Lead(II) nitrate

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Lead(II) nitrate
Lead(II) nitrate 1.jpg
Lead(II)-nitrate-unit-cell-3D-balls.png
Lead(II)-nitrate-xtal-3D-SF.png
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.210 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 233-245-9
PubChem CID
RTECS number
  • OG2100000
UNII
UN number 1469
  • InChI=1S/2NO3.Pb/c2*2-1(3)4;/q2*-1;+2
    Key: RLJMLMKIBZAXJO-UHFFFAOYSA-N
  • [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Pb+2]
Properties
Pb(NO3)2
Molar mass 331.2 g/mol
Appearancecolorless or white
Density 4.53 g/cm3
Melting point 470 °C (878 °F; 743 K) [1] decomposes
376.5 g/L (0 °C)
597 g/L (25°C)
1270 g/L (100°C)
−74·10−6 cm3/mol [2]
1.782 [1]
Thermochemistry
−451.9 kJ·mol−1 [2]
Hazards
GHS labelling: [3]
GHS-pictogram-acid.svg GHS-pictogram-exclam.svg GHS-pictogram-silhouette.svg GHS-pictogram-pollu.svg
Danger
H302, H317, H318, H332, H360, H373, H410
P201, P202, P210, P220, P221, P260, P261, P264, P270, P271, P272, P273, P280, P281, P301+P312, P302+P352, P304+P312, P304+P340, P305+P351+P338, P308+P313, P310, P312, P314, P321, P330, P333+P313, P363, P370+P378, P391, P405, P501
NFPA 704 (fire diamond)
NFPA 704.svgHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
1
OX
Lethal dose or concentration (LD, LC):
500 mg/kg (guinea pig, oral) [4]
Safety data sheet (SDS) ICSC 1000
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Lead(II) nitrate is an inorganic compound with the chemical formula Pb(NO3)2. It commonly occurs as a colourless crystal or white powder and, unlike most other lead(II) salts, is soluble in water.

Contents

Known since the Middle Ages by the name plumbum dulce, the production of lead(II) nitrate from either metallic lead or lead oxide in nitric acid was small-scale, for direct use in making other lead compounds. In the nineteenth century lead(II) nitrate began to be produced commercially in Europe and the United States. Historically, the main use was as a raw material in the production of pigments for lead paints, but such paints have been superseded by less toxic paints based on titanium dioxide. Other industrial uses included heat stabilization in nylon and polyesters, and in coatings of photothermographic paper. Since around the year 2000, lead(II) nitrate has begun to be used in gold cyanidation.

Lead(II) nitrate is toxic and must be handled with care to prevent inhalation, ingestion and skin contact. Due to its hazardous nature, the limited applications of lead(II) nitrate are under constant scrutiny.

History

Lead nitrate was first identified in 1597 by the alchemist Andreas Libavius, who called the substance plumbum dulce, meaning "sweet lead", because of its taste. [5] It is produced commercially by reaction of metallic lead with concentrated nitric acid in which it is sparingly soluble. [6] [7] It has been produced as a raw material for making pigments such as chrome yellow (lead(II) chromate, PbCrO4) and chrome orange (basic lead(II) chromate, Pb2CrO5) and Naples yellow. These pigments were used for dyeing and printing calico and other textiles. [8] It has been used as an oxidizer in black powder and together with lead azide in special explosives. [9]

Production

Lead nitrate is produced by reaction of lead(II) oxide with concentrated nitric acid: [10]

PbO + 2 HNO3(concentrated) → Pb(NO3)2↓ + H2O

It may also be obtained evaporation of the solution obtained by reacting metallic lead with dilute nitric acid. [11]

Pb + 4 HNO3 → Pb(NO3)2 + 2 NO2 + 2 H2O

Solutions and crystals of lead(II) nitrate are formed in the processing of lead–bismuth wastes from lead refineries. [12]

Structure

Coordination sphere of the Pb ion Lead(II)-nitrate-xtal-Pb-coordination-3D-bs-17.png
Coordination sphere of the Pb ion
Crystal structure of Pb(NO3)2 [111] plane LeadNitrateCrystalStructure.png
Crystal structure of Pb(NO3)2[111] plane

The crystal structure of solid lead(II) nitrate has been determined by neutron diffraction. [13] [14] The compound crystallizes in the cubic system with the lead atoms in a face-centred cubic system. Its space group is Pa3Z=4 (Bravais lattice notation), with each side of the cube with length 784  picometres.

