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Lead(IV) oxide, commonly known as lead dioxide, is an inorganic compound with the chemical formula PbO 2.It is an oxide where lead is in an oxidation state of +4. [1] It is a dark-brown solid which is insoluble in water. [2]
Lead oxides are a group of inorganic compounds with formulas including lead (Pb) and oxygen (O).. Common lead oxides include: Lead(II) oxide, PbO, litharge (red), massicot (yellow)
Lead(II) oxide, also called lead monoxide, is the inorganic compound with the molecular formula Pb O.PbO occurs in two polymorphs: litharge having a tetragonal crystal structure, and massicot having an orthorhombic crystal structure.
In chemistry, plumbite is the PbO 2− 2 oxyanion or hydrated forms, or any salt containing this anion. In these salts, lead is in the oxidation state +2. It is the traditional term for the IUPAC name plumbate(II).
Reaction of lead with sulfur or hydrogen sulfide yields lead sulfide. The solid has the NaCl-like structure (simple cubic), which it keeps up to the melting point, 1114 °C (2037 °F). If the heating occurs in presence of air, the compounds decomposes to give the monoxide and the sulfate. [7]
Hydrogen compounds are compounds containing the element hydrogen. In these compounds, hydrogen can form in the +1 and -1 oxidation states. Hydrogen can form compounds both ionically and in covalent substances. It is a part of many organic compounds such as hydrocarbons as well as water and other organic substances.
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However, it is soluble in hydrochloric acid present in the stomach, and is therefore toxic when ingested. It also dissolves in glacial acetic acid and a diluted mixture of nitric acid and hydrogen peroxide. When heated to 500 °C, it decomposes to lead(II) oxide and oxygen. At 580 °C, the reaction is complete. 2 Pb 3 O 4 → 6 PbO + O 2