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231:. Animals and humans can obtain the necessary iron from foods that contain it in assimilable form, such as meat. Other organisms must obtain their iron from the environment. However, iron tends to form highly insoluble iron(III) oxides/hydroxides in aerobic (
640:
Iron(III) is a d center, meaning that the metal has five "valence" electrons in the 3d orbital shell. The number and type of ligands bound to iron(III) determine how these electrons arrange themselves. With so-called "strong field ligands" such as
258:
The insolubility of iron(III) compounds is also responsible for the low levels of iron in seawater, which is often the limiting factor for the growth of the microscopic plants (
251:
that form soluble complexes with iron(III), that can be reabsorbed into the cell. (The other plants instead encourage the growth around their roots of certain bacteria that
544:
While iron(III) aquo complexes tend to convert to polymeric oxy-hydroxides, iron(III) complexes with other ligands form stable solutions. The complex with
624:, rust flakes off, because it is bulkier than the metal that formed it. Therefore, unprotected iron objects will in time be completely turned into rust.
828:
Boyd PW, Watson AJ, Law CS, et al. (October 2000). "A mesoscale phytoplankton bloom in the polar
Southern Ocean stimulated by iron fertilization".
487:
The aquo ligands on iron(III) complexes are labile. This behavior is visualized by the color change brought about by reaction with thiocyanate:
757:
472:
compounds prevent the polymerization. These same ligands can even dissolve iron(III) oxides and hydroxides. One of these ligands is
888:
792:
480:
also solubilizes ferric ion at neutral pH, although its complexes are less stable than those of EDTA. Many chelating ligands - the
476:, which is often used to dissolve iron deposits or added to fertilizers to make iron in the soil available (soluble) to plants.
910:
30:
685:. Tetrahedral complexes are high spin. The magnetism of ferric complexes can show when they are high or low spin.
130:, that naked ion does not exist except under extreme conditions. Iron(III) centres are found in many compounds and
677:
has only five unpaired electrons. It is high-spin. With chloride, iron(III) forms tetrahedral complexes, e.g. (
594:
217:
613:
216:. Many organisms, from bacteria to humans, store iron as microscopic crystals (3 to 8 nm in diameter) of
34:
196:
All known forms of life require iron, which usually exists in Fe(II) or Fe(III) oxidation states. Many
837:
761:
608:
is a mixture of iron(III) oxide and oxide-hydroxide that usually forms when iron metal is exposed to
368:
165:
131:
342:
758:"Iron integral to the development of life on Earth – and the possibility of life on other planets"
861:
730:
702:
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87:
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has only one unpaired electron. It is low-spin. With so-called "weak field ligands" such as
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812:
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269:
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ions surrounding the Fe core. Relative to lower oxidation states, ferric is less common in
79:
72:
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694:
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236:
841:
564:
201:
904:
259:
205:
807:
H. Marschner and V. Römheld (1994): "Strategies of plants for acquisition of iron".
865:
708:
662:
646:
568:
286:
138:
481:
356:
248:
244:
169:
134:, where Fe(III) is bonded to several ligands. A molecular ferric complex is the
337:
ions. In these complexes, the protons are acidic. Eventually these solutions
551:
338:
213:
209:
119:
636:
d-orbital splitting scheme for low- and high spin octahedral Fe(III) complex
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that further converts to polymeric oxide-hydroxide via the process called
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is soluble and can sustain reduction to it iron(II) derivative:
473:
75:
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can thrive in such environments by secreting compounds called
200:
in living beings contain iron(III) centers. Examples of such
575:, is a very complicated material that contains iron(III).
359:
out of the solution as solids. That reaction liberates
713:
Pages displaying short descriptions of redirect targets
699:
Pages displaying short descriptions of redirect targets
484:- are produced naturally to dissolve iron(III) oxides.
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Iron(III) is found in many minerals and solids, e.g.,
645:, the five electrons pair up as best they can. Thus
727:
Pages displaying wikidata descriptions as a fallback
616:oxide layers that are formed by other metals, like
739: – The element iron in its +2 oxidation state
325:. Iron(III) nitrate dissolved in water to give
883:(2nd ed.). Oxford: Butterworth-Heinemann.
783:Berg, Jeremy Mark; Lippard, Stephen J. (1994).
787:. Sausalito, Calif: University Science Books.
262:) that are the basis of the marine food web.
224:, from which it can be recovered as needed.
8:
255:iron(III) to the more soluble iron(II).)
