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Bromine monofluoride is a quite unstable interhalogen compound with the chemical formula BrF. It can be produced through the reaction of bromine trifluoride (or bromine pentafluoride) and bromine. Due to its lability, the compound can be detected but not isolated: [2] BrF 3 + Br 2 → 3 BrF BrF 5 + 2 Br 2 → 5 BrF Br 2(l) + F 2(g) → 2 BrF (g)
In a highly exothermic reaction, BrF 3 reacts with water to form hydrobromic acid and hydrofluoric acid: BrF 3 + 2 H 2 O → 3 HF + HBr + O 2. BrF 3 is a fluorinating agent, but less reactive than ClF 3. [10] Already at -196 °C, it reacts with acetonitrile to give 1,1,1-trifluoroethane. [11] BrF 3 + CH 3 CN → CH 3 CF 3 + 1 ⁄ 2 Br 2 + 1 ...
ClF and BrF can both be produced by the reaction of a larger interhalogen, such as ClF 3 or BrF 3 and a diatomic molecule of the element lower in the periodic table. Among the hexatomic interhalogens, IF 5 has a higher boiling point (97 °C) than BrF 5 (40.5 °C), although both compounds are liquids at room temperature .
Refractory oxides tend to be only partially fluorinated, but here the derivatives KBrF 4 and BrF 2 SbF 6 remain reactive. Bromine trifluoride is a useful nonaqueous ionising solvent, since it readily dissociates to form BrF + 2 and BrF − 4 and thus conducts electricity. [43] Bromine pentafluoride (BrF 5) was first synthesised in 1930
A molecule is composed of one or more chemical bonds between molecular orbitals of different atoms. A molecule may be polar either as a result of polar bonds due to differences in electronegativity as described above, or as a result of an asymmetric arrangement of nonpolar covalent bonds and non-bonding pairs of electrons known as a full ...
The fluorine–fluorine bond of the difluorine molecule is relatively weak when compared to the bonds of heavier dihalogen molecules. The bond energy is significantly weaker than those of Cl 2 or Br 2 molecules and similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines. [8]
Bromine pentafluoride, BrF 5 This page was last edited on 19 February 2017, at 20:27 (UTC). Text is available under the Creative Commons Attribution-ShareAlike ...
The polarizability of an atom or molecule is defined as the ratio of its induced dipole moment to the local electric field; in a crystalline solid, one considers the dipole moment per unit cell. [1] Note that the local electric field seen by a molecule is generally different from the macroscopic electric field that would be measured externally.