Lead(II) compounds are characteristic of the inorganic chemistry of lead.
Even strong oxidizing agents like fluorine and chlorine react with lead to give only PbF₂ and PbCl₂. Lead(II) ions are usually colorless in solution, and partially hydrolyze to form Pb(OH)⁺ and finally [Pb₄(OH)₄]⁴⁺ (in which the hydroxyl ions act as bridging ligands), but are not reducing agents as tin(II) ions are.
Techniques for identifying the presence of the Pb²⁺ ion in water generally rely on the precipitation of lead(II) chloride using dilute hydrochloric acid.
As the chloride salt is sparingly soluble in water, in very dilute solutions the precipitation of lead(II) sulfide is achieved by bubbling hydrogen sulfide through the solution.

Lead monoxide exists in two polymorphs, litharge α-PbO (red) and massicot β-PbO (yellow), the latter being stable only above around 488 °C.
Litharge is the most commonly used inorganic compound of lead.
There is no lead(II) hydroxide; increasing the pH of solutions of lead(II) salts leads to hydrolysis and condensation.

Lead commonly reacts with heavier chalcogens.
Lead sulfide is a semiconductor, a photoconductor, and an extremely sensitive infrared radiation detector.
The other two chalcogenides, lead selenide and lead telluride, are likewise photoconducting.
They are unusual in that their color becomes lighter going down the group.

Lead dihalides are well-characterized; this includes the diastatide and mixed halides, such as PbFCl.
The relative insolubility of the latter forms a useful basis for the gravimetric determination of fluorine.
The difluoride was the first solid ionically conducting compound to be discovered (in 1834, by Michael Faraday).
The other dihalides decompose on exposure to ultraviolet or visible light, especially the diiodide.
Many lead(II) pseudohalides are known, such as the cyanide, cyanate, and thiocyanate.
Lead(II) forms an extensive variety of halide coordination complexes, such as [PbCl₄]²⁻, [PbCl₆]⁴⁻, and the [Pb₂Cl₉]ₙ⁵ⁿ⁻ chain anion.

Lead(II) sulfate is insoluble in water, like the sulfates of other heavy divalent cations.
Lead(II) nitrate and lead(II) acetate are very soluble, and this is exploited in the synthesis of other lead compounds.
Lead(II) compounds are characteristic of the inorganic chemistry of lead. Even strong oxidizing agents like fluorine and chlorine react with lead to give only PbF₂ and PbCl₂. Lead(II) ions are usually colorless in solution, and partially hydrolyze to form Pb(OH)⁺ and finally [Pb₄(OH)₄]⁴⁺ (in which the hydroxyl ions act as bridging ligands), but are not reducing agents as tin(II) ions are. Techniques for identifying the presence of the Pb²⁺ ion in water generally rely on the precipitation of lead(II) chloride using dilute hydrochloric acid. As the chloride salt is sparingly soluble in water, in very dilute solutions the precipitation of lead(II) sulfide is achieved by bubbling hydrogen sulfide through the solution.
Lead monoxide exists in two polymorphs, litharge α-PbO (red) and massicot β-PbO (yellow), the latter being stable only above around 488 °C. Litharge is the most commonly used inorganic compound of lead. There is no lead(II) hydroxide; increasing the pH of solutions of lead(II) salts leads to hydrolysis and condensation.
Lead commonly reacts with heavier chalcogens. Lead sulfide is a semiconductor, a photoconductor, and an extremely sensitive infrared radiation detector. The other two chalcogenides, lead selenide and lead telluride, are likewise photoconducting. They are unusual in that their color becomes lighter going down the group.
Lead dihalides are well-characterized; this includes the diastatide and mixed halides, such as PbFCl. The relative insolubility of the latter forms a useful basis for the gravimetric determination of fluorine. The difluoride was the first solid ionically conducting compound to be discovered (in 1834, by Michael Faraday). The other dihalides decompose on exposure to ultraviolet or visible light, especially the diiodide. Many lead(II) pseudohalides are known, such as the cyanide, cyanate, and thiocyanate. Lead(II) forms an extensive variety of halide coordination complexes, such as [PbCl₄]²⁻, [PbCl₆]⁴⁻, and the [Pb₂Cl₉]ₙ⁵ⁿ⁻ chain anion.
Lead(II) sulfate is insoluble in water, like the sulfates of other heavy divalent cations. Lead(II) nitrate and lead(II) acetate are very soluble, and this is exploited in the synthesis of other lead compounds.
Lead