The Compound Fecl3 is Made of
The Compound Fecl3 is Made of
![]() Iron(III) chloride (hydrate) |
|||
![]() Iron(Iii) chloride (anhydrous) |
|||
|
|||
Names | |||
---|---|---|---|
IUPAC names
Fe(Three) chloride |
|||
Other names
|
|||
Identifiers | |||
CAS Number |
|
||
3D model (JSmol) |
|
||
ChEBI |
|
||
ChemSpider |
|
||
ECHA InfoCard | 100.028.846 |
||
EC Number |
|
||
PubChem |
|
||
RTECS number |
|
||
UNII |
|
||
UN number |
|
||
CompTox Dashboard |
|
||
InChI
|
|||
SMILES
|
|||
Properties | |||
Chemical formula |
FeCliii |
||
Molar mass |
|
||
Appearance | Dark-green-black by reflected calorie-free; royal-red by transmitted light; xanthous solid as hexahydrate; chocolate-brown as aqueous solution | ||
Odor | Slight HCl | ||
Density |
|
||
Melting bespeak | 307.half dozen °C (585.seven °F; 580.viii Thou) (anhydrous) 37 °C (99 °F; 310 M) (hexahydrate)[i] |
||
Humid point |
|
||
Solubility in water |
912g/L (anhydrous or hexahydrate, 25°C)[1] | ||
Solubility in
|
|
||
Magnetic susceptibility (χ) |
+xiii,450·x−6 cm3/mol[2] |
||
Viscosity | 12 cP (40% solution) | ||
Structure | |||
Crystal structure |
Hexagonal, hR24 | ||
Infinite group |
R3, No. 148[3] | ||
Lattice constant |
a = 0.6065nm, α = xc°, β = 90°, γ = 120° |
||
Formula units (Z) |
6 | ||
Coordination geometry |
Octahedral | ||
Hazards[5] [half dozen] [Note ane] |
|||
GHS labelling: |
|||
Pictograms |
![]() ![]() |
||
Point discussion |
Danger | ||
Hazard statements |
H290, H302, H314 |
||
Precautionary statements |
P234, P260, P264, P270, P273, P280, P301+P312, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P390, P405, P406, P501 |
||
NFPA 704 (fire diamond) |
2
|
||
Flash signal | Non-flammable | ||
NIOSH (United states health exposure limits): |
|||
REL (Recommended) |
TWA onemg/m3 [4] |
||
Safety data sheet (SDS) | ICSC |
||
Related compounds | |||
Other anions |
|
||
Other cations |
|
||
Related coagulants |
|
||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references |
Iron(III) chloride
is the inorganic chemical compound with the formula
FeCl3
. As well called
ferric chloride, information technology is a common compound of atomic number 26 in the +3 oxidation land. The anhydrous compound is a crystalline solid with a melting point of 307.6 °C. The color depends on the viewing angle: by reflected calorie-free the crystals announced nighttime greenish, only by transmitted low-cal they appear royal-red.
Structure and properties
[edit]
Anhydrous
[edit]
Anhydrous iron(Iii) chloride has the
BiI3
structure, with octahedral Fe(Iii) centers interconnected by two-coordinate chloride ligands.[3]
Iron(III) chloride has a relatively depression melting point and boils at around 315 °C. The vapor consists of the dimer
Iron2Cl6
(similar aluminium chloride) which increasingly dissociates into the monomeric
FeClthree
(with D3h
point group molecular symmetry) at college temperature, in competition with its reversible decomposition to requite fe(II) chloride and chlorine gas.[8]
Hydrates
[edit]
In addition to the anhydrous material, ferric chloride forms four hydrates. All forms of fe(III) chloride feature two or more chlorides as ligands, and 3 hydrates feature
[FeCl4]−
.[9]
-
dihydrate:
FeClthree·2H2O
has the structural formula
trans–[FeCl2(H2O)4][FeCl4]. -
FeClthree·2.5HiiO
has the structural formula
cis–[FeCl2(HiiO)iv][FeCl4]·H2O. -
FeCliii·3.5H2O
has the structural formula
cis–[FeCl2(HiiO)4][FeCl4]·3H2O. -
hexahydrate:
FeClthree·6HiiO
has the structural formula
trans–[FeCl2(H2O)4]Cl·2H2O.[10]
Aqueous solution
[edit]
Aqueous solutions of ferric chloride are characteristically yellow, in contrast to the stake pinkish solutions of
[Atomic number 26(H2O)6]3+
. According to spectroscopic measurements, the main species in aqueous solutions of ferric chloride are the octahedral complex
[FeCl2(HtwoO)4]+
(stereochemistry unspecified) and the tetrahedral
[FeCl4]−
.[9]
Grooming
[edit]
Anhydrous iron(III) chloride may be prepared past treating iron with chlorine:[11]
-
ii Fe + iii Cl2
→ 2 FeCliii
Solutions of iron(3) chloride are produced industrially both from iron and from ore, in a closed-loop process.
