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{{chembox {{chembox
| Verifiedfields = changed
| Watchedfields = changed | Watchedfields = changed
| verifiedrevid = 417264594 | verifiedrevid = 441024062
| ImageFile1 = Oxid olovnatý.JPG | ImageFile1 = Oxid olovnatý.JPG
| ImageSize1 = 244 | ImageSize1 = 244
Line 7: Line 8:
| ImageSize2 = 180 | ImageSize2 = 180
| IUPACName = Lead(II) oxide | IUPACName = Lead(II) oxide
| OtherNames = Lead monoxide<br />]<br />]<br />Plumbous oxide | OtherNames = Lead monoxide<br/>]<br/>]<br/>Plumbous oxide<br/>Galena
| Section1 = {{Chembox Identifiers | Section1 = {{Chembox Identifiers
| CASNo = 1317-36-8 | CASNo = 1317-36-8
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Ref = {{cascite|correct|CAS}}
| PubChem = | ChemSpiderID = 140169
| UNNumber = 3288 | ChEBI = 81045
| RTECS = OG1750000 | EC_number = 215-267-0
| KEGG = C17379
}}
| PubChem = 14827
| UNNumber = 3288 2291 3077
| RTECS = OG1750000
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 4IN6FN8492
| StdInChI=1S/O.Pb
| StdInChIKey = YEXPOXQUZXUXJW-UHFFFAOYSA-N
| SMILES = O=
}}
| Section2 = {{Chembox Properties | Section2 = {{Chembox Properties
| Formula = PbO | Formula = PbO
| MolarMass = 223.20 g/mol | MolarMass = 223.20 g/mol
| Appearance = red or yellow powder | Appearance = red or yellow powder
| Density = 9.64 g/cm<sup>3</sup> <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref> | Density = 9.53 g/cm<sup>3</sup>
| MeltingPtC = 888 | MeltingPtC = 888
| BoilingPtC = 1477 | BoilingPtC = 1477
| Solubility = α-PbO: 0.0504 g/L (25 °C)<br/>β-PbO: 0.1065 g/L (25 °C)<ref name=Greninger1977>{{cite book |author1=Dorothy Greninger |author2=Valerie Kollonitsch |author3=Charles Howard Kline |title=Lead Chemicals |publisher=] |year=1977 |url=https://books.google.com/books?id=pOQgAQAAIAAJ |page=52}}</ref>
| Solubility = insoluble
| SolubleOther = insoluble in dilute ]s <br /> soluble in concentrated alkalis <br /> soluble in ] | SolubleOther = insoluble in dilute ]s, ]<br/>soluble in concentrated alkalis <br/> soluble in ], ]
| MagSus = {{val|4.20|e=-5|u=cm<sup>3</sup>/mol}}}}
}}
| Section3 = {{Chembox Structure | Section3 = {{Chembox Structure
| Coordination = | Coordination =
| CrystalStruct = ], ] | CrystalStruct = ], ]
| SpaceGroup = P4/nmm, No. 129 | SpaceGroup = P4/nmm, No. 129}}
}}
| Section7 = {{Chembox Hazards | Section7 = {{Chembox Hazards
| ExternalMSDS = | ExternalSDS =
| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}
| EUIndex = 082-001-00-6
| GHSSignalWord = Danger
| EUClass = Repr. Cat. 1/3<br />Harmful ('''Xn''')<br />Dangerous for the environment ('''N''')
| HPhrases = {{H-phrases|302|332|351|360Df|362|373|410}}
| RPhrases = {{R61}}, {{R20/22}}, {{R33}}, {{R62}}, {{R50/53}}
| PPhrases = {{P-phrases|201|202|260|261|263|264|270|271|273|281|301+312|304+312|304+340|308+313|312|314|330|391|405|501}}
| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}}
| NFPA-H = 3 | NFPA-H = 3
| NFPA-F = 0 | NFPA-F = 0
| NFPA-R = 0 | NFPA-R = 0
| NFPA-O = | NFPA-S =
| FlashPt = Non-flammable | FlashPt = Non-flammable
| LDLo = 1400&nbsp;mg/kg (dog, oral)<ref name=IDLH>{{IDLH|7439921|Lead compounds (as Pb)}}</ref>}}
}}
| Section8 = {{Chembox Related | Section8 = {{Chembox Related
| OtherAnions = ]<br />]<br />] | OtherAnions = ]<br/>]<br/>]
| OtherCations = ]<br />]<br />] | OtherCations = ]<br/>]<br/>]<br/>]
| OtherFunctn = ]<br />] | OtherFunction = ]<br/>]
| Function = ] ]s | OtherFunction_label = ] ]s
| OtherCpds = ]<br />] | OtherCompounds = ]<br/>]}}}}
}}
}}


