Jdtcujk

Lead(II) oxide
	; ;
	; ;
Names;
	; IUPAC name; Lead(II) oxide;
	Other names; Lead monoxide; Litharge; Massicot; Murda sang; Plumbous oxide; Galena;
Identifiers;
; CAS Number;	; ; 1317-36-8 Y; ; ;
; ChemSpider;	; 140169; ;
; ECHA InfoCard;	; 100.013.880;
; ; PubChem CID; ;	; 14827; ;
; RTECS number;	OG1750000;
; UN number;	3288;
; ; CompTox Dashboard (EPA); ;	; DTXSID0029638 ; ;
Properties;
; Chemical formula;	PbO ;
; Molar mass;	223.20 g/mol ;
Appearance;	red or yellow powder;
; Density;	9.53 g/cm3;
; Melting point;	888 °C (1,630 °F; 1,161 K) ;
; Boiling point;	1,477 °C (2,691 °F; 1,750 K) ;
; Solubility in water;	0.017 g/L;
; Solubility;	insoluble in dilute alkalis, alcohol; soluble in concentrated alkalis ; soluble in HCl, ammonium chloride;
; ; Magnetic susceptibility (χ);	; 6995420000000000000♠42.0×10−6 cm3/mol;
Structure;
; Crystal structure;	; Tetragonal, tP4;
; Space group;	P4/nmm, No. 129;
Hazards;
; Safety data sheet;	; ICSC 0288;
; ; EU classification (DSD) (outdated); ;	Repr. Cat. 1/3; Toxic (T); Harmful (Xn); Dangerous for the environment (N);
; R-phrases (outdated);	; R61, R20/22, R33, R62, R50/53;
; S-phrases (outdated);	; S53, S45, S60, S61;
; NFPA 704;	; ; ; ; ; ; ; ; ; 0; ; ; 3; ; ; 0; ; ;
; Flash point;	Non-flammable ;
	Lethal dose or concentration (LD, LC):;
; ; LDLo (lowest published);	1400 mg/kg (dog, oral);
Related compounds;
; Other anions; ;	; Lead sulfide; Lead selenide; Lead telluride;
; Other cations; ;	; Carbon monoxide; Silicon monoxide; Tin(II) oxide;
; Related lead oxides; ;	; Lead(II,II,IV) oxide; Lead dioxide;
; Related compounds;	; Thallium(III) oxide; Bismuth(III) oxide;
	; Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).;
	; N verify (what is YN ?);
	; Infobox references;
;	;

Lead(II) oxide, also called lead monoxide, is the inorganic compound with the molecular formula PbO. PbO occurs in two polymorphs: litharge having a tetragonal crystal structure, and massicot having an orthorhombic crystal structure. Modern applications for PbO are mostly in lead-based industrial glass and industrial ceramics, including computer components. It is an amphoteric oxide.

Preparation

PbO may be prepared by heating lead metal in air at approximately 600 °C. At this temperature it is also the end product of oxidation of other lead oxides in air:^[3]

PbO₂293 °C→ Pb₁₂O₁₉351 °C→ Pb₁₂O₁₇375 °C→ Pb₃O₄605 °C→ PbO

Thermal decomposition of lead(II) nitrate or lead(II) carbonate also results in the formation of PbO:

2 Pb(NO₃)₂ → 2 PbO + 4 NO₂ + O₂

PbCO₃ → PbO + CO₂

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 high temperature (1,000 °C) the sulfide is converted to the oxide:^[4]

2 PbS + 3 O₂ → 2 PbO + 2 SO₂

Metallic lead is obtained by reducing the PbO with carbon monoxide at around 1,200 °C:^[5]

PbO + CO → Pb + CO₂

Structure

As determined by X-ray crystallography, both polymorphs, tetragonal and orthorhombic feature a pyramidal four-coordinate lead center. In the tetragonal form the four Pb-O bonds have the same length, but in the orthorhombic two are shorter and two longer. The pyramidal nature indicates the presence of a stereochemically active lone pair of electrons.^[6] When PbO occurs in tetragonal lattice structure it is called litharge; and when the PbO has orthorhombic lattice structure it is called massicot. The PbO can be changed from massicot to litharge or vice versa by controlled heating and cooling.^[7] 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.^[8] The tetragonal and orthorhombic forms of PbO occur naturally as rare minerals.

