Cytochrome c-catalyzed oxidation of organic molecules by hydrogen peroxide.

Cytochrome c catalyzed the oxidation of various electron donors in the presence of hydrogen peroxide (H2O2), including 2-2'-azino-bis(3-ethylbenzthiazoline-6-sulfonic acid) (ABTS), 4-aminoantipyrine (4-AP), and luminol. With ferrocytochrome c, oxidation reactions were preceded by a lag phase corresponding to the H2O2-mediated oxidation of cytochrome c to the ferric state; no lag phase was observed with ferricytochrome c. However, brief preincubation of ferricytochrome c with H2O2 increased its catalytic activity prior to progressive inactivation and degradation. Superoxide (O2-) and hydroxyl radical (.OH) were not involved in this catalytic activity, since it was not sensitive to superoxide dismutase (SOD) or mannitol. Free iron released from the heme did not play a role in the oxidative reactions as concluded from the lack of effect of diethylenetriaminepentaacetic acid. Uric acid and tryptophan inhibited the oxidation of ABTS, stimulation of luminol chemiluminescence, and inactivation of cytochrome c. Our results are consistent with an initial activation of cytochrome c by H2O2 to a catalytically more active species in which a high oxidation state of an oxo-heme complex mediates the oxidative reactions. The lack of SOD effect on cytochrome c-catalyzed, H2O2-dependent luminol chemiluminescence supports a mechanism of chemiexcitation whereby a luminol endoperoxide is formed by direct reaction of H2O2 with an oxidized luminol molecule, either luminol radical or luminol diazoquinone.     

The enhancement of iron-dependent luminol peroxidation by 2,2′-Dipyridyl and nitrilotriacetate

The generation of radicals from luminol and H₂O₂, in the presence of iron and iron chelates was monitored by measuring the chemiluminescence produced by further oxidation of these radicals. 2,2′-Dipyridyl enhanced the production of chemiluminescence in the presence of FeSO₄, farritin and haemosiderin but not FeCI₃ or horseance of both FeSO₄ and FeCI₃ but not ferritin or haemosiderin. The enhancement of chemiluminescence by iron chelation may have analytical applications and the process by which these iron chelates are able to generate radicals from the nitrogenous base luminol may be similar to that responsible for their toxic effects on DNA.     

Anti-oxidant activity of spermine and spermidine re-evaluated with oxidizing systems involving iron and copper ions

This study was designed to investigate the direction of redox reactions of spermine and spermidine in the presence of iron and copper. The redox activity of spermine and spermidine was assessed using a variety of methods, including their ability to: (1) reduce Fe(3+) to Fe(2+) ions; (2) protect deoxyribose from oxidation by Fe(2+)-ethylene diaminetetraacetic acid, Fe(3+)-ethylene diaminetetraacetic acid systems with and without H(2)O(2); (3) protect DNA from damage caused by Cu(2+)-H(2)O(2), and Fe(2+)-H(2)O(2) with and without ascorbic acid; (4) inhibit H(2)O(2)-peroxidase-induced luminol dependent chemiluminescence; (5) scavenge diphenyl-picryl-hydrazyl radical. Spermine and spermidine at concentration 1mM reduced 1.8+/-0.3 and 2.5+/-0.1 nmol of Fe(3+) ions during 20 min incubation. Both polyamines enhanced deoxyribose oxidation. The highest enhancement of 7.6-fold in deoxyribose degradation was found for combination of spermine with Fe(3+)-ethylene diaminetetraacetic acid. An 10mM spermine and spermidine decreased CuSO(4)-H(2)O(2)-ascorbic acid- and FeSO(4)-H(2)O(2)-ascorbic-induced DNA damage by 73+/-6, 69+/-4% and 90+/-5, 53+/-4%, respectively. They did not protect DNA from CuSO(4)-H(2)O(2) and FeSO(4)-H(2)O(2). Spermine apparently increased the CuSO(4)-H(2)O(2)-dependent injury to DNA. Polyamines attenuated H(2)O(2)-peroxidase-induced luminol dependent chemiluminescence. Total light emission from specimens containing 10mM spermine or spermidine was attenuated by 85.3+/-1.5 and 87+/-3.6%. During 20 min incubation 1mM spermine or spermidine decomposed 8.1+/-1.4 and 9.2+/-1.8% of diphenyl-picryl-hydrazyl radical. These results demonstrate that polyamines of well known anti-oxidant properties may act as pro-oxidants and enhance oxidative damage to DNA components in the presence of free iron ions and H(2)O(2).     

