Abstract
Alkaline phosphatases play a crucial role in phosphate acquisition by microorganisms. To expand our understanding of catalysis by this class of enzymes we have determined the structure of the widely-occurring microbial alkaline phosphatase PhoX. The enzyme contains a complex active site cofactor comprising two antiferromagnetically-coupled Fe3+ ions, three Ca2+ ions, and a μ3-bridging oxo group. Notably, the main part of the cofactor resembles synthetic oxide-centered triangular metal complexes. Structures of PhoX-ligand complexes reveal how the active site metal ions bind substrate and implicate the cofactor oxo group in the catalytic mechanism. The presence of iron in PhoX raises the possibility that iron bioavailability limits microbial phosphate acquisition.
Phosphate-containing macromolecules and metabolites are essential components of living cells. Under conditions of phosphate deficiency microorganisms obtain phosphate from biologically-derived organic compounds by producing extra-cytoplasmic alkaline phosphatases (1, 2). Prominent amongst these enzymes are phosphate monoesterases of the PhoA and PhoX families which are found in all three domains of life. The archetypal PhoA enzyme of Escherichia coli has been extensively studied (2) but PhoX alkaline phosphatases are minimally characterized and do not exhibit sequence similarity to other phosphotransfer enzymes. Genes encoding PhoX are abundant in ocean bacteria (3-5) and are also present in bloom-forming cyanobacteria (6), human pathogens (7, 8), and eukaryotic green algae including the model organism Chlamydomonas reinhardtii (9).
To establish the active site architecture of PhoX we have undertaken structural analysis of the enzyme from Pseudomonas fluorescens Pf0-1 (10). Recombinant P. fluorescens PhoX is a phosphomonoesterase with no phosphodiesterase activity and is able to cleave phosphorus-nitrogen bonds but not phosphorus-carbon bonds (Fig. S1A). The purified PhoX protein is purple in color with several broad absorbance bands in the visible spectrum, indicating the presence of a prosthetic group (Fig. 1A). Addition of the non-hydrolysable substrate analogue adenosine-5′-(β,γ-methylene)triphosphate (AMP-PCP) causes changes in the visible spectrum (Fig. 1A) showing that the prosthetic group is associated with the substrate-binding site. We determined crystal structures for native PhoX and for PhoX in complex with AMP-PCP, phosphate, and the putative transition state mimic vanadate. All four structures were determined to high resolution (1.1-1.5 Å) from crystals grown at the catalytic pH optimum of 8 (Figs. S1B, S2A, S3, Tables S1, S2).
PhoX folds as a 6-bladed β-propeller (Fig. 2A). The active site of the enzyme lies at the bottom of the cavity at the center of the propeller and is accessible from only one face of the propeller through a channel (Fig. 2B). The active site in the native PhoX structure contains four metal ions, and a further metal ion is present in the structures of the three PhoX-ligand complexes. Proton-induced X-ray emission spectroscopy of a sample of the PhoX-phosphate complex detected 3.4±0.3 atoms of calcium and 1.6±0.1 atoms of iron per complex with no other candidate elements (Co, Ni, Zn, Mg, Mn) detectable. Individual metal ion sites in the PhoX structures were assigned as three Ca and two Fe ions on the basis of their coordination geometry and anomalous scattering at different wavelengths (Fig. S2B,C). All metal sites are fully occupied and the B factors for the Ca ions do not differ significantly from those for the Fe ions. The ions FeA, FeB, and CaA form a triangle at the bottom of the active site cavity (Figs. 2 and 3). Ions CaB and (in the ligand complexes only) CaC lie above the plane of the first three ions and to one side of the cavity, with the plane containing the three Ca ions being almost perpendicular to that of the FeAFeBCaA triangle. All five metal ions are co-ordinated by oxygen atoms provided either by the side chains of conserved residues, by water, or by the ligand molecules (Figs. 2C, S3, S4A,D,E, Table S3). FeA is additionally ligated by a thiolate side chain from invariant Cys179. Substitution of individual amino acids co-ordinating FeA, FeB, CaB, or CaC resulted in PhoX variants with either no, or trace, catalytic activity (Table S4).