Reactions

The red and yellow forms of this material are related by a small change in enthalpy:

PbO(red) → PbO(yellow) ΔH = 1.6 kJ/mol

PbO is amphoteric, which means that it reacts with both acids and with bases. With acids, it forms salts of Pb²⁺ via the intermediacy of oxo clusters such as [Pb₆O(OH)₆]⁴⁺. With strong bases, PbO dissolves to form plumbite (also called plumbate(II)) salts:^[9]

PbO + H₂O + OH⁻ → [Pb(OH)₃]⁻

Applications

The kind of lead in lead glass 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 refractive index of the glass, decreasing the viscosity of the glass, increasing the electrical resistivity of the glass, and increasing the ability of the glass to absorb X-rays. Adding PbO to industrial ceramics (as well as glass) makes the materials more magnetically and electrically inert (raises the Curie temperature) and is often used for this purpose.^[10] Historically PbO was also used extensively in ceramic glazes for household ceramics, and it is still used, but not extensively any more. Other less dominant applications include the vulcanization of rubber and the production of certain pigments and paints.^[11] PbO is used in cathode ray tube glass to block X-ray emission, but mainly in the neck and funnel because it can cause discoloration when used in the faceplate. Strontium oxide is preferred for the faceplate.^{[citation needed]}

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.^[12]

Niche or declining uses

A mixture of PbO with glycerine sets to a hard, waterproof cement that has been used to join the flat glass sides and bottoms of aquariums, and was also once used to seal glass panels in window frames. It is a component of lead paints.

In powdered tetragonal litharge form, it can be mixed with linseed oil and then boiled to create a weather-resistant sizing used in gilding. 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.

PbO is used in certain condensation reactions in organic synthesis.^[13]

PbO is the input photoconductor in a video camera tube called the Plumbicon.

Health issues

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 bioaccumulate in plants and in mammals.^[14]

References

^ Blei(II)-oxid. Merck

^ "Lead compounds (as Pb)". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH)..mw-parser-output cite.citation{font-style:inherit}.mw-parser-output .citation q{quotes:"""""""'""'"}.mw-parser-output .citation .cs1-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-limited a,.mw-parser-output .citation .cs1-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration{color:#555}.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration span{border-bottom:1px dotted;cursor:help}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/12px-Wikisource-logo.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output code.cs1-code{color:inherit;background:inherit;border:inherit;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;font-size:100%}.mw-parser-output .cs1-visible-error{font-size:100%}.mw-parser-output .cs1-maint{display:none;color:#33aa33;margin-left:0.3em}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-format{font-size:95%}.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-right{padding-right:0.2em}

^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^{[page needed]}

^ Abdel-Rehim, A. M. (2006). "Thermal and XRD analysis of Egyptian galena". Journal of Thermal Analysis and Calorimetry. 86 (2): 393–401.

^ Lead Processing @ Universalium.academic.ru. Alt address: Lead processing @ Enwiki.net.

^ Wells, A. F. (1984), Structural Inorganic Chemistry (5th ed.), Oxford: Clarendon Press, ISBN 0-19-855370-6
^{[page needed]}

^ A simple example is given in A Text Book of Inorganic Chemistry, by Anil Kumar De, year 2007, page 383. A more complex example is in The Chemistry of Metal Alkoxides, published by Kluwer Academic Publishers, year 2002, section 9.4 on lead alkoxides, page 115.

^ Lead manufacturing in Britain, by David John Rowe, year 1983, page 16.

^ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5
^{[page needed]}

^ Chapter 9, "Lead Compounds", in the book Ceramic and Glass Materials: Structure, Properties and Processing, published by Springer, year 2008.

