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:''Ferruginous redirects here. For the bird, see Ferruginous Hawk''
Altogether there are sixteen known iron oxides.[1] These compounds are either oxides (Wüstite, Hematite, β-Fe2O3, Maghemite, γ-Fe2O3, ε-Fe2O3, Magnetite, Ferrihydrite), or hydroxides and oxide-hydroxides (Goethite, Akaganéite, Lepidocrocite, Feroxyhyte,
Bernalite, Schwertmannite and green rusts).
Some of these oxides are used in ceramic applications, particularly in glazing. Many metal oxides provide the colours in glazes after being fired at high temperatures.
Iron oxides yield pigments (see ) that are widely used in the cosmetic field. They are considered to be nontoxic, moisture resistant, and nonbleeding. Iron oxides graded safe for cosmetic use are produced synthetically in order to avoid the inclusion of ferrous or ferric oxides, and impurities normally found in naturally occurring iron oxides.
An array of statistics, including production, description, prices, consumption and foreign trade can be found at http://minerals.usgs.gov/minerals/pubs/commodity/iron_oxide/
★ Iron(II) oxide (FeO) or ferrous oxide is also known as wüstite in its mineral form. The black-coloured powder in particular can cause explosions as it readily ignites.
★ Iron(III) oxide (Fe2O3) or ferric oxide is also known as hematite or maghemite in its mineral form, or rouge as an industrial chemical. Purified, it is used as a coating in magnetic audio and computer media. In a dry or alkaline environment it can cause passivation and inhibits rust, yet it is also a component of rust.
★ Iron(II,III) oxide (Fe3O4) or ferrous ferric oxide is also known as magnetite or lodestone in its mineral form. Magnetite is an iron ore. This form of iron oxide tends to occur when iron corrodes underwater, and so is often found inside tanks or below the waterline of ships.
It is not difficult to extract iron from ore as compared to the similarly abundant elements aluminum and titanium.
1. The iron oxides: structure, properties, reactions, occurrences and uses, , RM, Cornell, Wiley VCH, 2003, ISBN 3-527-30274-3
★ http://chemed.chem.purdue.edu/demos/demosheets/12.3.html
Iron oxide pigment
Altogether there are sixteen known iron oxides.[1] These compounds are either oxides (Wüstite, Hematite, β-Fe2O3, Maghemite, γ-Fe2O3, ε-Fe2O3, Magnetite, Ferrihydrite), or hydroxides and oxide-hydroxides (Goethite, Akaganéite, Lepidocrocite, Feroxyhyte,
Bernalite, Schwertmannite and green rusts).
Some of these oxides are used in ceramic applications, particularly in glazing. Many metal oxides provide the colours in glazes after being fired at high temperatures.
Iron oxides yield pigments (see ) that are widely used in the cosmetic field. They are considered to be nontoxic, moisture resistant, and nonbleeding. Iron oxides graded safe for cosmetic use are produced synthetically in order to avoid the inclusion of ferrous or ferric oxides, and impurities normally found in naturally occurring iron oxides.
An array of statistics, including production, description, prices, consumption and foreign trade can be found at http://minerals.usgs.gov/minerals/pubs/commodity/iron_oxide/
| Contents |
| Iron oxides |
| References |
| External links |
Iron oxides
★ Iron(II) oxide (FeO) or ferrous oxide is also known as wüstite in its mineral form. The black-coloured powder in particular can cause explosions as it readily ignites.
★ Iron(III) oxide (Fe2O3) or ferric oxide is also known as hematite or maghemite in its mineral form, or rouge as an industrial chemical. Purified, it is used as a coating in magnetic audio and computer media. In a dry or alkaline environment it can cause passivation and inhibits rust, yet it is also a component of rust.
★ Iron(II,III) oxide (Fe3O4) or ferrous ferric oxide is also known as magnetite or lodestone in its mineral form. Magnetite is an iron ore. This form of iron oxide tends to occur when iron corrodes underwater, and so is often found inside tanks or below the waterline of ships.
It is not difficult to extract iron from ore as compared to the similarly abundant elements aluminum and titanium.
References
1. The iron oxides: structure, properties, reactions, occurrences and uses, , RM, Cornell, Wiley VCH, 2003, ISBN 3-527-30274-3
External links
★ http://chemed.chem.purdue.edu/demos/demosheets/12.3.html
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