Table 2 Comparison of optical transitions measured and calculated
for the PhCOCl radical anion and the benzoyl radical (in parenth-
eses: oscillator strength; s \ shoulder, b \ broad band)
formed for a structure ““in vacuoÏÏ and that the position of the
absorption band of the anion is difficult to measure accu-
rately, because of the soluteÏs self-absorption. Additionally, the
observed red-shift of approximately 50 nm for the dissociation
reaction agrees well with the calculated shift of about 60 nm
(the calculations usually reproduce tendencies better than
absolute values).
The spectrum of the benzoyl radical measured in this work
compares well with the spectrum found (absorption peak at
370 nm) in laser Ñash photolysis experiments.1
j
(exp)/
j(calc)/
max
nm
Transient
nm
B300 (s)
B370 (b)
290(0.60)
370(0.13)
313(0.11)
353(0.34)
Air-saturated solutions of benzoyl chloride
In air-saturated electron-irradiated neat solutions oxygen
reacts with the primary anionic species [k(e
(2.5 ^ 0.2) ] 1010 dm3 mol~1 s~1, this work: decay of solvat-
ed electrons in neat THF followed at 700 nm with increasing
] O ) \
solv, THF
2
oxygen-sensitive (see later)] points to an ionic species, and (iii)
it shows a Ðrst-order decay with a rate constant independent
of the solute concentration, which is expected for the disso-
ciation reaction [cf. eqn. (3)]. The spectrum of the long-lived
component (Fig. 2, spectrum at 5 ls), which appears after the
decay of the radical anion, is attributed to benzoyl radicals
produced according to eqn. (3).
To support our assignment, semi-empirical quantum chemi-
cal calculations were performed (see Table 2). The calculations
give the strongest transition at 290 nm for the benzoyl chlo-
ride radical anion, and at 353 nm for the benzoyl radical.
Although these values di†er slightly from the experimental
values (330 and 380 nm), the result is satisfactory taking into
account that the quantum-chemical calculations are per-
O
concentration; k(CH CN~~ ] O )7 \ 1 ] 1011 dm3
2
3
2
mol~1 s~1] as well as with the solvent radicals. Long-lived
absorption (lifetime [0.5 ls) due to solvent peroxy radicals is
observed in air-saturated neat solutions only below 350 nm as
shown in Fig. 3 (L).
In solutions containing PhCOCl, the grow-in of a new tran-
sient with a pronounced peak around 400 nm (and a shoulder
below 330 nm) is observed (Fig. 3, left inset). Its formation rate
is a function of the oxygen concentration (Fig. 3, inset at 380
nm) and the corresponding rate constant was estimated from
the superimposed time proÐles at 380 nm as follows: (i) com-
paring di†erent spectral regions the underlying short-lived
absorbance observed in nitrogen-saturated solutions was
found to be una†ected by oxygen (cf. Fig. 3, inset at 310 nm)
and therefore its decay rate in nitrogen-saturated solutions
was used in the Ðtting procedure, (ii) the decay of the new
band proved to be independent of oxygen concentration and a
corresponding decay rate of 4 ] 105 s~1 was derived in
oxygen-saturated solutions, (iii) Ðnally, the formation rate at
each concentration was determined by Ðtting the sum of three
exponential functions with two Ðxed time constants to the
experimental curves. Taking an oxygen concentration of
2.1 ] 10~3 mol dm~3 for air-saturated THF,8 a bimolecular
rate constant of (1.6 ^ 0.3) ] 109 dm3 mol~1 s~1 was esti-
mated for this reaction. The new band is assigned to benzoyl-
peroxy radicals formed according to eqn. (5).
Fig. 3 Transient optical absorption spectra observed 0.5 ls after
electron pulse irradiation (100 Gy per pulse) of air-saturated THF
solutions. (L) Neat THF; (@) 0.1 mol dm~3 PhCOCl and (…, left
inset) spectrum of benzoylperoxy radical corrected for solvent peroxy
radicals. Right insets: time proÐles of the absorbance at 310 and 380
Carbon-centered peroxy radicals usually show unspeciÐc UV-
absorption, but absorption bands in the near-UV or even in
the visible region have been found to be characteristic of
vinylperoxy and phenylperoxy radicals.9 The origin of these
absorption bands is discussed in terms of possible overlap of
the odd electron with the p-system of the vinyl double bond
or of the phenyl ring. In the present case such an overlap is
possible with the p-system either of the C2O double bond or
of the phenyl ring.
nm for
a
0.5 mol dm~3 PhCOClÈTHF solution [bottom, N -
2
saturated; top, air-saturated; middle, N Èair 1 ] 1 (only for 380 nm)].
2
The decay of benzoylperoxy radicals in THF is nearly
pseudo-Ðrst-order (k \ 4 ] 105 s~1) and independent of
benzoyl chloride concentration and dose; therefore, we
assume hydroperoxide formation via hydrogen abstraction
from the solvent.
Similar results were found in time-resolved IR experiments,
following the formation and decay of benzoylperoxy radicals
after laser Ñash photolysis of 2-hydroxy-2-methyl-1-
phenylpropan-1-one (Darocure 1173)Èhexane solution (cf. Fig.
4).10 The decay of the benzoylperoxy radicals (cf. Fig. 4) shows
a half-life of approximately 2 ls, i.e. the rate of 3.5 ] 105 s~1
compares well with our measurements (k \ 4 ] 105 s~1).
Owing to the limited time resolution (approximately 50 ns, for
experimental details see e.g. ref. 11) the formation rate can
Fig. 4 Decay of benzoylperoxy radicals followed at 1820 cm~1 after
laser Ñash photolysis (355 nm, 30 mJ per pulse, 7 ns) of air-saturated
Darocure-1173Èhexane solution.10 The inset shows the formation of
the benzoylperoxy radical band and the concomitant decay of the
benzoyl radical band at 1830 cm~1.
Phys. Chem. Chem. Phys., 2000, 2, 1425È1430
1427