10.1002/chem.201902651
Chemistry - A European Journal
FULL PAPER
the experimentally observed reactivity has been found which is,
in our opinion, a strong argument to rule out this reaction pathway.
After an exhaustive computational investigation of the non-
radical pathways with no consistent reaction mechanism found,
we focused on radical mechanism(s). The simplest pathway
assumes homolytic cleavage of F2 into two F· atoms. The
experimental value of the F2 bond dissociation enthalpy in
vacuum is 36.9 kcal.mol–1 [39] at 298.15 K. Corresponding Gibbs
free energy in vacuum is 29.6 kcal.mol–1. We assume that the
value in acetonitrile would be similar since the computed
COSMO-RS solvation energy for the F2 molecule in acetonitrile is
+1.3 kcal.mol–1, whereas the F· solvation free energy has been
computed as +0.6 kcal.mol–1, thus pointing to the overall change
in solvation free energy for the F2 → 2 F· reaction close to 0
kcal.mol–1. F2 dissociation is then presumably the highest barrier
along the radical reaction pathway. The F· radical then attacks
the SF3 group to form radical C (Scheme 5) in a barrier-less
process. We postulate that it is the stability of C, calculated as Ar
SF3 + 1/2 F2 → Ar-SF4· (free) energy change, that determines the
overall kinetics of the reaction. The experimentally observed order
of reactivity (inferred from the yields and selectivities listed in
Table 2) is nicely reproduced for 5a (X=H) > 5q (X= CN) > 5o (X
= NO2). For the 5r and 5y (5y has not studied in this work, but
reported in the literature),[23] the agreement is worse. Calculations
predict that 5r should be less reactive than 5q and on the contrary,
5y almost as reactive as 5q. However, this does not seem to be
the case in experiments. At the moment, we do not have an
explanation for the computed discrepancy for 5y and 5r. The
propagation step (TS6) is then associated with negligible
activation energy of 0.1–0.6 kcal.mol–1 with respect to the radical
intermediate C, which translates into 8.2–9.1 kcal.mol–1 in
activation Gibbs free energy due to the entropic terms. No clear
correlation between the computed barriers and the experimentally
observed reactivity is seen for this step and we do not consider it
as the rate determining. The termination is expectedly barrier-less.
In analogy with the structure of the closed-shell 5 and of the
blocks, such as SF5-substituted benzonitrile or benzoic acid,
ortho-substituted aromatics with rather bulky groups (previously
considered to be unreactive), and bis(pentafluorosulfa-
nyl)benzenes were prepared using elemental fluorine in one step.
The hybrid batch-flow process was developed and in terms of
isolated yield and selectivity it compared favorably to the
traditional batch process. A detailed computational study using
various density functional and wave function methods revealed
the reaction mechanism of the final and decisive step of the
studied fluorinations: conversion of the ArSF3 into ArSF5.
Excluding three non-radical pathways we postulate that the
reaction proceeds via the radical mechanism after homolytic
cleavage of the F-F. The remaining (propagation, termination)
steps are (almost) barrier-less and the overall kinetics is,
according to the computed data, determined by the stability of the
ArSF4· species. Experimentally observed order of reactivities has
been reproduced for three compounds studied computationally
while questions arise concerning the systems with the fluor-
containing X group in ortho- position. It must be emphasized that
we see a lot of room for further computational modeling of other
potential reaction channels that might be accompanied by the
elaborate experimental identification of all side-products, and may
include kinetic modeling. However, such analysis is beyond the
scope of this study.
Acknowledgements
This work was supported by the Czech Academy of Sciences
(Research Plan RVO: 61388963), by the Initial Training Network,
FLUOR21, funded by the FP7 Marie Curie Actions of the
European Commission (FP7-PEOPLE-2013-ITN-607787) and by
the Czech Science Foundation (18-00215J). We would like to
thank Professor Josef Michl (IOCB Prague) and Professor
Graham Sandford (Durham University, UK) for allowing J.A. to
use their F2 facility.
+
ArSF4 intermediates, in the equilibrium structures of radicals C
(molecular geometries deposited in the SI), fluorine atoms prefer
four equatorial positions with respect to the main molecular axis.
This leads, in the case of 5o (and slightly in the case of 5r) to a
steric clash, which is resolved, in the case of 5o – by
deplanarization of the NO2 group which comes at the cost of ~5 8
kcal.mol–1. This is, in qualitative terms, an explanation of the
sluggish reactivity observed for the 5o experimentally. We
postulate, while admitting the absence of a tangible computational
(or experimental) proof, that the reaction of 5y (and perhaps also
5r) may not follow the above-postulated reaction mechanism and
the origin of the sluggish reactivity towards the ArSF5 products is
the different reaction channel that leads to other products.
Keywords: pentafluorosulfanyl • sulfur pentafluoride • radical
fluorination • elemental fluorine • mechanism
[1]
L. J. Sæthre, N. Berrah, J. D. Bozek, K. J. Børve, T. X. Carroll, E. Kukk,
G. L. Gard, R. Winter, T. D. Thomas, J. Am. Chem. Soc. 2001, 123,
10729–10737.
[2]
[3]
W. A. Sheppard, J. Am. Chem. Soc. 1962, 84, 3072–3076.
M. V. Westphal, B. T. Wolfstädter, J.-M. Plancher, J. Gatfield, E. M.
Carreira, ChemMedChem 2015, 10, 461–469.
[4]
C. Hansch, R. M. Muir, T. Fujita, P. P. Maloney, F. Geiger, M. Streich, J.
Am. Chem. Soc. 1963, 85, 2817–2824.
[5]
[6]
P. R. Savoie, J. T. Welch, Chem. Rev. 2015, 115, 1130–1190.
P. J. Crowley, G. Mitchell, R. Salmon, P. A. Worthington, Chimia 2004,
58, 138–142.
[7]
[8]
[9]
S. Altomonte, M. Zanda, J. Fluorine Chem. 2012, 143, 57–93.
W. A. Sheppard, J. Am. Chem. Soc. 1962, 84, 3064–3072.
R. D. Bowden, P. J. Comina, M. P. Greenhall, B. M. Kariuki, A. Loveday,
D. Philp, Tetrahedron 2000, 56, 3399–3408.
Conclusions
In conclusions, the scope of the direct fluorination of aromatic
disulfides and thiols for the preparation of SF5-benzenes was
investigated.
[10] P. Kirsch, M. Bremer, M. Heckmeier, K. Tarumi, Angew. Chem., Int. Ed.
1999, 38, 1989–1992.
Over
twenty
new
examples
of
[11] J. Wessel, G. Kleemann, K. Seppelt, Chem. Ber. 1983, 116, 2399–2407.
(pentafluorosulfanyl)benzenes ranging from simple building
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