The consequences of hydroxyl radical formation on the stoichiometry and kinetics of ferrous iron oxidation by human apoferritin

Despite previous detection of hydroxyl radical formation during iron deposition into ferritin, no reports exist in the literature concerning how it might affect ferritin function. In the present study, hydroxyl radical formation during Fe(II) oxidation by apoferritin was found to be contingent on the "ferroxidase" activity (i.e., H subunit composition) exhibited by apoferritin. Hydroxyl radical formation was found to affect both the stoichiometry and kinetics of Fe(II) oxidation by apoferritin. The stoichiometry of Fe(II) oxidation by apoferritin in an unbuffered solution of 50 mM NaCl, pH 7.0, was approximately 3.1 Fe(II)/O(2) at all iron-to-protein ratios tested. The addition of HEPES as an alternate reactant for the hydroxyl radical resulted in a stoichiometry of about 2 Fe(II)/O(2) at all iron-to-protein ratios. HEPES functioned to protect apoferritin from oxidative modification, for its omission from reaction mixtures containing Fe(II) and apoferritin resulted in alterations to the ferritin consistent with oxidative damage. The kinetic parameters for the reaction of recombinant human H apoferritin with Fe(II) in HEPES buffer (100 mM) were: K(m) = 60 microM, k(cat) = 10 s(-1), and k(cat)/K(m) = 1.7 x 10(5) M(-1) x (-1). Collectively, these results contradict the "crystal growth model" for iron deposition into ferritin and, while our data would seem to imply that the ferroxidase activity of ferritin is adequate in facilitating Fe(II) oxidation at all stages of iron deposition into ferritin, it is important to note that these data were obtained in vitro using nonphysiologic conditions. The possibility that these findings may have physiological significance is discussed.     

Iron(II) and hydrogen peroxide detoxification by human H-chain ferritin. An EPR spin-trapping study

Overexpression of human H-chain ferritin (HuHF) is known to impart a degree of protection to cells against oxidative stress and the associated damage to DNA and other cellular components. However, whether this protective activity resides in the protein's ability to inhibit Fenton chemistry as found for Dps proteins has never been established. Such inhibition does not occur with the related mitochondrial ferritin which displays much of the same iron chemistry as HuHF, including an Fe(II)/H(2)O(2) oxidation stoichiometry of approximately 2:1. In the present study, the ability of HuHF to attenuate hydroxyl radical production by the Fenton reaction (Fe(2+) + H(2)O(2) --> Fe(3+) + OH(-) + *OH) was examined by electron paramagnetic resonance (EPR) spin-trapping methods. The data demonstrate that the presence of wild-type HuHF during Fe(2+) oxidation by H(2)O(2) greatly decreases the amount of .OH radical produced from Fenton chemistry whereas the ferroxidase site mutant 222 (H62K + H65G) and human L-chain ferritin (HuLF) lack this activity. HuHF catalyzes the pairwise oxidation of Fe(2+) by the detoxification reaction [2Fe(2+) + H(2)O(2) + 2H(2)O --> 2Fe(O)OH(core) + 4H(+)] that occurs at the ferroxidase site of the protein, thereby preventing the production of hydroxyl radical. The small amount of *OH radical that is produced in the presence of ferritin (相似文献   

