Carbon monofluoride
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'''Carbon monofluoride''' ('''CF''', '''CF<sub>x</sub>''', or '''(CF)<sub>x</sub>'''), also called '''polycarbon monofluoride''', '''polycarbon fluoride''', '''poly(carbon monofluoride)''', and '''graphite fluoride''', is a material formed by high-temperature reaction of [[fluorine]] gas with [[graphite]], [[charcoal]], or [[pyrolytic carbon]] powder. Its [[CAS number]] is {{CASREF|CAS=51311-17-2}}. In contrary to [[graphite intercalation compounds]] it is a [[covalent]] graphite compound.
Carbon is stable in fluorine atmosphere up to about 400 °C, but between 420-600 °C reaction takes place to give sub[[stoichiometric]] carbon monofluoride, CF<sub>0.68</sub> appearing dark grey. With increasing temperature and fluorine pressure stoichiometries up to CF<sub>1.12</sub> are formed. With increasing fluorine content the colour changes from dark grey to cream white indicating the loss of the aromatic character. The fluorine atoms are located in an alternating fashion above and under the former [[graphene]] plane, which is now buckled due to formation of [[covalent]] carbon-fluorine bonds. Reaction of carbon with fluorine at even higher temperature successively destroys the graphite compound to yield a mixture of gaseous [[fluorocarbon]]s such as e.g. tetrafluorocarbon, CF<sub>4</sub>, and tetrafluoroethylene, C<sub>2</sub>F<sub>4</sub>. <ref>[http://www.bbc.co.uk/dna/h2g2/A6359060 BBC - h2g2 - Carbon and its Inorganic Compounds<!-- Bot generated title -->]</ref>
In a similar fashion the recently found [[carbon]] [[allotrope]] [[fullerene]], C<sub>60</sub> reacts with fluorine gas to give fullerene fluorides with stoichiometries up to C<sub>60</sub>F<sub>48</sub> <ref>[http://www3.interscience.wiley.com/cgi-bin/abstract/84002199/ABSTRACT]O. V. Boltalina et al. Two isomers of C<sub>60</sub>F<sub>48</sub>: An Indented Fullerene, ''Int Ed. Angew.Chem. 40'' '''2001''', 2285 </ref>.
A precursor of carbon monofluoride is the '''fluorine-graphite intercalation compound''', also called '''fluorine-GIC'''.
Other intercalation fluorides of carbon are:
* [[poly(dicarbon fluoride)]] ((C<sub>2</sub>F)<sub>n</sub>)
* [[tetracarbon monofluoride]] (TCMF, C<sub>4</sub>F)
==Application==
Carbon monofluoride is used as a high [[energy density]] [[cathode]] material in [[lithium battery|lithium batteries]] of the "BR" type. Other uses are a [[wear]] reduction additive for [[lubricant]]s, and weather-resistant additive for [[paint]]s. Graphite fluoride is also used as both [[oxidizing agent]] and [[combustion modifier]] in [[rocket propellant]]s and [[pyrolant]]s <ref>[http://www3.interscience.wiley.com/cgi-bin/abstract/110531872/ABSTRACT] E.-C. Koch, Metal/Fluorocarbon Pyrolants: VI. Combustion Behaviour and Radiation Properties of Magnesium/Poly(Carbon Monofluoride) Pyrolant, ''Prop.,Expl.,Pyrotech. 30'' '''2005''', 209</ref>
==References==
A useful monograph on graphite fluorides has been written by Watanabe and coworkers <ref>N. Watanabe
T. Nakajima,H. Touhara, Graphite Fluorides, Elsevier, 1988 [http://www.elsevier.com/wps/find/bookdescription.librarians/500042/description#toc]
</ref>
<references/>
==External links==
[[Category:Inorganic carbon compounds]]
[[Category:Fluorides]]