- Dissolving iron ore in muriatic acid
-
Iron3Oiv
+ eight HCl → FeCl2
+ two FeClthree
+ 4 HtwoO
-
Iron3Oiv
- Oxidation of iron(II) chloride with chlorine
-
2 FeCl2
+ Cl2
→ 2 FeCliii
-
2 FeCl2
- Oxidation of iron(Two) chloride with oxygen and hydrochloric acid
-
4 FeCl2
+ Oii
+ 4 HCl → iv FeCl3
+ ii H2O
-
4 FeCl2
Heating hydrated atomic number 26(Iii) chloride does non yield anhydrous ferric chloride. Instead, the solid decomposes into hydrochloric acid and iron oxychloride. Hydrated atomic number 26(Iii) chloride can be converted to the anhydrous grade by treatment with thionyl chloride.[12]
Similarly, dehydration can be effected with trimethylsilyl chloride:[thirteen]
-
FeCl3·6H2O + 12 (CH3)iiiSiCl → FeClthree
+ six ((CHiii)3Si)iiO + 12 HCl
Reactions
[edit]
A brown, acidic solution of atomic number 26(III) chloride
When dissolved in water, iron(III) chloride give a strongly acidic solution.[xiv]
[9]
When heated with fe(III) oxide at 350 °C, iron(3) chloride gives atomic number 26 oxychloride.[xv]
-
FeCl3
+ Atomic number 262O3
→ 3FeOCl
The anhydrous salt is a moderately strong Lewis acid, forming adducts with Lewis bases such as triphenylphosphine oxide; e.g.,
FeCl3(OPPh3)2
where Ph is phenyl. It also reacts with other chloride salts to give the yellow tetrahedral
[FeCl4]−
ion. Salts of
[FeCl4]−
in hydrochloric acid can be extracted into diethyl ether.
Redox reactions
[edit]
Fe(III) chloride is a mild oxidizing amanuensis, for example, information technology oxidizes copper(I) chloride to copper(Two) chloride.
-
FeCl3
+ CuCl → FeClii
+ CuCltwo
In a comproportionation reaction, it reacts with iron to course iron(II) chloride:
-
two FeCl3
+ Fe → 3 FeCltwo
A traditional synthesis of anhydrous ferrous chloride is the reduction of FeClthree
with chlorobenzene:[16]
-
two FeCliii
+ C6H5Cl → 2 FeCl2
+ C6HfourCl2
+ HCl
With carboxylate anions
[edit]
Oxalates react rapidly with aqueous iron(III) chloride to give
[Fe(CiiO4)3]3−
. Other carboxylate salts form complexes; e.thousand., citrate and tartrate.
With alkaline metal alkoxides
[edit]
Alkali metal alkoxides react to give the metal alkoxide complexes of varying complexity.[17]
The compounds can exist dimeric or trimeric.[18]
In the solid stage a variety of multinuclear complexes have been described for the nominal stoichiometric reaction betwixt
FeClthree
and sodium ethoxide:[19]
[xx]
-
FeCl3
+ iii [CH3CH2O]−Na+
→ Fe(OCH2CH3)3
+ three NaCl
With organometallic compounds
[edit]
Iron(III) chloride in ether solution oxidizes methyl lithium
LiCH3
to give first light greenish yellow lithium tetrachloroferrate(3)
Li[FeCliv]
solution and so, with further improver of methyl lithium, lithium tetrachloroferrate(2)
Li2[FeCl4]:[21]
-
2 FeCl3
+ LiCH3
→ FeClii
+ Li[FeCl4] + •CH3
-
Li[FeCl4] + LiCH3
→ Litwo[FeCl4] + •CH3
The methyl radicals combine with themselves or react with other components to give generally ethane
CiiH6
and some marsh gas
CH4
.
