Degradation of Chlorinated Phenols by Zero Valent Iron and Bimetals of Iron: A Review
Degradation of Chlorinated Phenols by Zero Valent Iron and Bimetals of Iron: A Review
Environmental Engineering Research. 2011. Dec, 16(4): 187-203
Copyright ©2011, Korean Society of Environmental Engineering
This is an Open Access article distributed under the terms of the Creative Commons Attribution Non-Commercial License ( which permits unrestricted non-commercial use, distribution, and reproduction in any medium, provided the original work is properly cited.
  • Received : September 10, 2011
  • Accepted : November 20, 2011
  • Published : December 31, 2011
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About the Authors
Buddhika, Gunawardana
Department of Civil and Environmental Engineering, University of Auckland, Private Bag 92019, Auckland, New Zealand
Naresh, Singhal
Department of Civil and Environmental Engineering, University of Auckland, Private Bag 92019, Auckland, New Zealand
Peter, Swedlund
Department of Chemistry, University of Auckland, Private Bag 92019, Auckland, New Zealand

Chlorophenols (CPs) are widely used industrial chemicals that have been identified as being toxic to both humans and the environ-ment. Zero valent iron (ZVI) and iron based bimetallic systems have the potential to efficiently dechlorinate CPs. This paper reviews the research conducted in this area over the past decade, with emphasis on the processes and mechanisms for the removal of CPs, as well as the characterization and role of the iron oxides formed on the ZVI surface. The removal of dissolved CPs in iron-water systems occurs via dechlorination, sorption and co-precipitation. Although ZVI has been commonly used for the dechlorination of CPs, its long term reactivity is limited due to surface passivation over time. However, iron based bimetallic systems are an effective alternative for overcoming this limitation. Bimetallic systems prepared by physically mixing ZVI and the catalyst or through reductive deposition of a catalyst onto ZVI have been shown to display superior performance over unmodified ZVI. Nonetheless, the efficiency and rate of hydro-dechlorination of CPs by bimetals depend on the type of metal combinations used, properties of the metals and characteristics of the target CP. The presence and formation of various iron oxides can affect the reactivities of ZVI and bimetals. Oxides, such as green rust and magnetite, facilitate the dechlorination of CPs by ZVI and bimetals, while oxide films, such as hematite, maghemite, lepidocrocite and goethite, passivate the iron surface and hinder the dechlorination reaction. Key environmental parameters, such as solution pH, presence of dissolved oxygen and dissolved co-contaminants, exert significant impacts on the rate and extent of CP dechlorination by ZVI and bimetals.
1. Introduction
Chlorinated phenols (CPs) are industrial chemicals with wide applications, such as pesticides, herbicides, disinfectants, biocides and wood preservatives [1 , 2] . The group of CPs com-prise of 19 different chlorinated phenolic compounds, includ-ing pentachlorophenol (PCP), 3 tetrachlorophenols (TeCP), 6 trichlorophenols (TCP), 6 dichlorophenols (DCP), and 3 mono-chlorophenols (MCP) [3] . CPs are industrially produced by direct chlorination of phenol with chlorine gas, as well as other reac-tions, such as hydrolysis and hydrodechlorination, or by chlori-nation of less chlorinated phenols in the presence of aluminium or iron trichloride [4 , 5] . CPs are also by products of industrial processes, such as the bleaching of pulp using chlorine or chlo-rine dioxide [6] and during the production of higher chlorinated phenols [3] . CPs have been detected in groundwater, surface water, waste water, air and soils as a result of their improper dis-posal, leaching from landfills and the incineration of chlorinated wastes [3] .
CPs have been identified as priority toxic pollutants by the U.S. Environmental Protection Agency under the Clean Water Act [4 , 7 - 9] due to their environmental persistence, low biode-gradability and potential health hazard. The toxicity of CPs in-creases with the degree of chlorination, but decreases with the degree of their dissociation [4] . As a result, at low pH, where the non-dissociated form of CP is dominant, their toxicity is greater. While PCP has been identified as the most toxic chlorophenol [10] , many CPs are of environmental concern due to their acute toxicity and resistance to degradation [1 , 2] . In addition to PCP, which has a maximum contaminant level in drinking water of 1 ppb, 2, 4, 6-TCP and 2, 4-DCP are also in the list of drinking water contaminants [11] . CPs have been identified by the Inter-national Agency for Research on Cancer as possible carcinogens [3] and some studies involving the exposure to PCP via inhala-tion and dermal contact have shown the development of specific cancers, such as non-Hodgkin’s lymphoma, multiple myeloma, soft tissue sarcoma and liver cancer [12] . A case study of sawmill workers in New Zealand exposed to PCP reported neuropsycho-logical effects and respiratory diseases in some cases [13] . PCP is also acutely toxic to aquatic microorganisms and fish [10] . Even though the implementation of legislative controls and discharge standards in several countries has curtailed the emissions of CPs from commercial applications, they continue to be identified as common contaminants in surface and groundwater bodies [14] . The environmental prevalence of CPs is attributed to their recalcitrance that results from the carbon-halogen bond, which is cleaved with great difficulty, and the stability of the aromatic structure. Some environmentally significant physical-chemical properties of CPs are presented in Table 1 [15] .
Several methods have been developed for treating CP-con-taminated media, including sonication, ozonation [16 - 18] , elec-trochemical treatment [6 , 19] , advanced chemical oxidation by Fenton’s reagent [4 , 20] , advanced oxidation [4] , bioremediation [18 , 21 - 23] , phytodegradation [24] , reductive dechlorination by zero valent metals [5 , 25 - 31] and sorption by materials, such as almond shell residues [32] , coal fly ash [33] , and biosorbents [34 , 35] . Furthermore, combinations of treatments have also been used to enhance CP degradation. Examples of such approaches include nanoscale zero valent iron coupled with microwave en-ergy [36] or ultrasound [37] , biodegradation following chemical oxidation pre-treatment [38] , sequencing chemically reactive media (palladium coated iron) with biological reactive media (sand seeded with anaerobic bacteria) [39] and simultaneous anaerobic-aerobic biodegradation [40] .
Of the various treatment approaches, the treatment of CP contaminated groundwater using zero valent metals (ZVMs) is particularly attractive due to its low cost coupled with high ef-ficiency and passive mode of treatment. Accordingly, CP degra-dation by various ZVMs, including iron, zinc, magnesium, and aluminium, has previously been investigated [5 , 25 , 26 , 29 , 30 , 41] . CP degradation is dependent on the choice of an appropri-ate metal [42] . Table 2 lists the standard electrode reduction po-tentials of various metals in aqueous solution at 25℃ [43 , 44] . The electrode potential is the difference between the charge on an electrode and the charge in the solution [44] , and metals with higher reduction potentials have a greater ability for degrading chlorinated contaminants in water. However, concerns over the environmental impact and decrease in surface reactivity may limit the use of some promising metals. For example, despite the high reduction potential of zero valent zinc (ZVZn) (-0.763 V), its use has been less than zero valent iron (ZVI) due to the con-cern over water contamination by Zn 2+ ions and the decreased ZVZn reactivity by passivation due to the rapid formation of zinc oxides on its reaction with oxygen [45] . The use of zero valent aluminium (ZVAl) for the oxidative degradation of CPs is limited to acidic conditions due to the insolubility of aluminium oxide (Al 2 O 3 ) layers within the 4 to 9 pH range. Furthermore, concerns over Al 3+ ion toxicity to aquatic systems and humans limit the application of ZVAl for the treatment of CPs. In addition, when ZVMs are used in aqueous media, a balance between the metal reactivity with contaminant and with water needs to be main-tained. For example, Sn and Zn are preferable to Mg for treating chlorinated carbons, such as CCl 4 , as their reactivity with water is lower, but they maintain sufficient reactivity with the contami-nant; Mg oxidation by water overcomes its high reactivity with the contaminant [42] .
Among the different ZVMs, ZVI stands out due to its rela-tively high reactivity with halogenated compounds, low instal-lation and operation costs and low environmental impact [26 , 28] . Accordingly, ZVI is commonly used as a reactive medium in permeable reactive barriers (PRBs) [46 - 48] , as a cost-effective passive treatment approach often used for in situ remediation of contaminated soil and groundwater [39] , and has been shown to treat chlorinated aliphatics [49] , chlorinated methanes [50] , and chlorinated alkanes and alkenes [51] . Some modifications of ZVI include nano sized ZVI [52 , 53] and bimetallics of ZVI with catalysts, such as palladium (Pd) or nickel (Ni) [25 , 28 , 54 - 59] . This paper has reviewed the literature over the past decade to highlight the main features of the reductive degradation of CPs by ZVI/bimetallic iron. Special emphasis has been given to the mechanisms for the removal of CPs, the characteristics and role of iron oxides in the degradation of CPs, and the effect of envi-ronmental parameters and matrix characteristics.
Selected physical-chemical properties of chlorophenols at 25℃[15]
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Selected physical-chemical properties of chlorophenols at 25℃ [15]
Selected standard electrode reduction potential values in aqueous solution at 25℃[4344]
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Selected standard electrode reduction potential values in aqueous solution at 25℃ [43 44]
2. Use of ZVI for Reductive Dechlorination of Chlorophenols
While ZVI of all sizes have been used over the past decade to effectively dechlorinate many different chlorinated organic compounds [26 , 60 - 64] , later research has aimed at enhancing the degradation using smaller sized ZVI, with several studies having been conducted using microscale ZVI [25 , 26 , 28 , 30 , 39 , 65] and more recently using nanoscale ZVI [31 , 52 , 53 , 66 , 67] . A brief summary of the different types of ZVI used is presented in Table 3 . The use of a smaller particle size results in a larger sur-face area and; potentially, increased chemical reactivity [67] as the electronic properties of micro- and nano-scale particles can differ from those of larger particles. The physical and chemical properties of micro to nano sized iron particles are influenced by the atoms located on the iron surface rather than those deeper in the bulk iron material, resulting in more active particles [63] . In addition, nano particles, in contrast to micro scale particles, offer a higher density of reactive sites due to their larger specific surface areas [66] . As nano ZVI are able to stay in suspension for a longer duration, they can be injected into deep or stratified contaminated zones [68] .
