![]() ![]() Cobalt nitrate hexahydrate (Co(NO 3) 2♶H 2O) is a red deliquescence crystal that is easily soluble in water, and its molecule contains cobalt(II) hydrated ions ( 2+) and free nitrate ions. Cobalt(II) nitrate exists in the anhydrous form and the hydrate form, of which the hexahydrate is the most common. Ĭobalt can easily react with nitric acid to form cobalt(II) nitrate Co(NO 3) 2. Hydrogen bonding of water stabilizes this molecule. This compound can be obtained by reacting (N 5) 6(H 3O) 3(NH 4) 4Cl or Na(H 2O)(N 5)]♲H 2O and (NO 3) 2 at room temperature. It decomposes at 50~145 ☌ to form cobalt(II) azide, becoming anhydrous and releasing nitrogen, and exploding when heated further. Cobalt pentazolide Co(N 5) 2 was discovered in 2017, and it exists in the form of the hydrate ♴H 2O. Cobalt(II) and azide can form Co(NĤ complexes. Cobalt(II) azide (Co(N 3) 2) is another binary compound of cobalt and nitrogen that can explode when heated. ![]() Cobalt reacts with phosphorus or arsenic to form Co 2P, CoP, CoAs 2 and other substances. Nitrides Cobalt(II) nitrate hexahydrateĬobalt powder reacts with ammonia to form two kinds of nitrides, Co 2N and Co 3N. Soluble cobalt salts react with sodium hydroxide to obtain cobalt(II) hydroxide (Co(OH) 2): Co(NO 3) 2 + 2 NaOH → Co(OH) 2↓ + 2 NaNO 3Ĭobalt(II) hydroxide can be oxidized to the Co(III) compound CoO(OH) under alkaline conditions. Oxides and hydroxides Cobalt(II,III) oxideĬobalt can form various oxides, such as CoO, Co 2O 3 and Co 3O 4. It is a fluorinated reagent and reacts violently with water. The potential from F 2 to F − is as high as +2.87 V, and cobalt(III) fluoride (CoF 3) can exist stably. Therefore, the interaction of Co 3+ with Cl− produces Co 2+ and releases chlorine gas. , the potential is +1.92 V, which is higher than that of Cl 2 to Cl − (+1.36 V). The complex of cobalt halides and triethylphosphine ((C 2H 5) 3P) can absorb nitric monoxide in benzene to form the diamagnetic material Co(NO)X 2(P(C 2H 5) 3) ![]() ![]() Because the color change of cobalt(II) chloride in different hydrates, it can be used to manufacture color-changing silica gel.Īnhydrous cobalt halides react with nitric oxide at 70~120 ☌ to generate 2 (X = Cl, Br or I). Anhydrous cobalt(II) chloride is blue, while the hexahydrate is red-purple. In addition to the anhydrous forms, these cobalt halides also have hydrates. Inorganic compounds Halides Red-orange CoCl 2♶H 2Oįour halides of cobalt(II) are known, which are cobalt(II) fluoride (CoF 2) which is a pink solid, cobalt(II) chloride (CoCl 2) which is a blue solid, cobalt(II) bromide (CoBr 2) which is a green solid, and cobalt(II) iodide (CoI 2) which is a blue-black solid. In addition, there are cobalt compounds in high oxidation states +4, +5 and low oxidation states -1, 0, +1. In the compound, the most stable oxidation state of cobalt is the +2 oxidation state, and in the presence of specific ligands, there are also stable compounds with +3 valence. Finally, based on the different observations reported in the literature, we provide a critical review about the scope and limitations of this widely used chemical hypoxia model to be informative to all researchers interested in the field.Ĭhemical hypoxia cobalt chloride hypoxia inducible factor prolyl hydroxylases.Cobalt compounds are chemical compounds formed by cobalt with other elements. The different current hypotheses that explain the establishment of hypoxic conditions using CoCl 2 are also described. The regulation of hypoxia inducible factors by oxygen and the role of CoCl 2 are explained to understand the most accepted bases of the CoCl 2 -induced hypoxia model. This review describes the characteristics of the model, as well as the biochemical and molecular bases that support it. This model has several advantages, and currently, there is a substantial amount of scattered information about how this model works. One of the most commonly used models is cobalt chloride-induced chemical hypoxia because it stabilizes hypoxia inducible factors 1α and 2α under normoxic conditions. Several alternative models have been used to mimic hypoxia. Although a decrease in oxygen concentration is the optimal hypoxia model, the problem faced by many researchers is access to a hypoxia chamber or a CO 2 incubator with regulated oxygen levels, which is not possible in many laboratories. The use of hypoxia models in cell culture has allowed the characterization of the hypoxia response at the cellular, biochemical and molecular levels. ![]()
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