| 词条 | Green rust |
| 释义 |
Other varieties reported in the literature are bromide {{chem|Br|-}},[10] fluoride {{chem|F|-}},[10] iodide {{chem|I|-}},[14] nitrate {{chem|N|O|3|-}},[15] and selenate.[1] Green rust was first recognized as a corrosion crust on iron and steel surfaces.[2] It occurs in nature as the mineral fougerite.[1] StructureThe crystal structure of green rust can be understood as the result of inserting the foreign anions and water molecules between brucite-like layers of iron(II) hydroxide, {{chem|Fe}}({{chem|OH}})2. The latter has an hexagonal structure, with layer sequence AcBAcB... , where A and B are planes of hydroxide ions, and c those of {{chem|Fe|2+}} (iron(II), ferrous) cations. In the green rust, some {{chem|Fe|2+}} cations get oxidized to {{chem|Fe|3+}} (iron(III), ferric). Each triple layer AcB, which is electrically neutral in the hydroxide, becomes positively charged. The anions then intercalate between those triple layers and restore neutrality.[1] There are two basic structures of green rust, "type 1" and "type 2".[20] Type 1 is exemplified by the chloride and carbonate varieties. It has a rhombohedral crystal structure similar to that of pyroaurite. The layers are stacked in the sequence AcBiBaCjCbAkA ...; where A, B, and C represent {{chem|HO|-}} planes, a, b, and c are layers of mixed {{chem|Fe|2+}} and {{chem|Fe|3+}} cations, and i, j, and k are layers of the intercalated anions and water molecules.[1][22][23] The c crystallographic parameter is 22.5-22.8 Å for the carbonate, and about 24 Å for the chloride.[4] Type 2 green rust is exemplified by the sulfate variety. It has a hexagonal crystal structure, with layers probably stacked in the sequence AcBiAbCjA...[1][10][22] Chemical propertiesIn oxidizing environment, green rust generally turns into {{chem|Fe|3+}} oxyhydroxides, namely α-{{chem|Fe|O|OH}} (goethite) and γ-{{chem|Fe|O|OH}} (lepidocrocite).[22] Oxidation of the carbonate variety can be retarded by wetting the material with hydroxyl-containing compounds such as glycerol or glucose, even though they do not penetrate the structure.[3] Some variety of green rust is stabilized also by an atmosphere with high {{chem|C|O|2}} partial pressure.[3][31] Sulfate green rust has been shown to reduce nitrate {{chem|N|O|3|-}} and nitrite {{chem|N|O|2|-}} in solution to ammonium {{chem|N|H|4|+}}, with concurrent oxidation of {{chem|Fe|2+}} to {{chem|Fe|3+}}. Depending on the cations in the solution, the nitrate anions replaced the sulfate in the intercalation layer, before the reduction. It was conjectured that green rust may be formed in the reducing alkaline conditions below the surface of marine sediments and may be connected to the disappearance of oxidized species like nitrate in that environment.[32][33][34] Suspensions of carbonate green rust and orange γ-{{chem|Fe|O|OH}} in water will react over a few days produce a black precipitate of magnetite {{chem|Fe|3|O|4}}.[35] OccurrenceIron and steel corrosionGreen rust compounds were identified in green corrosion crusts that form on iron and steel surfaces, in alternating aerobic and anaerobic conditions, by water containing anions such as chloride, sulfate, carbonate, or bicarbonate.[2][4][11][20][22][41][42][43] They are believed to be intermediates in the oxidative corrosion of iron to form iron(III) oxyhydroxides (ordinary brown rust). The green rust may be formed either directly from metallic iron or from iron(II) hydroxide {{chem|Fe}}({{chem|OH}})2 .[4] SoilOn the basis of Mössbauer spectroscopic analysis, green rust minerals are suspected to occur as minerals in certain bluish-green soils that are formed in alternating redox conditions, and turn ochre once exposed to air.