Permeation of phospholipid membranes by peroxynitrite

Quantitative kinetic models have been developed for the reaction between peroxynitrite and membrane lipids in vesicles and for transmembrane oxidation of reactants located within their inner aqueous cores. The models were used to analyze TBARS formation and oxidation of entrapped Fe(CN)(6)(4)(-) ion in egg lecithin liposomes and several artificial vesicles. The analyses indicate that permeation of the bilayers by ONOOH and NO(2)(*), a radical formed by homolysis of the ONOOH bond, is unusually rapid but that permeation by ONOO(-) and CO(3)(*)(-), a radical formed when CO(2) is present, is negligible. Bicarbonate protects the vesicles against both membrane and Fe(CN)(6)(4)(-) oxidation by rapid competitive CO(2)-catalyzed isomerization of ONOOH to NO(3)(-); this effect is partially reversed by addition of nitrite ion, which reacts with CO(3)(*)(-) to generate additional NO(2)(*). Under medium conditions mimicking the physiological milieu, a significant fraction of the oxidants escape to inflict damage upon the vesicular assemblies. Rate constants for several elementary reaction steps, including transmembrane diffusion rates for ONOOH and NO(2)(*), were estimated from the bicarbonate dependence of the oxidative reactions.     

Chemiluminescence determination of pharmacologically active compounds by capillary electrophoresis.

A simple and rapid capillary electrophoresis with direct chemiluminescence method has been developed for the determination of five natural pharmacologically active compounds including rutin, protocatechuic aldehyde, chlorogenic acid, luteolin and protocatechuic acid. The luminol as a component of the separation electrolyte buffer was introduced at the head of the separation capillary. The separation of five compounds was carried out in a fused-silica capillary with 15.0 mmol/L tetraborate, 1.0 mmol/L SDS and 0.42 mmol/L luminol (pH 8.5). The analytes was determined by enhancing the chemiluminescence of luminol with 0.13 mmol/L K3Fe(CN)6 in 0.05 mol/L NaOH, which was introduced at the post-column stage. The voltage applied was 16 kV. Under the optimum conditions, the analytes were separated within 10 min. The excellent linearity was obtained over two to three orders of magnitude with a detection limit (signal:noise = 3) of 0.012-0.055 micromol/L for all five analytes. The method was successfully used in the analysis of pharmaceutical and biological samples, and the assay results were satisfactory.     

Effects of dietary factors on iron uptake from ferritin by Caco-2 cells

Biofortification of staple foods with iron (Fe) in the form of ferritin (Ft) is now possible, both by conventional plant breeding methods and transgenic approaches. Ft-Fe from plants and animals is absorbed well (25-30%) by human subjects, but little is known about dietary factors affecting its absorption. We used human intestinal Caco-2 cells and compared Fe absorption from animal Ft and FeSO4 to determine the effects of inhibitors and enhancers, such as phytic acid, ascorbic acid, tannic acid, calcium and heme. When postconfluent cells were coincubated with 59Fe-labeled (1 microM) FeSO4 and dietary factors, at different molar ratios of dietary factor to Fe (phytic acid:Fe, 10:1; ascorbic acid:Fe, 50:1; tannic acid:Fe, 50:1; calcium:Fe, 10:1 and hemin:Fe, 10:1), all inhibited uptake from FeSO4, except ascorbate, confirming earlier studies. In contrast, these dietary factors had little or no effect on Fe uptake from undigested Ft or Ft digested in vitro at pH 4, except tannins. However, results after in vitro digestion of Ft at pH 2 were similar to those obtained for FeSO4. These results suggest that Fe uptake occurs from both undigested as well as digested Ft but, possibly, via different mechanisms. The Fe-Ft stability shown here could minimize Fe-induced oxidation of Fe-supplemented food products.     

Effects of Ceruloplasmin on Superoxide-Dependent Iron Release from Ferritin and Lipid Peroxidation

Ceruloplasmin (CP) effectively inhibited superoxide and ferritin-dependent peroxidation of phospholipid liposomes, using xanthine oxidase or gamma irradiation of water as sources of superoxide. In addition, CP inhibited superoxide-dependent mobilization of iron from ferritin. suggesting that CP inhibited lipid peroxidation by decreasing the availability of iron from ferritin. CP also exhibited some superoxide scavenging activity as evidenced by its inhibition of superoxide-dependent cytochrome c reduction. However, superoxide scavenging by CP did not quantitatively account for its inhibitory effects on iron release. The effects of CP on iron-catalyzed lipid peroxidation in systems containing exogenously added ferrous iron was also investigated. CP exhibited prooxidant and antioxidant effects; CP stimulated at lower concentrations, reached a maximum. and inhibited at higher concentrations. However. the addition of apoferritin inhibited CP and Fe(II)-catalyzed lipid peroxidation at all concentrations of CP. In addition, CP catalyzed the incorporation of Fe(II) into apoferritin. Collectively these data suggest that CP inhibits superoxide and ferritin-dependent lipid peroxidation via its ability to incorporate reductively-mobilized iron into ferritin.     

