Iron(II) perchlorate
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| Names | |
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| IUPAC name
Iron(II) diperchlorate
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Other names
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.034.263 |
| EC Number |
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| Fe(ClO4)2 | |
| Molar mass | 254.75 g/mol |
| Appearance | Green crystals |
| Density | 2.15 g/cm3 |
| Melting point | 100 °C (212 °F; 373 K) |
| 98 g/100 mL (25 °C)[1] | |
| Structure[2] | |
| Orthorhombic | |
| Pmn21 | |
a = 7.79 Å, b = 13.48 Å, c = 5.24 Å
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| Hazards | |
| GHS labelling: | |
 
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| Danger | |
| H272, H315, H319, H335 | |
| P210, P220, P221, P261, P264, P271, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P370+P378, P403+P233, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other cations
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Manganese(II) perchlorate Cobalt(II) perchlorate Nickel(II) perchlorate |
Related compounds
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Iron(III) perchlorate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Iron(II) perchlorate is the inorganic compound with the formula Fe(ClO4)2·6H2O. A green, water-soluble solid, it is produced by the reaction of iron metal with dilute perchloric acid followed by evaporation of the solution:[3]
- Fe + 2 HClO4 + 6 H2O → Fe(ClO4)2·6H2O + H2
Although the ferrous cation is a reductant and the perchlorate anion is a strong oxidant, in the absence of atmospheric oxygen, dissolved ferrous perchlorate is stable in aqueous solution because the electron transfer between both species Fe2+ and ClO−4 is hindered by severe kinetic limitations. Being a weak Lewis base, the perchlorate anion is a poor ligand for the aqueous Fe2+ and does not contribute to the electron transfer by favoring the formation of an inner sphere complex giving rise to a possible reorganisation of the activated complex. The resulting high activation energy prohibits a thermodynamically spontaneous redox reaction (∆Gr < 0).
However, in aqueous solution, and under air, iron(II) perchlorate slowly oxidizes to iron(III) oxyhydroxide.[4]
The hexahydrate consists of discreet hexa-aquo-iron(II) divalent cations and perchlorate anions. It crystallizes with an orthorhombic structure.[2] It has minor phase transitions at 245 and 336 K.[5]
Uses
[edit]In organic chemistry, iron(II) perchlorate can be used as a source of ferrous ions for the Fenton oxidation.[1]
References
[edit]- ^ a b Mark W. Zettler; Daniela Sustac Roman (2014). "Iron(II) Perchlorate". Encyclopedia of Reagents for Organic Synthesis (EROS). doi:10.1002/047084289X.ri064.pub2.
- ^ a b Ghosh, Minakshi; Ray, Siddhartha (1981). "Twinning, disorder and phase transition in ferrous Perchlorate hexahydrate crystals". Zeitschrift für Kristallographie – Crystalline Materials. 155 (1–2): 129–137. Bibcode:1981ZK....155..129G. doi:10.1524/zkri.1981.155.1-2.129.
- ^ B.K. Chaudhuri (1975). "A new type of phase transition in M(ClO4)2(H2O)6 M = Fe, Co, Ni and Mn". Solid State Communications. 16 (6): 767–772. doi:10.1016/0038-1098(75)90071-X.
- ^ Philip George (1954). "The oxidation of ferrous perchlorate by molecular oxygen". Journal of the Chemical Society (Resumed): 4349–4359. doi:10.1039/JR9540004349.
- ^ D. P. Chiang; C. H. Peng; J. K. Mei; I. M. Jiang; S. C. Lin; Y. C. Chen; H. T. Liu; Y. F. Chen; W. S. Tse (2008). "Raman spectra of crystalline iron perchlorate hexahydrate". Journal of Raman Spectroscopy. 39 (3): 344–348. doi:10.1002/jrs.1801.
| Fe(-II) | |||
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| Fe(0) | |||
| Fe(I) |
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| Fe(0,II) | |||
| Fe(II) |
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| Fe(0,III) | |||
| Fe(II,III) | |||
| Fe(III) |
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| Fe(IV) | |||
| Fe(VI) | |||
| Purported | |||
Salts and covalent derivatives of the perchlorate ion | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
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