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Fluorographene
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<p>Fluorographene (or perfluorographane, graphene fluoride) is a <a href="/facts/Fluorocarbon/jA9N6aoT">fluorocarbon</a> derivative of <a href="/facts/Graphene/QDGUBaPt">graphene</a>. It is a two dimensional <a href="/facts/Carbon/ukrgQexo">carbon</a> sheet of <a href="/facts/Orbital_hybridisation/Fl7sz8Jm">sp3 hybridized</a> <a href="/facts/Carbon/ukrgQexo">carbons</a>, with each carbon atom bound to one <a href="/facts/Fluorine/YUV0Fb8m">fluorine</a>. The chemical formula is (CF)n. In comparison, Teflon (<a href="/facts/Polytetrafluoroethylene/jesBNXKq">polytetrafluoroethylene</a>), -(CF2)n-, consists of carbon "chains" with each carbon bound to two fluorines. </p><p>Unlike fluorographene, graphene is <a href="/facts/Saturated_and_unsaturated_compounds/tde2C216">unsaturated</a> (<a href="/facts/Orbital_hybridisation/Fl7sz8Jm">sp2 hybridized</a>) and completely carbon. The <a href="/facts/Hydrocarbon/Dcg95Ju5">hydrocarbon</a> analogue to fluorographene is sp3 hybridized <a href="/facts/Graphane/3QMVg24s">graphane</a>. Similar to other fluorocarbons (e.g. <a href="/facts/Perfluorohexane/S2FC7yI5">perfluorohexane</a>), fluorographene is highly insulating. Fluorographene is thermally stable, resembling <a href="/facts/Polytetrafluoroethylene/jesBNXKq">polytetrafluoroethylene</a>; however, chemically it is reactive. It can be transformed back into graphene by reaction with <a href="/facts/Potassium_iodide/6023uFnx">potassium iodide</a> at high temperatures. During reactions of fluorographene with <a href="/facts/Sodium_hydroxide/xjtdYtq7">NaOH</a> and <a href="/facts/Sodium_hydrosulfide/xFnzITR9">NaSH</a> simultaneous reductive defluorination and substitution are observed. The reactivity of fluorographene represents a facile way towards graphene derivatives. </p>