The rate of dechlorination of many chemicals by ZVI has been reported to decrease with lowering of the degree of chlorination [49 , 50] ; more chlorinated CPs would be expected to dechlori-nate faster [5] . Also, the degradation rate would be expected to increase for larger iron surface area to solution volume ratios [49 , 62] . The ZVI surface has been proposed to contain reactive and non-reactive sites [69 - 73] ; an effective reaction requires the contaminant molecule to come into contact with a reactive site. Reactive sites represent locations on the ZVI surface that de-grade the solute by breaking the bonds in the reactant [69 , 70 , 72] , while non-reactive sites are assumed to be largely respon-sible for the adsorption of contaminant molecules onto the ZVI [70] , without causing chemical degradation [72] . Exposed graph-ite inclusions have been reported to be responsible for the non-
Summary of different types of micro scale ZVI used in previous researchZVI: zero valent iron, PCP: pentachlorophenol, TCE: trichloroethene, CP: chlorinated phenol.
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Summary of different types of micro scale ZVI used in previous research ZVI: zero valent iron, PCP: pentachlorophenol, TCE: trichloroethene, CP: chlorinated phenol.
reactive sorption of trichloroethene (TCE) and tetrachloroethyl-ene (PCE) onto cast iron [69] . On the basis of available corrosion literature, Gotpagar et al. [73] hypothesized that defects/abnor-malities present on the surface of iron contribute to the reactive sites. Based on the modelling of the sorption of TCE onto reac-tive and non-reactive sites, with degradation only by the reactive sites, the reactive sites were estimated to account for only 2% of the total number of sites on the surface of ZVI [70] , while Bi et al. [71] estimated that only about 2% of the TCE sorption occurred at reactive sites. To complicate matters, when iron is in contact with water, the formation of oxide films on the ZVI surface may mask the reactive and non-reactive sites [74] . The formation of an oxide film can impede the transport and degradation of the organic contaminants by ZVI.
- 2.1. Processes and Mechanisms of Organic Contaminant Removal in Iron-Water Systems
The removal of dissolved contaminants in iron-water sys-tems occurs by the following four mechanisms:
1) Dechlorination: degradation of the contaminant and forma-tion of intermediates;
2) Sorption: accumulation of the contaminant molecules by ad-sorption or complex formation, without their degradation;
3) Precipitation: immobilization of the contaminant due to the formation of insoluble compounds;
4) Co-precipitation: nonspecific removal of the contaminant via entrapment in the matrix of precipitating or recrystallizing iron oxides/hydroxides on the ZVI surface.
Some common reaction pathways for the removal of dis-solved contaminants (RX) in ZVI/water systems based on above mechanisms are listed in Table 4 [74] . The mechanisms of de-chlorination, sorption and co-precipitation are discussed below, but precipitation has been ignored as this mechanism has pri-marily been reported in relation to the removal of heavy metals.
Summary of possible reaction pathways for aqueous phase contaminant (RX) removal in a ZVI/water system[74]Red - reduced form of chlorinated organic compound, FeOOH and Fex(OH)y(3x-y)–iron (oxy)hydroxides.ZVI: zero valent iron.
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Summary of possible reaction pathways for aqueous phase contaminant (RX) removal in a ZVI/water system [74] Red - reduced form of chlorinated organic compound, FeOOH and Fex(OH)y(3x-y)–iron (oxy)hydroxides. ZVI: zero valent iron.
- 2.1.1. Dechlorination
The chemical reduction of chlorinated organic compounds by ZVI-water systems is a surface mediated reaction, which re-sults in direct reduction of the contaminant [47 , 50 , 75] . Conse-quently, the removal of an organic contaminant by ZVI requires direct contact between the contaminant and reactive sites on the ZVI surface. Several steps are involved during the reaction of a chlorinated contaminant with ZVI [76] . The process of de-chlorination of a contaminant by ZVI is schematically illustrated in Fig. 1 .
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Schematic of the dechlorination of chlorinated organic compounds by zero valent iron (ZVI).
The contaminant molecules first diffuse through the solution to the ZVI surface, where they adsorb onto the reactive sites ( Fig. 1 A). Secondly, electrons are transferred from ZVI to the contami-nant molecules and produce lesser chlorinated compounds and various oxides on the surface, with the release of chloride ( Fig. 1 B). Lastly, some lesser chlorinated products diffuse from the ZVI surface into solution ( Fig. 1 C). Based on measurements of the large activation energy required for the reaction, Deng et al. [77] concluded that the reduction of vinyl chloride (VC) by ZVI in aqueous systems was controlled by a chemical reaction at the iron surface, instead of the diffusion of VC to the bulk solution. The dechlorination of CPs by ZVI generally follows first order ki-netics [17 , 26 , 28] .
Fig. 2 presents the proposed reaction pathway by which PCP is dechlorinated by ZVI. Data showing the dechlorination of 2, 3, 4, 6-TeCP by ZVI to form TCP, DCP, and MCP is presented in Fig. 3 . Equations 1-3 below represent the mechanism for the re-moval of a model chlorinated compound, RCl, via ZVI oxidation coupled with reductive dechlorination of the organic compound
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Proposed reaction pathway for pentachlorophenol (PCP) dechlorination by zero valent iron (ZVI). TeCP: tetrachlorophenols TriCP: trichlorophenols DCP: dichlorophenols CP: chlorophenols.
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Dechlorination of 2 3 4 6-Tetrachlornol by acid pre-treated iron. TeCP: tetrachlorophenols TCP: trichlorophenols DCP: dichlo-rophenols MCP: monochlorophenols.
[50] . The anodic reaction for the dissolution of ZVI is illustrated in Equation 1, reductive dechlorination of the chlorinated com-pound by ZVI in the presence of proton donors (for example wa-ter) is presented in Equation 2 and the net reductive dechlorina-tion of the chlorinated compound by ZVI is given in Equation 3.
  • Fe0→Fe2++ 2e-(1)
  • RCl+ 2e-+H+→RH+Cl-(2)
  • Fe0+RCl+H+→Fe2++RH+Cl-(3)
When oxygen is present, the cathodic reduction of oxygen occurs (Equation 4), while ZVI is oxidised to Fe 2+ and/or Fe 3+ ions, with a rise in the solution pH (Equation 5). Furthermore, under weak acidic to near neutral and oxygenated conditions the Fe 2+ ions in water further oxidise to ferric hydroxide; thereby, decreasing the solution pH (Equation 6) [78] . In addition, water can act as an oxidant (Equation 7) and; under anoxic conditions, ZVI corrosion will result in the production of hydrogen and an increase in the solution pH (Equation 8) [50] .
  • O2+ 2H2O+ 4e-→ 4OH-(4)
  • 2Fe0+O2+ 2H2O→ 2Fe2++ 4OH-(5)
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  • 2H2O+ 2e-→H2(g) + 2OH-(7)
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The above reactions lead to an increase in the solution pH, while producing reductants (Fe 2+ and H 2 ) with the potential for further dechlorination. However, dechlorination by dissolved Fe 2+ occurs slowly and can be further decreased by the presents of ligands in solution due to the formation of complexes with Fe 2+ ions [79] . In the absence of a catalyst, H 2 is not an effective reductant and its build-up on the metal surface can inhibit the corrosion of ZVI; thereby, slowing the dechlorination reaction [50] . A survey of the literature relating to the reduction of chlori-nated hydrocarbons by iron materials indicated that direct elec-tron transfer as well as an indirect mechanism involving atomic hydrogen participate in dechlorination [80 , 81] .
Negatively charged chloride ions are released during de-chlorination, which adsorb onto the oxide films and penetrate through the pores/defects on the oxides. This causes dispersion of the oxide films; thereby, increasing their permeability and en-hancing the movement of ions across the oxide films. Chloride ions are essential for the initiation of pitting and crevice corro-sion. Enhanced degradation rates of chlorinated compounds by ZVI may be due to enhanced metal dissolution and electron transfer due to pitting corrosion [82] . Furthermore, the chem-istry of the ZVI surface during the dechlorination reaction is similar to the classical crevice corrosion of steel in the presence of chloride ions [83] . The oxidation of iron releases electrons, which reduces dissolved oxygen to hydroxide ions. In addition, dissolved oxygen depletion in crevices leads to an increase in the
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Sorption of 2 3 4 6-Tetrachlorophenol (TeCP) onto (A) Un-modified ZVI (B) Acid-pre-treated zero valent iron (ZVI).
concentration of metal cations in the small crevices, which at-tract and increase the diffusion of negatively charged chloride ions from the bulk solution into the crevices. This process leads to an increase in the rate of metal dissolution [84] . Conversely, during this process, the formation of insoluble metal hydroxides can lead to coating of the exterior surface of ZVI and reduce the rate of metal dissolution [73] .
- 2.1.2. Sorption
In addition to dechlorination, CPs dissolved in solution can be removed via sorption onto the ZVI surface [26 , 85] . Fig. 4 shows the amounts of 2, 3, 4, 6-TeCP sorbed onto unmodified and acid pretrated ZVI. In some cases, the sorption onto ZVI can be sufficiently strong to prevent the diffusion of sorbed re-actant molecules back into solution. In such cases, the sorbed molecules can hinder the access of dissolved CPs to recative sites on the ZVI surface, attenuating the degradation process. The sorption onto ZVI may be a significant removal mechanism, with some studies having reported the removal of over 50% of the initial PCP mass via this process [26] . TCE and PCE sorb pri-marily onto the non-reactive sites of ZVI [72] . The adsorption of CPs onto iron oxides occurs via the phenolate group [86] . A high solution pH leads to decreased surface reactivity and enhanced adsorption of TeCPs onto the ZVI surface [87] . Under moder-ately acidic conditions (pH around 5.4), the adsorption of CPs is influenced by their degree of dissociation; CPs with lower pKa values have lower solubilities in water and show greater tenden-cies to adsorb onto iron oxides [87] . Contaminants with greater hydrophobicity are more susceptible to sorption, irrespective of their reactivity with ZVMs [25] . The adsorption of CPs dissolved in water to iron oxides is less than that of those in the gaseous phase, suggesting that hydrophobic CPs have a modest capac-ity to compete with water for adsorption onto hydrophilic oxide surface sites [86] .
- 2.1.3. Co-precipitation
Co-precipitation refers to contaminant entrapment in the iron oxides/hydroxides precipitating or recrystallizing on the ZVI surface. The co-precipitation of contaminants during iron corrosion is a fundamental mechanism of dissolved contami-nant removal by ZVI [88] . At pH values within the range 4 to 9, ZVI corrosion results in the formation of an oxide film on its sur-face. At lower pH values, the oxide films are relatively porous, unstable and detachable, while at higher pH values, the oxide films are more stable. At neutral pH, various iron oxides (green rusts, hydroxides, and oxyhydroxides) can precipitate, poten-tially entrapping dissolved organic compounds on the ZVI sur-face. In contrast to earlier studies, which considered oxide films as inhibitory to contaminant removal [50 , 75] , co-precipitation can lead to the oxide films acting as contaminant scavengers; contaminant removal may not necessarily be limited to surface mediated processes [89] .