^ Carr, Dodd S., "Lead Compounds", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a15_249

^ Sutherland, Charles A.; Milner, Edward F.; Kerby, Robert C.; Teindl, Herbert; Melin, Albert; Bolt, Hermann M., "Lead", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a15_193.pub2

^ Corson, B. B. (1936). "1,4-Diphenylbutadiene". Organic Syntheses. 16: 28.; Collective Volume, 2, p. 229

^ "Lead (II) oxide". International Occupational Safety and Health Information Centre. Retrieved 2009-06-06.

External links

Case Studies in Environmental Medicine - Lead Toxicity

ToxFAQs: Lead

National Pollutant Inventory - Lead and Lead Compounds Fact Sheet

Webelements PbO

[1] Blei(II)-oxid. Merck

[IDLH-2] "Lead compounds (as Pb)". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH)..mw-parser-output cite.citation{font-style:inherit}.mw-parser-output .citation q{quotes:"""""""'""'"}.mw-parser-output .citation .cs1-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-limited a,.mw-parser-output .citation .cs1-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration{color:#555}.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration span{border-bottom:1px dotted;cursor:help}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/12px-Wikisource-logo.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output code.cs1-code{color:inherit;background:inherit;border:inherit;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;font-size:100%}.mw-parser-output .cs1-visible-error{font-size:100%}.mw-parser-output .cs1-maint{display:none;color:#33aa33;margin-left:0.3em}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-format{font-size:95%}.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-right{padding-right:0.2em}

[3] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^{[page needed]}

[4] Abdel-Rehim, A. M. (2006). "Thermal and XRD analysis of Egyptian galena". Journal of Thermal Analysis and Calorimetry. 86 (2): 393–401.

[5] Lead Processing @ Universalium.academic.ru. Alt address: Lead processing @ Enwiki.net.

[6] Wells, A. F. (1984), Structural Inorganic Chemistry (5th ed.), Oxford: Clarendon Press, ISBN 0-19-855370-6
^{[page needed]}

[7] A simple example is given in A Text Book of Inorganic Chemistry, by Anil Kumar De, year 2007, page 383. A more complex example is in The Chemistry of Metal Alkoxides, published by Kluwer Academic Publishers, year 2002, section 9.4 on lead alkoxides, page 115.

[8] Lead manufacturing in Britain, by David John Rowe, year 1983, page 16.

[Holl-9] Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5
^{[page needed]}

[10] Chapter 9, "Lead Compounds", in the book Ceramic and Glass Materials: Structure, Properties and Processing, published by Springer, year 2008.

[11] Carr, Dodd S., "Lead Compounds", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a15_249

[12] Sutherland, Charles A.; Milner, Edward F.; Kerby, Robert C.; Teindl, Herbert; Melin, Albert; Bolt, Hermann M., "Lead", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a15_193.pub2

[13] Corson, B. B. (1936). "1,4-Diphenylbutadiene". Organic Syntheses. 16: 28.; Collective Volume, 2, p. 229

[14] "Lead (II) oxide". International Occupational Safety and Health Information Centre. Retrieved 2009-06-06.

v t e Lead compounds
Pb(II)	PbBr₂ Pb(C₅H₅)₂ Pb(C₂H₃O₂)₂ PbCl₂ PbCO₃ PbCrO₄ PbF₂ PbHAsO₄ PbI₂ Pb(NO₃)₂ Pb(N₃)₂ PbO Pb(OH)₂ Pb₃(PO₄)₂ PbS Pb(SCN)₂ PbSe PbSO₄ PbTe PbTiO₃ plumbite PbC₂ (hypothetical)
Pb(II,IV)	Pb₃O₄
Pb(IV)	Pb(C₂H₃O₂)₄ PbCl₄ PbF₄ PbH₄ PbO₂ PbS₂ plumbate Pb(OH)₄ (hypothetical)