Uses
[edit]
Industrial
[edit]
Iron(III) chloride is used in sewage treatment and drinking water production as a coagulant and flocculant.[22]
In this awarding,
FeCl3
in slightly basic water reacts with the hydroxide ion (OH−
) to form a floc of atomic number 26(Iii) hydroxide (Fe(OH)3
), too formulated equally FeO(OH) (ferrihydrite), that tin can remove suspended materials.
-
[Atomic number 26(H2O)6]3+
+ 4 OH−
→ [Fe(OH)4(H2O)2]−
+ 4 H2O → [FeO(OH)ii(H2O)]−
+ 6 H2O
It is also used every bit a leaching agent in chloride hydrometallurgy,[23]
for example in the product of Si from FeSi (Silgrain procedure by Elkem).[24]
Another of import awarding of iron(Iii) chloride is etching copper in two-pace redox reaction to copper(I) chloride and then to copper(II) chloride in the product of printed circuit boards (PCB).[25]
-
FeCliii
+ Cu → FeCltwo
+ CuCl -
FeClthree
+ CuCl → FeCl2
+ CuCl2
Atomic number 26(III) chloride is used equally catalyst for the reaction of ethylene with chlorine, forming ethylene dichloride (1,2-dichloroethane), an important article chemical, which is mainly used for the industrial production of vinyl chloride, the monomer for making PVC.
-
H2C=CH2
+ Cl2
→ ClCHiiCH2Cl
Laboratory apply
[edit]
In the laboratory iron(Iii) chloride is commonly employed as a Lewis acid for catalyzing reactions such as chlorination of effluvious compounds and Friedel–Crafts reaction of aromatics.[
commendation needed
]
It is less powerful than aluminum chloride, merely in some cases this mildness leads to higher yields, for case in the alkylation of benzene:
The ferric chloride test is a traditional colorimetric examination for phenols, which uses a 1% iron(III) chloride solution that has been neutralized with sodium hydroxide until a slight precipitate of FeO(OH) is formed.[26]
The mixture is filtered before use. The organic substance is dissolved in water, methanol or ethanol, and so the neutralized iron(III) chloride solution is added—a transient or permanent coloration (usually royal, green or blue) indicates the presence of a phenol or enol.
This reaction is exploited in the Trinder spot exam, which is used to indicate the presence of salicylates, particularly salicylic acid, which contains a phenolic OH group.
This test can be used to notice the presence of gamma-hydroxybutyric acid and gamma-butyrolactone,[27]
which crusade it to turn red-dark-brown.
Other uses
[edit]
- Used in anhydrous class as a drying reagent in certain reactions.
- Used to detect the presence of phenol compounds in organic synthesis; e.chiliad., examining purity of synthesized Aspirin.
- Used in water and wastewater treatment to precipitate phosphate as iron(Iii) phosphate.
- Used in wastewater treatment for odour control.
- Used by American coin collectors to place the dates of Buffalo nickels that are so badly worn that the appointment is no longer visible.
- Used by bladesmiths and artisans in pattern welding to etch the metal, giving it a contrasting effect, to view metal layering or imperfections.
- Used to etch the widmanstatten pattern in fe meteorites.
- Necessary for the carving of photogravure plates for printing photographic and fine art images in intaglio and for carving rotogravure cylinders used in the press manufacture.
- Used to brand printed excursion boards (PCBs) by etching copper.
- Used to strip aluminum coating from mirrors.
- Used to etch intricate medical devices.
- Used in veterinary practice to treat overcropping of an animal’s claws, particularly when the overcropping results in bleeding.
- Reacts with cyclopentadienylmagnesium bromide in ane grooming of ferrocene, a metal-sandwich complex.[28]
- Sometimes used in a technique of Raku ware firing, the iron coloring a pottery piece shades of pink, brown, and orange.
