IRON OXIDE

 

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Iron oxide is just rust to you and me, but ferric oxide to chemists.  Although it exists in abundance in nature, it is impossible to purify to acceptable safety standards.  As a result, all iron oxide today is synthetically prepared.  Depending on how iron oxide is prepared, it can develop different colors: yellow, red, brown and black.  Different colors of iron oxide depend upon the oxidative state of the iron atom, with Fe+3 appearing brown and Fe+2 appearing red.  Different colors of iron oxide also depend upon the amount of water added to the iron atom (iron hydroxides).  This variation gives rise to the yellow, red, brown, and black colors.

Application:

Iron oxide is an insoluble mineral pigment.  Consequently, its use in foods is limited.  In comparison, iron oxide is used extensively in the cosmetic industry where it is combined with titanium dioxide to make a host of red, pink, beige, tan, and black colors.  It is also combined with mica, making a wide variety of &#;pearlescent&#; colors used extensively in the cosmetic industry.

Class of chemical compounds composed of iron and oxygen

Electrochemically oxidized iron (rust)

Iron oxides are chemical compounds composed of iron and oxygen. Several iron oxides are recognized. Often they are non-stoichiometric. Ferric oxyhydroxides are a related class of compounds, perhaps the best known of which is rust.[1]

Iron oxides and oxyhydroxides are widespread in nature and play an important role in many geological and biological processes. They are used as iron ores, pigments, catalysts, and in thermite, and occur in hemoglobin. Iron oxides are inexpensive and durable pigments in paints, coatings and colored concretes. Colors commonly available are in the "earthy" end of the yellow/orange/red/brown/black range. When used as a food coloring, it has E number E172.

Stoichiometries

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Iron oxide pigment. The brown color indicates that iron is at the oxidation state +3. Green and reddish brown stains on a limestone core sample, respectively corresponding to oxides/hydroxides of Fe2+ and Fe3+.

Iron oxides feature as ferrous (Fe(II)) or ferric (Fe(III)) or both. They adopt octahedral or tetrahedral coordination geometry. Only a few oxides are significant at the earth's surface, particularly wüstite, magnetite, and hematite.

Thermal expansion

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• goethite (α-FeOOH)
• akaganéite (β-FeOOH)
• lepidocrocite (γ-FeOOH)
• feroxyhyte (δ-FeOOH)
• ferrihydrite (Fe5HO8 · 4 H2O approx., or 5 Fe2O3 · 9 H2O, better recast as FeOOH · 0.4 H2O)
• high-pressure pyrite-structured FeOOH.

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  Once dehydration is triggered, this phase may form FeO2Hx (0 < x < 1).

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• green rust (Fe

  III
  x

  Fe

  II
  y

  OH3x + y &#; z (A&#;)z where A&#; is Cl&#; or 0.5

  SO

  2&#;

  4

  )

Reactions

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In blast furnaces and related factories, iron oxides are converted to the metal. Typical reducing agents are various forms of carbon. A representative reaction starts with ferric oxide:[9]

2 Fe2O3 + 3 C &#; 4 Fe + 3 CO2

In nature

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Iron is stored in many organisms in the form of ferritin, which is a ferrous oxide encased in a solubilizing protein sheath.[10]

Species of bacteria, including Shewanella oneidensis, Geobacter sulfurreducens and Geobacter metallireducens, use iron oxides as terminal electron acceptors.[11]

Uses

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Almost all iron ores are oxides, so in that sense these materials are important precursors to iron metal and its many alloys.

Iron oxides are important pigments, coming in a variety of colors (black, red, yellow). Among their many advantages, they are inexpensive, strongly colored, and nontoxic.[12]

Magnetite is a component of magnetic recording tapes.

See also

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References

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