However, they can be produced at home by using bleach, and can be stabilized by precipitation with barium. These are only stable in strongly basic solutions and will degrade after about a day. This can be used to make fake blood as a party trick.īoth oxidation states readily from complexes with water, cyanide, nitrous oxide (ferrous only) and oxalates (ferric only) įerrates(VI) are compounds of iron in the +6 state. When an iodide-containing solution is added to a solution containing ferric ion, iron(II) iodide and iron precipitate.Ī relatively sensitive test for ferric iron is the addition of thiocyanates, which form a deep red complex. Iron(III) iodide is unstable with respect to disproportionation. Ferric compounds, such as iron(III) chloride, are strongly Lewis acidic. A small amount of acid will turn this solution clear as the 2+ is converted to 3+. One example is iron(III) nitrate: it is lavender in the solid state, but dissolves to form a rust-colored solution, with the dominant iron species being 2+. However, interesting color changes may occur due to complex formation. This is a source of annoyance for most chemists. The ferric state of iron is only soluble in acidic solutions and will quickly convert to hydrous iron(III) oxide if the acidity is reduced. Solid iron(II) sulfate may oxidize in air to form iron(III) oxide deposits. In basic solution, however, iron(II) oxide will precipitate and be oxidized by water to iron(III) oxide. The ferrous state of iron is normally soluble in water and is resistant to oxidation in acidic solution.
Iron metal will react with diluted acids, such as hydrochloric acid, but passivates in contact with concentrated acids, such as nitric acid or phosphoric acid. In solution, iron tends to form ferrous salts, but the addition of hydrogen peroxide (and often atmospheric oxygen) will promote the formation of ferric compounds. It will also react with sulfur at elevated temperatures if finely divided to form iron sulfide (FeS). Iron reacts with the halogens to form its halide salts. Magnetite may be produced by ignition of steel wool. It also will form mixed valence compounds like magnetite (Fe 3O 4), that contain both ferrous and ferric state iron in their structure. Iron reacts with air in the presence of water to form Fe 2O 3, commonly known as rust. Other oxidation states are possible present no interest to the amateur chemist. Iron forms compounds most commonly found in it's ferrous(II) and ferric(III) oxidation states, but it can exist in the (IV) and (VI) valence states as ferrates. Very pure single-crystal iron, used for research purposes, is far weaker structurally than aluminum metal. It is known to exist in four allotropes, and it may exist in a fifth. It is commonly known to be ferromagnetic, the word being partially derived from the Latin word for iron.
It has a melting point of 1538 degrees C.
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