'''Lead(II) oxide''' is the ] with the ] ]]. Lead(II) oxide occurs in two ]s, red, having a ] and yellow, having an ]. Both forms occur naturally as rare ]: the red form is known as ] and the yellow form is known as ].<ref name="Holl">{{Holleman&Wiberg}}</ref> '''Lead(II) oxide''', also called '''lead monoxide''', is the inorganic compound with the molecular formula ]]. PbO occurs in two ]s: ] having a ], and ] having an ]. Modern applications for PbO are mostly in ]-based industrial ] and industrial ceramics, including computer components. It is an ] oxide.<ref name=Ullmann/>


== Types ==
==Preparation and structure==
Lead oxide exists in two types:
PbO may be prepared by heating lead metal in air at approx. 600 °C. At this temperature it is also the end product of oxidation of other ]s in air:<ref>N.N. Greenwood, A. Earnshaw, "Chemistry of Elements", 2nd edition, Butterworth-Heinemann, 1997.</ref>


* Red tetragonal (α-PbO), obtained at temperatures below {{Convert|486|C|F}}
:PbO<sub>2</sub> –(293 °C)→ Pb<sub>12</sub>O<sub>19</sub> –(351 °C)→ Pb<sub>12</sub>O<sub>17</sub> –(375 °C)→ Pb<sub>3</sub>O<sub>4</sub> –(605 °C)→ PbO
* Yellow orthorhombic (β-PbO), obtained at temperatures above {{Convert|486|C|F}}


==Synthesis==
Thermal decomposition of lead(II) nitrate or lead carbonate also results in the PbO formation:
PbO may be prepared by heating lead metal in air at approximately {{convert|600|C|F|-2}}. At this temperature it is also the end product of decomposition of other ] in air:<ref name="G&E">{{Greenwood&Earnshaw2nd|pages=382-387}}</ref>
:2 Pb(NO<sub>3</sub>)<sub>2</sub> → 2 PbO + 4 NO<sub>2</sub> + O<sub>2</sub>
:<chem>PbO2-> Pb12O19 -> Pb12O17 -> Pb3O4 -> PbO</chem>
:PbCO<sub>3</sub> → PbO + CO<sub>2</sub>


Thermal decomposition of ] or ] also results in the formation of PbO:
As determined by ], the compound features pyramidal four-coordinate Pb center. The pyramidal nature indicates the presence of a stereo-chemically active ] of electrons.<ref>{{Wells1984}}</ref>
:2&nbsp;{{chem|Pb|(NO|3|)|2}} → 2&nbsp;PbO + 4&nbsp;{{chem|link=nitrogen dioxide|NO|2}} + {{chem|O|2}}
:{{chem|PbCO|3}} → PbO + {{CO2|link=yes}}

PbO is produced on a large scale as an intermediate product in refining raw lead ores into metallic lead. The usual lead ore is ] (]). At a temperature of around {{convert|1000|C|F|-2}} the sulfide is converted to the oxide:<ref>{{cite journal|title=Thermal and XRD analysis of Egyptian galena|journal=Journal of Thermal Analysis and Calorimetry|year=2006|volume=86|issue=2|pages=393–401|last1=Abdel-Rehim|first1=A. M. |doi=10.1007/s10973-005-6785-6|s2cid=96393940}}</ref>
:2&nbsp;PbS + 3&nbsp;{{chem|O|2}} → 2&nbsp;PbO + 2&nbsp;{{SO2|link=yes}}

