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Manganese(II) nitrate is the precursor to manganese(II) carbonate (MnCO 3), which is used in fertilizers and as a colourant. The advantage of this method, based on the use of ammonia (NH 3) and carbon dioxide (CO 2) as reaction intermediates, being that the side product ammonium nitrate (NH 4 NO 3) is also useful as a fertilizer. [1]
The color of chemicals is a physical property of chemicals that in most cases comes from the excitation of electrons due to an absorption of energy performed by the chemical. The study of chemical structure by means of energy absorption and release is generally referred to as spectroscopy .
A particularly common oxidation state for manganese in aqueous solution is +2, which has a pale pink color. Many manganese(II) compounds are known, such as the aquo complexes derived from manganese(II) sulfate (MnSO 4) and manganese(II) chloride (MnCl 2). This oxidation state is also seen in the mineral rhodochrosite (manganese(II) carbonate ...
A flame test involves introducing a sample of the element or compound to a hot, non-luminous flame and observing the color of the flame that results. [4] The compound can be made into a paste with concentrated hydrochloric acid, as metal halides, being volatile, give better results. [5] Different flames can be tried to verify the accuracy of ...
Mn(OH) 2: 3.221×10 −4: Manganese(II) nitrate: Mn(NO 3) 2: 102: 118: 139: 206: Manganese(II) oxalate: MnC 2 O 4 ·2H 2 O: 0.02: 0.024: 0.028: 0.033: Manganese(II) sulfate: MnSO 4: 52.9: 59.7: 62.9: 62.9: 60: 53.6: 45.6: 40.9: 35.3 Mercury(I) azide: Hg 2 (N 3) 2: 0.02727: Mercury(I) bromide: Hg 2 Br 2: 1.352×10 −6: Mercury(I) carbonate: Hg ...
The most important is Mn 3 N 2, which catalyzes nitrogen fixation and is a high-temperature antiferromagnet. The others are Mn 6 N 5–6, Mn 4 N, [1] [2] and Mn 2 N. [3] The compounds generally form as surface layer during combustion of manganese metal in nitrogen or ammonia gas, and homogenous samples can be difficult to obtain.
MnO 2 + H 2 → MnO + H 2 O MnO 2 + CO → MnO + CO 2. Upon heating to 450 °C, manganese(II) nitrate gives a mixture of oxides, denoted MnO 2−x, which can be reduced to the monoxide with hydrogen at ≥750 °C. [6] MnO is particularly stable and resists further reduction. [7] MnO can also be prepared by heating the carbonate: [8] MnCO 3 → ...
4 + 4 OH − → 4 MnO 2− 4 + 2 H 2 O + O 2. Potassium manganate is prepared industrially, as an intermediate to potassium permanganate, by dissolving manganese dioxide in molten potassium hydroxide with potassium nitrate or air as the oxidizing agent. [2] 2 MnO 2 + 4 OH − + O 2 → 2 MnO 2− 4 + 2 H 2 O