Lead tetrachloride

Names
IUPAC name

Lead(IV) chloride

Identifiers

CAS Number

* 13463-30-4

3D model (JSmol)

* Interactive image

ChemSpider |

* 109913

PubChem CID

* 123310

InChI

* InChI=1S/4ClH.Pb/h4*1H;/q;;;;+4/p-4

Key: PJYXVICYYHGLSW-UHFFFAOYSA-J

SMILES

* Cl[Pb](Cl)(Cl)Cl

Properties

Chemical formula

| PbCl4
Molar mass | 349.012 g/mol[1]
Appearance  | yellow oily liquid[2]
Density | 3.2 g⋅cm−3[1]
Melting point |  −15 °C (5 °F; 258 K)[1] stable below 0 °C (32 °F; 273 K)[2]
Boiling point |  50 °C (122 °F; 323 K)[1] decomposes

Solubility in water

| Reacts
Solubility | hydrochloric acid
Structure

Coordination geometry

| 4

Molecular shape

| tetrahedral[3]
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| -328.9 kJ/mol

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Infobox references

Tracking categories (test):

* SizeSet

Lead tetrachloride, also known as lead(IV) chloride, has the molecular formula PbCl4. It is a yellow, oily liquid which is stable below 0 °C, and decomposes at 50 °C.[2] 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.[4]

## Contents

* 1 Synthesis
* 2 Reaction with water
* 3 Stability
* 4 Toxicity
* 5 References

## Synthesis

Lead tetrachloride can be made by reacting lead(II) chloride PbCl2, and hydrochloric acid HCl, in the presence of chlorine gas (Cl2),[5] 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 \+ 2HCl
(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 because the central atom is bigger (Pb is bigger than C) so there is less cluttering and water can easily access it.[3] 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:[3]

PbCl4 → PbCl2 \+ Cl2(g)

There are reports that this reaction can proceed explosively and that the compound is best stored under pure sulfuric acid at -80 °C in the dark.[6]

The stability of the +4 oxidation state decreases as we travel down this group of the periodic table.[3] 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.[7]

## Toxicity

Lead is a cumulative poison.[4] 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).[8] Lead can be absorbed by the body through several routes, primarily inhalation but also ingestion and dermal contact. Lead compounds are also teratogens.[9]

## References

1. ↑ 1.0 1.1 1.2 1.3 "Lead compounds: Lead Tetrachloride". WebElements.com. http://www.webelements.com/compounds/lead/lead_tetrachloride.html. Retrieved 10 October 2012.
2. ↑ 2.0 2.1 2.2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 381. ISBN 978-0-08-037941-8.
3. ↑ 3.0 3.1 3.2 3.3 "The Chlorides of Carbon, Silicon and Lead". chemguide.co.uk. http://www.chemguide.co.uk/inorganic/group4/chlorides.html. Retrieved 10 October 2012.
4. ↑ 4.0 4.1 Emsley, John (2000). The Elements. Oxford: Oxford University Press. p. 114. ISBN 978-0-19-855819-4.
5. ↑ Neu, John T.; Gwinn, William D. (October 1958). "Raman Spectra of Germanium Tetrachloride and Lead Tetrachloride". Journal of the American Chemical Society 70 (10): 3464–3465. doi:10.1021/ja01190a073.
6. ↑ The Chemistry of Germanium: Tin and Lead E. G. Rochow, E. W. Abel Elsevier, 2014, ISBN 1483187586, ISBN 9781483187587
7. ↑ Miessler, Gary L. (2011). inorganic Chemistry. Boston: Prentice Hall. pp. 275, 289–290. ISBN 978-0-13-612866-3.
8. ↑ National Toxicology Program, Department of Health and Human Services (2011). Report on Carcinogens, Twelfth Edition (2011) - Lead and Lead Compounds. p. 251. https://ntp.niehs.nih.gov/ntp/roc/content/profiles/lead.pdf.
9. ↑ "Environmental Health & Safety - 1: General Information About Chemical Safety". Princeton UNiversity. http://web.princeton.edu/sites/ehs/hazardcommguide/1.htm. Retrieved 11 October 2012.

* 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

Salts and covalent derivatives of the chloride ion

HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | BCl3
B2Cl4 | CCl4 | NCl3
ClN3 | Cl2O
ClO2
Cl2O7 | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | SiCl4 | P2Cl4
PCl3
PCl5 | S2Cl2
SCl2
SCl4 | Cl2 | Ar
KCl | CaCl
CaCl2 | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl2
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5 | Se2Cl2
SeCl4 | BrCl | KrCl
RbCl | SrCl2 | YCl3 | ZrCl3
ZrCl4 | NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl4 | RuCl3 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
CsCl | BaCl2 |  | HfCl4 | TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | Re3Cl9
ReCl4
ReCl5
ReCl6 | OsCl4 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
AuCl3 | Hg2Cl2,
HgCl2 | TlCl | PbCl2,
PbCl4 | BiCl3 | PoCl2,
PoCl4 | AtCl  | RnCl2
FrCl | RaCl2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaCl3 | CeCl3 | PrCl3 | NdCl2,
NdCl3 | PmCl3 | SmCl2,
SmCl3 | EuCl2,
EuCl3 | GdCl3 | TbCl3 | DyCl2,
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3 | LuCl3
AcCl3 | ThCl4 | PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl3 | Fm  | Md  | No  | LrCl3

0.00

(0 votes)

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Lead_tetrachloride&oldid=559014"
*[CID]: Compound ID
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template