Iron oxidation chemistry in ferritin. Increasing Fe/O2 stoichiometry during core formation

The origin of previously observed variations in stoichiometry of iron oxidation during the oxidative deposition of iron in ferritin has been poorly understood. Knowledge of the stoichiometry of Fe(II) oxidation by O2 is essential to establishing the mechanism of iron core formation. In the present work, the amount of Fe(II) oxidized was measured by M?ssbauer spectrometry and the O2 consumed by mass spectrometry. The number of protons produced in the reaction was measured by "pH stat" titration and hydrogen peroxide production by the effect of the enzyme catalase on the measured stoichiometry. For protein samples containing low levels of iron (24 Fe(II)/protein) the stoichiometry was found to be 1.95 +/- 0.18 Fe(II)/O2 with H2O2 being a product, viz. Equation 1. 2Fe2+ + O2 + 4H2O----2FeOOH + H2O2 + 4H+ (1) EPR spin trapping experiments showed no evidence of superoxide radical formation. The stoichiometry markedly increased with additional iron (240-960 Fe/protein), to a value of 4 Fe(II)/O2 as in Equation 2. 4Fe2+ + O2 + 6H2O----4FeOOH + 8H+ (2) As the iron core is progressively laid down, the mechanism of iron oxidation changes from a protein dominated process with H2O2 being the primary product of O2 reduction to a mineral surface dominated process where H2O is the primary product. These results emphasize the importance of the apoferritin shell in facilitating iron oxidation in the early stage of iron deposition prior to significant development of the polynuclear iron core.     

Detection of methyl parathion using immuno-chemiluminescence based image analysis using charge coupled device

A novel method based on immuno-chemiluminescence and image analysis using charge coupled device (CCD) for the qualitative detection of methyl parathion (MP) with high sensitivity (up to 10 ppt) is described. MP antibodies raised in poultry were used as a biological sensing element for the recognition of MP present in the sample. The immuno-reactor column was prepared by packing in a glass capillary column (150 microl capacity) MP antibodies immobilized on Sepharose CL-4B through periodate oxidation method. Chemiluminescence principle was used for the detection of the pesticide. Light images generated during the chemiluminescence reaction were captured by a CCD camera and further processed for image intensity, which was correlated with pesticide concentrations. K(3)Fe(CN)(6) was used as a light enhancer to obtain detectable light images. Different parameters including concentrations of K(3)Fe(CN)(6), luminol, urea H(2)O(2), antibody, addition sequence of reactants and incubation time to obtain best images were optimized. The results obtained by image analysis method showed very good correlation with that of competitive ELISA for methyl parathion detection. Competitive ELISA method was used as a reference to compare the results obtained by CCD imaging.     

DNA damage by 5-aminolevulinic and 4,5-dioxovaleric acids in the presence of ferritin

Cellular accumulation of 5-aminolevulinic acid (ALA), the first specific intermediate of heme biosynthesis, is correlated in liver biopsy samples of acute intermittent porphyria affected patients with an increase in the occurrence of hepatic cancers and the formation of ferritin deposits in hepatocytes. 5-Aminolevulinic acid is able to undergo enolization and to be subsequently oxidized in a reaction catalyzed by iron complexes yielding 4,5-dioxovaleric acid (DOVA). The released superoxide radical (O(*-)(2)) is involved in the formation of reactive hydroxyl radical ((*)OH) or related species arising from a Fenton-type reaction mediated by Fe(II) and Cu(I). This leads to DNA oxidation. The metal catalyzed oxidation of ALA may be exalted by the O(*-)(2) and enoyl radical-mediated release of Fe(II) ions from ferritin. We report here the potentiating effect of ferritin on the ALA-mediated cleavage of plasmid DNA and the enhancement of the formation of 8-oxo-7, 8-dihydro-2'-deoxyguanosine (8-oxodGuo). Plasmid pBR322 was incubated with ALA and varying amounts of purified ferritin. DNA damage was assessed by gel electrophoresis analysis of the open and the linear forms of the plasmid from the native supercoiled structure. Addition of either the DNA compacting polyamine spermidine or the metal chelator ethylenediaminetetraacetic acid (EDTA) inhibited the damage. It was also shown that ALA in the presence of ferritin is able to increase the oxidation of the guanine moiety of monomeric 2'-deoxyguanosine (dGuo) and calf thymus DNA (CTDNA) to form 8-oxodGuo as inferred from high performance liquid chromatography (HPLC) measurements using electrochemical detection. The formation of the adduct dGuo-DOVA was detected in CTDNA upon incubation with ALA and ferritin. In a subsequent investigation, the aldehyde DOVA was also able to induces strand breaks in pBR322 DNA.     