- 2.2. Challenges to Implementation of ZVI Technology
While ZVI is effective at treating CPs dissolved in water, it does not effectively degrade dense non-aqueous phase liquids (DNAPLs) in a source area. Because the ZVI surface is hydrophil-ic, while CPs are typically hydrophobic, the interaction between ZVI and separate phase CPs tends to be absent [63 , 90] . Further-more, the rate of reduction is greatly influenced by surface char-acteristics of ZVI, such as the morphology, presence of impuri-ties, specific surface area and crystallinity [76] . One of the major challenges in the use of ZVI is the decrease in the iron reactivity over time, which has been attributed to:
1) Changes in the iron surface morphology [73] ;
2) Surface passivation due to saturation of the reactive sites with metal oxides or other species, depending on the solution composition, and the generation and accumulation of lesser chlorinated by products [82] ;
3) Precipitation of metal hydroxides (e.g., Fe(OH) 2 and Fe(OH) 3 ) and metal carbonates (e.g., FeCO 3 ) on the iron surface [62 , 65] .
Low rates of dechlorination by ZVI have also been partially attributed to the excessive sorption of contaminants to nonreac-tive sites and the impeding of electron transfer by oxide layers [73] . However, the reactivity of the ZVI surface can be sustained in the presence of some oxides, such as magnetite (Fe 3 O 4 ) and green rust (Fe [II]/Fe [III] hydroxide), while the presence of goe-thite (α-FeOOH) and hematite (α-Fe 2 O 3 ) decrease the reactivity [91 - 93] . The formation and role of iron oxides in the removal of CPs is further discussed in Section 4. The inhibition of iron cor-rosion and reduction reactions can also result from excessive H 2 accumulation on the iron surface [50] . Furthermore, the deg-radation of chlorinated aromatic compounds and compounds with lesser degrees of chlorination by ZVI occurs at slower rates
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Dechlorination of chlorophenols by acid pre treated iron. TCP: trichlorophenols TeCP: tetrachlorophenols PCP: pentachloro-phenol.
[56 , 65] . This sequence is illustrated for the degradations of PCP, 2, 3, 4, 6-TeCP, and 2, 4, 6-TCP in Fig. 5 . The accumulation of chlorinated by products due to low ZVI reactivity with lesser chlorinated contaminants can give rise to toxicological concern. Lastly, competition with co-contaminants, such as nitrate and chromate, can inhibit or decrease the reduction of chlorinated compounds [61 , 94] .
The use of nano ZVI in real applications is hindered by the rapid agglomeration of nano particles to micro scale particles and the larger aggregates in water [67] and the propensity of nano ZVI particles to interact with the subsurface media [68] . These processes may affect the mobility and reactivity of the nano particles, limiting their capacity to dechlorinate the con-taminants. An approach proposed to mitigate this issue involves enhancing the stability of the nano iron particles using natural clay minerals and zeolite [95] . However, in comparison to micro scale iron particles the lifespan of nano iron particles is expected to be smaller due to the relatively faster background corrosion [96] .
3. Use of Bimetals
Bimetallic systems have been investigated as a means of over-coming the limitations associated with the unmodified ZVI used to degrade chlorinated organics [25 , 26 , 28 , 37 , 54 , 97 - 99] . These systems are a combination of two metals - a primary metal and a secondary metal, selected based on their standard reduction po-tentials ( Table 2 ); the secondary metal is electropositive relative to the primary metal. In bimetallic systems, the primary metal, such as ZVI, is known to serve as the electron donor, while the secondary metal (Pd, platinum (Pt) or Ni) acts as a catalyst [45] . During the reaction, the secondary metal is not consumed, but increases the rate and efficiency of the reaction [45 , 58 , 100 - 102] . The incorporation of the catalyst contributes to increase the sur-face area and number of reactive sites on the ZVI surface [58 , 100] . Catalysts, such as Pd and Ni, have a void orbit, which allows for the formation of complex compounds by combining with the chloride atoms of chlorinated molecules; thus, reducing the ac-tivation energy and increasing the dechlorination reaction rate, while limiting the production of chlorinated intermediate com-
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Pentachlorophenol (PCP) degradation by unmodified zero valent iron (ZVI) acid washed ZVI and Ni/Fe bimetal.
pounds [45 , 99] . The presence of a secondary metal may also provide a surface that is less prone to fouling and that can con-tinue to supply electrons for the complete oxidation-reduction process [73] . In the presence of a catalytic metal, dechlorination of chlorinated organic compounds occurs via hydrogenation [96] . The catalytic reactivity of bimetals and the dechlorination rate depend on the properties of the chlorinated contaminants and the ZVI [26 , 56] . For example, while Kim and Carraway [26] observed that bimetallic systems were poorer at dechlorinating PCP than unmodified iron, Fig. 6 presents data that show ZVI bi-metals can lead to faster PCP dechlorination than unmodified or acid washed ZVI. Similarly, differences in molecular structures cause isomers of chlorophenols to show different dechlorination rates upon reacting with bimetals [56] .
Several bimetallic combinations have been studied for their efficiencies to degrade chlorinated organic compounds, includ-ing ZVI/Pd (Fe/Pd), ZVI/Ni (Fe/Ni), ZVI/Copper (Fe/Cu), and Magnesium /Palladium (Mg/Pd) [63] . Table 5 summarizes the degradation rate constants for selected chlorinated aliphatics and aromatics by different metallic media. Increasing the cata-lytic metal loading on the iron surface has been observed to in-crease the dechlorination efficiency [37 , 78 , 103] . This effect was attributed to the increased availability of the catalyst, where a higher catalytic metal load results in greater dispersion of the catalyst on the ZVI surface as well as increases in the surface area and number of dechlorination sites [56 , 103] .
- 3.1. Different Methods of Bimetallic Systems
Simple bimetallic systems prepared by physically mixing the primary metal (for example ZVI) and the catalyst (Ni) at pre-determined weight ratios have been shown to display superior performance [30 , 31 , 45 , 96 , 104 , 105] . For example, a mixture of nano-Ni and nano-ZVI showed greater PCP dechlorination than nano-ZVI particles alone [31] . However, bimetallics are usually prepared via reductive deposition by doping a catalytic metal, such as Pd, Pt or Ni (which are not active by themselves), onto the primary reactive metal, such as ZVI or ZVZn [25 , 26 , 28 , 53] . The reductive adsorption of the catalytic metal onto the iron sur-face is depicted in Equations 9 [78] and 10 [54] :
Summary of reaction rate constants in the degradation of several chlorinated aliphatic and aromatic compounds by various metals/metal combinationsNP: data not provided, PCP: pentachlorophenol, ZVI: zero valent iron, ZVZn: zero valent zinc, TeCP: tetrachlorophenols, TCP: trichlorophenols, DDT: dichloro-diphenyl-trichloroethane.
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Summary of reaction rate constants in the degradation of several chlorinated aliphatic and aromatic compounds by various metals/metal combinations NP: data not provided, PCP: pentachlorophenol, ZVI: zero valent iron, ZVZn: zero valent zinc, TeCP: tetrachlorophenols, TCP: trichlorophenols, DDT: dichloro-diphenyl-trichloroethane.
  • Pd4++ 2Fe0→Pd0+ 2Fe2+(9)
  • 2Fe0+Ni2+→Ni0+ 2Fe2+(10)
A bimetallic system can contain several galvanic cells on the primary metal; thus, increasing the rate of corrosion of the iron, which leads to an increased rate of dechlorination [52] . However, some studies have reported that physical mixing of two metals did not result in an increased rate of degradation of chlorinated aromatic compounds [45] . Comparisons of the reactivities of physical mixtures of nano-Ni and nano-ZVI with nano-ZVI alone and with Ni coated nano-ZVI showed that the Ni coated nano-ZVI gave the highest dechlorination activity [96] .
- 3.2. Processes and Mechanisms of Organic Contaminant Removal in Bimetallic Systems
Several mechanisms have been proposed to explain the im-proved dechlorination rates observed with bimetallic systems. Fig. 7 presents the various mechanisms for the hydrodechlori-nation of CPs by bimetallic particles [29 , 106] . Fig. 7 A illustrates the dechlorination via direct electron transfer from ZVI to the chlorinated molecule. A common hypothesis attributes the en-hanced reactivity of bimetals to the formation of galvanic cou-ples between the ZVI and catalyst due to the flow of electrons from ZVI to the catalyst driven by the difference in their elec-trode potentials. In the case of bimetals containing iron, ZVI acts as the anode and the catalyst as the cathode [45 , 84 , 96 , 100 , 107 , 108] . Although a higher rate of ZVI corrosion would be expected in the presence of a catalyst, with a weaker reductant, possessing a positive reduction potential compared to ZVI, the dissolutions of ZVI and Ni would be significantly lower in the Ni/Fe bimetal compared to the individual metals [96] ; the presence of ZVI has been reported to inhibit Ni corrosion [96 , 108] .
Another hypothesis attributes hydrogen adsorption onto the catalyst surface for the enhanced dechlorination by the bimet-als. This hypothesis assumes that chlorinated organic molecules are adsorbed onto the catalyst surface, where reduction of the chlorinated organic compounds occurs on the surface of the catalytic metal, but not at the interface of the catalyst and ZVI ( Fig. 7 B) [96 , 106 , 109 - 111] . In a bimetallic system ( ZVIC ), the hy-drogen adsorbed onto the surface ( H ads ) could be the result of the dissociative chemisorption of the H 2 produced by the reduc-tion of water (Equation 11) or that produced as an intermediate (Equation 12) [110] . When in contact with water, ZVI produces molecular hydrogen by anodic corrosion. This molecular hydro-gen is dissociatively adsorbed onto the catalyst to form a metal hydride (M-H), which subsequently dehalogenates the adsorbed target substrate - this process is known as hydrodechlorination [97] . The reactions occurring in a bimetallic system containing Ni as the catalyst can be represented by Equation 1 and Equa-tions 13-15 [96 , 112 , 113] . H* denotes the formation of atomic hydrogen and its involvement during metal hydride formation.