Electron paramagnetic resonance (EPR) spectroscopy was used to determine the oxidation state of the PhoX iron atoms (Fig. 1B). The native PhoX protein was EPR silent. However, partial reduction of the protein with dithionite led to the appearance of a g=4.3 EPR signal characteristic of monomeric high spin Fe3+. This behavior suggests that PhoX contains a pair of high spin Fe3+ ions rendered EPR-silent by magnetic coupling, with reduction of one of the Fe3+ ions to the EPR-silent Fe2+ state revealing the EPR signal from the remaining Fe3+ ion. Because the two ions in the resulting mixed valence state no longer interact magnetically it can be inferred that the Fe2+ ion has been released from the active site cofactor. Thus, only the fully oxidized Fe3+-Fe3+ state of the PhoX cofactor is catalytically viable. Further addition of sodium dithionite led to reduction of the remaining Fe3+ ion, rendering PhoX EPR silent again.
Within the FeAFeBCaA triangle lies an atom that is within bonding distance of all three metal ions (Fig. 2C; Table S3). The close to in-plane geometry suggests that this atom is an oxide ion (O2−). This is confirmed by the structural identity between this part of the PhoX active site and Fe2CaO(CCl3COO)6(THF)4, an inorganic complex containing a μ3-oxo-bridged Fe3+Fe3+Ca2+ cluster with O-donor co-ordination (11)(Fig. S5). The presence of a bridging oxo group explains the strong antiferromagnetic coupling of the two Fe3+ ions observed by EPR spectroscopy (Fig. 1B). The intense visible absorption bands observed for PhoX (Fig. 1A) are, likewise, characteristic of an oxo-bridged dinuclear Fe3+ unit (12), although Cys179 thiolate-to-FeA3+ ligand-to-metal charge transfer bands are also expected to contribute to the visible spectrum (13). The purple color of PhoX is, thus, distinct in origin from that of the well-known purple acid phosphatases in which the visible absorption is due to a tyrosinate-to-Fe3+ charge transfer (14).
PhoX had previously been considered to be an exclusively Ca-dependent enzyme based on the results of metal ion reconstitution experiments (e.g (7, 8, 15)) (although a biosynthetic requirement for Fe in P. fluorescens Phox biosynthesis had been reported (16)). In agreement with these earlier reconstitution studies, we found that the enzymatic activity of P. fluorescens PhoX was abolished by the metal ion chelator EDTA and that activity could be restored by the addition of Ca2+ ions alone (Fig. S1C). However, EDTA treatment perturbed, rather than abolished, the visible transitions arising from the FeA-FeB pair, indicating that the Fe3+ ions remain bound to PhoX in the presence of EDTA (Fig. 1C). This conclusion was confirmed by EPR spectroscopy, which showed that only a small proportion (12% by spin quantitation) of the Fe bound to PhoX is extracted by 50mM EDTA (Fig. 1B). Addition of Ca2+ ions to EDTA-treated enzyme restored the visible spectrum (Fig. 1C).
The PhoX-ligand complex structures show that the active site metal ions form a scaffold that binds the terminal phosphoryl group of the substrate molecule. In the phosphate and vanadate complexes all five metal ions have bonding interactions with the three terminal oxygen atoms of the ligand (Figs. 2C, 3C, S4B,C). In these structures the ligand sits on the FeAFeBCaA unit, with each terminal oxygen atom of the ligand placed above one of the three metal ions. In the AMP-PCP-bound structure the phosphate group has a tilted orientation relative to the FeAFeBCaA plane and there is no interaction with CaA (Fig. 3B). This binding mode permits both the terminal and β-phosphate groups of AMP-PCP to make bonding interactions with CaA and CaB (Fig. 3B). Modeling studies (not shown) suggest that even for substrates without multiple phosphate groups an initial tilted binding mode will usually be favored in order to avoid steric clashes with CaA and CaB. The sole conformational change in the protein that takes place on ligand binding to PhoX is movement of the guanidinium head group of conserved Arg385 to form a bonding interaction with one of the terminal oxygen atoms of the ligand (Fig. 2C). Replacing this arginine residue with alanine impairs PhoX activity suggesting Arg385 contributes to catalysis (Table S4).
