Über Orthoferrate(IV)

Scholder, R.; Bunsen, H. v.; Zeiss, W.

doi:10.1002/zaac.19562830132

Cited by 31 publications

(19 citation statements)

References 5 publications

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“…In 1956, Scholder et al (9) have disclosed the existence of Na FeO , synthesized by annealing a mixture of sodium oxide Na O and Fe O for 30 min at 1503C and 1 h at 4503C, under a stream of, dried and carbon dioxide free, oxygen. Neither physical properties nor structural characterization are reported and the authors only noted that Na FeO is extremely hygroscopic and quickly decomposes in air.…”

Section: Introductionmentioning

confidence: 99%

Synthesis, Crystal and Magnetic Structures of the Sodium Ferrate (IV) Na4FeO4 Studied by Neutron Diffraction and Mössbauer Techniques

Jeannot

Malaman

Gerardin

et al. 2002

Journal of Solid State Chemistry

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Section: Introductionmentioning

confidence: 99%

Synthesis, Crystal and Magnetic Structures of the Sodium Ferrate (IV) Na4FeO4 Studied by Neutron Diffraction and Mössbauer Techniques

Jeannot

Malaman

Gerardin

et al. 2002

Journal of Solid State Chemistry

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“…The temperature dependence of the conductivities is characterized by a weakly activated lowtemperature and a stronger activated high-temperature region. The electronic properties of the title system are interpreted in terms of a collective electronic state which is determined by strong correlation effects associated with the ( *) 3 ( *) 1 configuration of Fe 4؉ and a pronounced tendency to delocalize the * electrons arising from the strong covalency of iron-oxygen bonding.…”

mentioning

confidence: 99%

Electronic State, Magnetism, and Electrical Transport Behavior of Sr3−xAxFe2O7(x≤0.4,A=Ba, La)

Adler

1997

Journal of Solid State Chemistry

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“…In recent years, iron with +6 oxidation state (Fe(VI)), commonly called ferrate (Fe VI O 4 2-), has received much attention because of its usefulness in organic synthesis and "super-iron" batteries (Delaude and Laszlo, 1996;Sharma, 2002aLicht et al, 2002). In the laboratory, Fe(VI) can be produced by three types of synthetic techniques; a dry method, heating of various potassium-and iron containing minerals (Scholder et al, 1956;Scholder, 1962); electrolyzing an alkaline solution with an iron anode (Bouzek et al, 2000); and a wet method oxidizing a basic solution of Fe(III) salt by hypochlorite (Thompson et al, 1951).…”

Section: Iron(vi)mentioning

confidence: 99%

Use of Iron(VI) and Iron(V) as Oxidants and Disinfectants in Water Treatment

Sharma¹

2005

proc water environ fed

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A technology involving environmentally friendly oxidants, ferrates (Fe(VI), Fe VI O 4 2-and Fe(V), (Fe V O 4 3-)) can meet criteria of water treatment. Fe(VI) and Fe(V) have high oxidizing power, selectivity, and upon decomposition produce a non-toxic by-product, Fe(III). Fe(VI) is easily be prepared by oxidizing Fe(III) by hypochlorite in alkaline medium. Fe(V) is produced by oneelectron reduction of Fe(VI) using three different methods: chemical (e.g. Fe(II)), electron beam (eaq ), and photocatalytic (conduction band electron).Fe(VI) exhibits a multitude of advantageous properties; these include higher reactivity and selectivity as an oxidant, disinfectant, antifoulant, and coagulant. Examples include treatment of cyanides and toxic metals, and inactivation of microorganisms. Rates of oxidation increase with a decrease in pH and are related to protonation of Fe VI O 4 2-. Oxidation of sulfur-and nitrogencontaining pollutants by Fe(VI) can be accomplished in seconds to minutes with formation of non-hazardous products. Fe(VI) can easily oxidize the amino acid components of microcystins and is a suitable disinfectant for detoxifying toxins in water. Fe(V) is more powerful oxidant than is Fe(VI). The oxidation of pollutants and amino acids with Fe(V) is 3-5 orders of magnitude faster than with Fe(VI). Removal of pollutants by Fe(V) can be completed in microseconds to millisecond time scales. The use of ionizing radiation and photocatalytic techniques in the presence of Fe(VI) results in Fe(V) formation and may have synergistic effects on the oxidation of pollutants and removal of toxins in water. Fe(V) can be useful in inactivation of microbial contaminants that are resistant to chlorination, chloramines, and Fe(VI). This paper gives examples of the multi-functional properties of Fe(VI) and Fe(V) to treat water and wastewater.

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Über Orthoferrate(IV)

Abstract: Darstellung und Eigenschaften folgender Ferrate(IV) werden beschrieben: Na4FeO4, Sr2FeO4, Ba2FeO4, Ba3FeO5.

Cited by 31 publications

References 5 publications

Synthesis, Crystal and Magnetic Structures of the Sodium Ferrate (IV) Na4FeO4 Studied by Neutron Diffraction and Mössbauer Techniques

Synthesis, Crystal and Magnetic Structures of the Sodium Ferrate (IV) Na4FeO4 Studied by Neutron Diffraction and Mössbauer Techniques

Electronic State, Magnetism, and Electrical Transport Behavior of Sr3−xAxFe2O7(x≤0.4,A=Ba, La)

Use of Iron(VI) and Iron(V) as Oxidants and Disinfectants in Water Treatment

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