  • 2ZVIC+H2→ 2ZVIC–Hads(11)
  • ZVIC+H2O+e-→ZVIC–Hads+OH-(12)
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Mechanisms for the hydrodechlorination of chlorophenols by bimetallic systems. ZVI: zero valent iron [29 106].
  • Ni+H* →Ni–H(14)
  • Ni–H+R–Cl→Ni+R–H+Cl-(15)
A three step process has been proposed for the dechlorina-tion that occurs within bimetallic systems [99] . First, hydrogen gas is produced from the corrosion of ZVI in water, while the sec-ond step involves the transport and adsorption of chlorinated contaminant molecules onto the catalyst surfaces via bonding between the chlorine and the catalyst surface. The last step is de-chlorination, which involves the incorporation of hydrogen into the contaminant molecule and the release of chloride ions into solution. Another hypothesis paralleling that suggested above is that contaminant molecules adsorbed onto the ZVI surface are dechlorinated at the catalyst/ZVI interface ( Fig. 7 C) [106] .
Furthermore, some studies have postulated that rather than the atomic hydrogen adsorbed on the reductant surface, the atomic hydrogen absorbed/intercalated within the lattice of the catalytic metal is the dominant reductant responsible for the re-ductive dechlorination of the chlorinated compounds adsorbed onto the catalyst surface [52 , 106 , 110 , 114] . The enhanced re-activity of the bimetallic particles has been attributed to the adsorption of chlorinated contaminant and the generation and
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Dechlorination of pentachlorophenol (PCP) tetrachlorophe-nols (TeCP) and trichlorophenols (TCP) by a Ni/Fe bimetal.
storage of reactive hydrogen molecules on the metal surface. Under this hypothesis, the metal with the lower potential in the bimetal will preferentially dissolve and release electrons (e.g., Zn dissolution will occur in the Pd/Zn pair), while the other metal, with the relatively higher (positive) reduction potential, will act as the catalyst [73] . A consensus on the most likely hypothesis for the enhanced dechlorination by bimetals is currently lack-ing;clear experimental studies examining the above hypotheses are limited, and doping of ZVI with catalytic metals has been seen to not always result in an enhanced rate of degradation. For example, lowering of the PCP and 1, 1, 1-trichloroethane reduc-tion rates reportedly occurred when ZVI was modified with Pd, Pt, Ni or Cu [26] .
The dechlorination of CPs by bimetallics follows first order kinetics [ 28 , 54 - 57 , 59 ], and the rate constants have shown to be dependent on the degree of chlorination of the organic com-pound. A hypothesis explaining this behaviour is that the energy required to break the C-Cl bond differs for penta- tetra-, tri-, di-and mono-chlorophenols. In bimetallic systems, the rate and extent of degradation decreases with higher degrees of chlorina-tion, i.e., the order for the rates of degradation is MCP > DCP >TCP > PCP [25 , 97 , 115] . The more chlorinated compounds expe-rience greater repulsion between electrons on the metal surface and the negatively charged chlorine of the chlorinated organic molecule, leading to greater sorption of the lesser chlorinated organics [81] . As a result, in bimetallic systems, where indirect reduction through atomic hydrogen predominates, more chlo-rinated compounds may exhibit lower degradation rates com-pared to the less chlorinated compounds [81] . There is another hypothesis for the increased rate of degradation on lowering of the dechlorination, which is based on the assumption that dechlorination occurs in two steps. The first step is the cleav-age of the C-Cl bond resulting in the formation of a transient electron-deficient carbocation on the phenol ring; the second is the bonding of the carbocation with an electrophile, such as a hydrogen from the metal hydrides formed on the iron surface, to complete its octet configuration [97] . A greater number of chlorines on the phenol ring intensify the positive charge arising from C-Cl cleavage, which destabilizes the carbocation; there-by, lowering the rate of dechlorination [97] . However, contrary to the above observation, other studies have shown the inverse trend with lesser chlorinated compounds degrading at lower rates [ 101 , 116 ]. Fig. 8 presents data illustrating such an effect for the degradations of PCP, TeCP, and TCP using a Ni/Fe bimetal, where the rate and extent of PCP degradation was higher com-pared to those of TeCP and TCP. Therefore, the only consistent conclusion is that the efficiency and rate of hydrodechlorination of CPs by bimetallic systems are dependent on certain factors, such as the type and characteristics of the metal combinations used and the characteristics of the target contaminant.
- 3.3. Advantages of Using Bimetals
Bimetals can efficiently catalyse dechlorination reactions and reduce the amount of toxic chlorinated by products [56 , 78 , 96] , and further progress dechlorination reactions towards completion [45] . The dominant reaction for the dechlorination of chlorinated compounds in bimetallic systems is via hydrogen reduction rather than the electron transfer process from ZVI at the solid/liquid interface [45 , 56 , 78 , 102] . Furthermore, the ad-dition of a catalytic metal renders stability to the iron particles by lowering the oxidation of ZVI and formation of iron oxides on the surface [107] . While Fe/Pd particles were not observed to undergo a colour change upon exposure to air, ZVI particles rap-idly underwent surface oxidation, turning from black to reddish-brown within a few hours [45] . Similarly, ZVI particles lost their reactivity within a few days, while the activity of Fe/Pd particles was maintained beyond two weeks [52] and Pd doping eliminat-ed the passivation of the Zn surface [45] .
- 3.4. Limitations of Using Bimetallic Particles
Bimetallic surfaces can lose their reactivity over time through disintegration of the catalyst due to ZVI dissolution, the forma-tion of a hydrogen gas layer on the bimetallic surface due to excessive hydrogen production in the system, the formation of iron oxides on the surface [59] , and the sorption of chlorinated organic compounds [117] . During dechlorination, the formation of ferrous and ferric hydroxides on the iron surface can passivate the bimetallic surface by hindering the transport of chlorinated molecules as well as blocking access to reactive sites on its sur-face [62] . Additionally, the rate of dechlorination can decrease over time due to the formation of hydrates and oxides on the bimetal surfaces [37 , 59 , 96] . Some investigators have argued that the formation of iron oxide, occlusion of organic molecules and accumulation of hydrogen are temporary, reversible effects, which can be concealed by controlling the solution pH under anoxic conditions [59 , 117] .
4. Formation, Characterisation and Role of the Iron Oxide Films
The development of iron oxide films occurs naturally when ZVI comes in to contact with air and water. Likewise, when groundwater flows through a reactive barrier filled with ZVI or a bimetal, iron corrosion and other chemical reactions can lead to the formations of different iron oxide films on the ZVI surface [89] . The type and characteristics of the iron oxide films formed depend on the environmental conditions, such as groundwater chemistry, solution pH and availability of dissolved oxygen. As an example, in a ZVI/water system maintained at near neutral pH, oxides, such as magnetite and hematite, hydroxides, such as ferrous and ferric hydroxide, and oxyhydroxides, such as goe-thite and green rusts, are formed [74] . The properties of the ox-ide films, such as their electronic conductivity and porosity, can influence the corrosion of iron in natural waters [118] , and the formation of some oxides can enhance or decrease the reactivity of the iron surface [119] . The formation of oxides can also lower the porosity of the reactive medium in PRBs; considering the pH range 4 to 9 in natural waters, the oxides formed at a low pH are relatively porous (i.e., unprotective) and removable compared to the more stable and protective oxides formed at higher pH val-ues [120] . Numerous oxides can form on ZVI, including magne-tite, green rust (chloride and sulphate), lepidocrocite, goethite,maghemite, akageneite, wustite and ferrihydrite [31 , 91 , 94 , 119 , 121 - 129] . Table 6 provides a summary of selected characteristics of some of these oxides [130 - 132] .
The characteristics of iron oxides can affect the effectiveness of the catalytic metal deposited onto the ZVI surface. Further-more, iron oxides can sorb dissolved organic compounds. Ha-logenated hydrocarbons usually sorb via hydrophobic bonding rather than complex formation with iron oxides. Chlorinated organic molecules containing other functional groups can strongly sorb via interactions between the reactive sites on ox-ides and the functional groups [133] . Such interactions depend on the affinity of the contaminant molecules for the sorption sites, shape and polarity of the molecule, and the location of the functional group [133] . Furthermore, dissolved organics can also be removed from solution via co-precipitation, a process in which contaminants initially adsorb onto fresh iron oxides, but are later entrapped within the oxide as it matures [74] .
Iron oxide films play several different roles [47 , 94 , 119 , 122 , 126 , 134 - 137] . Oxide precipitates can passivate the iron surface by creating a barrier between the contaminant molecules and the ZVI surface, hindering the electron transfer process and suppressing dechlorination [122] . Passivation of iron surfaces occurs via the formation of oxides/oxyhydroxides, such as he-matite, maghemite, lepidocrocite and goethite [94 , 135 , 138] . The passivating oxide films are multilayered, nanocrytalline microstructures, typically consisting of an inner magnetite layer and an outer maghemite or hematite layer [91 , 122 , 135 , 139] . Conversely, some iron oxides can act as semiconductive films by contributing electrons from their conduction band to the dechlorination reaction; thereby, promoting contaminant re-
Selected characteristics of iron oxidesSpecific surface areas and symmetries compiled from Cornell and Schwertmann[132]; EBG(energy necessary to excite an electron from thevalence band to the conduction band) from Hernandez[130]; Density values from Balasubramaniam et al.[131].
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Selected characteristics of iron oxides Specific surface areas and symmetries compiled from Cornell and Schwertmann [132]; EBG (energy necessary to excite an electron from thevalence band to the conduction band) from Hernandez [130]; Density values from Balasubramaniam et al. [131].
duction [122] . Oxides, such as magnetite and green rust, allow electron transfer and facilitate the dechlorination reaction [94 , 119 , 135 , 138] . However, green rusts are unstable and will trans-form over time to relatively more stable oxides, such as goethite, lepidocrocite, maghemite or magnetite, depending on certain factors, such as the solution pH, and rates of oxidation and de-hydroxylation [132 , 140 - 142] . Similarly, while magnetite is elec-trically conductive, its formation can lead to ZVI passivation if it hinders the release of Fe 2+ to the bulk solution [91] . Conversely, precipitation of the passivating iron oxides can in some cases (e.g., when it occurs on non-reactive sites of the ZVI surface) re-sult in little or no decrease in the reactivity of ZVI [70] . In addi-tion to the commonly accepted mechanisms for the dechlorina-tion of organic compounds - direct electron transfer from ZVI or indirect electron transfer through the oxide layer, iron oxides can act as coordinating surfaces to reduce contaminants using the electrons contributed by surface bound Fe 2+ or by surface reac-tive sites of Fe 2+ ions formed in oxide films (structural Fe 2+ ) due to the release of electrons [122 , 143] .
