Lead tetrachloride
| Lead tetrachloride | ||
|---|---|---|
-chloride-from-xtal-2002-3D-SF.png) | ||
| IUPAC name Lead(IV) chloride | ||
| Identifiers | ||
| CAS number | 13463-30-4 | |
| Properties | ||
| Molecular formula | PbCl4 | |
| Molar mass | 349.012 g/mol[1] | |
| Appearance | yellow oily liquid at room temperature[1] | |
| Density | 3.2 g⋅cm−3[1] | |
| Melting point | −15 °C[1] (stable below 0 °C[1]) | |
| Boiling point | 50 °C[1] | |
| Solubility in water | Reacts | |
| Solubility | hydrochloric acid | |
| Structure | ||
| Coordination geometry |
4 | |
| Molecular shape | tetrahedral[2] | |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | ||
| Infobox references | ||
Lead tetrachloride, also known as lead(IV) chloride, has the molecular formula PbCl4. It is an unstable, inorganic compound and is a yellow, oily liquid at room temperature.[1] It has a tetrahedral configuration, with lead as the central atom. The Pb–Cl covalent bonds have been measured to be 247 pm and the bond energy is 243 kJ⋅mol−1.[3]
Synthesis
Lead tetrachloride can be made by reacting lead(II) chloride PbCl2, and hydrochloric acid HCl, in the presence of chlorine gas (Cl2),[4] leading to the formation of chloroplumbic acid H2PbCl6. It is then converted to the ammonium salt (NH4)2PbCl6 by adding ammonium chloride (NH4Cl). Finally, the solution is treated with concentrated sulfuric acid H2SO4, to separate out lead tetrachloride. This series of reactions is conducted at 0°C. The following equations illustrate the reaction:
- PbCl2 + 2HCl + Cl2 → H2PbCl6
- H2PbCl6 + 2 NH4Cl → (NH4)2PbCl6
- (NH4)2PbCl6 + H2SO4 → PbCl4+ 2HCl + (NH4)2SO4
Reaction with water
Unlike carbon tetrachloride, another group IV (IUPAC: group 14) chloride, lead tetrachloride reacts with water. This is due to the fact that the central atom is bigger (Pb is bigger than C) so there is less cluttering and water can easily access it.[2] Also, because of the presence of empty d orbitals on the Pb atom, oxygen can bind to it before a Pb–Cl bond has to break, thus requiring less energy. The overall reaction is thus as follow:
- PbCl4 + 2H2O → PbO2(s) + 4HCl(g)
Stability
Lead tetrachloride tends to decompose further into lead dichloride and chlorine gas:[2]
- PbCl4 → PbCl2 + Cl2(g)
This is due to the fact that the stability of the +4 oxidation state decreases as we travel down this group of the periodic table.[2] Thus while carbon tetrachloride is a stable compound, with lead the oxidation state +2 is favored and PbCl4 quickly becomes PbCl2. Indeed, the inert pair effect causes lead to favor its +2 oxidation state: Pb atom loses all its outermost p electrons and ends up with a stable, filled s subshell.[5]
Toxicity
Lead is a cumulative poison.[3] Only limited evidence have been shown of lead's carcinogenic effect, but lead tetrachloride, as well as all other lead compounds, is "reasonably anticipated to be human carcinogens" according to the Report on Carcinogens, Twelfth Edition (2011).[6] Lead can be absorbed by the body through several routes, primarily inhalation but also ingestion and dermal contact. Lead compounds are also teratogens.[7]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 1.5 1.6 "Lead compounds: Lead Tetrachloride". WebElements.com. Retrieved 10 October 2012.
- ↑ 2.0 2.1 2.2 2.3 "The Chlorides of Carbon, Silicon and Lead". chemguide.co.uk. Retrieved 10 October 2012.
- ↑ 3.0 3.1 Emsley, John (2000). The Elements. Oxford: Oxford University Press. p. 114. ISBN 0198558198.
- ↑ Neu, John T.; William D. Gwinn (October 1958). "Raman Spectra of Germanium Tetrachloride and Lead Tetrachloride". ACS 70 (10): 3464–3465. doi:10.1021/ja01190a073. Retrieved 10 October 2012.
- ↑ Miessler, Gary L. (2011). inorganic Chemistry. Boston: Prentice Hall. pp. 275, 289–290. ISBN 970-0-13-612866-3 Check
|isbn=value (help). - ↑ National Toxicology Program, Department of Health and Human Services (2011). Report on Carcinoens, Twelfth Edition (2011) - Lead and Lead Compounds. p. 251.
- ↑ "Environmental Health & Safety - 1: General Information About Chemical Safety". Princeton UNiversity. Retrieved 11 October 2012.
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