Thallium(I) hydroxide

Thallium(I) hydroxide[1]
Names
	IUPAC name thallium(I) hydroxide
	Other names thallous hydroxide
Identifiers
CAS Number	12026-06-1 ;
3D model (JSmol)	Interactive image;
ChemSpider	141413 ;
ECHA InfoCard	100.031.540
PubChem CID	160963;
UNII	847N2ZKW5S ;
CompTox Dashboard (EPA)	DTXSID10894114 ;
	InChI InChI=1S/H2O.Tl/h1H2;/q;+1/p-1 Key: QGYXCSSUHCHXHB-UHFFFAOYSA-M ; InChI=1/H2O.Tl/h1H2;/q;+1/p-1 Key: QGYXCSSUHCHXHB-REWHXWOFAR;
	SMILES [Tl+].[OH-];
Properties
Chemical formula	TlOH
Molar mass	221.390 g/mol
Appearance	yellow needles
Density	7.44 g/cm3
Melting point	decomposes at 139°C
Solubility in water	34.3 g/100g at 18°C
Hazards
Main hazards	Very toxic (T+) Corrosive (C) Dangerous for the environment (N)
EU classification (DSD) (outdated)	T+ C N
NFPA 704 (fire diamond)	0 4 1 COR
Thermochemistry
Std molar; entropy (So298)	88.0 J·mol−1·K−1
Std enthalpy of; formation (ΔfH⦵298)	-238.9 kJ·mol−1
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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	Infobox references

Thallium(I) hydroxide, also called thallous hydroxide, TlOH, is a hydroxide of thallium, with thallium in oxidation state +1.

Synthesis

Thallium(I) hydroxide is obtained from the decomposition of thallium(I) ethoxide in water.[2]

C₂H₅OTl + H₂O → TlOH + C₂H₅OH

This can also be done by direct reaction of thallium with ethanol and oxygen gas.

4 Tl + 2 C₂H₅OH + O₂ → 2 C₂H₅OTl + 2 TlOH

Another method is the reaction between thallium(I) sulfate and barium hydroxide.

Tl₂SO₄ + Ba(OH)₂ → 2 TlOH + BaSO₄

Properties

Thallous hydroxide is a strong base; it dissociates to the thallous ion, Tl⁺, except in strongly basic conditions. Tl⁺ resembles an alkali metal ion, A⁺, such as Li⁺ or K⁺.

References

Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–89, 5–16. ISBN 0-8493-0594-2.
Brauer, Georg; Baudler, Marianne (1975). Handbuch der Präparativen Anorganischen Chemie, Band I. (3rd ed.). Stuttgart: Ferdinand Enke. p. 883. ISBN 3-432-02328-6.

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[hand-1] Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–89, 5–16. ISBN 0-8493-0594-2.

[2] Brauer, Georg; Baudler, Marianne (1975). Handbuch der Präparativen Anorganischen Chemie, Band I. (3rd ed.). Stuttgart: Ferdinand Enke. p. 883. ISBN 3-432-02328-6.