v t e Oxides
Mixed oxidation states	Antimony tetroxide (Sb₂O₄) Cobalt(II,III) oxide (Co₃O₄) Europium(II,III) oxide (Eu₃O₄) Iron(II,III) oxide (Fe₃O₄) Lead(II,IV) oxide (Pb₃O₄) Manganese(II,III) oxide (Mn₃O₄) Silver(I,III) oxide (Ag₂O₂) Triuranium octoxide (U₃O₈) Carbon suboxide (C₃O₂) Mellitic anhydride (C₁₂O₉) Praseodymium(III,IV) oxide (Pr₆O₁₁) Terbium(III,IV) oxide (Tb₄O₇)
+1 oxidation state	Copper(I) oxide (Cu₂O) Caesium oxide (Cs₂O) Dicarbon monoxide (C₂O) Dichlorine monoxide (Cl₂O) Gallium(I) oxide (Ga₂O) Lithium oxide (Li₂O) Potassium oxide (K₂O) Rubidium oxide (Rb₂O) Silver oxide (Ag₂O) Thallium(I) oxide (Tl₂O) Sodium oxide (Na₂O) Water (hydrogen oxide) (H₂O)
+2 oxidation state	Aluminium(II) oxide (AlO) Barium oxide (BaO) Beryllium oxide (BeO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Europium(II) oxide (EuO) Germanium monoxide (GeO)) Iron(II) oxide (FeO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Palladium(II) oxide (PdO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Disulfur dioxide (S₂O₂) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Zinc oxide (ZnO)
+3 oxidation state	Aluminium oxide (Al₂O₃) Antimony trioxide (Sb₂O₃) Arsenic trioxide (As₂O₃) Bismuth(III) oxide (Bi₂O₃) Boron trioxide (B₂O₃) Cerium(III) oxide (Ce₂O₃) Dibromine trioxide (Br₂O₃) Chromium(III) oxide (Cr₂O₃) Dinitrogen trioxide (N₂O₃) Dysprosium(III) oxide (Dy₂O₃) Erbium(III) oxide (Er₂O₃) Europium(III) oxide (Eu₂O₃) Gadolinium(III) oxide (Gd₂O₃) Gallium(III) oxide (Ga₂O₃) Holmium(III) oxide (Ho₂O₃) Indium(III) oxide (In₂O₃) Iron(III) oxide (Fe₂O₃) Lanthanum oxide (La₂O₃) Lutetium(III) oxide (Lu₂O₃) Manganese(III) oxide (Mn₂O₃) Neodymium(III) oxide (Nd₂O₃) Nickel(III) oxide (Ni₂O₃) Phosphorus trioxide (P₄O₆) Praseodymium(III) oxide (Pr₂O₃) Promethium(III) oxide (Pm₂O₃) Rhodium(III) oxide (Rh₂O₃) Samarium(III) oxide (Sm₂O₃) Scandium oxide (Sc₂O₃) Terbium(III) oxide (Tb₂O₃) Thallium(III) oxide (Tl₂O₃) Thulium(III) oxide (Tm₂O₃) Titanium(III) oxide (Ti₂O₃) Tungsten(III) oxide (W₂O₃) Vanadium(III) oxide (V₂O₃) Ytterbium(III) oxide (Yb₂O₃) Yttrium(III) oxide (Y₂O₃)
+4 oxidation state	Americium dioxide (AmO₂) Carbon dioxide (CO₂) Carbon trioxide (CO₃) Cerium(IV) oxide (CeO₂) Chlorine dioxide (ClO₂) Chromium(IV) oxide (CrO₂) Dinitrogen tetroxide (N₂O₄) Germanium dioxide (GeO₂) Hafnium(IV) oxide (HfO₂) Lead dioxide (PbO₂) Manganese dioxide (MnO₂) Neptunium(IV) oxide (NpO₂) Nitrogen dioxide (NO₂) Osmium dioxide (OsO₂) Plutonium(IV) oxide (PuO₂) Praseodymium(IV) oxide (PrO₂) Protactinium(IV) oxide (PaO₂) Rhodium(IV) oxide (RhO₂) Ruthenium(IV) oxide (RuO₂) Selenium dioxide (SeO₂) Silicon dioxide (SiO₂) Sulfur dioxide (SO₂) Tellurium dioxide (TeO₂) Terbium(IV) oxide (TbO₂) Thorium dioxide (ThO₂) Tin dioxide (SnO₂) Titanium dioxide (TiO₂) Tungsten(IV) oxide (WO₂) Uranium dioxide (UO₂) Vanadium(IV) oxide (VO₂) Zirconium dioxide (ZrO₂)
+5 oxidation state	Antimony pentoxide (Sb₂O₅) Arsenic pentoxide (As₂O₅) Dinitrogen pentoxide (N₂O₅) Niobium pentoxide (Nb₂O₅) Phosphorus pentoxide (P₂O₅) Protactinium(V) oxide (Pa₂O₅) Tantalum pentoxide (Ta₂O₅) Vanadium(V) oxide (V₂O₅)
+6 oxidation state	Chromium trioxide (CrO₃) Molybdenum trioxide (MoO₃) Rhenium trioxide (ReO₃) Selenium trioxide (SeO₃) Sulfur trioxide (SO₃) Tellurium trioxide (TeO₃) Tungsten trioxide (WO₃) Uranium trioxide (UO₃) Xenon trioxide (XeO₃) Iridium trioxide (IrO₃)
+7 oxidation state	Dichlorine heptoxide (Cl₂O₇) Manganese heptoxide (Mn₂O₇) Rhenium(VII) oxide (Re₂O₇) Technetium(VII) oxide (Tc₂O₇)
+8 oxidation state	Osmium tetroxide (OsO₄) Ruthenium tetroxide (RuO₄) Xenon tetroxide (XeO₄) Iridium tetroxide (IrO₄) Hassium tetroxide (HsO₄)
Related	Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide
Oxides are sorted by oxidation state. Category:Oxides

