Fe3+ And O2- Chemical Formula

Chemical chemical compound

This commodity is nearly a red-colored oxide of atomic number 26. For other uses, see Red Iron.

Iron(III) oxide

Fe O
Names
IUPAC name Iron(Iii) oxide
Other names ferric oxide, haematite, ferric iron, red atomic number 26 oxide, rouge, maghemite, colcothar, fe sesquioxide, rust, ochre
Identifiers
CAS Number	1309-37-1 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:50819 Y
ChemSpider	14147 Northward
ECHA InfoCard	100.013.790
EC Number	215-168-2
E number	E172(ii) (colours)
Gmelin Reference	11092
KEGG	C19424 N
PubChem CID	518696
RTECS number	NO7400000
UNII	1K09F3G675 Y
CompTox Dashboard (EPA)	DTXSID0029632
InChI InChI=1S/2Fe.3O Y[inchi] Cardinal: JEIPFZHSYJVQDO-UHFFFAOYSA-N Y[inchi] InChI=ane/2Fe.3O/rFe2O3/c3-1-four-2(iii)5-1 Key: JEIPFZHSYJVQDO-ZVGCCQCPAC
SMILES O1[Fe]2O[Iron]1O2
Properties
Chemic formula	Iron two O 3
Molar mass	159.687 g·mol−1
Appearance	Red-brown solid
Odor	Odorless
Density	five.25 1000/cmiii [one]
Melting point	1,539 °C (ii,802 °F; 1,812 K)[one] decomposes 105 °C (221 °F; 378 Chiliad) β-dihydrate, decomposes 150 °C (302 °F; 423 K) β-monohydrate, decomposes 50 °C (122 °F; 323 K) α-dihydrate, decomposes 92 °C (198 °F; 365 Grand) α-monohydrate, decomposes[3]
Solubility in water	Insoluble
Solubility	Soluble in diluted acids,[ane] barely soluble in sugar solution[2] Trihydrate slightly soluble in aq. tartaric acid, citric acid, CH3COOH[3]
Magnetic susceptibility (χ)	+3586.0x10−6 cm3/mol
Refractive index (n D)	n1 = 2.91, north2 = three.19 (α, hematite)[4]
Structure
Crystal construction	Rhombohedral, hR30 (α-form)[five] Cubic bixbyite, cI80 (β-form) Cubic spinel (γ-form) Orthorhombic (ε-grade)[6]
Space group	R3c, No. 161 (α-course)[5] Iaiii, No. 206 (β-grade) Pna21, No. 33 (ε-grade)[6]
Indicate group	3m (α-form)[v] ii/m three (β-grade) mm2 (ε-form)[6]
Coordination geometry	Octahedral (Fethree+, α-grade, β-grade)[5]
Thermochemistry[vii]
Heat capacity (C)	103.9 J/mol·K[7]
Std molar entropy (S ⦵ 298)	87.4 J/mol·K[7]
Std enthalpy of formation (Δf H ⦵ 298)	−824.ii kJ/mol[seven]
Gibbs complimentary energy (Δf G ⦵)	−742.ii kJ/mol[7]
Hazards
GHS labelling:
Pictograms	[8]
Bespeak word	Alert
Hazard statements	H315, H319, H335 [8]
Precautionary statements	P261, P305+P351+P338 [8]
NFPA 704 (burn diamond)	[10] 0 0 0
Threshold limit value (TLV)	5 mg/thou3 [i] (TWA)
Lethal dose or concentration (LD, LC):
LD50 (median dose)	x thou/kg (rats, oral)[ten]
NIOSH (U.s. health exposure limits):
PEL (Permissible)	TWA 10 mg/chiliadiii [9]
REL (Recommended)	TWA 5 mg/m3 [9]
IDLH (Immediate danger)	2500 mg/m3 [9]
Related compounds
Other anions	Iron(3) fluoride
Other cations	Manganese(III) oxide Cobalt(Three) oxide
Related iron oxides	Iron(Two) oxide Iron(Ii,Iii) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Nverify (what is Y Due north  ?) Infobox references

