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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)
|
137.7 J/mol K | ||
Std molar
entropy (S⦵298) |
232.3 J/mol K | ||
Std enthalpy of
formation (ΔfH⦵298) |
-523 kJ/mol | ||
Gibbs free energy (ΔfG⦵)
|
-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]
The modern synthesis involves dechlorination of boron trichloride using copper. [2][ better source needed]
It can also be formed by the electrical discharge procedure of boron trichloride at low temperatures: [1] [3]
The most efficient synthesis technique uses no dechlorinating metal, instead passing radio-frequency AC current through gaseous boron trichloride. [4]
The compound is used as a reagent for the synthesis of organoboron compounds. For instance, diboron tetrachloride adds to ethylene: [5]
Diboron tetrachloride absorbs hydrogen quickly at room temperature: [3]
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]
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