4:["$","div",null,{"className":"min-h-screen bg-white flex flex-col","children":[["$","div",null,{"className":"px-6 pt-6 pb-4 border-b border-gray-100","children":[["$","div",null,{"className":"flex items-center gap-1.5 text-xs text-gray-400 mb-4","children":[["$","a",null,{"href":"/","className":"hover:text-[#26a69a] transition-colors","children":"Market"}],["$","span",null,{"children":"›"}],["$","span",null,{"className":"text-gray-600","children":"Iron(II) oxalate"}]]}],["$","div",null,{"className":"text-[10px] text-gray-400 uppercase tracking-widest mb-1","children":"Company Profile"}],["$","h1",null,{"className":"text-2xl font-bold text-gray-900","children":"Iron(II) oxalate"}],null]}],["$","div",null,{"className":"flex-1 px-6 py-6","children":[["$","p",null,{"className":"text-sm text-gray-600 leading-relaxed mb-8","children":"Ferrous oxalate (iron(II) oxalate) refers to the inorganic compound with the formula FeC2O4 (anhydrous) or FeC2O4·2H2O (dihydrate). These are yellow compounds. Characteristic of metal oxalate complexes, these compounds tend to be polymeric, hence their low solubility in water. The dihydrate is hygroscopic."}],["$","div",null,{"className":"columns-1 md:columns-2 gap-10","children":[["$","div","0",{"className":"mb-8 break-inside-avoid","children":[["$","div",null,{"className":"text-xs font-semibold text-gray-400 uppercase tracking-wide mb-3 border-b border-gray-100 pb-1","children":"Structure"}],["$","div",null,{"className":"text-sm text-gray-600 leading-relaxed wiki-content","dangerouslySetInnerHTML":{"__html":"Like other iron oxalates, ferrous oxalates feature octahedral Fe centers. The dihydrate is a coordination polymer, consisting of chains of oxalate-bridged ferrous centers, each with two aquo ligands. == Reactions =="}}]]}],["$","div","1",{"className":"mb-8 break-inside-avoid","children":[["$","div",null,{"className":"text-xs font-semibold text-gray-400 uppercase tracking-wide mb-3 border-b border-gray-100 pb-1","children":"Reactions"}],["$","div",null,{"className":"text-sm text-gray-600 leading-relaxed wiki-content","dangerouslySetInnerHTML":{"__html":"When heated to , the dihydrate dehydrates, and the anhydrous ferrous oxalate decomposes near . The products of thermal decomposition in a sealed environment are a mixture of iron oxides, pyrophoric iron, carbon dioxide, carbon monoxide, and water. Ferrous oxalates are precursors to iron phosphates, which are of value in batteries. ==Natural occurrence=="}}]]}],["$","div","2",{"className":"mb-8 break-inside-avoid","children":[["$","div",null,{"className":"text-xs font-semibold text-gray-400 uppercase tracking-wide mb-3 border-b border-gray-100 pb-1","children":"Natural occurrence"}],["$","div",null,{"className":"text-sm text-gray-600 leading-relaxed wiki-content","dangerouslySetInnerHTML":{"__html":"Anhydrous iron(II) oxalate is unknown among minerals . However, the dihydrate is known as humboldtine. A related mineral is stepanovite (), an unusual example of a naturally occurring ferrioxalate. ==See also=="}}]]}]]}],["$","div",null,{"className":"mt-8 pt-4 border-t border-gray-100","children":["$","a",null,{"href":"https://en.wikipedia.org/wiki/Iron(II)%20oxalate","target":"_blank","rel":"noopener noreferrer","className":"text-xs text-gray-400 hover:text-gray-600 transition-colors","children":"Source: Wikipedia ↗"}]}]]}],"$Lf"]}]