Chemical chemical compound

Iron(III) oxide in a vial

Fe(III) oxide or ferric oxide is the inorganic compound with the formula Fe_iiO_three. Information technology is ane of the three main oxides of iron, the other two being iron(Ii) oxide (FeO), which is rare; and iron(Two,III) oxide (Fe₃O_iv), which as well occurs naturally as the mineral magnetite. As the mineral known every bit hematite, Fe₂O_iii is the main source of fe for the steel industry. Fe₂O₃ is readily attacked by acids. Iron(III) oxide is oft called rust, and to some extent this label is useful, because rust shares several backdrop and has a similar composition; however, in chemistry, rust is considered an ill-defined textile, described as Hydrous ferric oxide.^[11]

Structure [edit]

Fe₂O₃ can be obtained in various polymorphs. In the chief one, α, iron adopts octahedral coordination geometry. That is, each Fe center is bound to six oxygen ligands. In the γ polymorph, some of the Iron sit on tetrahedral sites, with four oxygen ligands.

Blastoff phase [edit]

α-Fe₂O₃ has the rhombohedral, corundum (α-Al₂O₃) construction and is the well-nigh mutual form. It occurs naturally as the mineral hematite which is mined as the main ore of iron. It is antiferromagnetic below ~260 One thousand (Morin transition temperature), and exhibits weak ferromagnetism betwixt 260 K and the Néel temperature, 950 K.^[12] Information technology is easy to ready using both thermal decomposition and precipitation in the liquid phase. Its magnetic properties are dependent on many factors, e.1000. pressure level, particle size, and magnetic field intensity.

Gamma phase [edit]

γ-Fe₂O₃ has a cubic structure. It is metastable and converted from the alpha phase at loftier temperatures. Information technology occurs naturally every bit the mineral maghemite. It is ferromagnetic and finds application in recording tapes,^[13] although ultrafine particles smaller than 10 nanometers are superparamagnetic. It can exist prepared by thermal dehydratation of gamma iron(III) oxide-hydroxide. Another method involves the careful oxidation of atomic number 26(Ii,III) oxide (Fe₃O₄).^[13] The ultrafine particles can exist prepared by thermal decomposition of iron(III) oxalate.

Other solid phases [edit]

Several other phases have been identified or claimed. The β-phase is cubic trunk-centered (space group Ia3), metastable, and at temperatures above 500 °C (930 °F) converts to blastoff phase. It tin be prepared past reduction of hematite by carbon,^{[ clarification needed ]} pyrolysis of fe(III) chloride solution, or thermal decomposition of atomic number 26(III) sulfate.^[14]

The epsilon (ε) phase is rhombic, and shows properties intermediate between alpha and gamma, and may accept useful magnetic properties applicable for purposes such equally high density recording media for large information storage.^[fifteen] Preparation of the pure epsilon phase has proven very challenging. Textile with a high proportion of epsilon phase can exist prepared by thermal transformation of the gamma phase. The epsilon phase is also metastable, transforming to the alpha phase at betwixt 500 and 750 °C (930 and one,380 °F). It can also be prepared by oxidation of iron in an electrical arc or by sol-gel precipitation from atomic number 26(3) nitrate.^{[ citation needed ]} Research has revealed epsilon iron(III) oxide in ancient Chinese Jian ceramic glazes, which may provide insight into ways to produce that grade in the lab.^{[sixteen] [ not-principal source needed ]}

Additionally, at loftier pressure level an baggy form is claimed.^{[6] [ non-primary source needed ]}

Liquid phase [edit]

Molten Atomic number 26₂O₃ is expected to have a coordination number of close to 5 oxygen atoms about each atomic number 26 atom, based on measurements of slightly oxygen scarce supercooled liquid iron oxide droplets, where supercooling circumvents the need for the high oxygen pressures required above the melting bespeak to maintain stoichiometry.^[17]

Hydrated iron(3) oxides [edit]

