Diboron tetrachloride
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Names | |||
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Preferred IUPAC name
Diboron tetrachloride | |||
Systematic IUPAC name
Tetrachlorodiborane(4) | |||
Identifiers | |||
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Properties | |||
B2Cl4 | |||
Molar mass | 163.42 g·mol−1 | ||
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 | |||
Heat capacity (C)
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137.7 J/mol K | ||
Std molar
entropy (S⦵298) |
232.3 J/mol K | ||
Std enthalpy of (ΔfH⦵298)formation |
-523 kJ/mol | ||
Gibbs free energy (ΔfG⦵)
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-468.8 kJ/mol | ||
Related compounds | |||
Related compounds
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Diboron tetrafluoride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Diboron tetrachloride is a chemical compound with the formula B2Cl4. It is a colorless liquid.[1]
Synthesis
The modern synthesis involves dechlorination of
better source needed
]
It can also be formed by the electrical discharge procedure of boron trichloride at low temperatures:[1][3]
- BCl3 → BCl2 + Cl
- Cl + Hg (electrode) → HgCl or HgCl2
- 2 BCl2 → B2Cl4
The most efficient synthesis technique uses no dechlorinating metal, instead passing
AC current through gaseous boron trichloride.[4]
Reactions
The compound is used as a
- CH2=CH2 + B2Cl4 → Cl2B–CH2–CH2–BCl2
Diboron tetrachloride absorbs hydrogen quickly at room temperature:[3]
- 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.[4]
References
- ^ )
- ISBN 9780470132500.
- ^ ISSN 0002-7863.
- ^ ISSN 0009-2665.
- ISSN 0002-7863.