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Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO 3) 2 (H 2 O) x. The hydrates are hygroscopic blue solids . Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C.
Being the conjugate base of a strong acid (nitric acid, pK a = -1.4), nitrate has modest Lewis basicity.Two coordination modes are common: unidentate and bidentate.Often, bidentate nitrate, denoted κ 2-NO 3, is bound unsymmetrically in the sense that one M-O distance is clearly bonding and the other is more weakly interacting. [2]
H 2 N 2 O 2 + 2 H + + 2 e − ⇌ N 2 + 2 H 2 O; E 0 = +2.65 V. Oxidation reactions usually result in the formation of the nitrate ion, with nitrogen in oxidation state +5. For example, oxidation with permanganate ion can be used for quantitative analysis of nitrite (by titration): 5 NO − 2 + 2 MnO − 4 + 6 H + → 5 NO −
The synergic effect of the atomic thickness, high flexibility, stronger surface adsorption capability, electrical insulation, impermeability, high thermal and chemical stability of BN nanosheets can increase the Raman sensitivity by up to two orders, and in the meantime attain long-term stability and reusability not readily achievable by other ...
For example, the thermal decomposition of some metal nitrates generates NO 2: [14] Pb(NO 3) 2 → PbO + 2 NO 2 + 1 ⁄ 2 O 2. Alternatively, dehydration of nitric acid produces nitronium nitrate... 2 HNO 3 → N 2 O 5 + H 2 O 6 HNO 3 + 1 ⁄ 2 P 4 O 10 → 3 N 2 O 5 + 2 H 3 PO 4...which subsequently undergoes thermal decomposition: N 2 O 5 → ...
Hyponitrous acid (H 2 N 2 O 2) is a weak diprotic acid with the structure HON=NOH (pK a1 6.9, pK a2 11.6). Acidic solutions are quite stable but above pH 4 base-catalysed decomposition occurs via [HONNO] − to nitrous oxide and the hydroxide anion. Hyponitrites (involving the N 2 O 2−
The alkaline earth metal oxides are formed from the thermal decomposition of the corresponding carbonates. CaCO 3 → CaO + CO 2 (at approx. 900°C) In laboratory, they are obtained from hydroxides: Mg(OH) 2 → MgO + H 2 O. or nitrates: Ca(NO 3) 2 → CaO + 2NO 2 + 1/2O 2. The oxides exhibit basic character: they turn phenolphthalein red and ...
CaCO 3 → CaO + CO 2 The reaction is used to make quick lime, which is an industrially important product. Another example of thermal decomposition is 2Pb(NO 3) 2 → 2PbO + O 2 + 4NO 2. Some oxides, especially of weakly electropositive metals decompose when heated to high enough temperature.