Thallium(III) nitrate
Chemical compound
From Wikipedia, the free encyclopedia
Thallium(III) nitrate, also known as thallic nitrate, is a thallium compound with chemical formula Tl(NO3)3.[1] Normally found as the trihydrate, it is a colorless and highly toxic salt which hydrolyses in water to thallium(III) oxide.[2] It is a strong oxidizing agent useful in organic synthesis.
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| Names | |
|---|---|
| IUPAC name
thallium(III) trinitrate | |
| Other names
thallic nitrate | |
| Identifiers | |
3D model (JSmol) |
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.033.918 |
PubChem CID |
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| UNII | |
| UN number | 2727 |
CompTox Dashboard (EPA) |
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| Properties | |
| Tl(NO3)3 | |
| Molar mass | 390.398 g/mol |
| Appearance | colorless solid |
| Density | 3.36 g/cm3 |
| Melting point | 103 °C (217 °F; 376 K) |
| Boiling point | decomposes |
| reacts | |
| Structure | |
| hexagonal | |
| R3 | |
a = 11.821 Å, c = 10.889 Å | |
Lattice volume (V) |
1313.7 Å3 |
| Hazards | |
| GHS labelling: | |
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| Danger | |
| NFPA 704 (fire diamond) | |
| NIOSH (US health exposure limits): | |
IDLH (Immediate danger) |
15 mg/m3 |
| Safety data sheet (SDS) | Fisher Scientific |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Preparation
The trihydrate is prepared by dissolving thallium(III) oxide in concentrated nitric acid at 80 °C, followed by cooling of the resulting solution:[3]
- Tl2O3 + 6 HNO3 → 2 Tl(NO3)3 · 3 H2O
Thallous nitrate does not react with dinitrogen pentoxide to give the anhydrous salt; instead [NO][Tl(NO3)4] is formed.[4]
Structure
Thallium(III) nitrate trihydrate, Tl(NO3)3·3H2O, crystallizes in the hexagonal crystal system and consists of a nine-coordinate thallium center with three bidentate nitrate ligands and three monodentate water ligands.[5]
Organic synthesis
Despite its toxicity, thallium(III) nitrate is sometimes used in the laboratory, such as in the oxidation of methoxyl phenols to quinone acetals:[6]
Another use of thallium(III) nitrate is the oxidization of alkenes to acetals, cyclic alkenes to ring contracted aldehydes, and terminal alkynes to carboxylic acids. Ketones are also oxidized to carboxylic acids or esters in the presence of methanol. Illustrated below is an example of alkene oxidation to an acetal:[6][7]