Several hydrates of Iron(Iii) oxide exist. When alkali is added to solutions of soluble Atomic number 26(3) salts, a carmine-brown gelled precipitate forms. This is non Fe(OH)₃, just Fe₂O_three·H₂O (besides written as Fe(O)OH). Several forms of the hydrated oxide of Atomic number 26(III) be also. The cherry-red lepidocrocite (γ-Fe(O)OH) occurs on the outside of rusticles, and the orange goethite (α-Atomic number 26(O)OH) occurs internally in rusticles. When Atomic number 26_iiO₃·H₂O is heated, it loses its water of hydration. Further heating at 1670 1000 converts Atomic number 26₂O_iii to black Fe₃O₄ (Atomic number 26^IiIron^III _twoO₄), which is known as the mineral magnetite. Fe(O)OH is soluble in acids, giving [Iron(H_twoO)₆]³⁺ . In concentrated aqueous alkali, Fe₂O₃ gives [Fe(OH)_{half dozen}]³⁻.^[13]

Reactions [edit]

The most important reaction is its carbothermal reduction, which gives fe used in steel-making:

Iron₂O₃ + 3 CO → ii Fe + 3 CO_two

Another redox reaction is the extremely exothermic thermite reaction with aluminium.^[18]

2 Al + Fe_twoO_three → 2 Iron + Al₂O₃

This procedure is used to weld thick metals such equally rails of train tracks by using a ceramic container to funnel the molten fe in between two sections of track. Thermite is as well used in weapons and making small-scale-scale bandage-iron sculptures and tools.

Partial reduction with hydrogen at near 400 °C produces magnetite, a black magnetic material that contains both Fe(III) and Fe(II):^[19]

3 Fe₂O₃ + H_two → 2 Fe₃O₄ + H₂O

Iron(Three) oxide is insoluble in water but dissolves readily in strong acid, e.g. hydrochloric and sulfuric acids. It besides dissolves well in solutions of chelating agents such as EDTA and oxalic acid.

Heating atomic number 26(Three) oxides with other metal oxides or carbonates yields materials known as ferrates (ferrate (III)):^[19]

ZnO + Fe₂O₃ → Zn(FeO₂)₂

Preparation [edit]

Iron(III) oxide is a product of the oxidation of iron. It can be prepared in the laboratory by electrolyzing a solution of sodium bicarbonate, an inert electrolyte, with an iron anode:

iv Fe + 3 O₂ + 2 H₂O → 4 FeO(OH)

The resulting hydrated iron(3) oxide, written here as FeO(OH), dehydrates around 200 °C.^{[19] [twenty]}

2 FeO(OH) → Atomic number 26₂O_three + H_twoO

Uses [edit]

Iron industry [edit]

The overwhelming application of fe(III) oxide is as the feedstock of the steel and iron industries, e.g. the production of fe, steel, and many alloys.^[xx]

Polishing [edit]

A very fine pulverization of ferric oxide is known every bit "jeweler's rouge", "red rouge", or simply rouge. It is used to put the final polish on metallic jewelry and lenses, and historically as a cosmetic. Rouge cuts more slowly than some modernistic polishes, such equally cerium(4) oxide, but is still used in eyes fabrication and by jewelers for the superior cease it can produce. When polishing gilt, the rouge slightly stains the golden, which contributes to the advent of the finished piece. Rouge is sold equally a powder, paste, laced on polishing cloths, or solid bar (with a wax or grease folder). Other polishing compounds are also oftentimes called "rouge", even when they do non contain iron oxide. Jewelers remove the balance rouge on jewelry by use of ultrasonic cleaning. Products sold as "stropping compound" are frequently applied to a leather hone to assist in getting a razor edge on knives, straight razors, or any other edged tool.

Paint [edit]

2 different colors at unlike hydrate phase (α: red, β: yellow) of fe(III) oxide hydrate;^[three] they are useful as pigments.

Iron(Iii) oxide is also used as a pigment, under names "Paint Brown six", "Paint Brown 7", and "Pigment Cherry 101".^[21] Some of them, e.g. Paint Red 101 and Pigment Chocolate-brown 6, are canonical by the US Food and Drug Assistants (FDA) for use in cosmetics. Iron oxides are used every bit pigments in dental composites alongside titanium oxides.^[22]

Hematite is the characteristic component of the Swedish pigment color Falu reddish.