The primary mechanism of rate enhancement by phosphoryl transfer enzymes is thought to be provision of favorable geometric and electrostatic interactions with the transition state (1, 2). PhoX provides high valency metal ions that are appropriately positioned to interact with all three terminal oxygen atoms of the phosphoryl group, and in the vanadate complex the ligand is significantly distorted towards the presumed transition state geometry (Fig. S4C). Leaving group activation through co-ordination of the oxygen atom of the labile bond by CaC may also contribute to catalysis (Figs. 3C,E, S4B)(2).
Enzymatic phosphoryl transfer reactions involve in-line displacement of the leaving group by a nucleophile (2). Examination of the PhoX-ligand structures shows that the metal-bridging oxide ion is the only plausible candidate nucleophile (Figs. 3B-C, S4B,C). In the phosphate and vanadate complexes the oxide ion is positioned below the phosphorus atom and is directly in line with the scissile bond. It also blocks access of other potential nucleophiles to the substrate phosphorus atom trans to the leaving group in all three PhoX-ligand complexes (the calculated water-accessible surface area of the phosphorus atom in each case is 0.0 Å2). There is small molecule precedent for the hydrolysis of phosphate esters by an oxide ion bridging two Co3+ ions (17) and a metal-bridging oxide nucleophile has also been inferred to be present in one purple acid phosphatase (18). Oxide movement towards the phosphoryl P atom during catalysis would be facilitated by the weak CaA-oxide interaction and would be consistent with the observed movement of the oxide relative to the FeAFeBCaA plane in response to ligand binding at the active site (+0.4/−0.2 Å; Figs. 3A-C, S4B). Due to the difficulty in abstracting a μ-bridging oxygen atom from between two Fe3+ ions it is likely that the initial reaction product is resolved by a second in-line nucleophilic attack by a water molecule from the opposite side of the phosphorus atom (Fig. 3D). This water molecule would plausibly be activated by binding to CaC since this ion already interacts at the equivalent position with the oxygen atom of the substrate scissile bond (Figs. 3C,D, S4B). Nevertheless, we cannot exclude the possibility that the active site environment labilizes the μ-bridging oxygen atom to allow release of the initial product.
Our structural analysis suggests that PhoX has an almost exclusively inorganic mechanism in which the protein serves as a matrix for the catalytic metal ions. Unique features of the PhoX active site include a cofactor that combines Fe and Ca ions, Cys co-ordination to a Fe3+ ion that lacks a redox function, and the use of more than three metal ions to interact with a single phosphoryl group. It is also notable that the FeAFeBCaAO fragment of the cofactor resembles extensively-studied synthetic oxide-centered triangular metal complexes (19). Carboxylate-bridged Fe3+ pairs are used in other enzymes to catalyze redox reactions with oxygen (12) but in PhoX perform a non-redox role in which the high charge of the iron atoms is exploited to polarize the substrate. Like PhoX, some purple acid phosphatases use a di-iron center to carry out phosphoryl transfer reactions (20). However, in contrast to PhoX, the enzymatically active oxidation state of the iron pair is Fe3+-Fe2+ (21) and the catalytic nucleophile is probably a metal-bridging hydroxide ion (20).
Genes coding for PhoX and PhoA are not normally found in the same bacterium (4) suggesting that these two types of alkaline phosphatase have equivalent physiological roles. PhoA activity depends on Zn2+ ions, which are present at low abundance in many environments (22), and this has led to the hypothesis that organisms expressing PhoX have an advantage in P and Zn co-limited environments (15). However, our observation that PhoX requires Fe3+ ions as cofactors implies that PhoX activity will also be metal-limited by the low bioavailability of Fe in many environments (23). This hypothesis challenges the assumption that P and Fe have biochemically independent effects in co-limiting conditions (24) and raises the possibility that combined Zn-Fe-P co-limitation may occur in some environments through the requirement for either Zn or Fe for phosphate acquisition from organic phosphates. An environment where such considerations may apply is the Western North Atlantic where inorganic P and Zn concentrations are very low and Fe can also be in short supply (22, 25, 26).