The black dots represent the lead atoms, the white dots the nitrate groups 27 picometres above the plane of the lead atoms, and the blue dots the nitrate groups the same distance below this plane. In this configuration, every lead atom is bonded to twelve oxygen atoms (bond length: 281 pm). All N–O bond lengths are identical, at 127 picometres. [15]


Research interest in the crystal structure of lead(II) nitrate was partly based on the possibility of free internal rotation of the nitrate groups within the crystal lattice at elevated temperatures, but this did not materialise. [14]

Chemical properties and reactions

Solubility of lead nitrate in nitric acid at 26 °C. [16]

Lead nitrate decomposes on heating, a property that has been used in pyrotechnics . [9] It is soluble in water and dilute nitric acid.

Basic nitrates are formed in when alkali is added to a solution. Pb2(OH)2(NO3)2 is the predominant species formed at low pH. At higher pH Pb6(OH)5(NO3) is formed. [17] The cation [Pb6O(OH)6]4+ is unusual in having an oxide ion inside a cluster of 3 face-sharing PbO4 tetrahedra. [18] There is no evidence for the formation of the hydroxide, Pb(OH)2, in aqueous solution below pH 12.

Solutions of lead nitrate can be used to form co-ordination complexes. Lead(II) is a hard acceptor; it forms stronger complexes with nitrogen and oxygen electron-donating ligands. For example, combining lead nitrate and pentaethylene glycol (EO5) in a solution of acetonitrile and methanol followed by slow evaporation produced the compound [Pb(NO3)2(EO5)]. [19] In the crystal structure for this compound, the EO5 chain is wrapped around the lead ion in an equatorial plane similar to that of a crown ether. The two bidentate nitrate ligands are in trans configuration. The total coordination number is 10, with the lead ion in a bicapped square antiprism molecular geometry.

The complex formed by lead nitrate with a bithiazole bidentate N-donor ligand is binuclear. The crystal structure shows that the nitrate group forms a bridge between two lead atoms. [20] One interesting aspect of this type of complexes is the presence of a physical gap in the coordination sphere; i.e., the ligands are not placed symmetrically around the metal ion. This is potentially due to a lead lone pair of electrons, also found in lead complexes with an imidazole ligand. [21]

Applications

Lead nitrate has been used as a heat stabiliser in nylon and polyesters, as a coating for photothermographic paper, and in rodenticides. [10]

Heating lead nitrate is convenient means of making nitrogen dioxide

In the gold cyanidation process, addition of lead(II) nitrate solution improves the leaching process. Only limited amounts (10 to 100 milligrams lead nitrate per kilogram gold) are required. [22] [23]

In organic chemistry, it may be used in the preparation of isothiocyanates from dithiocarbamates. [24] Its use as a bromide scavenger during SN1 substitution has been reported. [25]

Safety

Lead(II) nitrate is toxic, and ingestion may lead to acute lead poisoning, as is applicable for all soluble lead compounds. [26] All inorganic lead compounds are classified by the International Agency for Research on Cancer (IARC) as probably carcinogenic to humans (Category 2A). [27] They have been linked to renal cancer and glioma in experimental animals and to renal cancer, brain cancer and lung cancer in humans, although studies of workers exposed to lead are often complicated by concurrent exposure to arsenic. [28] Lead is known to substitute for zinc in a number of enzymes, including δ-aminolevulinic acid dehydratase (porphobilinogen synthase) in the haem biosynthetic pathway and pyrimidine-5′-nucleotidase, important for the correct metabolism of DNA and can therefore cause fetal damage. [29]

Related Research Articles

<span class="mw-page-title-main">Silver nitrate</span> Chemical compound

Silver nitrate is an inorganic compound with chemical formula AgNO
3. It is a versatile precursor to many other silver compounds, such as those used in photography. It is far less sensitive to light than the halides. It was once called lunar caustic because silver was called luna by ancient alchemists who associated silver with the moon. In solid silver nitrate, the silver ions are three-coordinated in a trigonal planar arrangement.

