,
AmH ¼ 1.34 G, ApH ¼ 3.99 G) corresponding to the intermediate
radical (Int) formed in reaction 3. We have observed analogous
spectra before upon irradiation of MNP in benzene solution and
upon heating TB with AIBN, benzene and styrene;15 examples are
provided in Fig. S1 and S2 of the ESI.† As both of the signals are very
intense, we can use them to evaluate the concentrations of the
respective radicals: for DTBN the end component of the spectrum
was used for integration; for Int the third component was used.14b
During irradiation, the DTBN and the Int concentrations both
increase as a result of the trapping of tert-butyl radicals by MNP and
TB, respectively. After the irradiation is switched off the DTBN
concentration increases, while the Int concentration slowly decreases
(Fig. 2). This is because the intermediate radical has a finite lifetime
and it decomposes releasing tert-butyl radicals (reverse of reaction 3),
which are subsequently trapped by MNP forming DTBN (reaction
2).
If the irradiation time is noticeably less than the intermediate
lifetime (e.g., in the present work the irradiation time is 5 s whilst
the intermediate decays over several hundred seconds), we can
separately consider the processes of intermediate accumulation and
consumption; for DTBN all side reactions (Scheme 2) may be also
excluded due to short period of irradiation. Thus, the ratio of the
DTBN to Int formed during irradiation provides a measure of the
relative rates of tert-butyl radical addition to MNP versus to TB: that
is, [DTBN]0/[Int]0 ¼ krT[MNP]0/kad[TB]0. In this equation, [DTBN]0and [Int]0 are obtained by the extrapolation of the kinetic curves up
to zero time, [MNP]0 and [TB]0 are preset, and krT ¼ 3.3 � 106 L
mol�1 s�1,16 and hence kad can be obtained. Over the range of TB
concentrations 10�2 – 10�1 mol L�1 and at [MNP]¼ 10�2 mol L�1 the
average value of rate coefficient of tert-butyl radical addition to TB
was found to be equal to (5 � 1)�106 L mol�1 s�1; a collation of kad
values obtained under various TB concentrations is provided in Table
S1 of the ESI.† These results are in good qualitative agreement with
both experimental4 and theoretical6d values reported in the literature
for the addition of oligomeric and polymeric radicals to various
RAFT agents.
Provided the only pathway affecting the concentration of the Int
after switch-off is the fragmentation reaction (i.e. reverse of reaction
3), its rate coefficient kfr can be measured directly from the slope of
the kinetic curves of intermediate consumption after switch-off, when
Fig. 1 An ESR-spectrum observed upon irradiation by visible light
(through red light filter RL-15 with l > 650 nm) of the TB–MNP–benzene
system at 20 �C.
This journal is ª The Royal Society of Chemistry 2010
Fig. 2 Kinetic curves of accumulation and consumption of intermediate
radical Int (1) and DTBN (2) in the system TB–MNP–benzene after
switch-off of MNP photolysis: [TB] � 102 ¼ 1 (a) and 9 (b) and [MNP] ¼10�2 mol L�1 at 20 �C. Curves for other concentrations and full experi-
mental details are provided in the ESI†.
Scheme 2 The reactions taking place after switch-off irradiation of the
MNP–TB–benzene system at 20 �C.
Fig. 3 Semi-logarithmic plot of the kinetic curves 1 presented in Fig. 2a
and 2b, [TB] � 102 ¼ 1 mol L�1 (1) and 9 mol L�1 (2).
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plotted in semi-logarithmic form (Fig. 3): kfr ¼ (5 � 1)�10�3 s�1.
However, for this to be a valid direct measure of this rate coefficient,
it is important to consider the likelihood and effect of any additional
side reactions that might affect the Int concentration during switch
off. These possible reactions include re-addition of the tert-butyl
radical to the RAFT (reaction 3), and various possible termination
reactions (see Scheme 2, reactions 4, 6, 8 and 9).
The addition reaction (3) would contribute to an increase in the
intermediate concentration and cause the decay to occur over a
This journal is ª The Royal Society of Chemistry 2010
longer time period, leading us to underestimate the decay rate.
However, the experimental design of our current study largely
excludes the re-addition of tert-butyl radicals to TB, as the released
radicals are immediately trapped by the high spin trap concentration.
This is one of the key differences between the current case and the
earlier laser flash photolysis experiments of RAFT polymerization; in
the latter experiment there is no spin trap present and thus the released
radical can undergo re-addition, along with other reactions such as
propagation, termination, transfer, etc. However, for the sake of
rigor, we can take the addition reaction into account explicitly using
the correction factor p ¼ Rad/(RrT + Rad) ¼ kad[TB]/(krT[MNP] +
kad[TB]), where RrT and Rad are the rates of tert-butyl radical
addition to MNP and TB, correspondingly. For [TB] ¼ [MNP] ¼10�2 mol L�1 the p value is 0.6; i.e. the real kfr is slightly higher: kfr¼kfr
exp/p ¼ (8 � 2)�10�3 s�1.
The various termination reactions are more difficult to rule out
completely but it is important to note that if any of these do occur,
they would contribute to a decrease in the intermediate concentration
and cause the decay to occur over a shorter time period than in their
absence. In other words, in this experimental set-up, if Int termination
processes are important, our fragmentation rate coefficient provides an
upperbound to the true value. In fact the linear dependence of Fig. 3
indicates that at the chosen conditions all side reactions (4, 6, 8, 9)
involving intermediate radical can be largely excluded, and are
unlikely to be affecting the results. However, there is evidence that
termination processes are occurring to a small extent, and this is now
examined in detail.