=== From lead ===
There are two principal methods to make lead monoxide both of which resemble combustion of the lead at high temperature:<ref name=":0">{{Cite journal |last=Dix |first=J. E. |date=1987-02-01 |title=A comparison of barton-pot and ball-mill processes for making leady oxide |url=https://dx.doi.org/10.1016/0378-7753%2887%2980024-1 |journal=Journal of Power Sources |language=en |volume=19 |issue=2 |pages=157–161 |doi=10.1016/0378-7753(87)80024-1 |bibcode=1987JPS....19..157D |issn=0378-7753}}</ref>
;Barton pot method.
:The refined molten lead droplets are oxidized in a vessel under a forced air flow which carries them out to the separation system (e.g. ]) for further processing.<ref name=":0" /><ref name=":1">{{Cite book |last=Pavlov |first=D. |url=https://www.worldcat.org/oclc/978538577 |title=Lead-acid batteries : science and technology : a handbook of lead-acid battery technology and its influence on the product |date=2017 |isbn=978-0-444-59560-7 |edition=2 |location=Saint Louis |oclc=978538577}}</ref>{{Rp|page=245}} Oxides produced by this method are mostly a mixture of α-PbO and β-PbO. The overall reaction is:<blockquote>2{{Chem2|Pb + O2}}{{Overset|450&nbsp;°C (842&nbsp;°F)|→}}2PbO</blockquote>

;Ball mill method: The lead balls are oxidized in a cooled rotating drum. The oxidation is achieved by collisions of the balls. Just like in Barton pot method, the supply of air and separators may also be used.<ref name=":0" />{{r|:1|p=245}}

==Structure==
As determined by ], both polymorphs, ] and ] feature a pyramidal four-coordinate lead center. In the tetragonal form the four lead–oxygen bonds have the same length, but in the orthorhombic two are shorter and two longer. The pyramidal nature indicates the presence of a ] active ] of electrons.<ref>{{Wells5th}}{{page needed|date=June 2017}}</ref> When PbO occurs in tetragonal lattice structure it is called ]; and when the PbO has orthorhombic lattice structure it is called ]. The PbO can be changed from massicot to litharge or vice versa by controlled heating and cooling.<ref>A simple example is given in {{cite book |author=Anil Kumar De |title=A Textbook Of Inorganic Chemistry |chapter-url=https://books.google.com/books?id=PpTi_JAx7PgC&pg=PA383 |year=2007 |publisher=New Age International |isbn=978-81-224-1384-7 |pages=383 |chapter=§9.2.6 Lead (Pb): Lead Monoxide PbO }} A more complex example is in {{cite book |first=N.Y. |last=Turova |title=The Chemistry of Metal Alkoxides |chapter-url=https://books.google.com/books?id=rPzaMRjK8pQC&pg=PA115 |date=2002 |publisher=Springer |isbn=978-0-7923-7521-0 |pages=115 |chapter=§9.4 Germanium, tin, lead alkoxides}}</ref> The tetragonal form is usually red or orange color, while the orthorhombic is usually yellow or orange, but the color is not a very reliable indicator of the structure.<ref>{{cite book |first=David John |last=Rowe |title=Lead Manufacturing in Britain: A History |url=https://books.google.com/books?id=ZL4OAAAAQAAJ&pg=PA16 |date=1983 |publisher=Croom Helm |isbn=978-0-7099-2250-6 |pages=16}}</ref> The tetragonal and orthorhombic ] of PbO occur naturally as rare minerals.