<span class="mw-page-title-main">Copper(II) nitrate</span> Chemical compound

Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO3)2(H2O)x. The hydrates are blue solids. Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C. Common hydrates are the hemipentahydrate and trihydrate.

<span class="mw-page-title-main">Ceric ammonium nitrate</span> Chemical compound

Ceric ammonium nitrate (CAN) is the inorganic compound with the formula (NH4)2[Ce(NO3)6]. This orange-red, water-soluble cerium salt is a specialised oxidizing agent in organic synthesis and a standard oxidant in quantitative analysis.

<span class="mw-page-title-main">Lead(II) chloride</span> Chemical compound

Lead(II) chloride (PbCl2) is an inorganic compound which is a white solid under ambient conditions. It is poorly soluble in water. Lead(II) chloride is one of the most important lead-based reagents. It also occurs naturally in the form of the mineral cotunnite.

The uranyl ion is an oxycation of uranium in the oxidation state +6, with the chemical formula UO2+
2. It has a linear structure with short U–O bonds, indicative of the presence of multiple bonds between uranium and oxygen. Four or more ligands may be bound to the uranyl ion in an equatorial plane around the uranium atom. The uranyl ion forms many complexes, particularly with ligands that have oxygen donor atoms. Complexes of the uranyl ion are important in the extraction of uranium from its ores and in nuclear fuel reprocessing.

<span class="mw-page-title-main">Iron(III) nitrate</span> Chemical compound

Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO3)3.(H2O)n. Most common is the nonahydrate Fe(NO3)3.(H2O)9. The hydrates are all pale colored, water-soluble paramagnetic salts.

<span class="mw-page-title-main">Palladium(II) nitrate</span> Chemical compound

Palladium(II) nitrate is the inorganic compound with the formula Pd(NO3)2.(H2O)x where x = 0 or 2. The anhydrous and dihydrate are deliquescent solids. According to X-ray crystallography, both compounds feature square planar Pd(II) with unidentate nitrate ligands. The anhydrous compound, which is a coordination polymer, is yellow.

<span class="mw-page-title-main">Lead(II) thiocyanate</span> Chemical compound

Lead(II) thiocyanate is a compound, more precisely a salt, with the formula Pb(SCN)2. It is a white crystalline solid, but will turn yellow upon exposure to light. It is slightly soluble in water and can be converted to a basic salt (Pb(CNS)2·Pb(OH)2 when boiled. Salt crystals may form upon cooling. Lead thiocyanate can cause lead poisoning if ingested and can adversely react with many substances. It has use in small explosives, matches, and dyeing.

<span class="mw-page-title-main">Mercury(I) nitrate</span> Chemical compound

Mercury(I) nitrate is an inorganic compound, a salt of mercury and nitric acid with the formula Hg2(NO3)2. A yellow solid, the compound is used as a precursor to other Hg22+ complexes. The structure of the hydrate has been determined by X-ray crystallography. It consists of a [H2O-Hg-Hg-OH2]2+ center, with a Hg-Hg distance of 254 pm.

<span class="mw-page-title-main">Lead compounds</span> Type of compound

Compounds of lead exist with lead in two main oxidation states: +2 and +4. The former is more common. Inorganic lead(IV) compounds are typically strong oxidants or exist only in highly acidic solutions.

<span class="mw-page-title-main">Cerium nitrates</span> Chemical compound

Cerium nitrate refers to a family of nitrates of cerium in the +3 or +4 oxidation state. Often these compounds contain water, hydroxide, or hydronium ions in addition to cerium and nitrate. Double nitrates of cerium also exist.

<span class="mw-page-title-main">Actinide chemistry</span> Branch of nuclear chemistry

Actinide chemistry is one of the main branches of nuclear chemistry that investigates the processes and molecular systems of the actinides. The actinides derive their name from the group 3 element actinium. The informal chemical symbol An is used in general discussions of actinide chemistry to refer to any actinide. All but one of the actinides are f-block elements, corresponding to the filling of the 5f electron shell; lawrencium, a d-block element, is also generally considered an actinide. In comparison with the lanthanides, also mostly f-block elements, the actinides show much more variable valence. The actinide series encompasses the 15 metallic chemical elements with atomic numbers from 89 to 103, actinium through lawrencium.

