Iron(III) nitrate

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Iron(III) nitrate
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Chemical structure of ferric nitrate aquo complex
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Sample of ferric nitrate nonahydrate
Names
IUPAC name
Iron(III) nitrate
Other names
Ferric nitrate
Nitric acid, iron(3+) salt
Identifiers
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3D model (JSmol)
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  • InChI=1S/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;; checkY
    Key: SZQUEWJRBJDHSM-UHFFFAOYSA-N checkY
  • InChI=1/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;;
    Key: SZQUEWJRBJDHSM-UHFFFAOYAC
  • [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Fe+3]
Properties
Fe(NO3)3
Molar mass 403.999 g/mol (nonahydrate)
241.86 g/mol (anhydrous)
Appearance Pale violet crystals
hygroscopic
Density 1.68 g/cm3 (hexahydrate)
1.6429 g/cm3(nonahydrate)
Melting point 47.2 °C (117.0 °F; 320.3 K) (nonahydrate)
Boiling point 125 °C (257 °F; 398 K) (nonahydrate)
150 g/100 mL (hexahydrate)
Solubility soluble in alcohol, acetone
+15,200.0·10−6 cm3/mol
Structure
octahedral
Hazards[2]
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1
0
0
OX
Flash point non-flammable
NIOSH (US health exposure limits):
REL (Recommended)
 TWA 1 mg/m3[1]
Related compounds
Other anions
 Iron(III) chloride
Iron(III) sulfate
Related compounds
 Iron(II) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Template:Chembox Footer/trackingTemplate:Short description

Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO3)3.(H2O)n. Most common is the nonahydrate Fe(NO3)3.(H2O)9. The hydrates are all pale colored, water-soluble paramagnetic salts.

Hydrates

Iron(III) nitrate is deliquescent, and it is commonly found as the nonahydrate Fe(NO3)3·9H2O, which forms colourless to pale violet crystals. This compound is the trinitrate salt of the aquo complex [Fe(H2O)6]3+.[3] Other hydrates Fe(NO
3)
3·xH
2O, include:

  • tetrahydrate (x=4), more precisely triaqua dinitratoiron(III) nitrate monohydrate, Page Module:Chem2/styles.css has no content.[Fe(NO3)2(H2O)3]NO3·H2O, has complex cations wherein Fe3+ is coordinated with two nitrate anions as bidentate ligands and three of the four water molecules, in a pentagonal bipyramid configuration with two water molecules at the poles.[4]
  • pentahydrate (x=5), more precisely penta-aqua nitratoiron(III) dinitrate, Page Module:Chem2/styles.css has no content.[Fe(NO3)(H2O)5](NO3)2, in which the Fe3+ ion is coordinated to five water molecules and a unidentate nitrate anion ligand in octahedral configuration.[4]
  • hexahydrate (x=6), more precisely hexaaquairon(III) trinitrate, Page Module:Chem2/styles.css has no content.[Fe(H2O)6](NO3)3, where the Fe3+ ion is coordinated to six water molecules in octahedral configuration.[4]

Reactions

Iron(III) nitrate is a useful precursor to other iron compounds because the nitrate is easily removed or decomposed. It is for example, a standard precursor to potassium ferrate Page Module:Chem2/styles.css has no content.K2FeO4.[5]

When dissolved, iron(III) nitrate forms yellow solutions. When this solution is heated to near boiling, nitric acid evaporates and a solid precipitate of iron(III) oxide Fe
2O
3 appears.[6] Another method for producing iron oxides from this nitrate salt involves neutralizing its aqueous solutions.[7]

Preparation

The compound can be prepared by treating iron metal powder with nitric acid, as summarized by the following idealized equation:[8]

Page Module:Chem2/styles.css has no content.Fe + 4 HNO3 + 7 H2O → Fe(NO3)3(H2O)9 + NO

Applications

Ferric nitrate has no large scale applications. It is a catalyst for the synthesis of sodium amide from a solution of sodium in ammonia:[9]

Page Module:Chem2/styles.css has no content.2 NH3 + 2Na → 2 NaNH2 + H2

Certain clays impregnated with ferric nitrate have been shown to be useful oxidants in organic synthesis. For example, ferric nitrate on Montmorillonite—a reagent called Clayfen—has been employed for the oxidation of alcohols to aldehydes and thiols to disulfides.[10]

Ferric nitrate solutions are used by jewelers and metalsmiths to etch silver and silver alloys.

References

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  1. ^ Page Module:Citation/CS1/styles.css has no content.NIOSH Pocket Guide to Chemical Hazards. "#0346". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ Page Module:Citation/CS1/styles.css has no content.HSNO Chemical Classification Information Database, New Zealand Environmental Risk Management Authority, retrieved 2010-09-19.
  3. ^ Page Module:Citation/CS1/styles.css has no content.Hair, Neil J.; Beattie, James K. (1977). "Structure of Hexaaquairon(III) Nitrate Trihydrate. Comparison of Iron(II) and Iron(III) Bond Lengths in High-Spin Octahedral Environments". Inorganic Chemistry. 16 (2): 245–250. doi:10.1021/ic50168a006.
  4. ^ a b c H. Schmidt, A. Asztalos, F. Bok and W. Voigt (2012): "New Iron(III) Nitrate Hydrates: Page Module:Chem2/styles.css has no content.Fe(NO3|3·xH2O with x = 4, 5 and 6". Acta Crystallographica Section C - Inorganic Compounds, volume C68, pages i29-i33. Script error: No such module "CS1 identifiers".
  5. ^ Page Module:Citation/CS1/styles.css has no content.H. Lux (1963). "Potassium Ferrate (VI) K2FeO4". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1504.
  6. ^ Egon Matijević and Paul Scheiner (1978): "Ferric Hydrous Oxide Sols: III. Preparation of Uniform Particles by Hydrolysis of Fe(III)-Chloride, -Nitrate, and -Perchlorate solutions". Journal of Colloid and Interface Science, volume 63, issue 3, pages 509-524. Script error: No such module "CS1 identifiers".
  7. ^ Page Module:Citation/CS1/styles.css has no content.H. Lux (1963). "Iron (III) Hydroxide FeO(OH)". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1499.
  8. ^ Script error: No such module "Template wrapper".
  9. ^ Page Module:Citation/CS1/styles.css has no content.Hampton, K. G.; Harris, T. M.; Hauser, C. R. (1973). "2,4-Nonanedione". Organic Syntheses; Page Module:Citation/CS1/styles.css has no content.Collected Volumes, vol. 5, p. 848. As of 2007, 22 other entries describe similar preparations in Organic Syntheses
  10. ^ Cornélis, A. Laszlo, P.; Zettler, M. W. "Iron(III) Nitrate–K10 Montmorillonite Clay" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. Script error: No such module "CS1 identifiers"..

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