{{gallery|mode=packed-hover
|title=Crystal structure in litharge form<ref name="G&E" /><ref>{{ cite journal | doi = 10.1016/S0167-2738(01)00699-3 | journal = ] | year = 2001 | volume = 140 | pages = 115–123 | first1 = Caroline | last1 = Pirovano | first2 = M. Saiful | last2 = Islam | authorlink2 = Saiful Islam (professor) | first3 = Rose-Noëlle | last3 = Vannier | first4 = Guy | last4 = Nowogrocki | first5 = Gaëtan | last5 = Mairesse | title = Modelling the crystal structures of Aurivillius phases | issue = 1–2 }}</ref><ref>{{ cite web | url = https://www.ccdc.cam.ac.uk/structures/Search?Ccdcid=1653774&DatabaseToSearch=Published | title = ICSD Entry: 94333 | author = <!--Not stated--> | website = ]: Access Structures | publisher = ] | access-date = 2021-06-01 }}</ref>
|File:PbO-litharge-xtal-Pb-coordination-3D-bs-17.png|Pb coordinates ]
|File:PbO-litharge-xtal-O-coordination-3D-bs-17.png|O coordinates distorted-]
|File:PbO-litharge-xtal-unit-cell-3D-bs-17.png|Unit cell
|File:PbO-litharge-xtal-3x3x3-3D-bs-17.png|{{math|3×3×3}} unit cells
|File:PbO-litharge-xtal-3x3x3-a-3D-bs-17.png|Along the ]
|File:PbO-litharge-xtal-3x3x3-c-3D-bs-17.png|Along the ]
}}


==Reactions== ==Reactions==
Metallic lead is obtained by reducing PbO with ] at around {{convert|1200|C|F|-2}}:<ref>. Alt address: .</ref>
:PbO + CO → Pb + {{CO2}}

The red and yellow forms of this material are related by a small change in ]: The red and yellow forms of this material are related by a small change in ]:
PbO(red) → PbO(yellow) ''ΔH'' = 1.6 kJ/mol :PbO<sub>(red)</sub> → PbO<sub>(yellow)</sub> {{pad|5em}} Δ''H'' = 1.6&nbsp;kJ/mol


PbO is ], which means that it reacts with both acids and with bases. With acids, it forms salts of Pb<sup>2+</sup> via the intermediacy of oxo ]s such as <sup>4+</sup>. With strong base, PbO dissolves to form ](II) salts:<ref name="Holl"/> PbO is ], which means that it reacts with both acids and with bases. With acids, it forms salts of {{chem|Pb|2+}} via the intermediacy of oxo ]s such as {{chem||4+}}. With strong bases, PbO dissolves to form ] (also called plumbate(II)) salts:<ref name="Holl">{{Holleman&Wiberg}}{{page needed|date=June 2017}}</ref>
PbO + H<sub>2</sub>O + OH<sup>-</sup> → <sup>-</sup> :PbO + {{H2O}} + {{chem|OH|−}} → {{chem||−}}


==Applications== ==Applications==
The kind of lead in ] is normally PbO, and PbO is used extensively in making glass. Depending on the glass, the benefit of using PbO in glass can be one or more of increasing the ] of the glass, increasing the ] (i.&nbsp;e. reducing the ]) of the glass, decreasing the ] of the glass, increasing the electrical ] of the glass, and increasing the ability of the glass to absorb ]. Adding PbO to industrial ] (as well as glass) makes the materials more magnetically and electrically inert (by raising their ]) and it is often used for this purpose.<ref>Chapter 9, "Lead Compounds", in the book , published by Springer, year 2008.</ref> Historically PbO was also used extensively in ]s for household ceramics, and it is still used, but not extensively any more. Other less dominant applications include the ] of rubber and the production of certain pigments and paints.<ref name=Ullmann>{{Ullmann|first=Dodd S.|last=Carr|year=2005|title=Lead Compounds|doi=10.1002/14356007.a15_249}}</ref> PbO is used in ] glass to block ] emission, but mainly in the neck and funnel of the tube, because it can cause discoloration when used in the faceplate. ] and ] are preferred for the faceplate.<ref>{{Cite book|url=https://books.google.com/books?id=FvkqeL4IDMwC&q=lead+funnel&pg=PA9|title=Image Performance in CRT Displays|first=Kenneth|last=Compton|date=5 December 2003|publisher=SPIE Press|isbn=9780819441447|via=Google Books}}</ref>
PbO is produced on a large scale as an intermediate in the conversion of lead ores, mainly ] into metallic lead. The consumption of lead, and hence the processing of PbO, correlates with the number of automobiles because it remains the key component of automotive lead-acid batteries.<ref>Charles A. Sutherland, Edward F. Milner, Robert C. Kerby, Herbert Teindl, Albert Melin, Hermann M. Bolt “Lead” in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. {{DOI|10.1002/14356007.a15_193.pub2}}</ref>