Magnetic recording [edit]

Iron(Iii) oxide was the most common magnetic particle used in all types of magnetic storage and recording media, including magnetic disks (for information storage) and magnetic record (used in sound and video recording as well as data storage). Its apply in computer disks was superseded by cobalt alloy, enabling thinner magnetic films with college storage density.^[23]

Photocatalysis [edit]

α-Atomic number 26_iiO₃ has been studied as a photoanode for solar water oxidation.^[24] However, its efficacy is limited by a short diffusion length (2–4 nm) of photograph-excited accuse carriers^[25] and subsequent fast recombination, requiring a large overpotential to drive the reaction.^[26] Research has been focused on improving the h2o oxidation performance of Atomic number 26₂O_iii using nanostructuring,^[24] surface functionalization,^[27] or by employing alternate crystal phases such as β-Fe_twoO_three.^[28]

Medicine [edit]

Calamine lotion, used to care for mild itchiness, is chiefly equanimous of a combination of zinc oxide, interim as astringent, and nigh 0.5% iron(III) oxide, the production's agile ingredient, acting every bit antipruritic. The red color of atomic number 26(Iii) oxide is also mainly responsible for the lotion's pinkish color.

See as well [edit]

• Chalcanthum

References [edit]

1. ^ ^{a b c d} Haynes, p. four.69
2. ^ "A dictionary of chemical solubilities, inorganic". annal.org . Retrieved 17 November 2020.
3. ^ ^{a b c} Comey, Arthur Messinger; Hahn, Dorothy A. (Feb 1921). A Lexicon of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 433.
4. ^ Haynes, p. 4.141
5. ^ ^{a b c d} Ling, Yichuan; Wheeler, Damon A.; Zhang, Jin Zhong; Li, Yat (2013). Zhai, Tianyou; Yao, Jiannian (eds.). Ane-Dimensional Nanostructures: Principles and Applications. John Wiley & Sons, Inc. Hoboken, New Bailiwick of jersey: John Wiley & Sons, Inc. p. 167. ISBN978-one-118-07191-v.
6. ^ ^{a b c d} Vujtek, Milan; Zboril, Radek; Kubinek, Roman; Mashlan, Miroslav. "Ultrafine Particles of Iron(III) Oxides by View of AFM – Novel Road for Written report of Polymorphism in Nano-world" (PDF). Univerzity Palackého . Retrieved 12 July 2014.
7. ^ ^{a b c d eastward} Haynes, p. five.12
8. ^ ^{a b c} Sigma-Aldrich Co., Iron(Iii) oxide. Retrieved on 2014-07-12.
9. ^ ^{a b c} NIOSH Pocket Guide to Chemical Hazards. "#0344". National Institute for Occupational Safe and Health (NIOSH).
10. ^ ^{a b} "SDS of Iron(III) oxide" (PDF). KJLC. England: Kurt J Lesker Visitor Ltd. five January 2012. Retrieved 12 July 2014.
11. ^ PubChem. "Atomic number 26 oxide (Fe2O3), hydrate". pubchem.ncbi.nlm.nih.gov . Retrieved 11 November 2020.
12. ^ Greedan, J. Due east. (1994). "Magnetic oxides". In King, R. Bruce (ed.). Encyclopedia of Inorganic chemistry. New York: John Wiley & Sons. ISBN978-0-471-93620-6.
13. ^ ^{a b c} Housecroft, Catherine East.; Sharpe, Alan G. (2008). "Chapter 22: d-block metal chemistry: the offset row elements". Inorganic Chemistry (3rd ed.). Pearson. p. 716. ISBN978-0-thirteen-175553-6.
14. ^ "Machinery of Oxidation & Thermal Decomposition of Atomic number 26 Sulphides" (PDF).