After switching off the irradiation, the intermediate radical very
slowly vanishes over a 10–15 min period depending on the MNP and
TB concentrations; simultaneously the DTBN concentration
increases (Fig. 2). This latter effect is due to the production of tert-
butyl radicals during intermediate fragmentation. Thus, MNP should
quantitatively register the intermediate fragmentation events. In this
case the number of additional DTBN adducts formed should be
equal to the number of intermediate radicals consumed; indeed, this is
observed when equal amounts of MNP and TB are present (Fig. 2a).
However, as the ratio of TB to MNP increases, one observes that
there is a greater loss of intermediate radicals than the corresponding
increase in DTBN concentration (Fig. 2b). This could either be as
a result of the additional consumption of Int by termination reactions
such as 6, 8 or 9 in Scheme 2, or the consumption of the DTBN itself
via by termination reactions 5 and 7. The remaining process in
Scheme 2, termination reaction 4, consumes both Int and DTBN and
does not affect their concentration ratio.
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The reactions of DTBN and Int with NO radicals (reactions 5 and
6) can be ruled out as they require NO to be produced in significant
quantities through the decomposition of MNP; this will only occur
over a long duration of irradiation and at high MNP concentrations.
The reaction of DTBN with tert-butyl radicals (reaction 7) is well
known, and when it plays a visible role the DTBN kinetic curve
reaches its saturation limit. However, we have designed our experi-
mental conditions so that this reaction can also be neglected due to
the low concentration of tert-butyl radicals compared with MNP and
TB. This was confirmed by showing in an independent experiment
that the DTBN concentration increased linearly with growth of
irradiation time, and hence reaction 7 was not consuming DTBN.
This leaves the termination of the Int via coupling either with tert-
butyl radical (reaction 8) or with itself (reaction 9). Whilst both
reactions are plausible from a chemical perspective, under the present
reaction conditions reaction 8 can also be excluded. Even if its rate
coefficient is assumed to be of a similar magnitude to the rate coef-
ficient of tert-butyl radical reaction with DTBN, TB and MNP (106–
107 L mol�1 s�1); as the intermediate concentration is 3–4 orders of
magnitude lower than that of MNP and TB, reaction 4 cannot
compete with reactions of tert-butyl radical with TB and MNP under
these conditions.
Thus, the only plausible pathway for the consumption of inter-
mediate radicals in these experiments is their self-termination (reaction
9). Since this reaction becomes more likely as the Int concentration
increases, we examine the system with highest concentration of TB
(Fig. 2b). It is obvious that the termination rate kt00 can be calculated
as the difference between the rate of intermediate radical consump-
tion and the rate of DTBN accumulation. This leads to eqn (10):
k00¼��
d½Int�=dt
d½DTBN�=dtþ 1
�kfrkrT ½MNP�
½Int�ðkrT ½MNP� þ kad ½TB�Þ (10)
From the measured concentrations (Fig. 2b) and the measured rate
coefficients, this is equal to (6.5 � 3.0) � 102 L mol�1 s�1.
Finally, having measured the addition and fragmentation rate
coefficients, and verified that other reactions are not substantially
affecting the results, we can obtain the first directly measured
experimental equilibrium constant K¼ kad/kfr for reaction (3) as (6�4)�108 L mol�1. This can then be compared with quantum-chemical
calculations on the same system under the same conditions (i.e. at
20 �C in benzene solution). To this end, we used the same method-
ology as in our recent study of S–S0-bis(methyl-2-propionate)-tri-
thiocarbonate mediated polymerization of methyl acrylate;13 full
computational details are provided in the ESI.† The equilibrium
constant we obtain for the present system is 4.5�108 L mol�1, which
is in excellent agreement with the experimental results. This result
therefore further reinforces the accuracy and applicability of our
quantum-chemical methodology for model RAFT reactions.
Conclusions
In conclusion, we have used an ESR-based spin trapping
technique to provide the first direct experimental measurements
for the rate coefficients of the addition and fragmentation reactions of
tert-butyl dithiobenzoate. The results indicate that the fragmentation
processes of dithiobenzoate derived intermediate RAFT radicals can
be relatively slow, in agreement with the original predictions of the so-
called slow fragmentation model.6,9 The equilibrium constant of (6�
1440 | Polym. Chem., 2010, 1, 1437–1440
4) � 108 L mol�1 at 20 �C in benzene is in excellent agreement with
the corresponding quantum-chemical calculations for the same
reaction 4.5 � 108 L mol�1, mutually verifying the accuracy of the
experimental and theoretical results. Our results also confirm that
intermediate self-termination can occur, albeit at a relatively low
reaction rate (kt0 0¼ (6.5� 3.0)� 102 L mol�1 s�1), at least for the low
molecular weight model compound studied.
Acknowledgements
MLC gratefully acknowledges financial support from the Australian
Research Council under their Centres of Excellence program and
generous allocations of supercomputing time on the National Facility
of the National Computational Infrastructure. EC gratefully
acknowledges financial support from the Russian Foundation for
Basic Research (project No 08-03-00269).
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