PbO is used extensively in manufacturing of ]es and ]s as well as in fine dinnerware. For such applications, the PbO is converted in situ to ], which is less toxic. Other less dominating applications include the ] of rubber and the production of certain pigments and paints.<ref>Dodd S. Carr "Lead Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinhiem. {{DOI|10.1002/14356007.a15_249}}</ref> PbO is used in ] glass to block ] emission, but mainly in the neck and funnel because it can cause discoloration when used in the faceplate. ] is preferred for the faceplate.{{Fact|date=May 2007}}


The consumption of lead, and hence the processing of PbO, correlates with the number of automobiles, because lead remains the key component of automotive ].<ref>{{Ullmann|first1=Charles A.|last1=Sutherland|first2=Edward F.|last2=Milner|first3=Robert C.|last3=Kerby|first4=Herbert|last4=Teindl|first5=Albert|last5=Melin|first6=Hermann M.|last6=Bolt|title=Lead|doi=10.1002/14356007.a15_193.pub2}}</ref>


===Niche or declining uses=== ===Niche or declining uses===
A mixture of PbO with ] sets to a hard, waterproof cement that has been used to join the flat glass sides and bottoms of ], and was also once used to seal glass panels in window frames. It is a component of ]s. A mixture of PbO with ] sets to a hard, waterproof ] that has been used to join the flat glass sides and bottoms of ]s, and was also once used to seal glass panels in window frames. It is a component of ]s.


PbO was one of the raw materials for ]s, a type of ] preserved ]. but it has been gradually replaced due to health problems. It was an unscrupulous practice in some small factories but it became rampant in ] and forced many honest manufacturers to label their boxes "lead-free" after the scandal went mainstream in 2013.
PbO is used in certain ]s in ].<ref>{{OrgSynth

|author=Corson, B. B.
In powdered tetragonal litharge form, it can be mixed with ] and then boiled to create a weather-resistant ] used in ]. The litharge would give the sizing a dark red color that made the gold leaf appear warm and lustrous, while the linseed oil would impart adhesion and a flat durable binding surface.
|year=1936

|title=1,4-Diphenylbutadiene
PbO is used in certain ]s in ].<ref>{{OrgSynth| last=Corson |first=B. B. |year=1936 |title=1,4-Diphenylbutadiene |volume=16 |pages=28 |collvol=2 |collvolpages=229 |prep=CV2P0229}}</ref>
|volume=16

|pages=28
PbO is the input photoconductor in a video camera tube called the ].
|collvol=2
|collvolpages=229
|prep=CV2P0229}}</ref>


==Health issues== ==Health issues==
]
{{Main|Lead poisoning}} {{Main|Lead poisoning}}
Lead oxide may be fatal if swallowed or inhaled. It causes irritation to skin, eyes, and respiratory tract. It affects gum tissue, the central nervous system, the kidneys, the blood, and the reproductive system. It can ] in plants and in mammals.<ref>{{cite web |url= http://www.ilo.org/safework_bookshelf/english?d&nd=857171610 |title= Lead(II) oxide |access-date= 2009-06-06 |publisher= International Occupational Safety and Health Information Centre |archive-url= https://web.archive.org/web/20111215095749/http://www.ilo.org/safework_bookshelf/english?d&nd=857171610 |archive-date= 2011-12-15 |url-status= dead }}</ref>
]

Lead oxide may be fatal if swallowed or inhaled. It causes irritation to skin, eyes, and respiratory tract. It affects gum tissue, central nervous system, kidneys, blood, and reproductive system. It can ] in plants and in mammals.<ref>{{cite web| url = http://www.ilo.org/safework_bookshelf/english?d&nd=857171610| title = Lead (II) oxide| accessdate = 2009-06-06| publisher = International Occupational Safety and Health Information Centre}}</ref>
{{Clear}}


==References== ==References==
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==External links== ==External links==
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{{Lead compounds}} {{Lead compounds}}
{{Oxides}}


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