Acceptor side effects on the electron transfer at cryogenic temperatures in intact photosystem II

In intact PSII, both the secondary electron donor (Tyr(Z)) and side-path electron donors (Car/Chl(Z)/Cyt(b)(559)) can be oxidized by P(680)(+) at cryogenic temperatures. In this paper, the effects of acceptor side, especially the redox state of the non-heme iron, on the donor side electron transfer induced by visible light at cryogenic temperatures were studied by EPR spectroscopy. We found that the formation and decay of the S(1)Tyr(Z) EPR signal were independent of the treatment of K(3)Fe(CN)(6), whereas formation and decay of the Car(+)/Chl(Z)(+) EPR signal correlated with the reduction and recovery of the Fe(3+) EPR signal of the non-heme iron in K(3)Fe(CN)(6) pre-treated PSII, respectively. Based on the observed correlation between Car/Chl(Z) oxidation and Fe(3+) reduction, the oxidation of non-heme iron by K(3)Fe(CN)(6) at 0 degrees C was quantified, which showed that around 50-60% fractions of the reaction centers gave rise to the Fe(3+) EPR signal. In addition, we found that the presence of phenyl-p-benzoquinone significantly enhanced the yield of Tyr(Z) oxidation. These results indicate that the electron transfer at the donor side can be significantly modified by changes at the acceptor side, and indicate that two types of reaction centers are present in intact PSII, namely, one contains unoxidizable non-heme iron and another one contains oxidizable non-heme iron. Tyr(Z) oxidation and side-path reaction occur separately in these two types of reaction centers, instead of competition with each other in the same reaction centers. In addition, our results show that the non-heme iron has different properties in active and inactive PSII. The oxidation of non-heme iron by K(3)Fe(CN)(6) takes place only in inactive PSII, which implies that the Fe(3+) state is probably not the intermediate species for the turnover of quinone reduction.     

The interaction of Rubia cordifolia with iron redox status: a mechanistic aspect in free radical reactions.

The present publication investigates the antioxidant property and mechanistic aspect of alcoholic extract of R. cordifolia. The extract of R. cordifolia has shown significant inhibitory effect on FeSO4 induced lipid peroxidation. Study with iron redox status showed that R. cordifolia extract reduced or oxidixed; Fe3+ or Fe2+ respectively, in a dose dependent manner. Results with superoxide anion (O2-.) and hydroxyl radical (OH.), showed no radical scavenging activity. The alcoholic extract significantly maintains the reduced glutathione content both in time and dose dependent manner. It also reduced the rate of depletion of reduced glutathione (GSH) level in presence of ferrous sulphate (FeSO4) and cumene hydroperoxide (CHP). On the basis of these observations, it can be concluded that the antioxidant property of R. cordifolia is due to a direct interaction with iron.     

