Iron(II) fluoride: Difference between revisions

Latest revision as of 06:22, 16 February 2025

Iron(II) fluoride[edit]

3D model of the rutile unit cell, similar to the structure of Iron(II) fluoride

Iron(II) fluoride, also known as ferrous fluoride, is an inorganic compound with the chemical formula FeF_. It is a pale green crystalline solid that is used in various industrial applications, including as a catalyst in organic synthesis and in the manufacture of ceramics.

Structure[edit]

Iron(II) fluoride crystallizes in the rutile structure, which is a common structure for many metal fluorides and oxides. In this structure, each iron ion is surrounded by six fluoride ions in an octahedral geometry. The fluoride ions are shared between adjacent iron centers, forming a three-dimensional network.

Properties[edit]

Iron(II) fluoride is a pale green solid that is relatively stable in air. It is insoluble in water but can dissolve in acids. The compound is known for its high melting point and thermal stability, making it suitable for high-temperature applications.

Applications[edit]

Iron(II) fluoride is used in the production of ceramics and as a catalyst in various chemical reactions. It is also employed in the synthesis of certain organic compounds, where it can facilitate fluorination reactions.

Safety[edit]

As with many metal fluorides, iron(II) fluoride should be handled with care. It can be harmful if ingested or inhaled, and appropriate safety measures should be taken to avoid exposure.

Related pages[edit]

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-'''Iron(II) fluoride''', also known as '''ferrous fluoride''', is an inorganic compound with the formula FeF<sub>2</sub>. It is one of two main fluoride compounds of [[iron]], the other being [[iron(III) fluoride]] or ferric fluoride, with the formula FeF<sub>3</sub>. Iron(II) fluoride is a white to greenish solid that is highly soluble in water, producing a greenish solution. It is more commonly found in its hydrated form FeF<sub>2</sub>·4H<sub>2</sub>O.
+{{DISPLAYTITLE:Iron(II) fluoride}}
-==Properties==
+== Iron(II) fluoride ==
-Iron(II) fluoride exists in an anhydrous form as well as in a tetrahydrate form (FeF<sub>2</sub>·4H<sub>2</sub>O). The anhydrous form adopts a rutile structure, similar to many other metal dihalides. In this structure, the iron atoms are six-coordinate, surrounded by six fluoride ions in an octahedral geometry. The tetrahydrate form has a more complex structure.
+[[File:Rutile-unit-cell-3D-balls.png|thumb|right|3D model of the rutile unit cell, similar to the structure of Iron(II) fluoride]]
-The compound is relatively stable, but it can be oxidized by atmospheric oxygen to [[iron(III) fluoride]], especially in the presence of moisture.
+'''Iron(II) fluoride''', also known as '''ferrous fluoride''', is an inorganic compound with the chemical formula '''FeF_'''. It is a pale green crystalline solid that is used in various industrial applications, including as a catalyst in organic synthesis and in the manufacture of ceramics.
-==Synthesis==
+== Structure ==
-Iron(II) fluoride can be prepared by reacting [[iron]] or iron(II) compounds with [[hydrogen fluoride]] (HF). For example, iron metal reacts with hydrogen fluoride to produce iron(II) fluoride and hydrogen gas:
+Iron(II) fluoride crystallizes in the [[rutile]] structure, which is a common structure for many metal fluorides and oxides. In this structure, each iron ion is surrounded by six fluoride ions in an octahedral geometry. The fluoride ions are shared between adjacent iron centers, forming a three-dimensional network.
-\[ \text{Fe} + 2\text{HF} \rightarrow \text{FeF}_2 + \text{H}_2 \]
+== Properties ==
+Iron(II) fluoride is a pale green solid that is relatively stable in air. It is insoluble in water but can dissolve in acids. The compound is known for its high melting point and thermal stability, making it suitable for high-temperature applications.
-Alternatively, iron(II) chloride or iron(II) sulfate can be reacted with sodium fluoride or hydrofluoric acid to yield iron(II) fluoride.
+== Applications ==
+Iron(II) fluoride is used in the production of [[ceramics]] and as a catalyst in various chemical reactions. It is also employed in the synthesis of certain organic compounds, where it can facilitate fluorination reactions.
-==Applications==
+== Safety ==
-Iron(II) fluoride is used in several applications, including:
+As with many metal fluorides, iron(II) fluoride should be handled with care. It can be harmful if ingested or inhaled, and appropriate safety measures should be taken to avoid exposure.
-* As a catalyst in organic synthesis.
+== Related pages ==
-* In the manufacture of ceramics.
+* [[Iron(III) fluoride]]
-* As a reagent in the laboratory.
-* In lithium-ion batteries as a potential cathode material due to its high electrochemical stability and capacity.
-==Safety==
-Iron(II) fluoride should be handled with care, as it is toxic if ingested and can cause irritation to the skin and eyes. It is also hazardous when inhaled, as it can cause respiratory tract irritation. Proper personal protective equipment should be worn when handling this chemical.
-==See Also==
 * [[Fluoride]]
-* [[Iron compounds]]
+* [[Rutile]]
-* [[Hydrogen fluoride]]
+* [[Inorganic chemistry]]
-* [[Lithium-ion battery]]
 [[Category:Iron compounds]]
 [[Category:Fluorides]]
 [[Category:Inorganic compounds]]