In recent years, the effect of specific oxides on the reactiv-ity with chlorinated organic compounds has been investigated using pure iron oxides [143 - 146] . Magnetite degradation of PCP showed the reduction to be controlled by surface reaction mechanisms, such as sorption and oxidation [145] , and that the reactivity decreased with an increase in the particle size of mag-netite [144] . The rate of carbon tetrachloride dechlorination by magnetite increased on increasing the solution pH from 6 to 10 [143] . Nonetheless, the presence of co-contaminants affects the reactivity of iron oxides [134 , 145] . Different species present in a matrix (e.g., anions, ligands, other organic compounds) com-pete to adsorb onto the reactive sites available on the oxide sur-faces [145] , where strong adsorption of such co-contaminants could inhibit the dechlorination of the target compounds [134] .
Fig. 9 presents the Raman spectra of typical iron oxides de-tected on ZVI/bimetallic surfaces. The unwashed ZVI surface contained Wustite, while acid washing and Ni coating during the bimetal preparation resulted in increased proportions of mag-netite present on the respective surfaces. The higher reactivity of acid washed ZVI and Ni/Fe was partially attributed to the in-creased proportion of magnetite.
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Raman spectra of reference iron oxides. (a) Wustite (b) mag-netite and iron surfaces before exposing to pentachlorophenol (PCP) (c) unwashed zero valent iron (ZVI) (d) acid washed ZVI and (e) Ni/Fe bimetal.
5. Effect of Environmental Parameters and Matrix Characteristics
The solution pH is a critical environmental parameter af-fecting the degradation of CPs. The solubility of CPs in water generally increases at higher pH values [2 , 14] and the solution pH affects the rates of iron corrosion and oxide formation. Iron dissolves under acidic conditions, while under basic conditions iron oxides form and cause surface passivation [50 , 62] . The de-chlorination efficiency decreases with increasing solution pH [27 , 37 , 55 , 97 , 112 , 113] . Moreover, with bimetallic systems at basic pH conditions, less atomic hydrogen or metal hydride par-ticipate in the dechlorination reaction. Therefore, extremes of solution pH can influence the availability of reactive sites on the ZVI and bimetals for dechlorination.
Dissolved oxygen (DO) is another significant parameter af-fecting the dechlorination of CPs by ZVI and bimetals. The pres-ence of DO can hamper the dechlorination by ZVI and bimetals because oxygen is the preferred electron acceptor under oxic conditions [50] . In an oxic system, DO can compete with CPs for the electrons produced via ZVI oxidation [147] . Furthermore, the presence of DO can affect the formation and composition of the oxide films formed on ZVI/bimetallic surfaces [135] . Under oxic conditions, the rates of dechlorination tend to be significantly lower to those under anoxic conditions [112 , 136 , 148] .
The composition of contaminated groundwater can affect the efficiency of a ZVI or bimetallic system for treating CPs. Groundwater can contain several constituents that may po-tentially compete with CPs for electrons, such as natural or-ganic matter [149 , 150] and dissolved inorganic anions, such as nitrate, chloride, chromate, carbonate, phosphate, sulphate, and sulphide [124 , 126 , 151 , 152] . The presence of dissolved co-contaminants can affect the corrosion of ZVI and the interaction between CPs and ZVI/bimetals. Furthermore, the behaviour of CPs when present as an individual component may differ from that when present as a multi-component system. Anions, such as nitrate and chromate, can compete for reactive sites and de-crease the sorption capacity and reactivity of the ZVI/bimetallic surfaces due to the formation of passive iron oxides on the sur-face [61 , 94 , 153 , 154] .
6. Conclusions
CPs are a group of industrially important chemicals. Howev-er, due to their unique characteristics (e.g., aromaticity stability, hydrophobic nature, toxicity to humans and ecosystems and en-vironmental persistence), the treatment of CPs has been a chal-lenge. The use of ZVI is an emerging passive in situ treatment method for the treatment of dissolved CPs. The removal of CPs from solution occurs through multiple processes (dechlorina-tion, sorption and co-precipitation). However, some processes (e.g., surface passivation) have been observed to limit the long term reactivity of ZVI. Iron based bimetallics offer an attractive approach for overcoming these limitations. Bimetals prepared by physically mixing ZVI and catalyst or doping of the catalyst onto the ZVI surface can enhance the rate and efficiency of CP dechlorination and decrease the accumulation of less chlori-nated intermediate compounds. Iron oxides play various roles depending on their characteristics (e.g., passivate the iron sur-face, act as a semiconductor or coordinating surfaces). Depend-ing on the characteristics, oxide films can enhance or decrease the reactivity of the iron surface and affect the efficiency of the catalyst and porosity of the reactive medium. The solution pH and dissolved oxygen are critical parameters that affect the deg-radation of dissolved CP by ZVI and bimetals. In addition, when co-contaminants with different physicochemical properties are present in the solution, they interact with the processes occur-ring at the reactive and sorption sites on ZVI/bimetallic surfaces. Such interactions impose competitive effects and affect the rate of CPs degradation by ZVI or bimetals.
The lead author thankfully acknowledges the awarding of the New Zealand International Doctoral Research Scholarship and the University of Auckland International Doctoral Scholarship for her Ph.D. study.
Keane MA 2005 A review of catalytic approaches to waste mini-mization:case study--liquid-phase catalytic treatment of chlorophenols. J. Chem. Technol. Biotechnol. 80 1211 - 1222    DOI : 10.1002/jctb.1325
Arcand Y , Hawari J , Guiot SR 1995 Solubility of pentachloro-phenol in aqueous solutions: the pH effect. Water Res. 29 131 - 136    DOI : 10.1016/0043-1354(94)E0104-E
Agency for Toxic Substances and Disease Registry. 1999 Toxico-logical profile for chlorophenols. Agency for Toxic Substances and Disease Registry U.S Department of Health and Human Services Atlanta
Pera-Titus M , Garcia-Molina V , Banos MA , Gimenez J , Es-plugas S 2004 Degradation of chlorophenols by means of ad-vanced oxidation processes: a general review. Appl. Catal. B. Environ. 47 219 - 256    DOI : 10.1016/j.apcatb.2003.09.010
Kim YH , Carraway ER 2003 Dechlorination of chlorinated phe-nols by zero valent zinc. Environ. Technol. 24 1455 - 1463    DOI : 10.1080/09593330309385690
Patel UD , Suresh S 2008 Electrochemical treatment of penta-chlorophenol in water and pulp bleaching effluent. Sep. Pu-rif. Technol. 61 115 - 122    DOI : 10.1016/j.seppur.2007.10.004
Keith L , Telliard W 1979 Priority pollutants. I. A perspective view. Environ. Sci. Technol. 13 416 - 423    DOI : 10.1021/es60152a601
U.S. Environmental Protection Agency. c2011 Protection of envi-ronment:toxic pollutants [Internet]. U.S. Environmental Protection Agency Washington DC Available from: x?c=ecfr&rgn=div8&view=text&node=40: no=40.
U.S. Environmental Protection Agency. c2011 Priority pollutants [Internet]. U.S. Environmental Protection Agency Washington DC Available from:
Tanjore S , Viraraghavan T 1994 Pentachlorophenol--water pollu-tion impacts and removal technologies. Int. J. Environ. Stud. 45 155 - 164    DOI : 10.1080/00207239408710889
U.S. Environmental Protection Agency. c2011 Drinking water con-taminants [Internet]. U.S. Environmental Protection Agency Washington DC Available from:
U.S. Environmental Protection Agency. 2010 Toxicological review of pentachlorophenol: in support of summary information on the Integrated Risk Information System (IRIS). U.S. Environmental Protection Agency Washing-ton DC 288 -
McLean D , et al. , Eng A , et al. , Dryson E , et al. 2009 Morbidity in former sawmill workers exposed to pentachlorophenol (PCP): a cross-sectional study in New Zealand. Am. J. Ind. Med. et al. 52 271 - 281    DOI : 10.1002/ajim.20677
Wightman PG , Fein JB 1999 Experimental study of 246-Trichlo-rophenol and pentachlorophenol solubilities in aqueous solutions: derivation of a speciation-based chlorophenol solubility model. Appl. Geochem. 14 319 - 331    DOI : 10.1016/S0883-2927(98)00054-7
Shiu WY , Ma KC , Varhanícková D , Mackay D 1994 Chlorophenols and alkylphenols: a review and correlation of environmen-tally relevant properties and fate in an evaluative environ-ment. Chemosphere 29 1155 - 1224    DOI : 10.1016/0045-6535(94)90252-6
Anotai J , Wuttipong R , Visvanathan C 2007 Oxidation and detoxi-fication of pentachlorophenol in aqueous phase by ozona-tion. J. Environ. Manage. 85 345 - 349    DOI : 10.1016/j.jenvman.2006.10.001
