Editing Lead (section)

==== Lead(II) ====
[[File:Oxid_olovnatý.JPG|left|thumb|[[Lead(II) oxide]]|alt=Cream powder]]Lead(II) compounds are characteristic of the inorganic chemistry of lead. Even strong [[oxidizing agent]]s like fluorine and chlorine react with lead to give only [[Lead(II) fluoride|PbF<sub>2</sub>]] and [[Lead(II) chloride|PbCl<sub>2</sub>]].{{sfn|Greenwood|Earnshaw|1998|p=373}} Lead(II) ions are usually colorless in solution,{{sfn|Hunt|2014|p=215}} and partially hydrolyze to form Pb(OH)<sup>+</sup> and finally [Pb<sub>4</sub>(OH)<sub>4</sub>]<sup>4+</sup> (in which the [[Hydroxy group|hydroxyl]] ions act as [[bridging ligand]]s),{{sfn|King|1995|pp=43–63}}{{sfn|Bunker|Casey|2016|p=89}} but are not [[reducing agent]]s as tin(II) ions are. [[Qualitative inorganic analysis|Techniques]] for identifying the presence of the Pb<sup>2+</sup> 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 instead achieved by bubbling [[hydrogen sulfide]] through the solution.{{sfn|Whitten|Gailey|David|1996|pp=904–905}}

[[Lead(II) oxide|Lead monoxide]] exists in two [[Crystal polymorphism|polymorphs]], [[litharge]] α-PbO (red) and [[massicot]] β-PbO (yellow), the latter being stable only above around 488&nbsp;°C. Litharge is the most commonly used inorganic compound of lead.{{sfn|Greenwood|Earnshaw|1998|p=384}} There is no lead(II) hydroxide; increasing the pH of solutions of lead(II) salts leads to hydrolysis and condensation.{{sfn|Greenwood|Earnshaw|1998|p=387}} Lead commonly reacts with heavier chalcogens. [[Lead sulfide]] is a [[semiconductor]], a [[Photoconductivity|photoconductor]], and an extremely sensitive [[Particle detector|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.{{sfn|Greenwood|Earnshaw|1998|p=389}}

[[File:Red-lead-unit-cell-3D-balls.png|right|thumb|upright| Lead and [[oxygen]] in a tetragonal [[Crystal structure#Unit cell|unit cell]] of [[lead(II,IV) oxide]]|alt=Alternating dark gray and red balls connected by dark gray-red cylinders]]
Lead dihalides are well-characterized; this includes the diastatide{{sfn|Zuckerman|Hagen|1989|p=426}} and mixed halides, such as PbFCl. The relative insolubility of the latter forms a useful basis for the [[Gravimetric analysis|gravimetric]] determination of fluorine. The difluoride was the first solid [[Ionic conductivity (solid state)|ionically conducting]] compound to be discovered (in 1834, by [[Michael Faraday]]).{{sfn|Funke|2013}} The other dihalides decompose on exposure to ultraviolet or visible light, especially [[Lead(II) iodide|the diiodide]].{{sfn|Greenwood|Earnshaw|1998|p=382}} Many lead(II) [[Pseudohalogen|pseudohalides]] are known, such as the cyanide, cyanate, and [[Lead(II) thiocyanate|thiocyanate]].{{sfn|Greenwood|Earnshaw|1998|p=389}}{{sfn|Bharara|Atwood|2006|p=4}} Lead(II) forms an extensive variety of halide [[coordination complex]]es, such as [PbCl<sub>4</sub>]<sup>2−</sup>, [PbCl<sub>6</sub>]<sup>4−</sup>, and the [Pb<sub>2</sub>Cl<sub>9</sub>]<sub>''n''</sub><sup>5''n''−</sup> chain anion.{{sfn|Greenwood|Earnshaw|1998|p=382}}

[[Lead(II) sulfate]] is insoluble in water, like the sulfates of other heavy divalent [[Ion|cations]]. [[Lead(II) nitrate]] and [[lead(II) acetate]] are very soluble, and this is exploited in the synthesis of other lead compounds.{{sfn|Greenwood|Earnshaw|1998|p=388}}