Diboron tetrachloride
 | |
| Names | |
|---|---|
| Preferred IUPAC name
Diboron tetrachloride | |
| Systematic IUPAC name
Tetrachlorodiborane | |
| Identifiers | |
| 13701-67-2 | |
| ChemSpider | 123068 |
| Jmol interactive 3D | Image |
| PubChem | 139548 |
| |
| |
| Properties | |
| B2Cl4 | |
| Molar mass | 163.433 g/mol |
| Appearance | colorless liquid |
| Density | 1.5 g/cm3 (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 | |
| 137.7 J/mol K | |
| Std molar entropy (S |
232.3 J/mol K |
| Std enthalpy of formation (ΔfH |
-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 [77 °F], 100 kPa). | |
| Infobox references | |
Diboron tetrachloride is a chemical compound with the formula B2Cl4. It can be formed by the electrical discharge procedure of boron trichloride at low temperatures.[1]
Synthesis
The electrical discharge procedure of boron trichloride can be divided into three steps:[2]
- BCl3 → BCl2 + Cl
- Cl + Hg(electrode) → HgCl or HgCl2
- 2BCl2 → B2Cl4
Reactions
The compound is used as a reagent for the synthesis of organoboron compounds. For instance, diboron tetrachloride reacts with ethylene:[3]
- CH2=CH2 + B2Cl4 → Cl2BCH2CH2BCl2
The compound absorbs hydrogen quickly at room temperature:[2]
- 3 B2Cl4 + 6H2 → 2 B2H6 + 4 BCl3
References
- ↑ P. L. Timms (1972). Low Temperature Condensation. Advances in Inorganic Chemistry and Radiochemistry. p. 143. ISBN 0-12-023614-1.
- 1 2 Urry, Grant; Wartik, Thomas; Moore, R. E.; Schlesinger, H. I. (1954). Journal of the American Chemical Society 76 (21): 5293. doi:10.1021/ja01650a010. Missing or empty
|title=(help) - ↑ Urry, Grant; Kerrigan, James; Parsons, Theran D.; Schlesinger, H. I. (1954). Journal of the American Chemical Society 76 (21): 5299. doi:10.1021/ja01650a011. Missing or empty
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