227:Insufficient iron in the human diet causes
107:salts, containing the cation Fe. The word
27:The element iron in its +3 oxidation state
661:, the five electrons are unpaired. Thus
600:are extremely insoluble reflecting their
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879:Earnshaw, A.; Greenwood, N. N. (1997).
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811:, volume 165, issue 2, pages 261–274.
367:lowering the pH of its solutions. The
281:Typically iron(III) salts, like the "
7:
785:Principles of bioinorganic chemistry
560:Iron(III) minerals and other solids
25:
220:, inside a shell of the protein
37:contains the iron(III) complex
126:Although often abbreviated as
1:
546:1,10-phenanthrolinebipyridine
277:Iron(III) salts and complexes
235:) environment, especially in
86:is an alternative name for
927:
697: – Inorganic compound
500:] + SCN ⇌ [Fe(SCN)(H
881:Chemistry of the elements
725: – chemical compound
711: – Chemical compound
595:iron(III) oxide-hydroxide
218:iron(III) oxide hydroxide
637:
576:
556:
273:
132:coordination complexes
118:
54:
35:Potassium ferrioxalate
635:
567:
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529:is nearly colorless,
268:
33:
762:University of Oxford
355:. These hydroxides
192:Iron(III) in biology
166:organoiron chemistry
123:, meaning "iron".
113:is derived from the
103:is used instead for
911:Iron(III) compounds
842:2000Natur.407..695B
555:Redox reaction of .
405:OH] ⇌ [Fe(H
343:iron(III) hydroxide
817:10.1007/BF00008069
731:Iron(III) fluoride
703:Iron(III) chloride
638:
577:
571:, commonly called
557:
289:with the formulas
274:
88:iron(III) chloride
55:
836:(6805): 695–702.
764:. 7 December 2021
612:air. Unlike the
97:). The adjective
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850:10.1038/35037500
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384:] ⇌ [Fe(H
371:are elaborate:
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311:], and [Fe(H
270:Pourbaix diagram
237:calcareous soils
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723:Ferric fluoride
717:Iron(III) oxide
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593:(hematite) and
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272:of aqueous iron
202:metalloproteins
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188:is well known.
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95:
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84:Ferric chloride
80:oxidation state
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531:[Fe(SCN)(H
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299:Cl], [Fe(H
287:aquo complexes
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71:refers to the
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541:is deep red.
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766:. Retrieved
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709:Ferric oxide
663:aquo complex
647:ferricyanide
639:
578:
569:Ferric oxide
543:
516:
486:
482:siderophores
467:
357:precipitates
280:
257:
249:siderophores
226:
195:
139:ferrioxalate
127:
125:
108:
98:
83:
67:
66:
62:
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679:[Fe(Cl)
651:[Fe(CN)
614:passivating
604:structure.
422:2 [Fe(H
214:cytochromes
170:ferrocenium
744:References
369:equilibria
341:producing
233:oxygenated
212:, and the
210:ferredoxin
168:, but the
78:in its +3
667:[Fe(H
602:polymeric
519:[Fe(H
492:[Fe(H
470:chelating
397:[Fe(H
392:OH] + H
376:[Fe(H
339:hydrolyze
327:[Fe(H
291:[Fe(H
174:[Fe(C
159:bidentate
143:[Fe(C
63:iron(III)
59:chemistry
39:[Fe(C
18:Iron(III)
905:Category
858:11048709
689:See also
622:aluminum
618:chromium
517:Whereas
468:Various
361:hydrogen
283:chloride
241:Bacteria
222:ferritin
204:include
198:proteins
105:iron(II)
866:4368261
838:Bibcode
737:Ferrous
643:cyanide
628:Bonding
598:FeO(OH)
478:Citrate
417:] + H
353:olation
245:grasses
172:cation
162:oxalate
100:ferrous
73:element
887:
864:
856:
830:Nature
791:
346:Fe(OH)
285:" are
253:reduce
229:anemia
120:ferrum
110:ferric
68:ferric
862:S2CID
768:9 May
659:water
610:humid
581:oxide
508:] + H
459:+ 2 H
363:ions
136:anion
117:word
115:Latin
885:ISBN
854:PMID
789:ISBN
770:2022
620:and
606:Rust
573:rust
474:EDTA
446:(OH)
430:(OH)
413:(OH)
243:and
92:FeCl
76:iron
846:doi
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813:doi
82:.
65:or
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