- Used to test the pitting and cleft corrosion resistance of stainless steels and other alloys.
- Used in conjunction with NaI in acetonitrile to mildly reduce organic azides to chief amines.[29]
- Used in an animal thrombosis model.[30]
- Used in an experimental energy storage systems.[31]
- Historically information technology was used to make straight positive blueprints.[32]
[33] - A component of modified Carnoy’s solution used for surgical treatment of keratocystic odontogenic tumor (KOT).
- Used equally an additive to sodium chloride (NaCl) to produce clear crystals.
Safety
[edit]
Iron(III) chloride is harmful, highly corrosive and acidic. The anhydrous fabric is a powerful dehydrating agent.
Although reports of poisoning in humans are rare, ingestion of ferric chloride can result in serious morbidity and mortality. Inappropriate labeling and storage pb to accidental swallowing or misdiagnosis. Early on diagnosis is important, especially in seriously poisoned patients.
Natural occurrence
[edit]
The natural analogue of
FeCl3
is the rare mineral
molysite, normally related to volcanic and other-blazon fumaroles.[34]
[35]
FeClthree
is also produced as an atmospheric table salt droplets by reaction between iron-rich dust and hydrochloric acrid from bounding main salt. This iron salt aerosol causes most v% of naturally-occurring oxidization of methane and is thought to accept a range of cooling effects.[36]
The temper of the planet Venus is approximately 1%
FeCl3
.[37]
[38]
Encounter too
[edit]
- Verhoeff’s stain
- Ferrosilicon
Notes
[edit]
-
^
An alternative GHS nomenclature from the Japanese GHS Inter-ministerial Committee (2006)[7]
notes the possibility of respiratory tract irritation from
FeCl3
and differs slightly in other respects from the classification used hither.
References
[edit]
-
^
a
b
c
d
e
f
Haynes, William M., ed. (2011).
CRC Handbook of Chemistry and Physics
(92nd ed.). Boca Raton, FL: CRC Printing. p. 4.69. ISBNane-4398-5511-0.
-
^
Haynes, William Thousand., ed. (2011).
CRC Handbook of Chemistry and Physics
(92nd ed.). Boca Raton, FL: CRC Printing. p. iv.133. ISBN1-4398-5511-0.
-
^
a
b
Hashimoto S, Forster Chiliad, Moss SC (1989). “Structure refinement of an FeCl3
crystal using a thin plate sample”.
J. Appl. Crystallogr.
22
(2): 173–180. doi:10.1107/S0021889888013913.
-
^
NIOSH Pocket Guide to Chemic Hazards. “#0346”. National Found for Occupational Safe and Health (NIOSH).
-
^
HSNO Chemical Classification Data Database, New Zealand Environmental Risk Management Potency, retrieved
19 Sep
2010
-
^
Various suppliers, collated by the Baylor College of Dentistry, Texas A&K University. (accessed 2010-09-19) -
^
GHS nomenclature – ID 831, Japanese GHS Inter-ministerial Committee, 2006, retrieved
nineteen Sep
2010
-
^
Holleman AF, Wiberg E (2001). Wiberg N (ed.).
Inorganic Chemistry. San Diego: Academic Press. ISBN978-0-12-352651-9.
-
^
a
b
c
Simon A. Cotton fiber (2018). “Atomic number 26(3) chloride and its coordination chemical science”.
Journal of Coordination Chemical science.
71
(21): 3415–3443. doi:x.1080/00958972.2018.1519188. S2CID 105925459.
-
^
Lind, Yard. D. (1967). “Crystal Structure of Ferric Chloride Hexahydrate”.
The Journal of Chemical Physics.
47
(3): 990–993. Bibcode:1967JChPh..47..990L. doi:10.1063/i.1712067.
-
^
Tarr BR, Booth HS, Dolance A (1950).
Anhydrous Iron(Iii) Chloride. Inorganic Syntheses. Vol. 3. pp. 191–194. doi:10.1002/9780470132340.ch51.
-
^
Pray AR, Heitmiller RF, Strycker S, et al. (1990). “Anhydrous Metal Chlorides”.
