Potassium hexacyanoferrate (III) complex has octahedron geometry, and the ions are kinetically unstable due to dissociation in the solution. It also has monoclinic and orthorhombic crystals showed only one doublet on the spectrum in phases of high and low temperatures. The compound has photosensitive characteristics, it possesses bioelectric chemical properties, but they are poorly oxidized by common oxidizing reagent. The polytype of K3[Fe(CN)6] are discussed in reference to cobalt salts by x-ray diffraction and Roman scattering as well. The method of preparing Potassium ferricyanide crystals is also investigated as well. The most common applications for the ion in the industry and pharmaceutical companies are discussed as well. Introduction
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For instance, commercial meters that produced by pharmaceutical companies contain potassium hexacyanoferrate (III) that measures the glucose level of blood on the patients.5 Iron has tripositive oxidation state in the complex and it has low spin, which cyanide ligand experiences a strong field in nature. The geometry of the complex is octahedral which causes the compound unstable once the cyanide ions dissociates in solution.5 The instability of the complex in solution is due to cyanide ions moving in the solution. The movement of cyanide ions affects the central atom which is iron that stabilizes the complex. Potassium hexacyaferrate (III) reacts with silver and produces silver hexacyanoferrate.5 Silver hexacyanoferrate is used in photographic processes. Potassium hexacyanoferrate(III) reacts with other salts violently, for instance, sodium nitrite reacts with potassium hexacyanoferrate(III) where it oxidizes ammonia to react explosively. Potassium hexacyanoferrate (III) particularly reacts with strong acid and forms hexacyanic acid, and later on it decomposes to form toxic hydrogen cyanide.5
Potassium hexacyanoferrate (III) is water soluble compound. When heated it decomposes. Cyanide complexes are most stable ions and its vapor pressure is negligible at 200C.5The potassium permanganate, ozone and chlorine are poor oxidizing agent for potassium hexacyanoferrate
For instance, commercial meters that produced by pharmaceutical companies contain potassium hexacyanoferrate (III) that measures the glucose level of blood on the patients.5 Iron has tripositive oxidation state in the complex and it has low spin, which cyanide ligand experiences a strong field in nature. The geometry of the complex is octahedral which causes the compound unstable once the cyanide ions dissociates in solution.5 The instability of the complex in solution is due to cyanide ions moving in the solution. The movement of cyanide ions affects the central atom which is iron that stabilizes the complex. Potassium hexacyaferrate (III) reacts with silver and produces silver hexacyanoferrate.5 Silver hexacyanoferrate is used in photographic processes. Potassium hexacyanoferrate(III) reacts with other salts violently, for instance, sodium nitrite reacts with potassium hexacyanoferrate(III) where it oxidizes ammonia to react explosively. Potassium hexacyanoferrate (III) particularly reacts with strong acid and forms hexacyanic acid, and later on it decomposes to form toxic hydrogen cyanide.5
Potassium hexacyanoferrate (III) is water soluble compound. When heated it decomposes. Cyanide complexes are most stable ions and its vapor pressure is negligible at 200C.5The potassium permanganate, ozone and chlorine are poor oxidizing agent for potassium hexacyanoferrate