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2 → 2 PbO + 4 NO 2 + O 2 PbCO 3 → PbO + CO 2. PbO is produced on a large scale as an intermediate product in refining raw lead ores into metallic lead. The usual lead ore is galena (lead(II) sulfide). At a temperature of around 1,000 °C (1,800 °F) in air, the sulfide converted to the oxide: [4] 2 PbS + 2 O 2 → 2 PbO + 2 SO 2
Although an amphiprotic species must be amphoteric, the converse is not true. For example, a metal oxide such as zinc oxide, ZnO, contains no hydrogen and so cannot donate a proton. Nevertheless, it can act as an acid by reacting with the hydroxide ion, a base: ZnO + 2 OH − + H 2 O → [Zn(OH) 4] 2−. Zinc oxide can also act as a base:
Lead dioxide is used as an anode material in electrochemistry. β-PbO 2 is more attractive for this purpose than the α form because it has relatively low resistivity, good corrosion resistance even in low-pH medium, and a high overvoltage for the evolution of oxygen in sulfuric- and nitric-acid-based electrolytes.
Lead sesquioxide, Pb 2 O 3, which is a lead (II,IV) oxide as well (lead(II) metaplumbate(IV) [Pb 2+][PbO 2− 3]), reddish yellow Pb 12 O 19 , monoclinic, dark-brown or black crystals The so-called black lead oxide , which is a mixture of PbO and fine-powdered Pb metal and used in the production of lead–acid batteries .
4 Pb + SO 2 → R 3 PbO(SO)R R 3 PbCl + 1/2Ag 2 O (aq) → R 3 PbOH + AgCl R 2 PbCl 2 + 2 OH − → R 2 Pb(OH) 2 + 2 Cl −. R 2 Pb(OH) 2 compounds are amphoteric. At pH lower than 8 they form R 2 Pb 2+ ions and with pH higher than 10, R 2 Pb(OH) 3 − ions. Derived from the hydroxides are the plumboxanes: 2 R 3 PbOH + Na → (R 3 Pb) 2 O ...
Lead(II,IV) oxide is lead(II) orthoplumbate(IV) [Pb 2+] 2 [PbO 4− 4]. [3] It has a tetragonal crystal structure at room temperature, which then transforms to an orthorhombic (Pearson symbol oP28, Space group Pbam, No. 55) form at temperature 170 K (−103 °C). This phase transition only changes the symmetry of the crystal and slightly ...
2 PbO + PbS → 3 Pb + SO 2. Metallic lead is attacked (oxidized) only superficially by air, forming a thin layer of lead oxide that protects it from further oxidation. The metal is not attacked by sulfuric or hydrochloric acids. It dissolves in nitric acid with the evolution of nitric oxide gas to form dissolved Pb(NO 3) 2. 3 Pb + 8 H + + 8 NO −
PbO may be prepared by heating lead metal in air at approximately 600 °C (lead melts at only 300 °C). At this temperature it is also the end product of heating of other lead oxides in air. [ 5 ] This is often done with a set of bellows pumping air over molten lead and causing the oxidized product to slip or fall off the top into a receptacle ...