Inorganic Syntheses. Vol. 28. pp. 321–323. doi:10.1002/9780470132593.ch80. ISBN9780470132593.
-
^
Boudjouk P, And so JH, Ackermann MN, et al. (1992). “Solvated and Unsolvated Anhydrous Metal Chlorides from Metallic Chloride Hydrates”.
Inorganic Syntheses. Inorganic Syntheses. Vol. 29. pp. 108–111. doi:x.1002/9780470132609.ch26. ISBN9780470132609.
-
^
Housecroft, C. Due east.; Sharpe, A. 1000. (2012).
Inorganic Chemistry
(fourth ed.). Prentice Hall. p. 747. ISBN978-0-273-74275-3.
-
^
Kikkawa South, Kanamaru F, Koizumi M, et al. (1984). “Layered Intercalation Compounds”. In Holt SL Jr (ed.).
Inorganic Syntheses. John Wiley & Sons, Inc. pp. 86–89. doi:10.1002/9780470132531.ch17. ISBN9780470132531.
-
^
P. Kovacic and N. O. Brace (1960). “Iron(2) Chloride”.
Inorganic Syntheses. Inorganic Syntheses. Vol. half dozen. pp. 172–173. doi:10.1002/9780470132371.ch54. ISBN9780470132371.
-
^
Turova NY, Turevskaya EP, Kessler VG, et al., eds. (2002). “12.22.1 Synthesis”.
The Chemistry of Metallic Alkoxides. Springer Science. p. 481. ISBN0306476576.
-
^
Bradley DC, Mehrotra RC, Rothwell I, et al. (2001). “three.2.10. Alkoxides of later 3d metals”.
Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 69. ISBN9780121241407. OCLC 162129468.
-
^
Michael V, Grätz F, Huch V (2001). “Atomic number 269Othree(OCtwoHv)21•C2HfiveOH—A New Construction Type of an Uncharged Iron(III) Oxide-Alkoxide Cluster”.
Eur. J. Inorg. Chem.
2001
(2): 367. doi:10.1002/1099-0682(200102)2001:two<367::AID-EJIC367>three.0.CO;ii-V.
-
^
Seisenbaeva GA, Gohil S, Suslova EV, et al. (2005). “The synthesis of iron (Iii) ethoxide revisited: Characterization of the metathesis products of iron (Three) halides and sodium ethoxide”.
Inorg. Chim. Acta.
358
(12): 3506–3512. doi:ten.1016/j.ica.2005.03.048.
-
^
Berthold HJ, Spiegl HJ (1972). “Über die Bildung von Lithiumtetrachloroferrat(II) Li2FeCl4
bei der Umsetzung von Eisen(III)-chlorid mil Lithiummethyl (ane:1) in ätherischer Lösung”.
Z. Anorg. Allg. Chem.
(in High german).
391
(three): 193–202. doi:10.1002/zaac.19723910302.
-
^
Water Treatment Chemicals
(PDF). Akzo Nobel Base Chemicals. 2007. Archived from the original
(PDF)
on 13 August 2010. Retrieved
26 Oct
2007.
-
^
Park KH, Mohapatra D, Reddy BR (2006). “A report on the acidified ferric chloride leaching of a circuitous (Cu–Ni–Co–Iron) matte”.
Separation and Purification Technology.
51
(three): 332–337. doi:10.1016/j.seppur.2006.02.013.
-
^
Dueñas Díez Thou, Fjeld M, Andersen E, et al. (2006). “Validation of a compartmental population balance model of an industrial leaching procedure: The Silgrain process”.
Chem. Eng. Sci.
61
(1): 229–245. doi:x.1016/j.ces.2005.01.047.
-
^
Greenwood NN, Earnshaw A (1997).
Chemistry of the Elements
(2d ed.). Oxford: Butterworth-Heinemann. p. 1084. ISBN9780750633659.
-
^
Furniss BS, Hannaford AJ, Smith PW, et al. (1989).
Vogel’southward Textbook of Practical Organic Chemical science
(fifth ed.). New York: Longman/Wiley. ISBN9780582462366.