Dai Y , Li F , Ge F , Zhu F , Wu L , Yang X 2006 Mechanism of the enhanced degradation of pentachlorophenol by ultra-sound in the presence of elemental iron. J. Hazard. Mater. 137 1424 - 1429    DOI : 10.1016/j.jhazmat.2006.04.025
Tamer E , Hamid Z , Aly AM , Ossama ET , Bo M , Benoit G 2006 Se-quential UV-biological degradation of chlorophenols. Che-mosphere 63 277 - 284    DOI : 10.1016/j.chemosphere.2005.07.022
Dabo P , Cyr A , Laplante F , Jean F , Menard H , Lessard J 2000 Elec-trocatalytic dehydrochlorination of pentachlorophenol to phenol or cyclohexanol. Environ. Sci. Technol. 34 1265 - 1268    DOI : 10.1021/es9911465
De AK , Dutta BK , Bhattacharjee S 2006 Reaction kinetics for the degradation of phenol and chlorinated phenols using fenton's reagent. Environ. Prog. 25 64 - 71    DOI : 10.1002/ep.10104
Yang CF , Lee CM 2008 Pentachlorophenol contaminated ground-water bioremediation using immobilized Sphingomonas cells inoculation in the bioreactor system. J. Hazard. Mater. 152 159 - 165    DOI : 10.1016/j.jhazmat.2007.06.102
Singh S , Chandra R , Patel DK , Reddy MM , Rai V 2008 Investiga-tion of the biotransformation of pentachlorophenol and pulp paper mill effluent decolorisation by the bacterial strains in a mixed culture. Bioresour. Technol. 99 5703 - 5709    DOI : 10.1016/j.biortech.2007.10.022
Van Nooten T , Springael D , Bastiaens L 2008 Positive impact of microorganisms on the performance of laboratory-scale permeable reactive iron barriers. Environ. Sci. Technol. 42 1680 - 1686    DOI : 10.1021/es071760d
Headley JV , Peru KM , Du JL , Gurprasad N , McMartin DW 2008 Evaluation of the apparent phytodegradation of pentachlo-rophenol by Chlorella pyrenoidosa. J. Environ. Sci. Health A. Toxic. Hazard. Subst. Environ. Eng. 43 361 - 364    DOI : 10.1080/10934520701795491
Morales J , Hutcheson R , Cheng IF 2002 Dechlorination of chlo-rinated phenols by catalyzed and uncatalyzed Fe(0) and Mg(0) particles. J. Hazard. Mater. 90 97 - 108    DOI : 10.1016/S0304-3894(01)00336-3
Kim YH , Carraway ER 2000 Dechlorination of pentachlorophe-nol by zero valent iron and modified zero valent irons. Envi-ron. Sci. Technol. 34 2014 - 2017    DOI : 10.1021/es991129f
Patel UD , Suresh S 2008 Effects of solvent pH salts and resin fatty acids on the dechlorination of pentachlorophenol us-ing magnesium-silver and magnesium-palladium bimetal-lic systems. J. Hazard. Mater. 156 308 - 316    DOI : 10.1016/j.jhazmat.2007.12.021
Choi JH , Choi SJ , Kim YH 2008 Hydrodechlorination of 246-tri-chlorophenol for a permeable reactive barrier using ze-ro-valent iron and catalyzed iron. Korean J. Chem. Eng. 25 493 - 500    DOI : 10.1007/s11814-008-0083-5
Choi JH , Kim YH 2009 Reduction of 246-trichlorophenol with zero-valent zinc and catalyzed zinc. J. Hazard. Mater. 166 984 - 991    DOI : 10.1016/j.jhazmat.2008.12.004
Marshall WD , Kubatova A , Lagadec AJ , Miller DJ , Hawthorne SB 2002 Zero-valent metal accelerators for the dechlorination of pentachlorophenol (PCP) in subcritical water. Green Chem. 4 17 - 23    DOI : 10.1039/b108337f
Cheng R , et al. , Zhou W , et al. , Wang JL , et al. 2010 Dechlorination of penta-chlorophenol using nanoscale Fe/Ni particles: role of nano-Ni and its size effect. J. Hazard. Mater. et al. 180 79 - 85    DOI : 10.1016/j.jhazmat.2010.03.068
Estevinho BN , Ratola N , Alves A , Santos L 2006 Pentachlorophe-nol removal from aqueous matrices by sorption with al-mond shell residues. J. Hazard. Mater. 137 1175 - 1181    DOI : 10.1016/j.jhazmat.2006.04.001
Estevinho BN , Martins I , Ratola N , Alves A , Santos L 2007 Re-moval of 24-dichlorophenol and pentachlorophenol from waters by sorption using coal fly ash from a Portuguese thermal power plant. J. Hazard. Mater. 143 535 - 540    DOI : 10.1016/j.jhazmat.2006.09.072
Deng S , Ma R , Yu Q , Huang J , Yu G 2008 Enhanced removal of pentachlorophenol and 24-D from aqueous solution by an aminated biosorbent. J. Hazard. Mater.
Mathialagan T , Viraraghavan T 2009 Biosorption of pentachloro-phenol from aqueous solutions by a fungal biomass. Biore-sour. Technol. 100 549 - 558    DOI : 10.1016/j.biortech.2008.06.054
Jou CJ 2008 Degradation of pentachlorophenol with zero-va-lence iron coupled with microwave energy. J. Hazard. Mater. 152 699 - 702    DOI : 10.1016/j.jhazmat.2007.07.036
Zhang W , Quan X , Wang J , Zhang Z , Chen S 2006 Rapid and com-plete dechlorination of PCP in aqueous solution using Ni-Fe nanoparticles under assistance of ultrasound. Chemosphere 65 58 - 64    DOI : 10.1016/j.chemosphere.2006.02.060
Lee SH , Carberry JB 1992 Biodegradation of PCP enhanced by chemical oxidation pretreatment. Water Environ. Res 64 682 - 690    DOI : 10.2175/WER.64.5.4
Choi JH , Kim YH , Choi SJ 2007 Reductive dechlorination and biodegradation of 246-trichlorophenol using sequential permeable reactive barriers: laboratory studies. Chemosphere 67 1551 - 1557    DOI : 10.1016/j.chemosphere.2006.12.029
Chen YC , Lan HX , Zhan HY , Fu SY 2005 Simultaneous anaero-bic-aerobic biodegradation of halogenated phenolic com-pound under oxygen-limited conditions. J. Environ. Sci. 17 873 - 875
Bokare AD , Choi W 2009 Zero-valent aluminum for oxidative degradation of aqueous organic pollutants. Environ. Sci. Technol. 43 7130 - 7135    DOI : 10.1021/es9013823
Boronina T , Klabunde KJ , Sergeev G 1995 Destruction of organo-halides in water using metal particles: carbon tetrachloride/water reactions with magnesium tin and zinc. Environ. Sci. Technol. 29 1511 - 1517    DOI : 10.1021/es00006a012
Arning MD , Minteer SD , Zoski CG 2007 Electrode potentials. In: Handbook of electrochemistry. Elsevier Boston 813 - 827
Speight JG 2005 Lange's handbook of chemistry. 16th ed. McGraw-Hill New York 1572 -
Zhang WX , Wang CB , Lien HL 1998 Treatment of chlorinated organic contaminants with nanoscale bimetallic particles. Catal. Today 40 387 - 395    DOI : 10.1016/S0920-5861(98)00067-4
Gavaskar AR 1999 Design and construction techniques for per-meable reactive barriers. J. Hazard. Mater. 68 41 - 71    DOI : 10.1016/S0304-3894(99)00031-X
Henderson AD , Demond AH 2007 Long-term performance of ze-ro-valent iron permeable reactive barriers: a critical review. Environ. Eng. Sci. 24 401 - 423    DOI : 10.1089/ees.2006.0071
Thiruvenkatachari R , Vigneswaran S , Naidu R 2008 Permeable reactive barrier for groundwater remediation. J. Ind. Eng. Chem. 14 145 - 156
Gillham RW , Ohannesin SF 1994 Enhanced degradation of ha-logenated aliphatics by zero valent iron. Ground Water 32 958 - 967    DOI : 10.1111/j.1745-6584.1994.tb00935.x
Matheson LJ , Tratnyek PG 1994 Reductive dehalogenation of chlorinated methanes by iron metal. Environ. Sci. Technol. 28 2045 - 2053    DOI : 10.1021/es00061a012
Johnson TL , Scherer MM , Tratnyek PG 1996 Kinetics of haloge-nated organic compound degradation by iron metal. Envi-ron. Sci. Technol. 30 2634 - 2640    DOI : 10.1021/es9600901
Lien HL , Zhang WX 2001 Nanoscale iron particles for complete reduction of chlorinated ethenes. Colloids Surf. A. Physico-chem. Eng. Asp. 191 97 - 105    DOI : 10.1016/S0927-7757(01)00767-1
McDowall L 2005 Degradation of toxic chemicals by zero-valent metal nanoparticles--a literature review. Defence Science and Technology Organisation Australia
Ko SO , Lee DH , Kim YH 2007 Kinetic studies of reductive dechlo-rination of chlorophenols with Ni/Fe bimetallic particles. Environ. Technol. 28 583 - 593    DOI : 10.1080/09593332808618818
Wei J , Xu X , Liu Y , Wang D 2006 Catalytic hydrodechlorina-tion of 24-dichlorophenol over nanoscale Pd/Fe: reaction pathway and some experimental parameters. Water Res. 40 348 - 354    DOI : 10.1016/j.watres.2005.10.017
Liu Y , Yang F , Yue PL , Chen G 2001 Catalytic dechlorination of chlorophenols in water by palladium/iron. Water Res. 35 1887 - 1890    DOI : 10.1016/S0043-1354(00)00463-2
Zhou T , Li Y , Lim TT 2010 Catalytic hydrodechlorination of chlo-rophenols by Pd/Fe nanoparticles: comparisons with other bimetallic systems kinetics and mechanism. Sep. Purif. Technol. 76 206 - 214    DOI : 10.1016/j.seppur.2010.10.010
Tong SP , Wei H , Ma CA , Liu WP 2005 Rapid dechlorination of chlorinated organic compounds by nickel/iron bimetallic system in water. J. Zhejiang Univ. Science 6A 627 - 631    DOI : 10.1631/jzus.2005.A0627
Jovanovic GN , Plazl PŽ , Sakrittichai P , Al-Khaldi K 2004 Dechlori-nation of p-chlorophenol in a microreactor with bimetallic Pd/Fe catalyst. Ind. Eng. Chem. Res. 44 5099 - 5106
Arnold WA , Roberts AL 2000 Pathways and kinetics of chlorinat-ed ethylene and chlorinated acetylene reaction with Fe(0) particles. Environ. Sci. Technol. 34 1794 - 1805    DOI : 10.1021/es990884q
Schlicker O , Ebert M , Fruth M , Weidner M , Wüst W , Dahmke A 2000 Degradation of TCE with iron: the role of competing chromate and nitrate reduction. Ground Water 38 403 - 409    DOI : 10.1111/j.1745-6584.2000.tb00226.x
