244
B. Schwartz et al. / Inorganica Chimica Acta 370 (2011) 243–246
blocks} were obtained by vapor diffusing diethyl ether into a
dichloromethane solution of (Et4N)[FeII(CN)2(CO)2(PPh3)I] and
(BzPPh3)Cl and allowing the solutions to stand over 2 weeks at
ꢀ20 °C in refrigerator. A piece of crystal was coated in grease
and mounted on a Siemens (Bruker) SMART CCD area detector
5. Kinetics measurements
The kinetics of the substitution reaction was studied in THF
solution by a quantitative infrared spectroscopic method. Concen-
trations of (Et4N)fac-[FeII(CN)2(CO)3I] were kept at 0.010–0.030 M
and concentrations of PPh3 were kept at 0.10–1.00 M. In each mea-
surement, the concentration of PPh3 was at least 10 times more
than the concentration of (Et4N)fac-[FeII(CN)2(CO)3I]. Reactions
were performed in 100 mL round bottom flasks immersed in a
temperature controlled water bath ( 0.1 °C) at five different tem-
peratures: 20.7, 25.0, 30.0, 35.0 and 40.0 °C. At each temperature,
experiments were carried out at least five times with different
PPh3 concentrations. Infrared spectra for each experiment were ta-
ken periodically. The substitution reaction was monitored by the
decreasing of the carbonyl peak (2098 cmꢀ1) over time. Isosbestic
points were observed in each experiment, indicating no significant
accumulation of an intermediate. Plots of Ln(Abst ꢀ Abs1) against
time were linear over 3–5 half-lives, indicating the substitution
reaction was under pseudo-first-order condition. The rate con-
stants kobs were obtained by the slope of these plots. Plots of kobs
against [PPh3] were linear and yielded an overall second-order rate
constant k at each temperature. Activation parameters were deter-
mined from linear plots of the Eyring equation k = (kBT/h)[ex-
instrument with Mo K
a radiation. The data were collected at
173 K with scans of 0.3° per frame, with 10 s per frame such
x
that 1271 frames were collected for a hemisphere of data. The
first 50 frames were recollected at the end of the data collection
to monitor for decay; no significant decay was detected. Data out
to 2h of 56.00° were used. Cell parameters were retrieved using
SMART software and refined using SAINT software on all ob-
served reflections between 2h of 3° and the upper thresholds
[4,5]. Data reduction was performed with the SAINT software,
which corrects for Lorentz polarization and decay. Absorption
corrections were applied using SADABS [6]. The space groups for
all of the compounds were assigned unambiguously by analysis
of symmetry and systematic absences determined by the pro-
gram XPREP [7]. The crystal parameters are listed in Table 1. The
structure was solved by the direct method with SHELXS-97 and
subsequently refined against all data in the 2h ranges by full
matrix least squares on F2 using SHELXL-97 [8]. All non-hydrogen
atoms were refined anisotropically. Hydrogen atoms were
attached at idealized positions on carbon or nitrogen atoms ex-
cept for the disordered dichloromethane molecule and were
checked for missing symmetry by the PLATON program. Disordered
solvent molecules (CH2Cl2 and diethyl ether) were removed using
SQUEEZE [9].
p(ꢀ
D D
H–/RT + S–/R)]. Standard deviations of rate constants were
estimated by using linear least-squares error analysis with uniform
weighting of data points.
6. Results and discussions
4. Other physical measurement
Synthesis of the product (Et4N)[FeII(CN)2(CO)2(PPh3)I] was per-
formed in acetonitrile solution with ca. 25% excess of PPh3 at 40 °C.
Quantitative IR experiment showed that the conversion to the
product is almost 100%; however, the isolated yield was 54%.
[FeII(CN)2(CO)2(PPh3)I]ꢀ did not react further with PPh3, as ob-
served in the kinetics study, 10- to 100-fold PPh3 did not cause fur-
ther reaction. IR spectra of the reaction mixture and the isolated
product were identical, suggesting no other isomers were formed
during substitution.
Infrared spectra were recorded by a Thermo Nicolet 380 spec-
trometer. A NaCl cell with 0.12 mm path length was used for all
the solution IR measurements. Absorption spectra were recorded
by a Varian Cary 50 spectrophotometer at 200–800 nm range.
1H NMR and 31P NMR spectra were recorded by
Mercury400 MHz spectrometer.
a Varian
Crystal structure of [FeII(CN)2(CO)2(PPh3)I]ꢀ was established by
Table 1
its BzPPh3þ salt. (BzPPh3)[FeII(CN)2(CO)2(PPh3)I] was crystallized in
Crystal data and structure refinement for (BzPPh3)[FeII(CN)2(CO)2(PPh3)I].
ꢀ
a triclinic cell P1. The product anion has an octahedral geometry.
Empirical formula
Formula weight
Temperature (K)
Wavelength (Å)
Crystal system
Space group
Unit cell dimensions
a (Å)
C47H37FeIN2O2P2
906.48
173(2)
0.71073
triclinic
There are four diatomic ligands in the equatorial plane which are
assigned as two cis-cyanide and two cis-carbonyl ligands. The
distinctive difference between the Fe–CN and Fe–CO bond dis-
tances confirms our assignments [3,10–12]. PPh3 and iodide
ꢀ
P1
12.233(5)
13.154(5)
16.251(7)
75.820(7)
71.492(7)
74.862(7)
2356.0(17)
2
1.278
1.079
916
0.35 ꢁ 0.30 ꢁ 0.20
1.93–28.00
29171
b (Å)
c (Å)
a
(°)
b (°)
c
(°)
V (Å3)
Z
DCalc. (mg/m3)
Absorption coefficient (mmꢀ1
F(0 0 0)
)
Crystal size (mm3)
Theta range for data collection (°)
Reflections collected
Independent reflections (Rint
Completeness to theta = 28.33°
Refinement method
)
11 167 (0.0881)
98.0%
Full-matrix least-squares on F2
11 167/16/484
Data/restraints/parameters
Goodness-of-fit (GOF) on F2
0.997
Final R indices [I > 2
R indices (all data)
Largest difference in peak and hole
r
(I)]
R1 = 0.0758, wR2 = 0.2243
R1 = 0.0976, wR2 = 0.2401
3.957 and ꢀ0.993 e Åꢀ3
Fig. 1. ORTEP drawing of [FeII(CN)2(CO)2(PPh3)I]ꢀ at 50% probability level. Hydrogen
atoms are removed for clarity.