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| Names | |||
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| Preferred IUPAC name Diboron tetrachloride | |||
| Systematic IUPAC name Tetrachlorodiborane(4) | |||
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| Properties | |||
| Chemical formula | B2Cl4 | ||
| Molar mass | 163.42 g·mol | ||
| Appearance | colorless liquid | ||
| Density | 1.5 g/cm (0 °C) | ||
| Melting point | −92.6 °C (−134.7 °F; 180.6 K) | ||
| Boiling point | 65.5 °C (149.9 °F; 338.6 K) | ||
| Thermochemistry | |||
| Heat capacity (C) | 137.7 J/mol K | ||
| Std molar entropy (S298) |
232.3 J/mol K | ||
| Std enthalpy of formation (ΔfH298) |
-523 kJ/mol | ||
| Gibbs free energy (ΔfG) | -468.8 kJ/mol | ||
| Related compounds | |||
| Related compounds | Diboron tetrafluoride | ||
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Infobox references | |||
Diboron tetrachloride is a chemical compound with the formula B2Cl4. It is a colorless liquid.
Synthesis
The modern synthesis involves dechlorination of boron trichloride using copper.
It can also be formed by the electrical discharge procedure of boron trichloride at low temperatures:
- BCl3 → BCl2 + Cl
- Cl + Hg (electrode) → HgCl or HgCl2
- 2 BCl2 → B2Cl4
The most efficient synthesis technique uses no dechlorinating metal, instead passing radio-frequency AC current through gaseous boron trichloride.
Reactions
The compound is used as a reagent for the synthesis of organoboron compounds. For instance, diboron tetrachloride adds to ethylene:
- CH2=CH2 + B2Cl4 → Cl2B–CH2–CH2–BCl2
Diboron tetrachloride absorbs hydrogen quickly at room temperature:
- 3 B2Cl4 + 3 H2 → B2H6 + 4 BCl3
With boranes, it replaces a hydrogen to form dichloroborane(3) and a polyhedral dichloroborane. Heat induces disproportionation back to boron trichloride and a polyhedral boron(I) chloride.
References
- ^ P. L. Timms (1972). Low Temperature Condensation. Academic Press. p. 143. ISBN 0-12-023614-1.
{{cite book}}:|work=ignored (help) - Timms, Peter L. (1979). "Tetrachlorodiborane(4) (Diboron Tetrachloride)". Inorganic Syntheses. Vol. 19. pp. 74–78. doi:10.1002/9780470132500.ch14. ISBN 9780470132500.
- ^ Urry, Grant; Wartik, Thomas; Moore, R. E.; Schlesinger, H. I. (1954). "The Preparation and Some of the Properties of Diboron Tetrachloride, B2Cl4". Journal of the American Chemical Society. 76 (21): 5293–5298. doi:10.1021/ja01650a010. ISSN 0002-7863.
- ^ Morrison, John A. (1991-01-01). "Chemistry of the polyhedral boron halides and the diboron tetrahalides". Chemical Reviews. 91 (1): 35–48. doi:10.1021/cr00001a003. ISSN 0009-2665.
- Urry, Grant; Kerrigan, James; Parsons, Theran D.; Schlesinger, H. I. (1954). "Diboron Tetrachloride, B2Cl4, as a Reagent for the Synthesis of Organo-boron Compounds. I. The Reaction of Diboron Tetrachloride with Ethylene". Journal of the American Chemical Society. 76 (21): 5299–5301. doi:10.1021/ja01650a011. ISSN 0002-7863.
| Boron compounds | |
|---|---|
| Boron pnictogenides | |
| Boron halides | |
| Acids | |
| Boranes | |
| Boron oxides and sulfides | |
| Carbides | |
| Organoboron compounds | |
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