Chen JL , Al-Abed SR , Ryan JA , Li Z 2001 Effects of pH on dechlo-rination of trichloroethylene by zero-valent iron. J. Hazard. Mater. 83 243 - 254    DOI : 10.1016/S0304-3894(01)00193-5
Geiger Cherie L , Carvalho-Knighton K , Novaes-Card S , Ma-loney P , DeVor R 2009 A review of environmental applications of nanoscale and microscale reactive metal particles. ACS Symp. Ser. 1027 1 - 20
Cho HH , Park JW 2005 Effect of coexisting compounds on the sorption and reduction of trichloroethylene with iron. En-viron. Toxicol. Chem. 24 11 - 16    DOI : 10.1897/04-051R.1
Kim YH 1999 Reductive dechlorination of chlorinated aliphatic and aromatic compounds using zero valent metals: modified metals and electron medi-ators Texas A&M University College Station
Cheng R , Wang Jl , Zhang WX 2007 Comparison of reductive de-chlorination of p-chlorophenol using Fe0 and nanosized Fe0. J. Hazard. Mater. 144 334 - 339    DOI : 10.1016/j.jhazmat.2006.10.032
Noubactep C , Caré S 2010 On nanoscale metallic iron for ground-water remediation. J. Hazard. Mater. 182 923 - 927    DOI : 10.1016/j.jhazmat.2010.06.009
Lim TT , Zhu BW 2009 Practical applications of bimetallic na-noiron particles for reductive dehalogenation of haloorgan-ics: prospects and challenges. ACS Symp. Ser. 1027 245 - 261
Burris DR , Allen-King RM , Manoranjan VS , Campbell TJ , Lo-raine GA , Deng B 1998 Chlorinated ethene reduction by cast iron: sorption and mass transfer. J. Environ. Eng. 124 1012 - 1019    DOI : 10.1061/(ASCE)0733-9372(1998)124:10(1012)
Deng B , Hu S , Whitworth TM , Lee R 2003 Trichloroethylene re-duction on zero valent iron: probing reactive versus nonre-active sites. ACS Symp. Ser. 837 181 - 205
Bi E , Devlin JF , Huang B , Firdous R 2010 Transport and kinetic studies To characterize reactive and nonreactive sites on granular iron. Environ. Sci. Technol. 44 5564 - 5569    DOI : 10.1021/es101012p
Burris DR , Campbell TJ , Manoranjan VS 1995 Sorption of tri-chloroethylene and tetrachloroethylene in a batch reac-tive metallic iron-water system. Environ. Sci. Technol. 29 2850 - 2855    DOI : 10.1021/es00011a022
Gotpagar J , Lyuksyutov S , Cohn R , Grulke E , Bhattacha-ryya D 1999 Reductive dehalogenation of trichloroethylene with zero-valent iron: surface profiling microscopy and rate en-hancement studies. Langmuir 15 8412 - 8420    DOI : 10.1021/la990325x
Noubactep C 2008 A critical review on the process of con-taminant removal in Fe 0-H2O systems. Environ. Technol. 29 909 - 920    DOI : 10.1080/09593330802131602
Weber EJ 1996 Iron-mediated reductive transformations: in-vestigation of reaction mechanism. Environ. Sci. Technol. 30 716 - 719    DOI : 10.1021/es9505210
Su C , Puls RW 1999 Kinetics of trichloroethene reduction by ze-rovalent iron and tin: pretreatment effect apparent activa-tion energy and intermediate products. Environ. Sci. Tech-nol. 33 163 - 168    DOI : 10.1021/es980481a
Deng B , Burris DR , Campbell TJ 1999 Reduction of vinyl chlo-ride in metallic iron-water systems. Environ. Sci. Technol. 33 2651 - 2656    DOI : 10.1021/es980554q
Xu X , Zhou M , He P , Hao Z 2005 Catalytic reduction of chlori-nated and recalcitrant compounds in contaminated water. J. Hazard. Mater. 123 89 - 93    DOI : 10.1016/j.jhazmat.2005.04.002
Doong RA , Wu SC 1992 Reductive dechlorination of chlorinated hydrocarbons in aqueous solutions containing ferrous and sulfide ions. Chemosphere 24 1063 - 1075    DOI : 10.1016/0045-6535(92)90197-Y
Wang J , Farrell J 2003 Investigating the role of atomic hydrogen on chloroethene reactions with iron using tafel analysis and electrochemical impedance spectroscopy. Environ. Sci. Technol. 37 3891 - 3896    DOI : 10.1021/es0264605
Li T , Farrell J 2002 Mechanisms controlling chlorocarbon reduc-tion at iron surfaces. ACS Symp. Ser. 806 397 - 410
Kim JS , Shea PJ , Yang JE , Kim JE 2007 Halide salts accelerate deg-radation of high explosives by zerovalent iron. Environ. Pol-lut. 147 634 - 641    DOI : 10.1016/j.envpol.2006.10.010
Fontana MG , Greene ND 1978 Corrosion engineering. 2nd ed. McGraw-Hill New York
Jones DA 1996 Principles and prevention of corrosion. 2nd ed. Prentice Hall Upper Saddle River
Choi JH , Choi SJ , Kim YH 2008 Liquid-liquid extraction methods to determine reductive dechlorination of 246-trichloro-phenol by zero-valent metals and zero-valent bimetals. Sep. Sci. Technol. 43 3624 - 3636    DOI : 10.1080/01496390802219067
Bandara J , Mielczarski JA , Kiwi J 2001 I. Adsorption mechanism of chlorophenols on iron oxides titanium oxide and alu-minum oxide as detected by infrared spectroscopy. Appl. Catal. B. Environ. 34 307 - 320    DOI : 10.1016/S0926-3373(01)00224-7
Kung KH , McBride MB 1991 Bonding of chlorophenols on iron and aluminum oxides. Environ. Sci. Technol. 25 702 - 709    DOI : 10.1021/es00016a015
Noubactep C 2010 The fundamental mechanism of aqueous contaminant removal by metallic iron. Water SA 36 663 - 670
Noubactep C 2007 Processes of contaminant removal in “Fe0-H2O” systems revisited: the importance of co-precipitation Open Environ. J. 1 9 - 13    DOI : 10.2174/1874233500701010009
U.S. Environmental Protection Agency. 1998 Permeable reactive barrier technologies for contaminant remediation. U.S. Environmental Protection Agency Wash-ington DC
Farrell J , Kason M , Melitas N , Li T 2000 Investigation of the long-term performance of zero-valent iron for reductive dechlorination of trichloroethylene. Environ. Sci. Technol. 34 514 - 521    DOI : 10.1021/es990716y
Huang YH , Zhang TC , Shea PJ , Comfort SD 2003 Effects of oxide coating and selected cations on nitrate reduction by iron metal. J. Environ. Qual. 32 1306 - 1315    DOI : 10.2134/jeq2003.1306
Satapanajaru T , Comfort SD , Shea PJ 2003 Enhancing metola-chlor destruction rates with aluminum and iron salts during zerovalent iron treatment. J. Environ. Qual. 32 1726 - 1734    DOI : 10.2134/jeq2003.1726
Ritter K , Odziemkowski MS , Simpgraga R , Gillham RW , Irish DE 2003 An in situ study of the effect of nitrate on the reduction of trichloroethylene by granular iron. J. Contam. Hydrol. 65 121 - 136    DOI : 10.1016/S0169-7722(02)00234-6
Kiser JR , Manning BA 2010 Reduction and immobilization of chromium(VI) by iron(II)-treated faujasite. J. Hazard. Mater. 174 167 - 174    DOI : 10.1016/j.jhazmat.2009.09.032
Schrick B , Blough JL , Jones AD , Mallouk TE 2002 Hydrodechlo-rination of trichloroethylene to hydrocarbons using bime-tallic nickel-iron nanoparticles. Chem. Mater. 14 5140 - 5147    DOI : 10.1021/cm020737i
Patel UD , Suresh S 2007 Dechlorination of chlorophenols using magnesium-palladium bimetallic system. J. Hazard. Mater. 147 431 - 438    DOI : 10.1016/j.jhazmat.2007.01.029
Chen LH , Huang CC , Lien HL 2008 Bimetallic iron-aluminum particles for dechlorination of carbon tetrachloride. Che-mosphere 73 692 - 697    DOI : 10.1016/j.chemosphere.2008.07.005
Wang X , Chen C , Liu H , Ma J 2008 Characterization and evalua-tion of catalytic dechlorination activity of Pd/Fe bimetallic nanoparticles. Ind. Eng. Chem. Res. 47 8645 - 8651    DOI : 10.1021/ie701762d
Elliott DW , Zhang WX 2001 Field assessment of nanoscale bi-metallic particles for groundwater treatment. Environ. Sci. Technol. 35 4922 - 4926    DOI : 10.1021/es0108584
Muftikian R , Fernando Q , Korte N 1995 A method for the rapid dechlorination of low molecular weight chlorinated hydro-carbons in water. Water Res. 29 2434 - 2439    DOI : 10.1016/0043-1354(95)00102-Q
Li T , Farrell J 2000 Reductive dechlorination of trichloroethene and carbon tetrachloride using iron and palladized-iron cathodes. Environ. Sci. Technol. 34 173 - 179    DOI : 10.1021/es9907358
Agarwal S , Al-Abed SR , Dionysiou DD 2007 Enhanced corrosion-based Pd/Mg bimetallic systems for dechlorination of PCBs. Environ. Sci. Technol. 41 3722 - 3727    DOI : 10.1021/es062886y
Cheng SF , Wu SC 2000 The enhancement methods for the degradation of TCE by zero-valent metals. Chemosphere 41 1263 - 1270    DOI : 10.1016/S0045-6535(99)00530-5
Cheng SF , Wu SC 2001 Feasibility of using metals to remediate water containing TCE. Chemosphere 43 1023 - 1028    DOI : 10.1016/S0045-6535(00)00263-0
Cheng IF , Fernando Q , Korte N 1997 Electrochemical dechlori-nation of 4-chlorophenol to phenol. Environ. Sci. Technol. 31 1074 - 1078    DOI : 10.1021/es960602b
Wang CB , Zhang WX 1997 Synthesizing nanoscale iron particles for rapid and complete dechlorination of TCE and PCBs. Environ. Sci. Technol. 31 2154 - 2156    DOI : 10.1021/es970039c
Xu Y , Zhang WX 2000 Subcolloidal Fe/Ag particles for reductive dehalogenation of chlorinated benzenes. Ind. Eng. Chem. Res. 39 2238 - 2244    DOI : 10.1021/ie9903588
Lin CJ , Lo SL , Liou YH 2004 Dechlorination of trichloroethylene in aqueous solution by noble metal-modified iron. J. Haz-ard. Mater. 116 219 - 228    DOI : 10.1016/j.jhazmat.2004.09.005
Cwiertny DM , Bransfield SJ , Roberts AL 2007 Influence of the oxidizing species on the reactivity of iron-based bimetallic reductants. Environ. Sci. Technol. 41 3734 - 3740    DOI : 10.1021/es062993s