<span class="mw-page-title-main">Titanium(IV) nitrate</span> Chemical compound

Titanium nitrate is the inorganic compound with formula Ti(NO3)4. It is a colorless, diamagnetic solid that sublimes readily. It is an unusual example of a volatile binary transition metal nitrate. Ill defined species called titanium nitrate are produced upon dissolution of titanium or its oxides in nitric acid.

<span class="mw-page-title-main">Zirconium nitrate</span> Chemical compound

Zirconium nitrate is a volatile anhydrous transition metal nitrate salt of zirconium with formula Zr(NO3)4. It has alternate names of zirconium tetranitrate, or zirconium(IV) nitrate.

<span class="mw-page-title-main">Thorium(IV) nitrate</span> Chemical compound

Thorium(IV) nitrate is a chemical compound, a salt of thorium and nitric acid with the formula Th(NO3)4. A white solid in its anhydrous form, it can form tetra- and pentahydrates. As a salt of thorium it is weakly radioactive.

<span class="mw-page-title-main">Iron(II) nitrate</span> Chemical compound

Iron(II) nitrate is the nitrate salt of iron(II). It is commonly encountered as the green hexahydrate, Fe(NO3)2·6H2O, which is a metal aquo complex, however it is not commercially available unlike iron(III) nitrate due to its instability to air. The salt is soluble in water and serves as a ready source of ferrous ions.

<span class="mw-page-title-main">Plutonium(IV) nitrate</span> Chemical compound

Plutonium (IV) nitrate is an inorganic compound, a salt of plutonium and nitric acid with the chemical formula Pu(NO3)4. The compound dissolves in water and forms crystalline hydrates as dark green crystals.

Neptunium(IV) nitrate is an inorganic compound, a salt of neptunium and nitric acid with the chemical formula Np(NO3)4. The compound forms gray crystals, dissolves in water, and forms crystal hydrates.

<span class="mw-page-title-main">Transition metal nitrate complex</span> Compound of nitrate ligands

A transition metal nitrate complex is a coordination compound containing one or more nitrate ligands. Such complexes are common starting reagents for the preparation of other compounds.

Cobalt compounds are chemical compounds formed by cobalt with other elements.