Supplementary Material
Acknowledgements
We thank G. O’Toole for providing P. fluorescens Pf0-1 genomic DNA, J. Marcoux, B. Pilgrim, and A. Parkin for exploratory experiments, and F. Armstrong, T. Browning, J. McGrady, G. Henderson, D. Herschlag, C. Schofield, A. Thomson, C. Timmel, N. Williams, and R. Williams for valuable discussions. This work was funded by the University of Oxford, Pembroke College Oxford, Oxford Martin School Vaccine Design Institute, the Engineering and Physical Sciences Research Council, the Biotechnology and Biological Sciences Research Council (grant F02150X), and the European Molecular Biology Organization. Structure co-ordinates and X-ray data have been deposited in the PDB with accession codes 4a9v, 4amf, 4alf, and 3zwu.
References and Notes
- 1.Kamerlin SC, Sharma PK, Prasad RB, Warshel A. Why nature really chose phosphate. Quarterly reviews of biophysics. 2013;46:1–132. doi: 10.1017/S0033583512000157. [DOI] [PMC free article] [PubMed] [Google Scholar]
- 2.Lassila JK, Zalatan JG, Herschlag D. Biological phosphoryl-transfer reactions: understanding mechanism and catalysis. Annual review of biochemistry. 2011;80:669–702. doi: 10.1146/annurev-biochem-060409-092741. [DOI] [PMC free article] [PubMed] [Google Scholar]
- 3.Luo H, Benner R, Long RA, Hu J. Subcellular localization of marine bacterial alkaline phosphatases. Proceedings of the National Academy of Sciences of the United States of America. 2009;106:21219–21223. doi: 10.1073/pnas.0907586106. [DOI] [PMC free article] [PubMed] [Google Scholar]
- 4.Sebastian M, Ammerman JW. The alkaline phosphatase PhoX is more widely distributed in marine bacteria than the classical PhoA. The ISME journal. 2009;3:563–572. doi: 10.1038/ismej.2009.10. [DOI] [PubMed] [Google Scholar]
- 5.Orchard ED, Webb EA, Dyhrman ST. Molecular analysis of the phosphorus starvation response in Trichodesmium spp. Environmental microbiology. 2009;11:2400–2411. doi: 10.1111/j.1462-2920.2009.01968.x. [DOI] [PubMed] [Google Scholar]
- 6.Harke MJ, Berry DL, Ammerman JW, Gobler CJ. Molecular response of the bloom-forming cyanobacterium, Microcystis aeruginosa, to phosphorus limitation. Microbial ecology. 2012;63:188–198. doi: 10.1007/s00248-011-9894-8. [DOI] [PubMed] [Google Scholar]
- 7.van Mourik A, Bleumink-Pluym NM, van Dijk L, van Putten JP, Wosten MM. Functional analysis of a Campylobacter jejuni alkaline phosphatase secreted via the Tat export machinery. Microbiology. 2008;154:584–592. doi: 10.1099/mic.0.2007/012120-0. [DOI] [PubMed] [Google Scholar]
- 8.Roy NK, Ghosh RK, Das J. Monomeric alkaline phosphatase of Vibrio cholerae. Journal of bacteriology. 1982;150:1033–1039. doi: 10.1128/jb.150.3.1033-1039.1982. [DOI] [PMC free article] [PubMed] [Google Scholar]
- 9.Moseley JL, Chang CW, Grossman AR. Genome-based approaches to understanding phosphorus deprivation responses and PSR1 control in Chlamydomonas reinhardtii. Eukaryotic cell. 2006;5:26–44. doi: 10.1128/EC.5.1.26-44.2006. [DOI] [PMC free article] [PubMed] [Google Scholar]
- 10.Materials and methods are available on Science online.