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Jdtcujk

Lead(II) oxide

Contents

Preparation

Structure

Reactions

Applications

Niche or declining uses

Health issues

References

External links

Comments

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Names


IUPAC name Lead(II) oxide
Other names Lead monoxide Litharge Massicot Murda sang Plumbous oxide Galena
Identifiers
CAS Number	1317-36-8^Y
ChemSpider	140169
ECHA InfoCard	100.013.880
PubChem CID	14827
RTECS number	OG1750000
UN number	3288
CompTox Dashboard (EPA)	DTXSID0029638
Properties
Chemical formula	PbO
Molar mass	223.20 g/mol
Appearance	red or yellow powder
Density	9.53 g/cm³
Melting point	888 °C (1,630 °F; 1,161 K)
Boiling point	1,477 °C (2,691 °F; 1,750 K)
Solubility in water	0.017 g/L^[1]
Solubility	insoluble in dilute alkalis, alcohol soluble in concentrated alkalis soluble in HCl, ammonium chloride
Magnetic susceptibility (χ)	6995420000000000000♠42.0×10⁻⁶ cm³/mol
Structure
Crystal structure	Tetragonal, tP4
Space group	P4/nmm, No. 129
Hazards
Safety data sheet	ICSC 0288
EU classification (DSD) (outdated)	Repr. Cat. 1/3 Toxic (T) Harmful (Xn) Dangerous for the environment (N)
R-phrases (outdated)	R61, R20/22, R33, R62, R50/53
S-phrases (outdated)	S53, S45, S60, S61
NFPA 704	0 3 0
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD_Lo (lowest published)	1400 mg/kg (dog, oral)^[2]
Related compounds
Other anions	Lead sulfide Lead selenide Lead telluride
Other cations	Carbon monoxide Silicon monoxide Tin(II) oxide
Related lead oxides	Lead(II,II,IV) oxide Lead dioxide
Related compounds	Thallium(III) oxide Bismuth(III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is ^YN ?)
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Lead(II) oxide

Contents

Preparation

Structure

Reactions

Applications

Niche or declining uses

Health issues

References

External links

Comments

Post a Comment

Popular posts from this blog

Information security

Volkswagen Group MQB platform

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