M. Bonifacic et al., REACTION OF AQUACHROMIUM(II) IONS WITH 2,2'-BIPYRIMIDINE - A PULSE-RADIOLYSIS STUDY, Journal of the Chemical Society. Dalton transactions, (17), 1998, pp. 2879-2885
Chromium(Ir) ion was generated from Cr(NH3)(6)(3+) and hydrated electr
ons in the presence of 2,2'-bipyrimidine (bpm). The reaction of Cr(NH3
)(6)(3+) with e(-)(aq) has k = 4.9 x 10(10) dm(3) mol(-1) s(-1) at 25
degrees C. The Cr(NH3)(6)(2+) so produced loses all the ammonia ligand
s with k > 10(5) s(-1). A product complex with an absorption maximum a
t around 350 nm was formed in the reaction of chromium(II) ion and bpm
. In the presence of a moderate excess of bpm an equilibrium is establ
ished on the 0.1 ms timescale with K-app = k(f) [bpm]/k(b). Both the f
orward (k(f)) and back (k(b)) reactions are pH dependent in the range
3.5 to 8.6. At pH 3.5 and 8.6, k,has the values of 1.6 x 10(8) and 4.4
x 10(7) dm(3) mol(-1) s(-1) and k(b) of 4.3 x 10(4) and 3.2 x 10(3) s
(-1), respectively. The UV spectra of the reaction product(s) indicate
that the absorbing product contains chromium(III) and bipyrimidine ra
dical ligand. The first acid dissociation constant of chromium(II) ion
was determined as 1.4 x 10(-5) mol dm(-3). At pH less than or equal t
o 3.5, where all chromium species are predominantly in the aqua form,
the proposed reaction scheme is (H2O)(6)Cr2+ + bpm (k-1)reversible arr
ow(k1) (H2O)(5)Cr-II(bpm)(2+) (k-2)reversible arrow(k2) (H2O)(4)Cr-II(
bpm)(2+) (k-3)reversible arrow(k3) (H2O)(4)Cr-III(bpm(.-))(2+) where [
(H2O)(5)Cr-II(bpm)](2+) and [(H2O)(4)Cr-II(bpm)](2+) represent steady-
state intermediates present in stoichiometrically negligible concentra
tions. On the 0.1 ms timescale, [(H2O)(4)Cr-III(bpm(.-))](2+) is stabl
e but undergoes changes at longer times. The protonated bpm molecule,
H(+)bpm, is reduced by 1-hydroxy-1-methylethyl radicals, k = 5 x 10(9)
dm(3) mol(-1) s(-1), yielding a diprotonated bpm radical, H(2)bpm(.+)
. No reaction was observed between Cr(H2O)(6)(3+) and H(2)bpm(.+) in p
ulse radiolysis experiments, which places the rate constant for this r
eaction at <2 x 10(6) dm3 mol(-1) s(-1).