- 11.Prodius D, et al. Synthesis, structure and properties of heterotrinuclear carboxylate complexes [Fe2M(Ca, Sr, Ba)O(CCl3COO)6(THF)n] Polyhedron. 2006;25:2175–2182. [Google Scholar]
- 12.Solomon EI, et al. Geometric and electronic structure/function correlations in non-heme iron enzymes. Chemical reviews. 2000;100:235–349. doi: 10.1021/cr9900275. [DOI] [PubMed] [Google Scholar]
- 13.Oganesyan VS, Thomson AJ. Magnetic circular dichroism of symmetry and spin forbidden transitions of high-spin metal ions. J Chem Phys. 2000;113:5003–5017. [Google Scholar]
- 14.Gaber BP, Sheridan JP, Bazer FW, Roberts RM. Resonance Raman scattering from uteroferrin, the purple glycoprotein of the porcine uterus. The Journal of biological chemistry. 1979;254:8340–8342. [PubMed] [Google Scholar]
- 15.Kathuria S, Martiny AC. Prevalence of a calcium-based alkaline phosphatase associated with the marine cyanobacterium Prochlorococcus and other ocean bacteria. Environmental microbiology. 2011;13:74–83. doi: 10.1111/j.1462-2920.2010.02310.x. [DOI] [PubMed] [Google Scholar]
- 16.Monds RD, Newell PD, Schwartzman JA, O’Toole GA. Conservation of the Pho regulon in Pseudomonas fluorescens Pf0-1. Applied and environmental microbiology. 2006;72:1910–1924. doi: 10.1128/AEM.72.3.1910-1924.2006. [DOI] [PMC free article] [PubMed] [Google Scholar]
- 17.Williams NH, Lebuis AM, Chin J. A structural and functional model of dinuclear metallophosphatases. Journal of the American Chemical Society. 1999;121:3341–3348. [Google Scholar]
- 18.Schenk G, et al. Phosphate forms an unusual tripodal complex with the Fe-Mn center of sweet potato purple acid phosphatase. Proceedings of the National Academy of Sciences of the United States of America. 2005;102:273–278. doi: 10.1073/pnas.0407239102. [DOI] [PMC free article] [PubMed] [Google Scholar]
- 19.Cannon RD, White RP. Chemical and physical properties of triangular bridged metal complexes. Prog Inorg Chem. 1988;36:195–298. [Google Scholar]
- 20.Mitic N, et al. The catalytic mechanisms of binuclear metallohydrolases. Chemical reviews. 2006;106:3338–3363. doi: 10.1021/cr050318f. [DOI] [PubMed] [Google Scholar]
- 21.Wang DL, Holz RC, David SS, Que L, Jr., Stankovich MT. Electrochemical properties of the diiron core of uteroferrin and its anion complexes. Biochemistry. 1991;30:8187–8194. doi: 10.1021/bi00247a014. [DOI] [PubMed] [Google Scholar]
- 22.Jakuba RW, Moffett JW, Dyhrman ST. Evidence for the linked biogeochemical cycling of zinc, cobalt, and phosphorus in the western North Atlantic Ocean. Global Biogeochem Cy. 2008;22 [Google Scholar]
- 23.Moore CM, et al. Processes and patterns of oceanic nutrient limitation. Nat Geosci. 2013;6:701–710. [Google Scholar]
- 24.Saito MA, Goepfert TJ, Ritt JT. Some thoughts on the concept of colimitation: Three definitions and the importance of bioavailability. Limnol Oceanogr. 2008;53:276–290. [Google Scholar]
- 25.Wu JF, Sunda W, Boyle EA, Karl DM. Phosphate depletion in the western North Atlantic Ocean. Science. 2000;289:759–762. doi: 10.1126/science.289.5480.759. [DOI] [PubMed] [Google Scholar]
- 26.Moore CM, et al. Iron limits primary productivity during spring bloom development in the central North Atlantic. Global Change Biol. 2006;12:626–634. [Google Scholar]
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