-
^
Zhang SY, Huang ZP (2006). “A color test for rapid screening of gamma-hydroxybutyric acid (GHB) and gamma-butyrolactone (GBL) in beverage and urine”.
Fa Yi Xue Za Zhi.
22
(half dozen): 424–vii. PMID 17285863.
-
^
Kealy TJ, Pauson PL (1951). “A New Blazon of Organo-Iron Chemical compound”.
Nature.
168
(4285): 1040. Bibcode:1951Natur.168.1039K. doi:x.1038/1681039b0. S2CID 4181383.
-
^
Kamal A, Ramana K, Ankati H, et al. (2002). “Mild and efficient reduction of azides to amines: synthesis of fused [ii,1-b]quinazolines”.
Tetrahedron Lett.
43
(38): 6861–6863. doi:10.1016/S0040-4039(02)01454-5.
-
^
Tseng 1000, Dozier A, Haribabu B, et al. (2006). “Transendothelial migration of ferric ion in FeCliii
injured murine common carotid artery”.
Thromb. Res.
118
(ii): 275–280. doi:ten.1016/j.thromres.2005.09.004. PMID 16243382.
-
^
Manohar, Aswin K.; Kim, Kyu Min; Plichta, Edward; Hendrickson, Mary; Rawlings, Sabrina; Narayanan, S. R. (28 October 2015). “A High Efficiency Fe-Chloride Redox Flow Bombardment for Large-Scale Energy Storage”.
Journal of the Electrochemical Guild.
163
(1): A5118. doi:10.1149/2.0161601jes. ISSN 1945-7111. S2CID 100823390.
-
^
US Patent 241713, Pellet H, “Method of preparing paper”, published 1881
-
^
Lietze E (1888).
Modern Heliographic Processes. New York: D. Van Norstrand Company. pp. 65.
-
^
“Molysite”.
www.mindat.org.
-
^
“Listing of Minerals”.
world wide web.ima-mineralogy.org. March 21, 2011.
-
^
Oeste, Franz Dietrich; de Richter, Renaud; Ming, Tingzhen; Caillol, Sylvain (January 13, 2017). “Climate engineering science by mimicking natural dust climate control: the iron salt aerosol method”.
Earth Arrangement Dynamics.
8
(1): 1–54. Bibcode:2017ESD…..8….1O. doi:10.5194/esd-viii-1-2017 – via esd.copernicus.org.
-
^
Krasnopolsky, Five. A.; Parshev, 5. A. (1981). “Chemical composition of the atmosphere of Venus”.
Nature.
292
(5824): 610–613. Bibcode:1981Natur.292..610K. doi:x.1038/292610a0. S2CID 4369293.
-
^
Krasnopolsky, Vladimir A. (2006). “Chemical composition of Venus atmosphere and clouds: Some unsolved issues”.
Planetary and Space Science.
54
(xiii–14): 1352–1359. Bibcode:2006P&SS…54.1352K. doi:x.1016/j.pss.2006.04.019.
Further reading
[edit]
-
Lide DR, ed. (1990).
CRC Handbook of Chemical science and Physics
(71st ed.). Ann Arbor, MI, The states: CRC Press. ISBN9780849304712.
-
Stecher PG, Finkel MJ, Siegmund OH, eds. (1960).
The Merck Index of Chemicals and Drugs
(7th ed.). Rahway, NJ, USA: Merck & Co.
-
Nicholls D (1974).
Complexes and First-Row Transition Elements, Macmillan Press, London, 1973. A Macmillan chemistry text. London: Macmillan Press. ISBN9780333170885.
-
Wells AF (1984).
Structural Inorganic Chemistry. Oxford scientific discipline publications (5th ed.). Oxford, Great britain: Oxford University Press. ISBN9780198553700.
-
March J (1992).
Advanced Organic Chemistry
(quaternary ed.). New York: John Wiley & Sons, Inc. pp. 723. ISBN9780471581482.
-
Reich HJ, Rigby HJ, eds. (1999).
Acidic and Bones Reagents. Handbook of Reagents for Organic Synthesis. New York: John Wiley & Sons, Inc. ISBN9780471979258.
The Compound Fecl3 is Made of
Source: https://en.wikipedia.org/wiki/Iron%28III%29_chloride