15. ^ Tokoro, Hiroko; Namai, Asuka; Ohkoshi, Shin-Ichi (2021). "Advances in magnetic films of epsilon-iron oxide toward next-generation high-density recording media". Dalton Transactions. Royal Gild of Chemistry. 50 (2): 452–459. doi:10.1039/D0DT03460F. PMID 33393552. S2CID 230482821. Retrieved 25 January 2021.
16. ^ Dejoie, Catherine; Sciau, Philippe; Li, Weidong; Noé, Laure; Mehta, Apurva; Chen, Kai; Luo, Hongjie; Kunz, Martin; Tamura, Nobumichi; Liu, Zhi (2015). "Learning from the by: Rare ε-Fe_twoO₃ in the ancient black-glazed Jian (Tenmoku) wares". Scientific Reports. iv: 4941. doi:10.1038/srep04941. PMC4018809. PMID 24820819.
17. ^ Shi, Caijuan; Alderman, Oliver; Tamalonis, Anthony; Weber, Richard; You lot, Jinglin; Benmore, Chris (2020). "Redox-structure dependence of molten iron oxides". Communications Materials. ane (1): 80. Bibcode:2020CoMat...1...80S. doi:x.1038/s43246-020-00080-4.
18. ^ Adlam; Price (1945). Higher School Certificate Inorganic Chemistry. Leslie Slater Cost.
19. ^ ^{a b c} Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited past G. Brauer, Academic Press, 1963, NY. Vol. one. p. 1661.
20. ^ ^{a b} Greenwood, N. Due north.; Earnshaw, A. (1997). Chemical science of the Chemical element (2nd ed.). Oxford: Butterworth-Heinemann. ISBN978-0-7506-3365-9.
21. ^ Paint and Surface Coatings: Theory and Do. William Andrew Inc. 1999. ISBN978-ane-884207-73-0.
22. ^ Banerjee, Avijit (2011). Pickard's Transmission of Operative Dentistry. United States: Oxford University Press Inc., New York. p. 89. ISBN978-0-19-957915-0.
23. ^ Piramanayagam, Southward. North. (2007). "Perpendicular recording media for hd drives". Periodical of Applied Physics. 102 (i): 011301–011301–22. Bibcode:2007JAP...102a1301P. doi:10.1063/1.2750414.
24. ^ ^{a b} Kay, A., Cesar, I. and Grätzel, M. (2006). "New Benchmark for Water Photooxidation by Nanostructured α-Fe₂O₃ Films". Journal of the American Chemical Order. 128 (49): 15714–15721. doi:10.1021/ja064380l. PMID 17147381. {{cite journal}}: CS1 maint: multiple names: authors list (link)
25. ^ Kennedy, J.H. and Frese, Yard.Westward. (1978). "Photooxidation of Water at α-Iron_twoO₃ Electrodes". Journal of the Electrochemical Society. 125 (5): 709. doi:x.1149/1.2131532. {{cite journal}}: CS1 maint: multiple names: authors list (link)
26. ^ Le Formal, F. (2014). "Back Electron–Hole Recombination in Hematite Photoanodes for Water Splitting". Journal of the American Chemical Society. 136 (6): 2564–2574. doi:10.1021/ja412058x. PMID 24437340.
27. ^ Zhong, D.Thousand. and Gamelin, D.R. (2010). "Photoelectrochemical Water Oxidation by Cobalt Catalyst ("Co−Pi")/α-Fe₂O_three Composite Photoanodes: Oxygen Development and Resolution of a Kinetic Clogging". Periodical of the American Chemical Social club. 132 (12): 4202–4207. doi:ten.1021/ja908730h. PMID 20201513. {{cite journal}}: CS1 maint: multiple names: authors listing (link)
28. ^ Emery, J.D. (2014). "Diminutive Layer Deposition of Metastable β-Iron₂O_three via Isomorphic Epitaxy for Photoassisted Water Oxidation". ACS Applied Materials & Interfaces. 6 (24): 21894–21900. doi:10.1021/am507065y. OSTI 1355777. PMID 25490778.

External links [edit]

• NIOSH Pocket Guide to Chemical Hazards

Fe3+ And O2- Chemical Formula,

Source: https://en.wikipedia.org/wiki/Iron(III)_oxide

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