Determination of the electron affinities of alpha- and beta-naphthyl radicals using the kinetic method with full entropy analysis. The C-H bond dissociation energies of naphthalene
Ha. Lardin et al., Determination of the electron affinities of alpha- and beta-naphthyl radicals using the kinetic method with full entropy analysis. The C-H bond dissociation energies of naphthalene, J MASS SPEC, 36(6), 2001, pp. 607-615
The C-H bond dissociation energies for naphthalene were determined using a
negative ion thermochemical cycle involving the gas-phase acidity (DeltaH(a
cid)) and electron affinity (EA) for both the alpha- and beta -positions. T
he gas-phase acidity of the naphthalene alpha- and beta -positions and the
EAs of the alpha- and beta -naphthyl radicals were measured in the gas phas
e in a flowing afterglow-triple quadrupole apparatus. A variation of the Co
oks kinetic method was used to measure the EAs of the naphthyl radicals by
collision-induced dissociation of the corresponding alpha- and beta -naphth
ylsulfinate adducts formed by reactions in the now tube portion of the inst
rument. Calibration references included both x and a radicals, and full ent
ropy analysis was performed over a series of calibration curves measured at
collision energies ranging from 3.5 to 8 eV (center-of-mass). The measured
EAs are 33.0 +/- 1.4 and 31.4 +/- 1.0 kcal mol(-1) (1 kcal = 4.184 kJ) for
the alpha- and beta -naphthyl radicals, respectively. The gas-phase acidit
ies for naphthalene were measured by the DePuy silane cleavage method, whic
h utilizes the relative abundances of aryldimethylsiloxides and trimethylsi
loxide that result from competitive cleavages from a proposed pentacoordina
te hydroxysiliconate intermediate. The measured acidities are 394.0 +/- 5.0
and 397.6 +/- 4.8 kcal mol(-1) for the alpha- and beta -positions, respect
ively. The C-H bond dissociation energies calculated from the thermochemica
l cycle are 113.4 +/- 5.2 and 115.4 +/- 4.9 kcal mol(-1) for the alpha- and
beta -positions, respectively. These energies are, to within experimental
error, indistinguishable and are approximately the same as the first bond d
issociation energy for benzene. Copyright (C) 2001 John Wiley & Sons, Ltd.