Bransfield SJ , Cwiertny DM , Roberts AL , Fairbrother DH 2006 Influence of copper loading and surface coverage on the reactivity of granular iron toward 111-trichloroethane. En-viron. Sci. Technol. 40 1485 - 1490    DOI : 10.1021/es051300p
Graham LJ , Jovanovic G 1999 Dechlorination of p-chlorophenol on a Pd/Fe catalyst in a magnetically stabilized fluidized bed: implications for sludge and liquid remediation. Chem. Eng. Sci. 54 3085 - 3093    DOI : 10.1016/S0009-2509(98)00393-5
Tian H , Li J , Mu Z , Li L , Hao Z 2009 Effect of pH on DDT degra-dation in aqueous solution using bimetallic Ni/Fe nanopar-ticles. Sep. Purif. Technol. 66 84 - 89    DOI : 10.1016/j.seppur.2008.11.018
Cwiertny DM , Bransfield SJ , Livi KJ , Fairbrother DH , Rob-erts AL 2006 Exploring the influence of granular iron additives on 111-trichloroethane reduction. Environ. Sci. Technol. 40 6837 - 6843    DOI : 10.1021/es060921v
Hoke JB , Gramiccioni GA , Balko EN 1992 Catalytic hydrode-chlorination of chlorophenols. Appl. Catal. B. Environ. 1 285 - 296    DOI : 10.1016/0926-3373(92)80054-4
Patel U , Suresh S 2006 Dechlorination of chlorophenols by magnesium-silver bimetallic system. J. Colloid Interface Sci. 299 249 - 259    DOI : 10.1016/j.jcis.2006.01.047
Yuan G , Keane MA 2003 Catalyst deactivation during the liq-uid phase hydrodechlorination of 24-dichlorophenol over supported Pd: influence of the support. Catal. Today 88 27 - 36
Noubactep C 2010 The suitability of metallic iron for envi-ronmental remediation. Environ. Progr. Sustain. Energ. 29 286 - 291    DOI : 10.1002/ep.10406
Odziemkowski MS , Schuhmacher TT , Gillham RW , Reardon EJ 1998 Mechanism of oxide film formation on iron in simulating groundwater solutions: raman spectroscopic studies. Cor-ros. Sci. 40 371 - 389    DOI : 10.1016/S0010-938X(97)00141-8
Noubactep C , Schöner A 2010 Metallic iron for environmental remediation: learning from electrocoagulation. J. Hazard. Mater. 175 1075 - 1080    DOI : 10.1016/j.jhazmat.2009.09.152
Furukawa Y , Kim JW , Watkins J , Wilkin RT 2002 Formation of fer-rihydrite and associated iron corrosion products in perme-able reactive barriers of zero-valent iron. Environ. Sci. Tech-nol. 36 5469 - 5475    DOI : 10.1021/es025533h
Scherer MM , Balko BA , Tratnyek PG 1999 The role of oxides in reduction reactions at the metal-water interface. ACS Symp. Ser. 715 301 - 322
Erbs M , Bruun Hansen HC , Olsen CE 1998 Reductive dechlorina-tion of carbon tetrachloride using iron(II) iron(III) hydrox-ide sulfate (green rust). Environ. Sci. Technol. 33 307 - 311
Blowes DW , Ptacek CJ , Benner SG , McRae CW , Bennett TA , Puls RW 2000 Treatment of inorganic contaminants using per-meable reactive barriers. J. Contam. Hydrol. 45 123 - 137    DOI : 10.1016/S0169-7722(00)00122-4
Gu B , et al. , Phelps TJ , et al. , Liang L , et al. 1999 Biogeochemical dynamics in zero-valent iron columns:implications for permeable reac-tive barriers. Environ. Sci. Technol. et al. 33 2170 - 2177    DOI : 10.1021/es981077e
Roh Y , Lee SY , Elless MP 2000 Characterization of corrosion products in the permeable reactive barriers. Environ. Geol. 40 184 - 194    DOI : 10.1007/s002540000178
Kamolpornwijit W , Liang L , Moline GR , Hart T , West OR 2004 Identification and quantification of mineral precipitation in Fe 0 filings from a column study. Environ. Sci. Technol. 38 5757 - 5765    DOI : 10.1021/es035085t
Phillips DH , et al. , Nooten TV , et al. , Bastiaens L , et al. 2010 Ten year per-formance evaluation of a field-scale zero-valent iron per-meable reactive barrier installed to remediate trichloro-ethene contaminated groundwater. Environ. Sci. Technol. et al. 44 3861 - 3869    DOI : 10.1021/es902737t
Kohn T , Livi KJ , Roberts AL , Vikesland PJ 2005 Longevity of gran-ular iron in groundwater treatment processes: corrosion product development. Environ. Sci. Technol. 39 2867 - 2879    DOI : 10.1021/es048851k
Hernandez R 2002 Integration of zero-valent metals and chemi-cal oxidation for the destruction of 246 trinitrotoluene within aqueous matrices Missis-sippi State University Mississippi
Balasubramaniam R , Ramesh Kumar AV , Dillmann P 2003 Characterization of rust on ancient Indian iron. Curr. Sci. 85 1546 - 1555
Cornell RM , Schwertmann U 2003 The iron oxides structure properties reactions occurrences and uses. 2nd ed. Wiley-VCH Wein-heim 664 -
Brown GE , et al. , Henrich VE , et al. , Casey WH , et al. 1998 Metal oxide surfac-es and their interactions with aqueous solutions and micro-bial organisms. Chem. Rev. et al. 99 77 - 174
Johnson TL , Fish W , Gorby YA , Tratnyek PG 1998 Degradation of carbon tetrachloride by iron metal: complexation effects on the oxide surface. J. Contam. Hydrol. 29 379 - 398    DOI : 10.1016/S0169-7722(97)00063-6
Ritter K , Odziemkowski MS , Gillham RW 2002 An in situ study of the role of surface films on granular iron in the permeable iron wall technology. J. Contam. Hydrol. 55 87 - 111    DOI : 10.1016/S0169-7722(01)00187-5
Helland BR , Alvarez PJ , Schnoor JL 1995 Reductive dechlorina-tion of carbon tetrachloride with elemental iron. J. Hazard. Mater. 41 205 - 216    DOI : 10.1016/0304-3894(94)00111-S
Hansen HC , Koch CB , Nancke-Krogh H , Borggaard OK , Sø-rensen J 1996 Abiotic nitrate reduction to ammonium: key role of green rust. Environ. Sci. Technol. 30 2053 - 2056    DOI : 10.1021/es950844w
Liu CC , Tseng DH , Wang CY 2006 Effects of ferrous ions on the re-ductive dechlorination of trichloroethylene by zero-valent iron. J. Hazard. Mater. 136 706 - 713    DOI : 10.1016/j.jhazmat.2005.12.045
Davenport AJ , Oblonsky LJ , Ryan MP , Toney MF 2000 The struc-ture of the passive film that forms on iron in aqueous envi-ronments. J. Electrochem. Soc. 147 2162 - 2173    DOI : 10.1149/1.1393502
Farrell J , Melitas N , Kason M , Li T 2000 Electrochemical and col-umn investigation of iron-mediated reductive dechlorina-tion of trichloroethylene and perchloroethylene. Environ. Sci. Technol. 34 2549 - 2556    DOI : 10.1021/es991135b
Myneni SC , Tokunaga TK , Brown GE 1997 Abiotic selenium re-dox transformations in the presence of Fe(IIIII) oxides. Sci-ence 278 1106 - 1109    DOI : 10.1126/science.278.5340.1106
Benali O , Abdelmoula M , Refait P , Génin JM 2001 Effect of or-thophosphate on the oxidation products of Fe(II)-Fe(III) hydroxycarbonate: the transformation of green rust to fer-rihydrite. Geochim. Cosmochim. Acta 65 1715 - 1726    DOI : 10.1016/S0016-7037(01)00556-7
Danielsen KM , Hayes KF 2004 pH dependence of carbon tetra-chloride reductive dechlorination by magnetite. Environ. Sci. Technol. 38 4745 - 4752    DOI : 10.1021/es0496874
Vikesland PJ , Heathcock AM , Rebodos RL , Makus KE 2007 Particle size and aggregation effects on magnetite reac-tivity toward carbon tetrachloride. Environ. Sci. Technol. 41 5277 - 5283    DOI : 10.1021/es062082i
Xue X , Hanna K , Abdelmoula M , Deng N 2009 Adsorption and oxidation of PCP on the surface of magnetite: kinetic experi-ments and spectroscopic investigations. Appl. Catal. B. En-viron. 89 432 - 440    DOI : 10.1016/j.apcatb.2008.12.024
Amonette JE , Workman DJ , Kennedy DW , Fruchter JS , Gorby YA 2000 Dechlorination of carbon tetrachloride by Fe(II) associ-ated with goethite. Environ. Sci. Technol. 34 4606 - 4613    DOI : 10.1021/es9913582
Junyapoon S 2005 Use of zero-valent iron for wastewater treat-ment. KMITL Sci. Tech. J. 5 587 - 595
Ghauch A , Tuqan A 2009 Reductive destruction and decon-tamination of aqueous solutions of chlorinated antimi-crobial agent using bimetallic systems J. Hazard. Mater. 164 665 - 674    DOI : 10.1016/j.jhazmat.2008.08.048
Liu T , Tsang DC , Lo IM 2008 Chromium(VI) reduction kinetics by zero-valent iron in moderately hard water with humic acid: iron dissolution and humic acid adsorption. Environ. Sci. Technol. 42 2092 - 2098    DOI : 10.1021/es072059c
Tsang DC , Graham NJ , Lo IM 2009 Humic acid aggregation in zero-valent iron systems and its effects on trichloroethylene removal. Chemosphere 75 1338 - 1343    DOI : 10.1016/j.chemosphere.2009.02.058
Riley RG , Zachara JM 1992 Chemical contaminants on DOE lands and selection of contaminant mixtures for subsurface science research. U.S. Department of En-ergy Washington DC 77 -
Mackenzie PD , Horney DP , Sivavec TM 1999 Mineral precipita-tion and porosity losses in granular iron columns. J. Hazard. Mater. 68 1 - 17    DOI : 10.1016/S0304-3894(99)00029-1
Devlin JF , Allin KO 2005 Major anion effects on the kinetics and reactivity of granular iron in glass-encased magnet batch reactor experiments. Environ. Sci. Technol. 39 1868 - 1874    DOI : 10.1021/es040413q
D'Andrea P , Lai KC , Kjeldsen P , Lo IM 2005 Effect of groundwater inorganics on the reductive dechlorination of TCE by zero-valent iron. Water Air Soil Pollut. 162 401 - 420    DOI : 10.1007/s11270-005-7420-7