References

  1. 1 2 Patnaik, Pradyot (2003). Handbook of inorganic chemicals. New York: McGraw-Hill. p. 475. ISBN   0-07-049439-8. OCLC   50252041.
  2. 1 2 CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN   978-1-4987-5428-6. OCLC   930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)
  3. ↑ "Lead nitrate". pubchem.ncbi.nlm.nih.gov. Retrieved 19 December 2021.
  4. ↑ "Lead compounds (as Pb)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  5. ↑ Libavius, Andreas (1595). Alchemia Andreæ Libavii. Francofurti: Iohannes Saurius.
  6. ↑ Chisholm, Hugh, ed. (1911). "Lead"  . Encyclopædia Britannica . Vol. 16 (11th ed.). Cambridge University Press. pp. 314–320.
  7. ↑ Macgregor, John (1847). Progress of America to year 1846. London: Whittaker & Co. ISBN   0-665-51791-2.
  8. ↑ Partington, James Riddick (1950). A Text-book of Inorganic Chemistry. MacMillan. p. 838.
  9. 1 2 Barkley, J. B. (October 1978). "Lead nitrate as an oxidizer in blackpowder". Pyrotechnica. 4. Post Falls, Idaho: Pyrotechnica Publications: 16–18.
  10. 1 2 Greenwood, Norman N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. pp.  388, 456. ISBN   0-7506-3365-4.
  11. ↑ Othmer, D. F. (1967). Kirk-Othmer Encyclopedia of Chemical Technology. Vol. 12 (Iron to Manganese) (second completely revised ed.). New York: John Wiley & Sons. p. 272. ISBN   0-471-02040-0.
  12. ↑ "Product catalog; other products". Tilly, Belgium: Sidech. Archived from the original on 2007-07-01. Retrieved 2008-01-05.
  13. ↑ Hamilton, W. C. (1957). "A neutron crystallographic study of lead nitrate". Acta Crystallogr. 10 (2): 103–107. doi:10.1107/S0365110X57000304.
  14. 1 2 Nowotny, H.; G. Heger (1986). "Structure refinement of lead nitrate". Acta Crystallographica Section C . 42 (2): 133–35. doi:10.1107/S0108270186097032.
  15. ↑ Nowotny, H.; Heger, G. (15 February 1986). "Cấu trúc của chì nitrat". Acta Crystallographica Section C . 42 (2): 133–135. doi:10.1107/S0108270186097032 . Retrieved 15 July 2019.
  16. ↑ Ferris, L. M. (1959). "Lead nitrate—Nitric acid—Water system". Journal of Chemical & Engineering Data. 5 (3): 242. doi:10.1021/je60007a002.
  17. ↑ Pauley, J. L.; M. K. Testerman (1954). "Basic Salts of Lead Nitrate Formed in Aqueous Media". Journal of the American Chemical Society . 76 (16): 4220–4222. doi:10.1021/ja01645a062.
  18. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN   978-0-08-037941-8. p. 395
  19. ↑ Rogers, Robin D.; Andrew H. Bond; Debra M. Roden (1996). "Structural Chemistry of Poly (ethylene glycol). Complexes of Lead(II) Nitrate and Lead(II) Bromide". Inorg. Chem. 35 (24): 6964–6973. doi:10.1021/ic960587b. PMID   11666874.
  20. ↑ Mahjoub, Ali Reza; Ali Morsali (2001). "A Dimeric Mixed-Anions Lead(II) Complex: Synthesis and Structural Characterization of [Pb2(BTZ)4(NO3)(H2O)](ClO4)3 {BTZ = 4,4'-Bithiazole}". Chemistry Letters . 30 (12): 1234. doi:10.1246/cl.2001.1234.
  21. ↑ Shuang-Yi Wan; Jian Fan; Taka-aki Okamura; Hui-Fang Zhu; Xing-Mei Ouyang; Wei-Yin Sun & Norikazu Ueyama (2002). "2D 4.82 Network with threefold parallel interpenetration from nanometre-sized tripodal ligand and lead(II) nitrate". Chem. Commun. (21): 2520–2521. doi:10.1039/b207568g.
  22. ↑ Habashi, Fathi (1998). "Recent advances in gold metallurgy". Revisa de la Facultad de Ingeniera, Universidad Central de Venezuela. 13 (2): 43–54.
  23. ↑ "Auxiliary agents in gold cyanidation". Gold Prospecting and Gold Mining. Retrieved 2008-01-05.
  24. ↑ Dains, F. B.; Brewster, R. Q.; Olander, C. P. "Phenyl isothiocyanate". Organic Syntheses ; Collected Volumes, vol. 1, p. 447.
  25. ↑ Rapoport, H.; Jamison, T. (1998). "(S)-N-(9-Phenylfluoren-9-yl)alanine and (S)-Dimethyl-N-(9-phenylfluoren-9-yl)aspartate". Organic Syntheses ; Collected Volumes, vol. 9, p. 344.
  26. ↑ "Lead nitrate, Chemical Safety Card 1000". International Labour Organization, International Occupational Safety and Health Information Centre. March 1999. Retrieved 2008-01-19.
  27. ↑ "Inorganic and Organic Lead Compounds" (PDF). IARC Monographs on the Evaluation of Carcinogenic Risks to Humans. Suppl. 7. International Agency for Research on Cancer: 239. 1987. Archived from the original (PDF) on 2008-03-06. Retrieved 2008-01-19.
  28. ↑ World Health Organization, International Agency for Research on Cancer (2006). "Inorganic and Organic Lead Compounds" (PDF). IARC Monographs on the Evaluation of Carcinogenic Risks to Humans. 87. International Agency for Research on Cancer. ISBN   92-832-1287-8. Archived from the original (PDF) on 2007-10-21. Retrieved 2008-01-01.
  29. ↑ Mohammed-Brahim, B.; Buchet, J.P.; Lauwerys, R. (1985). "Erythrocyte pyrimidine 5'-nucleotidase activity in workers exposed to lead, mercury or cadmium". Int Arch Occup Environ Health. 55 (3): 247–52. doi:10.1007/BF00383757. PMID   2987134. S2CID   40092031.
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