Effect of metal ions on HIF-1alpha and Fe homeostasis in human A549 cells

Several metals are carcinogenic but little is known about the mechanisms by which they cause cancer. A pathway that may contribute to metal ion induced carcinogenesis is by hypoxia signaling, which involves a disruption of cellular iron homeostasis by competition with iron transporters or iron-regulated enzymes. To examine the involvement of iron in the hypoxia signaling activity of these metal ions we investigated HIF-1alpha protein stabilization, IRP-1 activity, and ferritin protein levels in human lung carcinoma A459 cells exposed to various agents in serum- and iron-free salt-glucose medium (SGM) or in normal complete medium. We also studied the effects of excess exogenous iron on these responses induced by nickel ion exposure. Our results show the following: (1) SGM enhanced metals-induced HIF-1alpha stabilization and IRP-1 activation (e.g., nickel and cobalt ions). (2) If SGM was reconstituted with a slight excess level (25 microM of FeSO(4)) of iron, this enhancing ability was significantly decreased. (3) The effect of a high level of exogenous iron (500 microM of FeSO(4)) on metal-induced hypoxia and iron metabolism was highly dependent on the order of addition. If treatment with the Fe and metal ions was simultaneous (co-treatment), the effects of nickel ion exposure were overwhelmed, since the added Fe reversed HIF-1alpha stabilization, decreased IRP-1 activity, and increased ferritin level. Pre-treatment with iron was not able to reverse the responses caused by nickel ion exposure. These results imply that it is important to consider the available iron concentration and suitable exposure design when studying metal-induced hypoxia or metal-induced disruption of Fe homeostasis.     

Stoichiometry of Fe(II) oxidation during ceruloplasmin-catalyzed loading of ferritin.

Ceruloplasmin catalyzed the incorporation of iron into apoferritin with a stoichiometry of 3.8 Fe(II)/O2. This value remained the same when ferritin containing varying amounts of iron was used. Contrary to the "crystal growth" model for ferritin formation, no iron incorporation into holoferritin was observed in the absence of ceruloplasmin. Fe(II)/O2 ratios close to 2 were obtained for iron incorporation into apo- and holoferritin in Hepes buffer, in the absence of ceruloplasmin, indicating the formation of reduced oxygen species. Sequential loading of ferritin in this buffer resulted in increasing oxidation of the protein as measured by carbonyl formation. Sequential loading of ferritin using ceruloplasmin did not result in protein oxidation and a maximum of about 2300 atoms of iron were incorporated into rat liver ferritin. This corresponded to the maximum amount of iron found in rat liver ferritin in vivo after injection with iron. These results provide evidence for ceruloplasmin as an effective catalyst for the incorporation of iron into both apo- and holoferritin. The possibility that these findings may have physiological significance is discussed.     

Site of OH radical attack on dihydrouracil and some of its methyl derivatives

The site of attack of OH radicals on dihydrouracil and five of its methylated derivatives was determined by pulse radiolysis using N,N,N',N'-tetramethylphenylenediamine (TMPD) to detect oxidizing radicals and tetranitromethane (TNM) as well as K3Fe(CN)6 to detect reducing radicals. In the case of dihydrouracil OH radicals abstract preferentially an H atom at C(6) to give the 6-yl radical (greater than or equal to 90 per cent) which at pH approximately 6.5 reduces TNM and K3Fe(CN)6 at almost diffusion-controlled rates. Only a small fraction of OH radicals abstract the H atom at C(5) (less than or equal to 10 per cent). The resulting 5-yl radical oxidizes TMPD to TMPD+ at pH 7-8. With the methylated derivatives of dihydrouracil, OH radicals react less selectively, especially in the case of N(1)-methyl derivatives. This methyl group is activated to a similar degree as the methylene group at C(6). In 1-Medihydrouracil the yield of N(1)-CH2 radicals is about 29 per cent, which has been deduced from the yield of formaldehyde formed after oxidation of this radical by TNM at pH approximately 6.5 and the subsequent hydrolysis. Radicals at the other methyl substituents are generated to a lesser extent (less than or equal to 10 per cent) and are relatively unreactive towards oxidizing agents such as TNM and K3Fe(CN)6 as well as towards the reducing agent TMPD. Although methyl substitution opens new routes for OH attack the preferred site of H abstraction remains C(6) (greater than 60 per cent).     