[45][46][47][48] The green rust has been conjectured to be present in the form of the mineral fougerite.[5] Biologically mediated formationHexagonal crystals of green rust (carbonate and/or sulfate) have also been obtained as a byproducts of bioreduction of ferric oxyhydroxides by dissimilatory iron-reducing bacteria, such as Shewanella putrefaciens, that couple the reduction of {{chem|Fe|3+}} with the oxidation of organic matter.[50] This process has been conjectured to occur in soil solutions and aquifers.[35] In one experiment, a 160 mM suspension of orange lepidocrocite γ-{{chem|Fe|O|O|H}} in a solution containing formate ({{chem|H|C|O|2|-}}), incubated for 3 days with a culture of S. putrefaciens, turned dark green due to the conversion of the hydroxide to GR({{chem|C|O|3|2-}}), in the form of hexagonal platelets with diameter ~7 µm. In this process, the formate was oxidized to bicarbonate {{chem|H|C|O|3|-}} which provided the carbonate anions for the formation of the green rust. The live bacteria were shown to be necessary for the formation of the green rust.[35] Laboratory preparationAir oxidation methodsGreen rust compounds can be synthesized at ordinary ambient temperature and pressure, from solutions containing iron(II) cations, hydroxide anions, and the appropriate intercalatory anions, such as chloride,[8][54][55][56] sulfate,[57][58][59][60] or carbonate.[61] The result is a suspension of ferrous hydroxide {{chem|Fe}}({{chem|OH}})2 in a solution of the third anion. This suspension is oxidized by stirring in air, or bubbling air through it.[47] Since the product is very prone to oxidation, it is necessary to monitor the process and exclude oxygen once the desired ratio of {{chem|Fe|2+}} and {{chem|Fe|3+}} is achieved.[3] One method first combines an iron(II) salt with sodium hydroxide {{chem|Na|O|H}} to form the ferrous hydroxide suspension. Then the sodium salt of the third anion is added, and the suspension is oxidized by stirring in air.[3][47][66] For example, carbonate green rust can be prepared by mixing solutions of iron(II) sulfate {{chem|Fe|S|O|4}} and sodium hydroxide; then adding sufficient amount of sodium carbonate {{chem|Na|2|C|O|3}} solution, followed by the air oxidation step.[66] Sulfate green rust can be obtained by mixing solutions of {{chem|Fe|Cl|2}}·4{{chem|H|2|O}} and {{chem|Na|O|H}} to precipitate {{chem|Fe}}({{chem|O|H}})2 then immediately adding sodium sulfate {{chem|Na|2|S|O|4}} and proceeding to the air oxidation step.[11][60] A more direct method combines a solution of iron(II) sulfate {{chem|Fe|S|O|4}} with {{chem|Na|O|H}}, and proceeding to the oxidizing step.[34] The suspension must have a slight excess of {{chem|Fe|S|O|4}} (in the ratio of 0.5833 {{chem|Fe|2+}} for each {{chem|HO|-}}) for the green rust to form; however, too much of it will produce instead an insoluble basic iron sulfate, iron(II) sulfate hydroxide {{chem|Fe|2|S|O|4}}({{chem|OH}})2·n{{chem|H|2|O}}.[58] The production of green rust is reduced as temperature increases.[72] Stoichometric Fe(II) - Fe(III) methodsAn alternate preparation of carbonate green rust first creates a suspension of iron(III) hydroxide {{chem|Fe}}({{chem|O|H}})3 in an iron(II) chloride {{chem|Fe|Cl|2}} solution, and bubbles carbon dioxide through it.[3] In a more recent variant, solutions of both iron(II) and iron(III) salts are first mixed, then a solution of {{chem|Na|OH}} is added, all in the stoichometric proportions of the desired green rust. No oxidation step is then necessary.[60] ElectrochemistryCarbonate green rust films have also been obtained from the electrochemical oxidation of iron plates.[61] ReferencesUnspecifc references:[76][77] 1 : Corrosion |
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