高铁酸盐

高铁酸盐
	IUPAC名; Ferrate(VI)
	系统名; Tetraoxoironbis(olate)[来源请求]
别名	铁酸盐
识别
CAS号	16836-06-9
PubChem	25000034
ChemSpider	21865127
SMILES	[O-][Fe]([O-])(=O)=O;
InChI	1/Fe.4O/q;;;2*-1/rFeO4/c2-1(3,4)5/q-2;
InChIKey	XGBDPAYTQGQHEW-WTZHFVRHAI
ChEBI	30992
性质
化学式	FeO42-
摩尔质量	119.843 g mol-1 g·mol⁻¹
	若非注明，所有数据均出自标准状态（25 ℃，100 kPa）下。

高铁酸盐的高铁酸根是无机阴离子，化学式[FeO₄]²⁻。它对光敏感，其化合物和溶液呈淡紫色，为已知对水稳定的极强氧化剂。尽管归为弱碱，高铁酸盐浓溶液仍有腐蚀性，且会烧伤皮肤，只能在强碱环境稳定存在。

命名法

ferrate通常指代高铁酸根，但也可以指其它含铁阴离子，当中许多比[FeO₄]²⁻盐常见。这包括有强还原性的四羰基铁酸二钠Na₂[Fe(CO)₄]和三价铁络合物四氯铁酸根[FeCl₄]⁻。铁的含氧阴离子铁(V)酸根[FeO₄]³⁻和铁(IV)酸根[FeO₄]⁴⁻也同样存在，但其研究较少。这些也称为高铁酸根。^[1]

合成

高铁酸盐可在碱性条件用强氧化剂在水溶液中氧化铁，或加热固态的铁屑和粉状硝酸钾的混合物而形成。^[2]

如在碱性溶液加热氢氧化铁与次氯酸钠制备高铁酸盐：^[3]

2Fe(OH)₃＋3OCl⁻＋4OH⁻　→　2[FeO₄]²⁻＋5H₂O＋3Cl⁻

通常让阴离子以钡盐形式沉淀出来，形成高铁酸钡。^[3]

性质

高铁酸根离子不稳定，在中性^[2]或酸性环境会分解为三价铁：^[3]

[FeO₄]²⁻＋3e⁻＋8H⁺　⇌　Fe³⁺＋4H₂O

还原过程中间体中铁的氧化态有+5和+4^[4]。这些阴离子甚至比高铁酸根活泼^[5]。高铁酸根在碱性条件更稳定，酸值为8或9时能存在8至9小时^[5]。

稀高铁酸盐水溶液为粉红色，浓时为深红或紫色^[4]^[6]。与高锰酸盐相比，高铁酸盐是更强的氧化剂^[7]，可将三价铬氧化成重铬酸盐^[8]，或将氨氧化成氮分子^[9]。

高铁酸盐是优秀的消毒剂，能移除并杀死病毒。^[10]

高铁酸根离子有两个不成对电子，有顺磁性。其为四面体形分子构型。^[4]

参见

高铁酸钾

参考资料

^ Graham Hill; John Holman. Chemistry in context 5th. Nelson Thornes. 2000: 202. ISBN 0-17-448276-0.
^ ^2.0 ^2.1 R. K. Sharma. Text Book Of Coordination Chemistry. Discovery Publishing House. 2007: 124–125. ISBN 81-8356-223-X.
^ ^3.0 ^3.1 ^3.2 Gary Wulfsberg. Principles of descriptive inorganic chemistry. University Science Books. 1991: 142–143. ISBN 0-935702-66-0.
^ ^4.0 ^4.1 ^4.2 Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman. Inorganic chemistry. Academic Press. 2001: 1457–1458. ISBN 0-12-352651-5.
^ ^5.0 ^5.1 Gary M. Brittenham. Raymond J. Bergeron , 编. The Development of Iron Chelators for Clinical Use. CRC Press. 1994: 37–38. ISBN 0-8493-8679-9.
^ John Daintith (编). Oxford dictionary of chemistry 5th. Oxford University Press. 2004: 235. ISBN 0-19-860918-3.
^ Kenneth Malcolm Mackay; Rosemary Ann Mackay; W. Henderson. Introduction to modern inorganic chemistry 6th. CRC Press. 2002: 334–335. ISBN 0-7487-6420-8.
^ Amit Arora. Text Book Of Inorganic Chemistry. Discovery Publishing House. 2005: 691–692. ISBN 81-8356-013-X.
^ Karlis Svanks. Oxidation of Ammonia in Water by Ferrates(VI) and (IV) (PDF). Water Resources Center, Ohio State University: 3. June 1976 [2010-05-04].
^ Stanley E. Manahan. Environmental chemistry 8th. CRC Press. 2005: 234. ISBN 1-56670-633-5.

[hill-1] Graham Hill; John Holman. Chemistry in context 5th. Nelson Thornes. 2000: 202. ISBN 0-17-448276-0.

[sharma-2] 2.0 ^2.1 R. K. Sharma. Text Book Of Coordination Chemistry. Discovery Publishing House. 2007: 124–125. ISBN 81-8356-223-X.

[wulfsberg-3] 3.0 ^3.1 ^3.2 Gary Wulfsberg. Principles of descriptive inorganic chemistry. University Science Books. 1991: 142–143. ISBN 0-935702-66-0.

[wiberg-4] 4.0 ^4.1 ^4.2 Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman. Inorganic chemistry. Academic Press. 2001: 1457–1458. ISBN 0-12-352651-5.

[bergeron-5] 5.0 ^5.1 Gary M. Brittenham. Raymond J. Bergeron , 编. The Development of Iron Chelators for Clinical Use. CRC Press. 1994: 37–38. ISBN 0-8493-8679-9.

[6] John Daintith (编). Oxford dictionary of chemistry 5th. Oxford University Press. 2004: 235. ISBN 0-19-860918-3.

[mackay-7] Kenneth Malcolm Mackay; Rosemary Ann Mackay; W. Henderson. Introduction to modern inorganic chemistry 6th. CRC Press. 2002: 334–335. ISBN 0-7487-6420-8.

[8] Amit Arora. Text Book Of Inorganic Chemistry. Discovery Publishing House. 2005: 691–692. ISBN 81-8356-013-X.

[9] Karlis Svanks. Oxidation of Ammonia in Water by Ferrates(VI) and (IV) (PDF). Water Resources Center, Ohio State University: 3. June 1976 [2010-05-04].

[10] Stanley E. Manahan. Environmental chemistry 8th. CRC Press. 2005: 234. ISBN 1-56670-633-5.

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