The ferroxidase center is essential for ferritin iron loading in the presence of phosphate and minimizes side reactions that form Fe(III)-phosphate colloids

Ferritin iron loading was studied in the presence of physiological serum phosphate concentrations (1 mM), elevated serum concentrations (2–5 mM), and intracellular phosphate concentrations (10 mM). Experiments compared iron loading into homopolymers of H and L ferritin with horse spleen ferritin. Prior to studying the reactions with ferritin, a series of control reactions were performed to study the solution chemistry of Fe²⁺ and phosphate. In the absence of ferritin, phosphate catalyzed Fe²⁺ oxidation and formed soluble polymeric Fe(III)-phosphate complexes. The Fe(III)-phosphate complexes were characterized by electron microscopy and atomic force microscopy, which revealed spherical nanoparticles with diameters of 10–20 nm. The soluble Fe(III)-phosphate complexes also formed as competing reactions during iron loading into ferritin. Elemental analysis on ferritin samples separated from the Fe(III)-phosphate complexes showed that as the phosphate concentration increased, the iron loading into horse ferritin decreased. The composition of the mineral that does form inside horse ferritin has a higher iron/phosphate ratio (~1:1) than ferritin purified from tissue (~10:1). Phosphate significantly inhibited iron loading into L ferritin, due to the lack of the ferroxidase center in this homopolymer. Spectrophotometric assays of iron loading into H ferritin showed identical iron loading curves in the presence of phosphate, indicating that the ferroxidase center of H ferritin efficiently competes with phosphate for the binding and oxidation of Fe²⁺. Additional studies demonstrated that H ferritin ferroxidase activity could be used to oxidize Fe²⁺ and facilitate the transfer of the Fe³⁺ into apo transferrin in the presence of phosphate.     

Light generation with Fenton's reagent. Its relationship to granulocyte chemiluminescence.

A simple chemical system consisting of FeSO4 and H2O2 (Fenton's reagent) was shown to emit light (chemiluminescence). The addition of tryptophan to the reaction markedly enhanced light production. Very little chemiluminescence was observed when H2O2 was omitted from the reaction and when ferric, instead of ferrous, ions were used. Hydroxyl radical (OH.) and singlet oxygen (1 deltagO2) quenchers suppressed chemiluminescence of the FeSO4 + tryptophan + H2O2 system; and, deuterium oxide (2H2O) enhanced chemiluminescence of both FeSO4 reactions. These observations suggest that a radical chain reaction involving both OH. and 1 deltag O2 is responsible for the chemiluminescent reactions. Six iron-containing proteins, some of which are located within granulocytes, all emitted light in the presence of H2O2. Since iron and H2O2 are present in metabolically stimulated granulocytes, it is likely that chemiluminescent reactions similar to the ones demonstrated in this study account for part of the chemiluminescence of activated granulocytes.     

A possible role for the conserved trimer interface of ferritin in iron incorporation.

Ferritin is a large protein, highly conserved among higher eukaryotes, which reversibly stores iron as a mineral of hydrated ferric oxide. Twenty-four polypeptides assemble to form a hollow coat with the mineral inside. Multiple steps occur in iron core formation. First, Fe2+ enters the protein. Then, several alternate paths may be followed which include oxidation at site(s) on the protein, oxidation on the core surface, and mineralization. Sequence variations occur among ferritin subunits which are classified as H or L; Fe2+ oxidation at sites on the protein appears to be H-subunit-specific or protein-specific. Other steps of ferritin core formation are likely to involve conserved sites in ferritins. Since incorporation of Fe2+ into the protein must precede any of the other steps in core formation, it may involve sites conserved among the various ferritin proteins. In this study, accessibility of Fe2+ to 1,10-phenanthroline, previously shown to be inaccessible to Fe2+ inside ferritin, was used to measure Fe2+ incorporation in two different ferritins under various conditions. Horse spleen ferritin (L/H = 10-20:1) and sheep spleen ferritin (L/H = 1:1.6) were compared. The results showed that iron incorporation measured as inaccessibility of Fe2+ to 1,10-phenanthroline increased with pH. The effect was the same for both proteins, indicating that a step in iron core formation common among ferritins was being measured. Conserved sites previously proposed for different steps in ferritin core formation are at the interfaces of pairs and trios of subunits. Dinitrophenol cross-links, which modify pairs of subunits and affect iron oxidation, had no effect on Fe2+ incorporation.(ABSTRACT TRUNCATED AT 250 WORDS)